The Lewis structure for disulfur monoxide, S2O, involves establishing eighteen valence electrons from the two sulfur atoms and the oxygen atom. The resulting structure shows each sulfur atom bonded to the central oxygen atom in a resonance structure, with each atom satisfying the octet rule.
Explanation:To draw the Lewis structure for disulfur monoxide (S2O), we begin by determining the total number of valence electrons. Sulfur has six, and with two sulfur atoms, that gives us twelve. Oxygen also has six valence electrons. So, the total is eighteen.
Next, we arrange the atoms to show the skeletal structure. For S2O, both sulfur atoms are bonded to the oxygen atom in the center. This behaves as a resonance structure. We then distribute the remaining electrons so each sulfur has eight: S-S=O
Note that each sulfur atom ends up with eight electrons (an octet), and the oxygen atom also has eight electrons.
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The Lewis structure of disulfur monoxide (S2O) has two sulfur atoms at the center, each connected by a single bond and an oxygen atom connected to a sulfur atom by a single bond. All elements fulfill the octet rule with the current structure and thus no resonance structure is required.
Explanation:The question is asking about the Lewis structure for the molecule disulfur monoxide (S2O). To create the Lewis structure, first count the number of valence electrons. Sulfur has 6 and oxygen has 6, so there is a total of 18 valence electrons in the molecule. We place sulfur atoms as the central atoms connected by a single bond and then place the oxygen atom adjacent to one of the sulfur atoms, also connected by a single bond.
Then, let's distribute remaining electrons to each atom to satisfy the octet rule. If there are too many electrons in the structure, make multiple bonds between S and O. However, in this case, S2O molecule can fully satisfy the octet rule with just single bonds. Double bonds are not needed. Similarly, there are no resonance structures for S2O according to the octet rule, as all the atoms achieve their necessary eight electrons with the initial structure.
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The place where an experiment is conducted is known as the ______. a. Labb. Workplace c. Test environment d. None of the above
Answer: option A. Lab.
Explanation:
Within each group of four atoms or ions presented below. select the species that are isoelectronic with each other:Note: you are not comparing the two columns, only selecting which within each column are isoelectronic with each other-not across the two columns.
Zn Ge²⁺
Fe³⁺ Cl⁻
Mn²⁺ B⁻
Ar C
Answer:
Fe³⁺ and Mn⁺²
B⁻ and C
Explanation:
Isoelectronic are species that have the same number of electrons. A neutral species has the same number of protons and electrons, and the number of protons in the atomic number (Z) found in the periodic table.
A cation (positive ions) lost the numbe of electrons indicate in its charge, and an anion (negative ions) gain the number of electrons indicate in its charge. So, let's identify the number of electrons (e-) in each one the atoms:
First column:
Zn: Z = 30, e- = 30
Fe³⁺: Z = 26, e- = 26 - 3 = 23
Mn⁺²: Z = 25, e- = 25 - 2 = 23
Ar: Z = 18
Isoelectronic: Fe³⁺ and Mn⁺²
Second column:
Ge⁺²: Z = 32, e- = 32-2 = 30
Cl⁻: Z = 17, e- = 17 + 1 = 18
B⁻: Z = 5, e- = 5 + 1 = 6
C: Z = 6, e- = 6
Isoelectronic B⁻ and C
Isoelectronic species are species that contain the same number of electrons.
Each column as we can see is made up of four chemical species which may be ions or neutral atoms. The species that are isoelectronic are those that contain the same number of electrons. We shall now examine the species in each column to determine which ones are isoelectronic.
In the first column, Fe³⁺ and Mn²⁺ are isoelectronic species, they both contain 23 electrons. In the second column, B⁻ and C are isoelectronic species, they both contain six electrons.
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Functional groups create active sites in molecules. The polar part of a molecule that can hydrogen bond to water is said be hydrophilic. Pi (π) bonds create active sites and will react with electron-deficient species. A electronegative heteroatom like nitrogen, oxygen, or a halogen makes a carbon atom ____________ . The nonpolar part of a molecule that is not attracted to water is said to be hydrophobic.
Answer:
Polar/Hydrophilic
Explanation:
Fluorine, Nitrogen and Oxygen are strong electronegative atoms and by definition, Electronegativity is the amount of pull or the high affinity of an atom to electrons.
Polar bond occurs when there is a high difference between the electronegativity value of both atoms that take part in the bond.
A polar molecule has a net dipole from the distribution of its positive and negayive charges. Hydrophobic and Hydrophilic (in chemistry, Polar) are terms dependent on the overall distribution of charge in its molecule.
Therefore, bonds between C-N, C-O and C-Cl are polar covalent bonds a d this is because of the jigh electronegativity possessed by Nitrogen, Oxygen and Chlorine.
The host says that the polar compounds get "stuck" at the hydrophobic core as the reason why polar compounds cannot cross the membrane. Sometimes people even describe this as the hydrophobic core "repels" polar compounds. This reasoning is WRONG! 1. Polar compounds are forming bonds with the water on the outside of the membrane. These bonds are called hydrogen 2. Can polar compounds interact in this same way with the hydrophobic tails of the phospholipids? (yes or no) no 3. Do interactions form between polar compounds and the hydrophobic tails? (yes or no) no 4. In order for a polar compound to enter into the hydrophobic space of the phospholipid tails, it would need to break the many bonds it has formed with the water and enter into a space where these bonds cannot form. Therefore, it is not a repelling action but a "lack of attraction."
Answer:
1. Some polar compounds form hydrogen bridge bonds with water.
2. Polar compounds DO NOT interact in the same way with hydrophobic phospholipid tails.
3. YES: interactions are formed between polar compounds and hydrophobic tails.
4. False
Explanation:
Hello!
Different types of intermolecular junctions can be formed in the molecules:
-Bridge hydrogen bond: It is formed between a hydrogen attached to a very electronegative element (such as oxygen in water) and another very electronegative element (such as oxygen, fluorine). Polar molecules that contain electronegative elements in their structure may form this junction with water.
-Dipole-dipole union: it is formed between polar molecules where the zone with positive charge density of one molecule approaches the zone with negative charge density of another.
-Dipole-induced dipole union: it is formed between polar molecules where the zone with positive charge density of a molecule causes a non-polar molecule to partially polarize. It is a weak union but becomes important in long hydrophobic chains. It is the union that is established between polar compounds and hydrophobic tails of phospholipids.
For a polar compound to enter the hydrophobic space of the phospholipid tails, the cell usually uses other transport systems other than passive transport such as transport by specialized proteins. Water, despite being a polar molecule, due to its small size it can pass through the membrane at low speed.
The bonds formed with water do not break in aqueous medium. the "lack of attraction" does not exist between the molecules, there is always attraction although it can be of different intensity.
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The question concerns the behavior of polar compounds with the phospholipid bilayer of cell membranes. Polar compounds can't interact with the hydrophobic core, not because the core repels them, but because they'd need to break their existing bonds with water and wouldn't be able to form new bonds within the hydrophobic core.
Explanation:The subject is about how polar compounds interact with the phospholipid bilayer, which forms the structure of cell membranes. Polar compounds form hydrogen bonds with the water molecules outside the membrane due to their polar nature. But they cannot form a similar kind of bond with the hydrophobic tails of the phospholipids, which form the core of the cell membrane.
Hydrophobic substances do not have the necessary conditions to form hydrogen bonds with polar compounds, making them unfavorable for such interactions. For a polar compound to pass through the hydrophobic layer, it would have to break the bonds it has with water and then fail to form any new bonds within the hydrophobic core. This would require a lot of energy and is not favorable, thus making it seem like the hydrophobic core 'repels' polar compounds, when in reality, it's a lack of attraction.
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How many protons and electrons are there in a neutral atom of each of the following elements?a. carbonb. fluorinec. tind. nickel
Answer:
a.Carbon :proton number =6
electron number =6
b. Fluorine: proton number=9
electron number =9
c. tin: proton number=50
electron number =50
d. nickel:proton number=28
electron number =28
Explanation:
In the neutral state of an atom the number of protons is always equal to the number of electrons and that whats makes it electrically neutral as the positive charges of protons balances the negative charges of electrons.
Butadiene c4h6 reacts with itself at 250 degrees celcius to form a dimer with the formula c8h12. The reaction is second order in c4h6. What is the rate law for the reaction?
Answer:
Rate = k * [C₄H₆]²
Explanation:
It is possible to write the reaction as:
2C₄H₆ → C₈H₁₂The differential rate law for a simple second order reaction of the type 2A → B is:
Rate = k * [A]²With the above information in mind, the rate law for the reaction of butadiene would be:
Rate = k * [C₄H₆]²Dimethyl sulfide is the most abundant biological sulfur compound emitted to the atmosphere. It is produced by phytoplankton and emitted over the oceans. Draw the structure of dimethyl sulfide.
The structure of Dimethyl sulfide is H3C-S-CH3. It is produced naturally by some marine algae.
Explanation:
DMS or dimethyl sulfide is formed by using two methyl groups combined with one sulfur atom. It is an organosulphur compound with a structural formula H3C-S-CH3.Most abundant biological sulfur compounds emitted to air and oceans by phytoplankton. DMS is produced naturally by the waste of dimethyl sulphoxide which is disposed into the sewer causing environmental odor problems.It is a flammable liquid that boils at 37 degrees celsius and a disagreeable smell produced from the cooking of certain vegetables also indicates bacterial contamination in the production of malt and brewing.
The periodicity of the properties of elements is chiefly due to the
I) numbers of electrons in the atoms of the elements
II) distribution of electrons in the atoms of the elements
III) numbers of neutrons in the atoms of the elements
a) I only
b) I and III only
c) all of these
d) II only
e) III only
f) II and III only
g) none of these
h) I and II only
The periodic properties of elements are chiefly due to the numbers of electrons in each element's atoms and the distribution of these electrons. These properties don't significantly relate to the neutrons in the atoms. Thus, the correct answer is h) I and II only.
Explanation:The periodicity of the properties of elements is chiefly due to the numbers of electrons in the atoms of the elements and the distribution of electrons in the atoms of the elements. In the periodic table, these properties are mainly arranged by the atomic number of the elements, which determines the number of electrons, and their electronic configuration. More specifically, the arrangement is based on the number of protons (nuclear charge) and how the electrons are distributed in energy levels/shells around the nucleus.
So, the answer is h) I and II only.
The number of neutrons does not significantly affect periodic properties as the nature of an atom is primarily defined by its number of protons and electrons.
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Final answer:
The answer is (h) I and II only, where periodicity is primarily due to the number and distribution of electrons, which are related to the atomic number. The number of neutrons does not impact periodicity.
Explanation:
The periodicity of the properties of elements is chiefly due to the distribution of electrons in the atoms of the elements and the overall number of electrons, which correspond to their atomic number. The correct answer to the question is hence, option (h) I and II only. The number of protons in an atom (which is equivalent to the number of electrons in a neutral atom) and how these electrons are distributed among the different energy levels, or shells, determine the chemical and physical properties of an element.
Various properties such as atomic radius, ionization energy, and electron affinity can be understood through the element's position on the periodic table. Neutrons do not affect the chemical properties of elements and are thus irrelevant to periodicity. The specific arrangement of electrons, particularly in the outermost shells or valence shells, influences how an element reacts chemically and thus its placement in the periodic table.
When your body metabolizes sugar (glucose), 2.8 MJ of heat is produced for every mole of sugar that is burned. How much heat will be released when 0.25 moles of glucose in a can of soda is metabolized? Express your answer in kilojoules (kJ) using the correct number of significant figures.
Answer: [tex]7.0\times 10^2kJ[/tex] will be released when 0.25 moles of glucose in a can of soda is metabolized
Explanation:
Heat of combustion is the amount of heat released on complete combustion of 1 mole of substance.
Given :
Amount of heat released on combustion 1 mole of glucose = 2.8 MJ = [tex]2.8\times 10^3kJ[/tex] [tex]1MJ=10^3kJ[/tex]
Thus we can say:
1 mole of glucose on combustion releases = [tex]2.8\times 10^6J[/tex]
Thus 0.25 moles of glucose on combustion releases =[tex]\frac{2.8\times 10^3kJ}{1}\times 0.25=7.0\times 10^2kJ[/tex]
Thus [tex]7.0\times 10^2kJ[/tex] will be released when 0.25 moles of glucose in a can of soda is metabolized
A chemist must prepare 275. mL of 1967, ?? aqueous copper(II) fluoride (Cur) working solution. He'll do this by pouring out some 2.63 T-aqueous copper(II) fluoride stock solution into a graduated cylinder and diluting it with distilled water. Calculate the volume in mL of the copper(II) fluoride stock solution that the chemist should pour out. Be sure your answer has the correct number of significant digits mL
Answer:
206 mL
Explanation:
In the annexed picture you can see your same question, just in another format.
First we calculate the total moles of CuF₂ that are required in the working solution:
1967 μM ⇒ 1967 / 10⁶ = 1.967 x10⁻³M
1.967 x10⁻³M * 0.275 L = 5.409x10⁻⁴ mol
Now we divide those moles by the concentration of the stock solution, to calculate the volume:
5.409x10⁻⁴ mol ⇒ 5.409x10⁻⁴ * 1000 = 0.5409 mmol
0.5409 mmol ÷ (2.63 mmol/L) = 0.206 L
0.206 L ⇒ 0.206 * 1000 = 206 mL
Indicate whether each of the following statements is TRUE or FALSE 1. A sharp melting point for a crystalline organic material always indicates a pure single compound 2. A molecular size impurity always lowers the melting point of an organic compound 3. If the addition of a sample of compound A to compound B does not change the melting point of B, A and B must be identical 4. An eutectic mixture has a sharp melting point Answer 4 Melting and freezing points of a pure compound are identical
Answer:1. False, 2. False, 3. True, 4. True
Explanation:
1. FALSE. Pure crystalline solids have sharp melting points, while the present of impurity lower the melting point. This is True, but the exception is a eutectic mixture. A properly mixed eutectic mixture have a sharp melting point also.
2. FALSE, although the present of impurity lower the melting point of a organic compound, but if a molecular size impurity with a significantly higher melting point and is present in large quantities the melting point of the organic compound will not be lowered.
3. TRUE, two compounds with same melting point, when mixed together will not change the melting point of either compounds. But if A has higher MP than B and the addition of A to B creates mixture with same melting point as pure A then the statement will be false.
4. TRUE, a properly mixed eutectic mixture will have a sharp melting point.
Melting point and freezing point of a pure compound will be identical because the liquid form of a pure substance when cooled it forms a stable arrangement that supercooling is prevented, freezing occur at the same temperature at which the pure solid phase melts
In a photoelectric effect experiment, electrons are ejected from a titanium surface (work function, 3 eV) following irradiation with UV light. The energy of the incident UV light is 7.2 x 10-19 J.
(a) Calculate the wavelength of the ejected electrons.
(b) Calculate the wavelength of the incident UV light.
(c) would an iron surface (Ф-4.7 eV require a longer or shorter wavelength of light to eject electrons with the same wavelength calculated in part (a)? Briefly explain.
Explanation:
According to the Einstein law, it is known that
[tex]h \times \nu = \phi + \frac{1}{2} mv^{2}[/tex]
where, h = energy of light
[tex]\phi[/tex] = work function
[tex]m v^{2}[/tex] = kinetic energy of electron
It is given that the value of [tex]h \nu[/tex] is [tex]7.2 \times 10^{-19} J[/tex]. And,
1 eV = [tex]1.6 \times 10^{-19} J[/tex]
Here, [tex]\phi[/tex] for titanium is 4.33 eV
= [tex](4.33 \times 1.6 \times 10^{-19})[/tex] J
= [tex]6.928 \times 10^{-19}[/tex] J
(a) First of all, kinetic energy will be calculated as follows.
[tex]\frac{1}{2}mv^{2} = h \nu - \phi[/tex]
= [tex](7.2 \times 10^{-19} - 6.92 \times 10^{-19})[/tex] J
= [tex]0.272 \times 10^{-19}[/tex] J
It is known that mass of electrons is equal to [tex]9.109 \times 10^{-31} kg[/tex].
Therefore, [tex]mv^{2} = 0.544 \times 10^{-19} J[/tex]
and, [tex](mv)^{2} = 9.109 \times 0.544 \times 10^{-19} \times 10^{-31}[/tex]
= [tex]4.955 \times 10^{-50}[/tex]
mv = [tex]2.225 \times 10^{-25}[/tex]
Now, the relation between wavelength and mv is as follows.
[tex]\lambda = \frac{6.626 \times 10^{-34}}{2.225 \times 10^{-25}}[/tex]
= [tex]2.98 \times 10^{-9} m[/tex]
Therefore, the wavelength of the ejected electrons is [tex]2.98 \times 10^{-9} m[/tex].
(b) It is known that relation between energy and wavelength is as follows.
E = [tex]h \nu = \frac{hc}{\lambda}[/tex]
[tex]\lambda = \frac{6.626 \times 10^{-34} \times 3 \times 10^{8}}{7.2 \times 10^{-19}}[/tex]
= [tex]\frac{6.626 \times 3 \times 10^{-26}}{7.2 \times 10^{-19}}[/tex]
= [tex]2.76 \times 10^{-7} m[/tex]
Hence, the wavelength of the ejected electrons is [tex]2.76 \times 10^{-7} m[/tex].
(c) For iron surface, [tex]\phi = 4.7 eV[/tex]
= [tex](4.7 \times 1.6 \times 10^{-19})[/tex] J
= [tex]7.52 \times 10^{-19}[/tex] J
Here, the value of [tex]\phi[/tex] is more than the value of UV light source. Hence, we need a shorter wavelength light as we know that,
[tex]E \propto \frac{1}{\lambda}[/tex]
Therefore, lesser will be the wavelength higher will be the energy.
Final answer:
In a photoelectric effect experiment, the wavelength of the ejected electrons can be calculated using the equation E = h / λ, where E is the energy of the electron, h is Planck's constant, and λ is the wavelength. The wavelength of the ejected electrons is found to be 13.8 femtometers. The wavelength of the incident UV light can be calculated using the same equation and is found to be 9.2 picometers. For an iron surface with a higher work function, a longer wavelength of light would be required to eject electrons with the same wavelength.
Explanation:
(a) To calculate the wavelength of the ejected electrons, we can use the equation E = h / λ, where E is the energy of the electron, h is Planck's constant (6.626 x 10^-34 J*s), and λ is the wavelength.
We can rearrange the equation to solve for λ: λ = h / E.
When we substitute the energy of the ejected electrons as given (3 eV = 4.8 x 10^-19 J), we get λ = (6.626 x 10^-34 J*s) / (4.8 x 10^-19 J) = 13.8 x 10^-15 m, or 13.8 femtometers.
(b) To calculate the wavelength of the incident UV light, we can use the same equation E = h / λ, but this time substitute the energy of the incident light (7.2 x 10^-19 J) and solve for λ. We get λ = (6.626 x 10^-34 J*s) / (7.2 x 10^-19 J) = 9.2 x 10^-16 m, or 9.2 picometers.
(c) The work function of an iron surface is provided (4.7 eV). Since the work function represents the minimum energy required to eject an electron, a longer wavelength of light would be required to eject electrons with the same calculated wavelength in part (a). This is because longer wavelength light corresponds to lower energy photons.
How many milliliters of a 2.0 molar sodium chloride solution would be needed to prepare 250 mL of 0.15 molar sodium chloride solution?
Answer:
18.75 mL
Explanation:
We must apply the dilute factor formula to solve this:
Diluted volume . Diluted M = Concentrated volume . concentrated M
250 mL . 0.15 M = Concentrated volume . 2 M
(250 mL . 0.15 M) / 2M = Concentrated volume
18.75 mL = Concentrated volume
Rubbing alcohol contains 585 g isopropanol (C3H7OH) in 1000 mL of solution (aqueous solution). Calculate the molarity.
Answer:
The molarity of the solution is 9.73 M
Explanation:
Step 1: Data given
Mass of isopropanol = 585 grams
Molar mass of isopropanol = 60.1 g/mol
Volume = 1000 mL = 1 L
Step 2: Calculate moles of isopropanol
Moles isopropanol = mass isopropanol / molar mass isopropanol
Moles isopropanol = 585 grams / 60.1 g/mol
Moles isopropanol = 9.73 moles
Step 3: Calculate molarity of the solution
Molarity = moles / volume
Molarity = 9.73 moles / 1L
Molarity = 9.73 M
The molarity of the solution is 9.73 M
Nitrogen dioxide decomposes to nitric oxide and oxygen via the reaction: 2NO2 → 2NO + O2 In a particular experiment at 300 °C, [NO 2 ] drops from 0.0100 to 0.00650 M in 100 s. The rate of disappearance of NO2 for this period is __________ M/s.
The correct answer is "0.000035 M/s". The rate of disappearance of NO₂ in the reaction is 0.000035 M/s, found by dividing the change in concentration of NO₂ (-0.00350 M) by the time period (100 s).
The rate of disappearance of NO₂ in the reaction 2NO₂
ightarrow 2NO₂ + NO₂ can be calculated using the change in concentration of NO₂ over time. We are given that the concentration of NO₂ drops from 0.0100 to 0.00650 M in 100 seconds.
First, we calculate the change in concentration (also known as the concentration difference):
Concentration difference = Final concentration - Initial concentration = 0.00650 M - 0.0100 M = -0.00350 M (a negative sign indicates disappearance).
To find the rate of disappearance, we divide the concentration difference by the time period:
Rate of disappearance = Concentration difference / Time period
Rate of disappearance = -0.00350 M / 100 s = -0.000035 M/s
Since we are interested in the rate of disappearance, we take the absolute value of the result, making it 0.000035 M/s.
The rate of disappearance of NO2 for the given period is [tex]\( 3.5 \times 10^{-5} \) M/s.[/tex]
To find the rate of disappearance of NO2, we need to calculate the change in concentration of NO2 over time. The reaction given is:
[tex]\[ 2NO_2 \rightarrow 2NO + O_2 \][/tex]
From the problem, we have the initial concentration of NO2 as 0.0100 M and the final concentration as 0.00650 M. The time taken for this change in concentration is 100 seconds.
The rate of disappearance of NO2 can be calculated using the formula:
[tex]\[ \text{Rate} = -\frac{\Delta [NO_2]}{\Delta t} \][/tex]
where [tex]\( \Delta [NO_2] \)[/tex] is the change in concentration of NO2, and [tex]\( \Delta t \)[/tex] is the change in time.
The change in concentration of NO2 is:
[tex]\[ \Delta [NO_2] = [NO_2]_{\text{initial}} - [NO_2]_{\text{final}} \][/tex]
[tex]\[ \Delta [NO_2] = 0.0100 \, \text{M} - 0.00650 \, \text{M} = 0.00350 \, \text{M} \][/tex]
The change in time is:
[tex]\[ \Delta t = t_{\text{final}} - t_{\text{initial}} \][/tex]
[tex]\[ \Delta t = 100 \, \text{s} - 0 \, \text{s} = 100 \, \text{s} \][/tex]
Now, we can calculate the rate:
[tex]\[ \text{Rate} = -\frac{0.00350 \, \text{M}}{100 \, \text{s}} \][/tex]
[tex]\[ \text{Rate} = -3.5 \times 10^{-5} \, \text{M/s} \][/tex]
The negative sign indicates that the concentration of NO2 is decreasing over time. However, the rate of disappearance is typically reported as a positive value, so we take the absolute value:
[tex]\[ \text{Rate} = 3.5 \times 10^{-5} \, \text{M/s} \][/tex]
The following reaction plays a key role in the destruction of ozone In the atmosphere:
Cl(g) + O3(g)--> ClO(g) + O2(g)
Given that S degree for CIO is 218.9J/(mol. K), use standard molar entropies (S degree) to calculate the delta S for this reaction.
Answer:
19.91 J/K
Explanation:
The entropy is a measure of the randomness of the system, and it intends to increase in nature, thus for a spontaneous reaction ΔS > 0.
The entropy variation can be found by:
ΔS = ∑n*S° products - ∑n*S° reactants
Where n is the coefficient of the substance. The value of S° (standard molar entropy) can be found at a thermodynamic table.
S°, Cl(g) = 165.20 J/mol.K
S°, O3(g) = 238.93 J/mol.K
S°, O2(g) = 205.138 J/mol.K
So:
ΔS = (1*205.138 + 1*218.9) - (1*165.20 + 1*238.93)
ΔS = 19.91 J/K
A chemist adds .25L of a .11M potassium dichromate solution to a reaction flask. Calculate the mass in grams of potassium dichromate the chemist has added to the flask. Round your answer to significant digits.
Answer: 8.2 grams of potassium dichromate the chemist has been added to the flask.
Explanation:
Molarity is defined as the number of moles of solute dissolved per liter of the solution.
To calculate the number of moles for given molarity, we use the equation:
[tex]\text{Molarity of the solution}=\frac{\text{Moles of solute}}{\text{Volume of solution (in L)}}[/tex] .....(1)
Molarity of potassium dichromate solution = 0.11 M
Volume of solution = 0.25 L
Putting values in equation 1, we get:
[tex]0.11M=\frac{\text{Moles of potassium dichromate}}{0.25L}\\\\{\text{Moles of potassium dichromate}}={0.11mol/L\times 0.25L}=0.028mol[/tex]
Mass of potassium dichromate =[tex]moles\times {\text {molar mass}}=0.028mol\times 294g/mol=8.2g[/tex]
Thus mass in grams of potassium dichromate the chemist has added to the flask is 8.2.
To calculate the mass of potassium dichromate, use the equation moles = volume (L) × concentration (mol/L), and then multiply the moles by the molar mass of K₂Cr2O7. Round your answer to the correct number of significant digits.
Explanation:To calculate the mass of potassium dichromate that the chemist added to the flask, we can use the equation:
moles = volume (L) × concentration (mol/L)
First, convert the volume to liters by dividing it by 1000. Then, use the equation with the given volume and concentration to find the moles of potassium dichromate. Finally, multiply the moles by the molar mass of potassium dichromate to get the mass in grams. The molar mass of K₂Cr2O7 is 294.185 g/mol.
mass = moles × molar mass
Make sure to round your answer to the correct number of significant digits based on the given information.
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If you want to dissolve 91.6 g of KCl in 200 g of water, what temperature should the water be?
Answer:
The temperature of water will be 60 degree Celsius.
Explanation:
For every chemical there present a particular solubility temperature. The phenomenon occurs as the positive charge is attracted towards the negative and hence gives rise to a cohesive structure. When the polar compounds as well as the ions gets added to the water, they start getting into smaller parts and hence dissolve and becomes solution. The partial charge of water starts attracting different parts of the compound and makes them soluble in water.
Final answer:
To dissolve 91.6 g of KCl in 200 g of water, a temperature higher than 25°C will likely be necessary, but an exact temperature cannot be provided without specific solubility data for KCl.
Explanation:
To determine the temperature at which 91.6 g of KCl (potassium chloride) will dissolve in 200 g of water, we need to refer to the solubility data for KCl. Solubility tables or graphs provide this information and show the amount of a solute that can dissolve in a solvent at various temperatures. Generally, the solubility of ionic compounds like KCl increases with temperature. Without specific solubility data for KCl at different temperatures, an exact answer cannot be provided. However, it is known that at 25°C (77°F), approximately 34 g of KCl will dissolve in 100 mL of water. Therefore, for 91.6 g of KCl, a temperature higher than 25°C will likely be necessary to dissolve the entire amount in 200 g of water. More accurate determination requires a solubility chart or experimental data for KCl.
A neutral atom and an ion of the same element have the same number of _______. They have a different number of _______ and hence reactivity.
Answer:
a. Protons
b. Electrons
Explanation:
The atomic number of an element is also the proton number. Since the atom is neutral, the proton number and the electron number are equal. But this is different for an ion in that the element has either gain or loss an electron and so, the electron number differ from the proton number.
Mole, in the context of this book, is taken in units of gram-mole. On this basis, how many atoms are there in a pound-mole of a substance
Final answer:
A pound-mole of a substance contains approximately 6.022 × 10²³ × 453.592 atoms, as Avogadro's number is used in the definition of a mole, which is based on grams, and needs to be converted using the pound-to-gram conversion factor.
Explanation:
The concept of mole is fundamental in chemistry for measuring quantities of substances. When referring to a pound-mole is equivalent to the number of atoms in a substance weighing one pound. However, Avogadro's number, which is 6.022 × 10²³, is defined based on the international standard mole unit, which is mass in grams. To convert between the pound-mole and the gram-mole, one must use the conversion factor between pounds and grams. Since 1 pound is equal to approximately 453.592 grams, a pound-mole will contain Avogadro's number multiplied by the ratio between the pound and grams (453.592). Therefore, there are approximately 6.022 × 10²³ × 453.592 atoms in a pound-mole of a substance.
What is the pH of 100 mL of a 50 mM solution of benzoic acid is added to 70 mL of a 50 mM NaOH solution?
Answer: The pH of the solution is 4.57
Explanation:
To calculate the number of moles for given molarity, we use the equation:
[tex]\text{Molarity of the solution}=\frac{\text{Moles of solute}\times 1000}{\text{Volume of solution (in mL)}}[/tex]
For benzoic acid:Molarity of benzoic acid = 50 mM = 0.05 M (Conversion factor: 1 M = 1000 mM)
Volume of solution = 100 mL
Putting values in above equation, we get:
[tex]0.05M=\frac{\text{Moles of benzoic acid}\times 1000}{100mL}\\\\\text{Moles of benozic acid}=\frac{(0.05\times 100)}{1000}=0.005mol[/tex]
For sodium hydroxide:Molarity of sodium hydroxide = 50 mM = 0.05 M
Volume of solution = 70 mL
Putting values in above equation, we get:
[tex]0.05M=\frac{\text{Moles of sodium hydroxide}\times 1000}{50mL}\\\\\text{Moles of sodium hydroxide}=\frac{0.05\times 70}{1000}=0.0035mol[/tex]
The chemical reaction for sodium hydroxide and benzoic acid follows the equation:
[tex]C_6H_5COOH+NaOH\rightarrow C_6H_5COONa+H_2O[/tex]
Initial: 0.005 0.0035
Final: 0.0015 - 0.0035
Volume of solution = 100 + 70 = 170 mL = 0.170 L (Conversion factor: 1 L = 1000 mL)
To calculate the pH of acidic buffer, we use the equation given by Henderson Hasselbalch:
[tex]pH=pK_a+\log(\frac{[salt]}{[acid]})[/tex]
[tex]pH=pK_a+\log(\frac{[C_6H_5COONa]}{[C_6H_5COOH]})[/tex]
We are given:
[tex]pK_a[/tex] = negative logarithm of acid dissociation constant of benzoic acid = 4.2
[tex][C_6H_5COONa]=\frac{0.0035}{0.170}[/tex]
[tex][C_6H_5COOH]=\frac{0.0015}{0.170}[/tex]
pH = ?
Putting values in above equation, we get:
[tex]pH=4.2+\log(\frac{0.0035/0.170}{0.0015/0.170})\\\\pH=4.57[/tex]
Hence, the pH of the solution is 4.57
Whenever a substance is oxidized,
1. it gains electrons.
2. some other substance must be reduced.
3. it is called the oxidizing agent.
4. hydronium ions are produced.
Answer: some other substance must be reduced.
Explanation:
Oxidation-reduction reaction or redox reaction is defined as the reaction in which oxidation and reduction reactions occur simultaneously.
Oxidation reaction is defined as the reaction in which a substance looses its electrons. The oxidation state of the substance increases.
[tex]M\rightarrow M^{n+}+ne^-[/tex]
The substance which gets oxidized itself reduces others and thus is called as reducing agent.
Reduction reaction is defined as the reaction in which a substance gains electrons. The oxidation state of the substance gets reduced.
[tex]M^{n+}+ne^-\rightarrow M[/tex]
The substance which gets itself reduced , oxidise others and thus is called as oxidising agent.
Oxidation is the loss of electrons and is usually coupled with the reduction of another substance, known as the oxidizing agent. The production of hydronium ions is not a core characteristic of all oxidation processes.
Explanation:Whenever a substance is oxidized, it means that it has lost electrons. This process is usually coupled with the reduction of another substance, which gains the electrons. Thus, statement 1 is incorrect, and statement 2 is correct: when a substance is oxidized, another substance must be reduced.
Statement 3 is also correct: a substance that is oxidized and causes the reduction of another substance is called the oxidizing agent. Statement 4 is incorrect: the production of hydronium ions is not a general characteristic of oxidation reactions, it’s specific to certain reactions that involve acids.
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Draw the structural formula for 1-octyne. Click the "draw structure" button to launch the drawing utility.
Answer:
Explanation:
1 - Octyne is a member of the Alkyne family. Alkyne has a general formular is CnH2n-2 which is a homologous series with a least one carbon - carbon triple bond.
Where n is the number of carbon atoms needed in the structure.
The "1" prefix is an indicator for where the triple bond of the compound will be found which is at carbon -1. Because of its triple bond it is termed an unsaturated hydrocarbon. Their properties include:
1. Highly reactivity
2. Hydrophobic compound.
Octa- decribes the number of carbon atoms present in the compound which is 8. Also note that, it is not a cycloalkyne but a straight chain compound with a triple bond at one end.
So using the general formular, CnH2n-2
For n = 8,
1-Octyne is C8H14
Below in the attac is the structural formula of 1 - Octyne
Answer:
Explanation:
1-Octyne is a member of the Alkyne series, Alkyne is a homologous series with the general molecular formula;
CnH2n-2
n is a positive whole number which equal to or greater than 2.
i.e n= number of carbon given
In the case of the compound given (1-Octyne), the prefix “Oct” means 8, which is the number of
carbon atoms present in the compond while the suffix “yne” is
coined from the family name “Alkyne”
Therefore, C8H(2x 8) – 2 = C8H16-2 = C8H14
It is an unsaturated hydrocarbon, each alkyne molecule contains four hydrogen atoms
corresponding to alkane and two hydrogen atom less than the corresponding alkene. This is because
each alkyne molecule contains a carbon-carbon triple bond, where two carbon atoms are bonded
to each other by the sharing of three pairs of electrons.
The Alkyne family show a higher degree of unsaturation than the alkenes, hence they are chemically
reactive than alkane and alkene .
In the isothermal reversible compression of 52.0 mmol of a perfect gas at 260 K, the volume of gas is reduced from 300 cm3 to 100 cm3 , calculate w for this process
Answer:
The work done is 123.5 J
Explanation:
Given that:-
Temperature = 260 K
The expression for the work done is:
[tex]W=-nRT \ln \left( \dfrac{V_2}{V_1} \right)[/tex]
Where,
n is the number of moles = 52.0 mmol = [tex]52.0\times 10^{-3}\ moles[/tex]
W is the amount of work done by the gas
R is Gas constant having value = 8.314 J / K mol
T is the temperature
V₁ is the initial volume = 300 cm³
V₂ is the final volume = 100 cm³
Applying in the equation as:
[tex]W=-52.0\times 10^{-3}\ moles\times 8.314\ J/Kmol\times 260\ K \ln \left( \dfrac{100\ cm^3}{300\ cm^3} \right)[/tex]
[tex]W=-52.0\times 10^{-3}\times 8.314\times 260 \ln \left( \dfrac{100}{300} \right)\ J=123.5\ J[/tex]
The work done is 123.5 J
The work done in the isothermal reversible compression of an ideal gas, where the volume of gas was reduced from 300 cm3 to 100 cm3 is about 284 J.
Explanation:In the given problem, we're dealing with isothermal reversible compression of an ideal gas. Under these conditions, the work done (w) can be calculated using the formula: w = -nRT ln(Vf/Vi), where n is the number of moles, R is the gas constant, T is the temperature, Vi is the initial volume, and Vf is the final volume.
Here, n = 52.0 mmol = 0.052 mol, R = 8.314 J / (mol·K) (in these units to match those of the problem), T = 260 K, Vi = 300 cm3 = 0.3 L, and Vf = 100 cm3 = 0.1 L.
Plugging these values into the formula, we get:
w = -0.052 mol * 8.314 J / (mol·K) * 260 K * ln(0.1/0.3)
Therefore, the work done in this isothermal reversible compression where the volume of gas was reduced from 300 cm3 to 100 cm3 is approximately 284 J.
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Which of the following gases is expected to be most soluble in water? Explain your reasoning. (a) CH4 (b) CCl4 (c) CHCl3
Answer: (c) CHCl3
Explanation:
From the rule : a polar solvent will dissolve a polar compound and a non polar solvent will also dissolves a non polar compound.
(a) CH4 is non- polar and water is a polar solvent. Therefore CH4 is not soluble in water
(b) CCl4 is non polar and water is a polar solvent. Therefore CCl4 is not soluble in wtaer
(c) CHCl3 is polar molecule and water is also a polar solvent.
Therefore CHCl3 is expected to be most soluble in water
Among CH4, CCl4, and CHCl3, CHCl3 (chloroform) is expected to be the most soluble in water due to its somewhat polar nature which corresponds with the polarity of water.
Explanation:The gas expected to be most soluble in water among CH4, CCl4, and CHCl3 is CHCl3. This is based on the principle of 'like dissolves like'. In terms of polarity, water is polar and CHCl3 (chloroform) is also somewhat polar due to the presence of chlorine atoms, which have higher electronegativity. Since polar molecules are more likely to dissolve in another polar substance, CHCl3 would be the most soluble of the given gases in water.
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A chemist mixes 96.2 g of chloroform with 31.2 g of acetone and 98.1 g of acetyl bromide. Calculate the percent by mass of each component of this solution Be sure each of your answer entries has the correct number of significant digits. acetyl bromide
The percent by mass of acetyl bromide in the given solution can be calculated by dividing its mass by the total mass of the solution and then multiplying by 100%, leading to a result of 43.5%.
Explanation:To calculate the percent by mass of each component in the solution, we first need to find the total mass of the solution. The total mass is the sum of the mass of chloroform, acetone, and acetyl bromide, which is 96.2 g + 31.2 g + 98.1 g = 225.5 g.
Next, we calculate the percent by mass for each substance by dividing the mass of each substance by the total mass and then multiplying it by 100%.
For acetyl bromide, it's (98.1 g / 225.5 g) * 100% = 43.5%.
Please note that the number of significant digits in the answer should match the lowest number of significant digits in the input, that's why it's rounded off to three significant digits.
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How many hydrogen atoms are in 35.0 grams of hydrogen gas? How many hydrogen atoms are in 35.0 grams of hydrogen gas? 4.25 × 1025 2.12 × 1025 1.05 × 1025 2.09 × 1025 none of the above
Answer:
1.05 × 10²⁵ atoms H₂
General Formulas and Concepts:
Atomic Structure
Reading a Periodic TableMolesStoichiometry
Using Dimensional AnalysisExplanation:
Step 1: Define
[Given] 35.0 g H₂
[Solve] atoms H₂
Step 2: Identify Conversions
Avogadro's Number - 6.022 × 10²³ atoms, molecules, formula units, etc.
[PT] Molar Mass of H - 1.01 g/mol
Molar Mass of H₂: 2(1.01) = 2.02 g/mol
Step 3: Convert
[DA] Set up: [tex]\displaystyle 35.0 \ g \ H_2(\frac{1 \ mol \ H_2}{2.02 \ g \ H_2})(\frac{6.022 \cdot 10^{23} \ atoms \ H_2}{1 \ mol \ H_2})[/tex]Simplify [Cancel out units]: [tex]\displaystyle 1.04342 \cdot 10^{25} \ atoms \ H_2[/tex]Step 4: Check
Follow sig fig rules and round. We are given 3 sig figs.
1.04342 × 10²⁵ atoms H₂ ≈ 1.04 × 10²⁵ atoms H₂
Topic: AP Chemistry
Unit: Atomic Structure
Final answer:
To find the number of hydrogen atoms in 35.0 grams of hydrogen gas, we calculated the moles of hydrogen gas and used Avogadro's number. We determined that there are 2.09 × 1025 hydrogen atoms in 35.0 grams of hydrogen gas.
Explanation:
To determine how many hydrogen atoms are in 35.0 grams of hydrogen gas, we use Avogadro's number and the concept of molar mass. The molar mass of hydrogen gas (H2) is 2.0158 grams per mole. First, we calculate the number of moles in 35.0 grams of hydrogen gas:
(35.0 grams H2) ÷ (2.0158 grams/mol) = 17.37 moles H2
Since each mole of hydrogen gas contains two hydrogen atoms, we need to multiply the number of moles by Avogadro's number, which is 6.022 × 1023 atoms/mol:
(17.37 moles H2) × (6.022 × 1023 molecules H2/mol) × (2 atoms H/molecule H2)
After calculating, we find that there are 2.09 × 1025 hydrogen atoms in 35.0 grams of hydrogen gas. Therefore, the correct answer is 2.09 × 1025.
Using the Bohr model, determine the energy in joules of the photon produced when an electron in a Li2+ ion moves from the orbit with n = 2 to the orbit with n = 1.
Answer:
1.472 x 10^-17 J energy of the photon is released (exothermic).
Explanation:
E = –kZ^2 / n^2
k = 2.18 x10^-18 J
Z = atomic number
Li2+ atomic number = 3
Ei = –(2.18 x 10^-18 J) x 3^2 / 2^2 = –4.905 x 10^-18 J
Ef = –(2.18 x 10^-18 J) x 3^2 / 1^2 = –1.962 x 10^-17 J
ΔE = |Ef – Ei| = |(–1.962 x 10^-17 J) – (–4.905 x 10^-18 J)| = 1.472x10^-17
1.472 x 10-17 J energy of the photon is released (exothermic).
Using the Bohr model, [tex]\rm 1.472\times 10^{-17 } J[/tex] is the energy in joules of the photon produced when an electron in a Li2+ ion moves from the orbit with n = 2 to the orbit with n = 1.
A photon is the basic unit of light and electromagnetic radiation. It is a quantum of energy and a carrier of electromagnetic force. Light was assumed to be a continuous wave in classical physics, but scientists found in the early twentieth century that light and other kinds of electromagnetic radiation behave as both waves and particles. This dual nature is a key concept in quantum mechanics.
E =[tex]\rm -kZ^2 / n^2[/tex]
k =[tex]\rm 2.18 \times10^{-18 }[/tex]J
Z = atomic number
[tex]\rm Li^{2+}[/tex] atomic number = 3
Ei =[tex]\rm -(2.18 \times 10^{-18} J) \times 3^2 / 2^2[/tex]
= [tex]\rm -4.905 \times 10^{-18}[/tex] J
Ef = [tex]\rm -(2.18 \times 10^{-18} J) \times 3^2 / 1^2[/tex]
=[tex]\rm -1.962 \times 10^{-17[/tex] J
ΔE = |Ef – Ei|
= |([tex]\rm -1.962 \times 10^{-17}[/tex] J) – ([tex]\rm -4.905 \times 10^{-18 } J[/tex])|
= [tex]\rm 1.472\times 10^{-17 }[/tex] J
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The molecular shape of the SiH2Cl2 molecule is approximately __________ and its dipole moment is ______ .
A. Tetrahedral, zero
B. Tetrahedral, greater than zero
C. trigonal planar, zero
D. trigonal planar, greater than zero
Answer:
A
Explanation:
The molecule would not have a net dipole moment because the dipole moments cancel out. Being a vector quantity, dipole moment is affected by the direction of the dipole. If the dipoles are such that they are oriented opposite each other, theory simply cancel out. Polarity of individual bonds in a molecule does not automatically imply that the molecule must poses a net dipolev moment. The polarity of the Si-H and Si-Cl bonds cancel out cause they are oriented opposite each other hence the molecule is non polar.
The molecular shape of the SiH2Cl2 molecule is approximately tetrahedral and its dipole moment is zero.
MOLECULAR SHAPE:Molecular shape of a molecule refers to the three-dimensional arrangement of the atoms that make up that molecule. In SiH2Cl2 molecule, silicon is a central atom that bonds to 2 atoms of hydrogen and chlorine atoms respectively. Hence, making it a tetrahedral molecule. The polarity of the Si-H and Si-Cl bonds cancel out in the SiH2Cl2 molecule because they are opposite charges, hence the molecule is non polar and have no dipole moment.Learn more about molecular geometry at: https://brainly.com/question/7558603?referrer=searchResultsional
An organic compound absorbs strongly in the IR at 1687 cm1. Its 'H NMR spectrum consists of two signals, a singlet at 2.1 ppm and a multiplet centered at 7.1 ppm. Its mass spectrum shows significant peaks at m/z 120, m/z 105, m/z 77, and m/z 43. This information is consistent with which of the following structures? IV Propose structures for the ions with m/z values of 120, 105,77 and 43 obtained in the mass spectrum of the compound you selected.
This question does not contain the structures of the molecules. The structures in Daylight SMILES format are:
I. C1=CC=CC=C1C(=O)C
II. C1=CC=CC=C1CC=O
III. C1=CC(C)=CC=C1C=O
IV. C1=CC=CC=C1CCC
V. C1=CC=CC=C1C(C)C
The structures are also attached
Answer:
The structure of compound IV is consistent with the information obtained analysis
Proposed structures for the ions with m/z values of 120, 105,77 and 43 are (also attached):
C1=CC=CC=C1C(=[OH0+])C |^1:7|
C1C([CH0+]=O)=CC=CC=1
C1[CH0+]=CC=CC=1
C(#[OH0+])C
respectively
Explanation:
The IR peak at 1687 cm⁻¹ is indicative of an α unsaturated carbonyl carbon. While the 1H NMR singlet is of the methyl group next to carbonyl and the multiplet near 7.1 ppm is a characteristic peak of benzene. This data shows points towards structure I.
Mass spectrum peak at 120 m/z is of molecular ion peak. In the case of carbonyl-containing molecule, this peak is observable. The signal at 105 shows the loss of a methyl group next to the carbonyl. m/z value of 77 is the characteristic cationic peak of benzene, while the peak at 43 infers the formation of acylium ion (RCO+) due to α-cleavage. All this data agrees with the structure of acetophenone (Structure 1)