This question requires the mass of sulfuric acid and a balance equation. The complete question is given below
Question:
According to the following reaction, how many grams of water are produced in the complete reaction of 24.1 grams of sulfuric acid?
H₂SO₄(aq) + Zn(OH)₂(s) ---------> ZnSO₄(aq) + 2H₂O(l)
Answer:
8.85 grams of water is obtained from 24.1 grams of sulfuric acid according to the given reaction
Explanation:
In this problem, the mass of water can be determined by using the balanced chemical equation.
Step 1: Write all data
Molar mass of water = 18 g
Molar mass of sulfuric acid = 98 g
Given mass of sulfuric acid = 24.1 g
Mass of water from reaction = ?
Step 2: Write statement for conversion
Given equation shows that
1 mole of H₂SO₄ gives 2 moles of water
Step 3: Convert moles into molar mass
Convert the moles into molar mass so, the statement becomes,
98 g of H₂SO₄ gives (2)(18) g of water
1 g of H₂SO₄ gives (2)(18)/98 g of water
Step 4: Use given data
24.1 g of H₂SO₄ gives (2)(18)(24.1)/98 g of water
amount of water = 8.85 g
Consider a mixture of four proteins with various molecular weights. A histone molecule weighs 15 kDa, 15 kDa, a p53 molecule weighs 53 kDa, 53 kDa, an actin molecule weighs 42 kDa, 42 kDa, and an IgG molecule weighs 150 kDa. 150 kDa. Arrange the molecules in order of their elution from a gel filtration column.
Answer:
IgGp53ActinHistoneExplanation:
In gel filtration chromatography a porous matrix is used as the stationary phase. The smaller molecules are able to diffuse into this matrix while the larger ones are not. For this reason the larger molecules will elute first, followed by the smaller ones in decreasing order of size.
In other words the largest molecule will elute first and the smallest molecule will elute last:
IgGp53ActinHistoneConstruct a simulated 1H NMR spectrum for ethyl acetate by dragging and dropping the appropriate splitting patterns into the boxes on the chemical shift baseline, and by dragging integration values into the small box above each signal. Items may be used more than once. Peak heights do not represent integration.
Answer:
Triplet at 1.15 ppm
Singlet at 2.02 ppm
Quartet at 4.10 ppm
Explanation:
In ethyl acetate there are three different sets of protons having different surrounding as compared to each other. The predicted ¹H-NMR of ethyl acetate is attached below and following are the signals shown by this compound,
(i) A singlet around 2.02 ppm is a characteristic peak shown by protons at carbon a. This is because there is no proton available on the adjacent carbon so there is no coupling.
(ii) A triplet around 1.15 ppm is a peak shown by protons at carbon c. This is because there are two proton present on the adjacent carbon so, according to (n+1) rule it will give a triplet peak.
(iii) A quartet around 4.10 ppm is a peak shown by protons at carbon b. This is because there are three proton present on the adjacent carbon so, according to (n+1) rule it will give a quartet peak. Also, as it is directly attached to oxygen atom hence, the chemical shift is downfielded or deshielded.
A mineral sample is obtained from a region of the country that has high arsenic contamination. An elemental analysis yields the following elemental composition:
Element Atomic Weight (g/mol) Percent Composition
Ca 40.078 22.3%
As 74.9216 41.6%
O 15.9994 35.6%
H 1.00794 60%
What is the empirical formula of this mineral?
Answer:
CaAsHO₄
Explanation:
The data has a mistake in one of the values there. I believe the mistake is on the hydrogen. So, I'm going to assume the value of Hydrogen is 0.6%, so the total percent composition would be 100.1% (Something better). All you have to do is replace the correct value of H (or the value with the mistaken option) and do the same procedure.
Now, to calculate the empirical formula, we can do this in three steps.
Step 1. Calculate the amount in moles of each element.
In these case, we just divide the percent composition with the molar mass of each one of them:
Ca: 22.3 / 40.078 = 0.5564
As: 41.6 / 74.9216 = 0.5552
O: 35.6 / 15.9994 = 2.2251
H: 0.6 / 1.00794 = 0.5953
Now that we have done this, let's calculate the ratio of mole of each of them. This is doing dividing the smallest number of mole between each of the moles there. In this case, the moles of As are the smallest so:
Ca: 0.5564/0.5552 = 1.0022
As: 0.5552/0.5552 = 1
O: 2.2251/0.5552 = 4.0077
H: 0.5953/0.5552 = 1.0722
Now, we round those numbers, and that will give us the number of atoms of each element in the empirical formula
Step 3. Write the empirical formula with the rounded numbers obtained
In this case we will have:
Ca: 1
As: 1
O: 4
H: 1
The empirical formula would have to be:
CaAsHO₄
You have a 275 mg sample of a compound that contains aluminum and a group 7A element (F, Cl, Br, I or At). This compound reacts with excess silver nitrate as follows ("X" represents the unknown element):
Complete Question:
You have a 275 mg sample of a compound that contains aluminum and a group 7A element (F, Cl, Br, I or At). This compound reacts with excess silver nitrate as follows (“X” represents the unknown element): AlX3 + 3 AgNO3 → 3 AgX + Al(NO3)3. This reaction forms 581 mg of AgX. Identify element X.
Answer:
Br
Explanation:
By the stoichiometry of the reaction, 1 mol of AlX3 will form 3 moles of AgX. If we call the molar mass of X as m, and by the periodic table the molar masses of Al is 26.982 g/mol, and of Ag is 107.87, thus the molar masses of the compounds will be:
AlX3 = 26.982 + 3m
AgX = 107.87 + m
And the mass relationship will be the number of moles multiplied by the molar mass. So, by a simple direct rule of three:
26.982 + 3m g of AlX3 ------------- 3*(107.87 + m) g of AgX
275 mg of AlX3 ----------- 581 mg
825*(107.87 + m) = 15676.542 + 1743m
88992.75 + 825m = 15676.542 + 1743m
-918m = -73316.208
m = 79.86 g/mol
So, comparing with the values of the masses of the group 7 elements, X must be Br (79.904 g/mol).
If the rate of formation of ammonia is 0.345 M/s, what is the rate of disappearance of N2?
Answer: The rate of disappearance of [tex]N_2[/tex] is 0.172 M/s
Explanation:
Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.
[tex]N_2(g)+3H_2(g)\rightarrow 2NH_3(g)[/tex]
The rate in terms of reactants is given as negative as the concentration of reactants is decreasing with time whereas the rate in terms of products is given as positive as the concentration of products is increasing with time.
Rate in terms of disappearance of [tex]N_2[/tex] = [tex]-\frac{1d[N_2]}{dt}[/tex]
Rate in terms of disappearance of [tex]H_2[/tex] = [tex]-\frac{1d[H_2]}{3dt}[/tex]
Rate in terms of appearance of [tex]NH_3[/tex] = [tex]\frac{1d[NH_3]}{2dt}[/tex]
The rate of formation of ammonia is = 0.345 M/s
[tex]\frac{1d[NH_3]}{dt}=0.345 M/s[/tex]
The rate of disappearance of [tex]N_2[/tex] is one by three times the rate of appearance of [tex]NH_3[/tex]
[tex]-\frac{1d[N_2]}{dt}=\frac{d[NH_3]}{2dt}[/tex]
[tex]-\frac{1d[N_2]}{dt}=\frac{0.345M/s}{2}=0.172M/s[/tex]
Thus the rate of disappearance of [tex]N_2[/tex] is 0.172 M/s
If the rate of formation of ammonia is 0.345 M/s, the rate of disappearance of nitrogen is 0.173 M/s.
Let's consider the balanced equation for the formation of ammonia.
N₂(g) + 3 H₂(g) ⇒ 2 NH₃(g)
The molar ratio of N₂ to NH₃ is 1:2. If the rate of formation of ammonia is 0.345 M/s, the rate of disappearance of nitrogen is:
[tex]\frac{0.345molNH_3}{L.s} \times \frac{1molN_2}{2molNH_3} = \frac{0.173molN_2}{L.s} = 0.173 M/s[/tex]
If the rate of formation of ammonia is 0.345 M/s, the rate of disappearance of nitrogen is 0.173 M/s.
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The frequency of stretching vibrations is correlated to the strength and stiffness of the bond between two atoms. This can be thought of as a ball-and-spring model. Using this knowledge, rank the following bonds in each part of the question by increasing frequency.
(a) Alkyne
(b) Alkane
(c) alkene
Answer:
a > c > b
Explanation:
As higher is the strength and stiffness of the bond between two atoms, more stable it is, and more difficult is to these bonds vibrate. So, the stretching vibration decreases when the strength and stiffness increases.
As more bonds are done between the atoms, more strength, and stiffness they have. So, the order of increase is:
simple bond > double bond > triple bond
And the increased frequency of vibration is:
triple bond > double bond > simple bond
An alkane is a hydrocarbon that has only simple bonds between carbons, an alkene is a hydrocarbon with one double bond between carbon, and an alkyne is a hydrocarbon with one triple bond. So, the increase in vibration of them is:
alkyne (a) > alkene (c) > alkane (b)
Answer: (A) < (C) < (B)
Ranking in order of increasing frequency.
Explanation:
what is the kinetic energy of a particle of mass m moving through space with velocity v?
Answer:
Kinetic Energy of the particle is half the mass of the particle multiplied by the square of the velocity of the particle
Explanation:
Kinetic Energy is given by 1/2mv^2
Where, m is the mass of the object and v is the velocity of the object
Answer: kinetic energy is equal to 1/2mv^2
Identify the power of ten that defines each of these prefixes. Input your answers as 10 x where x is the power of ten. nano- _______________. kilo- _______________. centi- _______________. micro- _______________. milli- _______________. mega- _______________.
Answer: The quantity of every prefix is written below as a power of ten.
Explanation:
In the metric system of measurement, the name of multiples and subdivision of any unit is done by combining the name of the unit with the prefixes.
For Example: deka, hecto and kilo means 10, 100 and 1000 respectively. Deci, centi and milli means one-tenth, one-hundredth, and one-thousandth respectively.
The quantity of these prefixes are written as the power of 10.
For the given prefixes:
Nano: The quantity will be [tex]10^{-9}[/tex]
Kilo: The quantity will be [tex]10^3[/tex]
Centi: The quantity will be [tex]10^{-2}[/tex]
Micro: The quantity will be [tex]10^{-6}[/tex]
Milli: The quantity will be [tex]10^{-3}[/tex]
Mega: The quantity will be [tex]10^6[/tex]
Hence, the quantity of every prefix is written above as a power of ten.
Write the rate law for the following elementary reaction:
2N2O5(g) - 2N204 Use k1 to stand for the rate constant.
Answer:
Rate law = k1 [N2O5]^2
Explanation:
Rate law only cares about reactants and rate law can only be determined experimentally or by using the coefficients of reactants in elementary reactions
If 2A---->B is an elementary reaction... rate law for this is rate=k[A]^2
So if we look at your question...2N2O5---->2N2O4 + 02 (I think you are missing O2 in question because otherwise equation is unbalanced)
Rate law = k1 [N2O5]^2
The rate law for the reaction 2N2O5(g) → 2N2O4(g) is rate = k1[N2O5]^2, indicating a second-order dependence on [N2O5]. For the reaction H2(g) + 2NO(g) → N2O(g) + H2O(g), the rate law is rate = k[NO]^2[H2], with the reaction being second order in NO and first order in H2.
Explanation:The rate law for an elementary reaction can be written directly from the stoichiometry of the reaction. Considering the provided elementary reaction 2N2O5(g) → 2N2O4(g), the rate law would be rate = k1[N2O5]^2, which indicates that the reaction is second order with respect to N2O5.
In general, for an elementary reaction like H2(g) + 2NO(g) → N2O(g) + H2O(g), the rate law given is rate = k[NO]^2[H2], which means that the reaction is second order with respect to NO (order of 2) and first order with respect to H2 (order of 1), making the overall order of the reaction three.
What is the mass % of ammonium chloride in a 1.73 M ammonium chloride aqueous solution at 20 °C?
The question is incomplete, here is the complete question:
What is the mass % of ammonium chloride in a 1.73 M ammonium chloride aqueous solution at 20 °C? The density of the solution is 1.0257 g/mL
Answer: The mass percent of ammonium chloride in solution is 9.03 %
Explanation:
We are given:
Molarity of ammonium chloride solution = 1.73 M
This means that 1.73 moles of ammonium chloride is present in 1 L or 1000 mL of solution.
To calculate the mass of solution, we use the equation:[tex]\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}[/tex]
Density of solution = 1.0257 g/mL
Volume of solution = 1000 mL
Putting values in above equation, we get:
[tex]1.0257g/mL=\frac{\text{Mass of solution}}{1000mL}\\\\\text{Mass of solution}=(1.0257g/mL\times 1000mL)=1025.7g[/tex]
To calculate the number of moles, we use the equation:[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]
Moles of ammonium chloride = 1.73 moles
Molar mass of ammonium chloride = 53.5 g/mol
Putting values in above equation, we get:
[tex]1.73mol=\frac{\text{Mass of ammonium chloride}}{53.5g/mol}\\\\\text{Mass of ammonium chloride}=(1.73mol\times 53.5g/mol)=92.6g[/tex]
To calculate the mass percentage of ammonium chloride in solution, we use the equation:[tex]\text{Mass percent of ammonium chloride}=\frac{\text{Mass of ammonium chloride}}{\text{Mass of solution}}\times 100[/tex]
Mass of solution = 1025.7 g
Mass of ammonium chloride = 92.6 g
Putting values in above equation, we get:
[tex]\text{Mass percent of ammonium chloride}=\frac{92.6g}{1025.7g}\times 100=9.03\%[/tex]
Hence, the mass percent of ammonium chloride in solution is 9.03 %
A chemist makes of magnesium fluoride working solution by adding distilled water to of a stock solution of magnesium fluoride in water. Calculate the concentration of the chemist's working solution. Round your answer to significant digits.
The question is incomplete, here is the complete question:
A chemist makes 600. mL of magnesium fluoride working solution by adding distilled water to 230. mL of a stock solution of 0.00154 mol/L magnesium fluoride in water. Calculate the concentration of the chemist's working solution. Round your answer to 3 significant digits.
Answer: The concentration of chemist's working solution is [tex]5.90\times 10^{-4}M[/tex]
Explanation:
To calculate the molarity of the diluted solution (chemist's working solution), we use the equation:
[tex]M_1V_1=M_2V_2[/tex]
where,
[tex]M_1\text{ and }V_1[/tex] are the molarity and volume of the stock magnesium fluoride solution
[tex]M_2\text{ and }V_2[/tex] are the molarity and volume of chemist's magnesium fluoride solution
We are given:
[tex]M_1=0.00154M\\V_1=230mL\\M_2=?M\\V_2=600mL[/tex]
Putting values in above equation, we get:
[tex]0.00154\times 230=M_2\times 600\\\\M_2=\frac{0.00154\times 230}{600}=5.90\times 10^{-4}M[/tex]
Hence, the concentration of chemist's working solution is [tex]5.90\times 10^{-4}M[/tex]
Calculate the amount of heat needed to boil 183.g of ethanol ( CH3CH2OH ), beginning from a temperature of 33.9°C . Round your answer to 3 significant digits. Also, be sure your answer contains a unit symbol.
To calculate the amount of heat needed to boil ethanol, use the formula Q = m * c * ΔT. Convert the temperature to Kelvin, calculate the change in temperature, and then apply the formula to find the amount of heat. The amount of heat needed to boil 183.g of ethanol is 20 kJ.
Explanation:To calculate the amount of heat needed to boil ethanol, we can use the equation:
Q = m * c * ΔT
Where Q is the amount of heat, m is the mass of ethanol, c is the specific heat capacity of ethanol, and ΔT is the change in temperature.
First, we need to calculate the change in temperature:
Convert the temperature from Celsius to Kelvin: 33.9°C + 273.15 = 306.05 KNext, subtract the boiling point of ethanol (78.4°C = 351.55 K) from the initial temperature: ΔT = 351.55 K - 306.05 K = 45.50 KNow we can calculate the amount of heat:
Find the specific heat capacity of ethanol: 2.44 J/g°CApply the formula: Q = 183.g * 2.44 J/g°C * 45.50 KFinally, round the answer to 3 significant digits: Q = 20000 J = 20 kJTherefore, the amount of heat needed to boil 183.g of ethanol is 20 kJ.
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A brick has a mass of and the Earth has a mass of . Use this information to answer the questions below. Be sure your answers have the correct number of significant digits. What is the mass of 1 mole of bricks? How many moles of bricks have a mass equal to the mass of the Earth?
Complete question
A brick has a mass of 4.0 kg and the Earth has a mass of 6.0 X 10²⁷ g. Use this information to answer the questions below. Be sure your answers have the correct number of significant digits. What is the mass of 1 mole of bricks? Round your answer to 2 significant digits. How many moles of bricks have a mass equal to the mass of the Earth? Round your answer to 2 significant digits.
Answer:
The mass of 1 mole of bricks = 24 X 10²⁶ g (2 significant digits), and
2.5 moles of bricks (2 significant digits) have a mass equal to the mass of the Earth.
Explanation:
Given mass of bricks = 4.0 kg
4.0kg of brick = 4000g
1 mole of any substance always contain 6.022 X 10²³ Avogadro's number
1 mole of bricks contains 6.022 X 10²³ bricks
Therefore, mass of 1 mole of brick = 6.022 X 10²³ X 4000g
= 4000 X 6.022 X 10²³ g
= 24088 X 10²³ g
The mass of 1 mole of bricks = 24 X 10²⁶ g (2 significant digits)
-----------------------------------------------------------------------------------------------------
⇒How many moles of bricks have a mass equal to the mass of the Earth?
Given mass of Earth = 6.0 X 10²⁷ g
24088 X 10²³ g --------> mass of 1 mole of bricks
6.0 X 10²⁷ g --------------> ?
= (6.0 X 10²⁷ g)/(24088 X 10²³ g)
= 2.4909 moles of bricks
≅ 2.5 moles of bricks ( 2 significant digits)
Therefore, 2.5 moles of bricks have a mass equal to the mass of the Earth
Answer
2.4x10^27 g
2.5 mol
The gas in a 250. mL piston experiences a change in pressure from 1.00 atm to 4.45 atm. What is the new volume (in mL) assuming the moles of gas and temperature are held constant
Answer:
56.2 mL
Explanation:
Given data
Initial volume (V₁): 250 mLInitial pressure (P₁): 1.00 atmFinal volume (V₂): ?Final pressure (P₂): 4.45 atmAssuming the gas has an ideal behavior, we can find the final volume using Boyle's law.
P₁ × V₁ = P₂ × V₂
V₂ = P₁ × V₁/P₂
V₂ = 1.00 atm × 250 mL/ 4.45 atm
V₂ = 56.2 mL
According to the question,
Volume,
[tex]V_1 = 250 \ mL[/tex][tex]V_2 = \ ?[/tex]Pressure,
[tex]P_1 = 1.00 \ atm[/tex][tex]P_2 = 4.45 \ atm[/tex]By using the Boyle's Law, we get
→ [tex]P_1 V_1 = P_2 V_2[/tex]
or,
→ [tex]V_2 = \frac{P_1V_1}{P_2}[/tex]
By putting the values, we get
[tex]= \frac{1.00\times 250}{4.45}[/tex]
[tex]= \frac{250}{4.45}[/tex]
[tex]= 56.2 \ mL[/tex]
Thus the above answer is right.
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A 27.40 g sample of liquid mercury is initially at 158.30°C. If the sample is heated at constant pressure ( = 1 atm), kJ of energy are needed to raise the temperature of the sample to 376.20°C. How much energy in kJ is required?
Answer:
energy required is 0.247kJ
Explanation:
The formula to use is Energy = nRdT;
Where n is number of mole
R is the molar gas constant
dT is the change in temperature
n = reacting mass of mercury / molar mass of mercury = 27.4/200.59 = 0.137
dT = final temperature - initial temperature = 376.20 - 158.30 = 217.90K
R = 8.314Jper mol per Kelvin
Energy = 0.137 x 8.314 x 217.90 = 247.12J
Energy in kJ= 247.12/1000= 0.247kJ
In a 4.00 L pressure cooker, water is brought to a boil. If the final temperature is 115 °C at 3.10 atm, how many moles of steam are in the cooker?
Answer: 0.39mol of the steam are in the cooker.
Explanation:Please see attachment for explanation
Given:
Volume, V = 4 LPressure, P = 3.10 atmTemperature, T = 115°C= 115+273
= 388 K
We know the relation,
→ [tex]PV = nRT[/tex]
or,
→ [tex]n = \frac{PV}{RT}[/tex]
By substituting the values, we get
[tex]= \frac{4\times 3.1}{0.082\times 388}[/tex]
[tex]= 0.39 \ mol[/tex]
[tex]= 0.39 \ mol[/tex]
Thus the above answer is correct.
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A mixture of xenon and oxygen gas is compressed from a volume of 99.0 L to a volume of 98.0 L, while the pressure is held constant at 69.0 atm. Calculate the work done on the gas mixture. Be sure your answer has the correct sign (positive or negative) and the correct number of significant digits
The work done on the gas mixture when it is compressed from 99.0 L to 98.0 L at a constant pressure of 69.0 atm is -69.0 atm L.
Explanation:In order to calculate the work done on a gas, we can use the equation:
Work = Pressure * Change in Volume
In this case, the pressure is held constant at 69.0 atm, and the change in volume is from 99.0 L to 98.0 L.
Using the formula, we can calculate the work as follows:
Change in Volume = Final Volume - Initial Volume = 98.0 L - 99.0 L = -1.0 LWork = Pressure * Change in Volume = 69.0 atm * -1.0 L = -69.0 atm LThe work done on the gas mixture is -69.0 atm L. The negative sign indicates that work is done on the system rather than by the system.
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An electron is confi ned to a linear region with a length of the same order as the diameter of an atom (about 100 pm). Calculate the minimum uncertainties in its position and speed.
Explanation:
The minimum uncertainty position is 100 nm.
Therefore, by Heisenberg Uncertainty principal
ΔxΔp≥h/2
Δp≥h/(2Δx)
we know that
h= [tex]1.0546\times10^{-34}[/tex] Js
Δx= [tex]100\times10^{-12} m[/tex]
therefore,
[tex]\Delta p =\frac{1.0546\times10^{-34}}{2\times12\times10^{-12}} = 5.3\times10^{-25} kgms^{-1}[/tex]
therefore,
[tex]\Delta v= \frac{\Delta p}{m} =\frac{5.3\times10^{-25}}{9.11\times10^{-31}}= 5.8\times10^{5} ms^{-1}[/tex]
Study this chemical reaction: FeSO4 (aq) + Zn (s) --> Fe (s) + ZnSO4 (aq) Then, write balanced half-reactions describing the oxidation and reduction that happen in this reaction.
oxidation:
reduction:
Answer: The oxidation and reduction half reactions are written below.
Explanation:
Oxidation reaction is defined as the chemical reaction in which an atom looses its electrons. The oxidation number of the atom gets increased during this reaction.
[tex]X\rightarrow X^{n+}+ne^-[/tex]
Reduction reaction is defined as the chemical reaction in which an atom gains electrons. The oxidation number of the atom gets reduced during this reaction.
[tex]X^{n+}+ne^-\rightarrow X[/tex]
For the given chemical reaction:
[tex]FeSO_4(aq.)+Zn(s)\rightarrow Fe(s)+ZnSO_4(aq.)[/tex]
The half reactions for the given reaction follows:
Oxidation half reaction: [tex]Zn(s)\rightarrow Zn^{2+}(aq.)+2e^-[/tex]
Reduction half reaction: [tex]Fe^{2+}(aq.)+2e^-\rightarrow Fe(s)[/tex]
Hence, the oxidation and reduction half reactions are written above.
The balanced half-reaction for oxidation in the reaction is Zn (s) -> Zn2+ (aq) + 2e-, signifying Zinc is being oxidised. The reduction half-reaction is Fe2+ (aq) + 2e- -> Fe (s) demonstrating Iron being reduced.
Explanation:In this chemical reaction:FeSO4 (aq) + Zn (s) --> Fe (s) + ZnSO4 (aq) two processes occur simultaneously; oxidation and reduction. Oxidation involves loss of electrons, and in this case, it is the Zinc metal that gets oxidized. It unites with Sulphate forming ZnSO4 and in the process gains a positive charge by losing 2 electrons.
The balanced half-reaction for oxidation is: Zn (s) --> Zn2+ (aq) + 2e-
Reduction on the other hand involves gain of electrons. Iron in this reaction gains electrons to form metallic iron (Fe). This can be represented by the following balanced half-reaction:
Fe2+ (aq) + 2e- --> Fe (s).
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Which of the following compounds would have the highest boiling point?
a. 1-propanol,
b. CH3CH2CH2OH ethanol,
c. CH3CH2OH dimethyl ether,
d. CH3OCH3 ethyl methyl ether,
e. CH3OCH2CH3
Answer:a. 1-propanol,
Explanation:
Boiling point depends on the relative molecular mass of the compound and the kind of intermolecular interactions present in the substance. 1-propanol has a relative molecular mass of 60 and posses strong intermolecular hydrogen bonding. The presence of hydrogen bonding is known to lead to an increase in boiling point. As a result of this, it is obvious that 1-propanol has the highest boiling point among other compounds in the list.
Final answer:
1-propanol has the highest boiling point among the mentioned compounds due to its ability to form hydrogen bonds, which significantly elevate its boiling point compared to the other options.
Explanation:
The question pertains to determining which of the listed compounds would have the highest boiling point. When comparing boiling points, factors such as molecular mass, polarity, and the presence of hydrogen bonding play crucial roles. Among the options, 1-propanol (C3H7OH) stands out because it is capable of hydrogen bonding, which significantly increases its boiling point compared to the other compounds listed, such as dimethyl ether (CH3OCH3) and ethyl methyl ether (CH3OCH2CH3), which primarily exhibit dipole-dipole interactions and London dispersion forces. Ethanol (CH3CH2OH) also exhibits hydrogen bonding but has a shorter carbon chain than 1-propanol, leading to a slightly lower boiling point.
Which of the following personal items are permitted to be at your workstation in the organic laboratory? Select all that apply. a. Pen or pencil b. Drinking water bottle c. I-Pad d. Lab manual e. Cell phone
Explanation:
While working in a laboratory it is necessary to be free from any kind of distraction. This is because a distraction while working in a laboratory can lead to serious consequences.
For this it is important to put all your electronic devices like mobile phones, tablets etc in your backpack. Also, you should not carry any kind of eatable, water bottle or anything into the lab.
This is because chemicals do react with food items. Hence, then food does not remain fit for consumption.
Thus, we can conclude that pen or pencil and lab manual personal items are permitted to be at your workstation in the organic laboratory.
Calculate the radius of a platinum atom in cm, given that Pt has an FCC crystal structure, a density of 21.4 g/cm3, and an atomic weight of 195.08 g/mol.
Answer:
Radius of platinum atom is [tex]1,38\times10^{-8} \ cm.[/tex]
Explanation:
We know, Density in solid state is also given by , [tex]\rho=\dfrac{Z\times M}{N_A\times a^3}[/tex]
Here, Z= total no of atom or molecule per unit cell. ( Z = 4 for FCC structure )
M = atomic weight = 195.08 gm/mol.
N_A= Avogadro's number = [tex]6.023\times 10^{23} .[/tex]
a= size of side of cube.
Also for, FCC crystal [tex]a=\sqrt2\times 2r[/tex] ....1
Since,[tex]\rho=\dfrac{Z\times M}{N_A\times a^3}\\[/tex]
Therefore, [tex]a^3=\dfrac{Z\times M}{N_A\times \rho}[/tex]
Putting all values , [tex]a=3.9\times 10^{-8} \ cm.[/tex]
Putting value of a in equation 1 we get,
[tex]r=\dfrac{a}{\sqrt2\times2}=1.38\times 10^{-8} \ cm.[/tex]
Hence, this is the required solution.
The radius of a platinum atom can be found using the density, atomic weight, and the nature of the crystal structure. The calculation involves finding the volume of an atom from the atomic weight, density and Avogadro's number and converting this volume to a radius by considering the atom as a sphere.
Explanation:The radius of a platinum atom can be calculated using the density, atomic weight, and the information about the crystal structure (in this case, face-centered cubic or FCC). Platinum (Pt) has a density (d) of 21.4 g/cm3 and an atomic weight (AW) of 195.08 g/mol.
First, let's calculate the number of atoms (n) in the unit cell of an FCC structure. An FCC unit cell has 4 atoms. Avogadro's number (Na) is 6.022 x 1023 mol-1.
The volume (V) of an atom can be calculated as follows: V = AW / (d * n * Na).Now we will calculate the radius (r) from the volume, considering the atom as a sphere: r = ((3*V) / (4*π))1/3.Keep in mind that the values have to be converted to cm in the end.
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A chemist adds of a M zinc nitrate solution to a reaction flask. Calculate the mass in grams of zinc nitrate the chemist has added to the flask. Round your answer to significant digits.
corrected question: A chemist adds 135mL of a 0.21M zinc nitrate solution to a reaction flask. Calculate the mass in grams of zinc nitrate the chemist has added to the flask. Round your answer to significant digits.
Answer:
5.37g
Explanation:
0.21M means ; 0.21mol/dm³
1dm³=1L , so we can say 0.21mol/L
if 0.21mol of Zinc nitrate is contained in 1L of water
x will be contained in 135mL of water
x= 0.21*135*10³/1
=0.02835moles
number of moles= mass/ molar mass
mass= number of moles *molar mas
molar mass of Zn(NO₃)₂=189.36 g/mol
mass= 0.02835 *189.36
mass=5.37g
Calculate the density, in g / mL , of a liquid that has a mass of 0.125 g and a volume of 0.000285 L
Answer:
ρ = 0.439 g/mL
Explanation:
Given data
Mass of the liquid: 0.125 gramsVolume of the liquid: 0.285 milliliters0.000285 L × (1000 mL/ 1 L) = 0.285 mL
The density (ρ) of a liquid is equal to its mass (m) divided by its volume (V).
ρ = m/V
ρ = 0.125 g/0.285 mL
ρ = 0.439 g/mL
The density of the liquid is 0.439 g/mL.
The density of a liquid, defined as mass per unit volume, with given mass of 0.125 grams and volume of 0.000285 liters, can be calculated using the formula: Density = mass/volume. After converting liters to milliliters, the density is approximately 0.439 g/mL.
Explanation:The question is asking for the calculation of the density of a liquid given its mass and volume. Density is a property of matter defined as mass per unit volume. It can be calculated using the formula: Density = mass/volume. In this case, the mass of the liquid is 0.125 grams and the volume is 0.000285 liters. But please note that the density should be presented in g/mL. Therefore, we need to convert the volume from liters to milliliters. 1 liter equals 1000 milliliters, so 0.000285 liters equals 0.285 milliliters. Using the formula, Density = 0.125 g / 0.285 mL which gives us a density of approximately 0.439 g/mL.
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While ethanol is produced naturally by fermentation, e.g. in beer- and wine-making, industrially it is synthesized by reacting ethylene with water vapor at elevated temperatures. A chemical engineer studying this reaction fills a flask with of ethylene gas and of water vapor. When the mixture has come to equilibrium she determines that it contains of ethylene gas and of water vapor. The engineer then adds another of water, and allows the mixture to come to equilibrium again. Calculate the pressure of ethanol after equilibrium is reached the second time. Round your answer to significant digits.
Answer:
Pressure of alcohol after reaching equilibrium the second time = 2.62atm
Explanation:
Detailed step by step with explanation is as shown in the attachment.
write out the acid dissociation reaction for hydrochloric acid. b) calculate the pH of a solution of 5.0 x 10^-4 M HCl. c) write out the acid dissociation reaction for sodium hydroxide. d) calculate the pH of a solution of 7.0 x 10^-5 M NaOH.
Answer:
The answer to your question is below
Explanation:
a) Acid dissociation reaction for HCl
HCl(g) + H₂O(l) ⇒ H⁺¹ (aq) + Cl⁻¹ (aq)
b) pH = -log [H⁺¹]
Concentration = 5 x 10⁻⁴
pH = -log [5 x 10⁻⁴]
pH = 3.3
c) Acid dissociation reaction
NaOH(s) + H₂O ⇒ Na⁺¹(aq) + OH⁻¹(aq)
d) pH
pOH = -log [7 x 10⁻⁵]
pOH = 4.2
pH = 14 - 4.2
pH = 9.8
The acid dissociation and pH for HCl and NaOH were detailed. For HCl, the reaction and solution pH were HCl -> H+ + Cl- and 3.3 respectively. For NaOH, the dissociation and solution pH were NaOH -> Na+ + OH- and 9.8 respectively.
Explanation:a) The acid dissociation reaction for hydrochloric acid (HCl) is as follows:
HCl → H+ + Cl-
b) The pH of a solution of hydrochloric acid can be calculated using the formula:
pH = -log[H+].
As HCl is a strong acid, it will completely ionize in water, meaning the concentration of H+ ions equals the concentration HCl. Therefore, the pH for a 5.0 x 10^-4 M HCl solution is -log(5.0 x 10^-4) = 3.3.
c) Sodium hydroxide is a base, not an acid, so its ionization does not involve releasing protons into the solution, but rather attracting them. It has the following dissociation reaction:
NaOH → Na+ + OH-.
d) As for the pH of a solution of 7.0 x 10^-5 M NaOH, we first need to find the pOH using the formula pOH = -log[OH-], since NaOH being a strong base completely ionizes. This equals -log(7.0 x 10^-5) = 4.2. Given that pH and pOH are related by the expression pH + pOH = 14 at 25°C, we can solve for the pH of the NaOH solution = 14 - pOH = 14 - 4.2 = 9.8.
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Calcium reacts with sulfur forming calcium sulfide. What is the theoretical yield (g) of CaS(s) that could be prepared from 8.54 g of Ca(s) and 2.33 g of sulfur(s)? Do not type units with your answer.
Answer:
5.242
Explanation:
Molar mass of Ca = 40.078 g/mol
Molar mass of S = 32.065 g/mol
Equation of reaction
Ca (s) + S(s) - CaS(s)
To find the limiting reagent
Mole of Ca = 8.54/40.078 (g/mol) = 0.213 mol
Mole of S = 2.33g / 32.065 (g/mol) = 0.072664 mol
From their mole ratio, sulphur is the limiting reagent
From the reaction
1 mole of calcium react with 1 mole of Sulphur to yield 1 mole of calcium sulphide
0.072664 mol of calcium will react with 0.072664 of sulphur to yield 0.072664 mole of CaS
Theoretical yield of CaS = 0.072664 × molar mass of CaS = 0.072664 × 72.143 g/mol = 5.242 g
Which of the following statements is true? I. Carbon forms covalent rather than ionic bonds. II. Carbon has an electronegativity value that is midway between that of the most metallic element and the most nonmetallic element. III. Carbon forms four bonds in virtually all its compounds. IV. A Si-Si bond is much stronger than a C-C bond. V. Relatively little heat is released when a C chain reacts and one bond replaces the other. Group of answer choices I, II, II, V I only II only III only IV only V only I and II I and III I and IV I and V II and III II and IV II and V III and IV III and V
Explanation:
Atomic number of carbon is 6 and its electronic distribution is 2, 4. As there are 4 valence electrons present in a carbon atom. Hence, it belongs to group 14 of the periodic table.
So, being a non-metal carbon atom tends to form covalent bonds. Also, the electronegativity value of carbon atom is mid-way between those of metals and non-metals.
In order to complete its octet, carbon atom tends to gain or share its 4 valence electrons. Therefore, it forms four bonds in all its compounds.
The Si-Si bond will be less stronger than C-C bond due to the larger size of silicon atom. As a result, there will be less overlapping between the silicon atoms due to which the bond formed will be weak in nature.
Whereas C-C bond is more stronger as a carbon atom is smaller in size as compared to silicon atom. As a result, more will be the overlapping between the carbon atoms. Hence, more stronger will be C-C bond than Si-Si bond.
As there will be covalent bonds present in a carbon chain and these bonds are weak as compared to ionic bonds. Hence, relatively little heat is released when a C chain reacts and one bond replaces the other.
Thus, we can conclude that out of the given options statements of I, II, III and V are true.
An acid that dissociates to the extent of 92% in water would be termed a strong acid.
True or Fasle?
Answer: False
Explanation:
Strong acid is defined as the acid which completely dissociates when dissolved in water. They have low pH. These releases ions in their aqueous states.
[tex]HNO_3(aq.)\rightarrow H^+(aq.)+NO_3^-(aq.)[/tex]
Weak acid is defined as the acid which does not completely dissociates when dissolved in water. They have high pH. These releases ions in their aqueous states.
[tex]CH_3COOH\rightleftharpoons CH_3COO^-+H^+[/tex]
Thus as the given acid is only 92% dissociated and cannot be completely dissociated, it is termed as a weak acid.
Final answer:
The given statement," An acid that dissociates to the extent of 92% in water would be termed a strong acid." is false.
Explanation:
In chemistry, the degree to which an acid dissociates in water classifies it as either strong or weak. An acid that dissociates 100% into ions when dissolved in water is deemed a strong acid. In contrast, acids that do not reach 100% dissociation are termed weak acids. An example of a weak acid is acetic acid (CH3COOH), which has a dissociation level significantly lower than 100% when dissolved in water.
Considering the given information, an acid that dissociates to the extent of 92% in water would not meet the criteria for a strong acid, as it does not fully dissociate. Thus, even with a high dissociation percentage such as 92%, this acid would still be classified as a weak acid. It is important to note that in practical terms a 92% dissociation indicates a relatively strong acid amongst weak acids, but it is not categorized as a strong acid in the technical sense.
In the following list, only __________ is not an example of a chemical reaction.
A) burning a plastic water bottle
B) the production of hydrogen gas from water
C) the tarnishing of a copper penny
D) chopping a log into sawdust
E) charging a cellular phone
Answer: Thus chopping a log into sawdust is not an example of a chemical reaction.
Explanation:
Physical reaction is a reaction in which there is no rearrangement of atoms and thus no new substance is formed. There is only change in physical state of the substance.
Example: chopping a log into sawdust as the shape and size of wood changes.
Chemical reaction is a reaction in which there is rearrangement of atoms and thus new substance is formed. There may or may not be a change in physical state.
Example: burning a plastic water bottle : as the plastic would combine with oxygen to give oxidised products.
the production of hydrogen gas from water: the chemical composition changes
the tarnishing of a copper penny: oxidation of copper takes place to give copper oxide.
charging a cellular phone: the electrical energy is used for a chemical reaction
Chopping a log into sawdust is an example of a physical change because it changes the size not the composition of the substance.
What are chemical reactions?Chemical reactions involve such kind change that leads to the formation of a new product (compound).
For example- the production of hydrogen gas from water, the burning of plastic produce gases.
Physical reactions:These reactions refer to the rearrangements of the atoms in a substance but do not to the formation of a new product such as temperature, phase, size, etc.
For example- chopping a log into sawdust
Therefore, chopping a log into sawdust is an example of a physical change because it changes the size not the composition of the substance.
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