Using the information provided in the chart determine which of these would have the highest pOH level? A) urine B) toothpaste C) rainwater D) household ammoni

The answer is D. 6 you multiply 2 and 3

Answer:

The correct answer is D

Explanation:

because you would take 2 and 3 and multiply them and get 6 or

3×2=6

Question 1:

1. One form of niobium oxide crystallizes in the unit cell shown above.

A. How many niobium atoms per unit cell? 3

B. How many oxygen atoms per unit cell? 3

C. What is the formula of niobium oxide? Nb2O5

Answer: A) 3 B) 3 C) Nb205

Question 2:

2. Quartz (left) and glass (right) are both forms of silicon dioxide. A piece of quartz breaks into a collection of smaller regular crystals with smooth faces. A piece of glass breaks into irregular shards. Use molecular structures to explain why the two solids break so differently. Select all that apply.

1. the bonding and geometry in quartz shows regular repeating patterns *

2.  the bonding and geometry in quartz shows irregular repeating patterns

3. the bonding and geometry in glass shows irregular repeating patterns *

4. the atomic geometries of the two solids can explain why they break so differently  *

5. the atomic geometries of the two solids cannot explain why they break so differently

6. the bonding and geometry in glass shows regular repeating patterns

Answer: 1,3,4

3. Solid silver adopts a face-centered cubic lattice. The metallic radius of a silver atom is 144 pm.

a. How many silver atoms occupy one unit cell of solid silver? 4

b. Calculate the length (in pm) of one side of the unit cell. 407

c. Calculate the volume (in m3) of one the unit cell.  6.74 x10^-29

d. What percentage (expressed to four significant figures) of the volume is empty? 25.95

Answer: a)4 b)407  c)6.74 x10^-29   d)25.95

4. Why hexane is insoluble in water? Select all that apply.

1. Water is polar solvent. *

2. Polar solvents dissolve both polar and non-polar compounds.

3. Polar solvents dissolve only polar compounds. *

4. Solubility does not depends on the polarity of the solvents and reagents.

5. Hexane is non-polar compound. *

Answer: 1,3,5

<3 goodluck

Final answer:

The empirical formula for the niobium oxide with oxide ions at the middle of each edge and niobium atoms at the center of each face is Nb2O, obtained by counting the ions per unit cell and adjusting for their location in the structure.

Explanation:

To determine the empirical formula of the niobium oxide, first, we need to consider how many ions are associated with each other in the cubic unit cell structure. A cubic unit cell with oxide ions at the middle of each edge and niobium atoms at the center of each face can be described as follows: each edge has 1/4 of an oxide ion since it is shared by 4 cubes, resulting in 1 oxide ion per unit cell (there are 12 edges, thus 12 x 1/4 = 3, but each oxygen is set twice, thus 3 / 2 = 1.5 but oxygen only gives 1 charge so we only take half). Each face-centered niobium contributes 1/2 of an atom to the unit cell since each face is shared between two unit cells, leading to 3 niobium atoms per unit cell (6 faces x 1/2 = 3). Therefore, for every 1 niobium atom, there is 0.5 of an oxide ion, and by multiplying both the niobium and oxide amounts by 2 to get whole numbers, we obtain the empirical formula Nb2O.

The coordination number of an ion in a crystalline structure is the number of counterions that surround it. In the niobium oxide unit cell described, the oxide ions are at the midpoint of each edge, and niobium atoms are at the center of each face. Without additional information, however, it is not possible to determine the exact coordination number, as this would depend on the 3D arrangement of the atoms within the cell.

Answer:

(a) The change in cell voltage is 0.05V

(b) The change in cell voltage is 0.03V

Explanation:

Redox reaction : It is defined as the reaction in which the oxidation and reduction reaction takes place simultaneously.

Oxidation reaction : It is defined as the reaction in which a substance looses its electrons. In this, oxidation state of an element increases.

Reduction reaction : It is defined as the reaction in which a substance gains electrons. In this, oxidation state of an element decreases.

Further explanation:

The image taken in context is attached below.

The standard reduction potentials for iron and silver are:

[tex]E^o_{(Fe^{2+}/Fe)}=-0.44V\\E^o_{(Ag^{+}/Ag)}=+0.80V[/tex]

In the given cell, the oxidation occurs at an anode which is a negative electrode and the reduction occurs at the cathode which is a positive electrode.

From the standard reduction potentials we conclude that, the substance having highest positive [tex]E^o[/tex] potential will always get reduced and will undergo reduction reaction.

So, silver will undergo reduction reaction will get reduced. Iron will undergo oxidation reaction and will get oxidized.

The given cell reactions are:

Oxidation half reaction (anode): [tex]Fe\rightarrow Fe^{2+}+2e^-[/tex]

Reduction half reaction (cathode): [tex]Ag^{+}+e^-\rightarrow Ag[/tex]

Thus, the anode and cathode will be [tex]E^o_{(Fe^{2+}/Fe)}[/tex]

and [tex]E^o_{(Ag^{+}/Ag)}[/tex] respectively.

The overall cell reaction will be,

[tex]2Ag^{+}+Fe\rightarrow Fe^{2+}+2Ag[/tex]

To calculate the [tex]E^o_{cell}[/tex] of the reaction, we use the equation:

[tex]E^o_{cell}=E^o_{cathode}-E^o_{anode}[/tex]

[tex]E^o=E^o_{(Ag^{+}/Ag)}-E^o_{(Fe^{2+}/Fe)}[/tex]

[tex]E^o=(+0.80V)-(-0.44V)=1.24V[/tex]

Now we have to calculate the cell potential.

Using Nernst equation :

[tex]E_{cell}=E^o_{cell}-\frac{0.0592}{n}\log \frac{[Fe^{2+}]}{[Ag^{+}]^2}[/tex]

where,

n = number of electrons in oxidation-reduction reaction = 2

[tex]E_{cell}[/tex] = emf of the cell = ?

Now put all the given values in the above equation, we get:

[tex]E_{cell}=1.24-\frac{0.0592}{2}\log \frac{(1M)}{(1M)^2}[/tex]

[tex]E_{cell}=1.24V[/tex]

Thus, the emf of cell potential is 1.24 V

Part (a):

The ion concentrations in the cathode half-cell [tex](Ag^+/Ag)[/tex] are increased by a factor of 10 from 1 M to 10 M.

The emf of the cell potential will be,

Using Nernst equation :

[tex]E_{cell}=E^o_{cell}-\frac{0.0592}{n}\log \frac{[Fe^{2+}]}{[Ag^{+}]^2}[/tex]

where,

n = number of electrons in oxidation-reduction reaction = 2

[tex]E_{cell}[/tex] = emf of the cell = ?

Now put all the given values in the above equation, we get:

[tex]E_{cell}=1.24-\frac{0.0592}{2}\log \frac{(1M)}{(10M)^2}[/tex]

[tex]E_{cell}=1.29V[/tex]

The change in cell voltage will be,

[tex]E_{cell}=1.29V-1.24V=0.05V[/tex]

Thus, the change in cell voltage is 0.05V

Part (b):

The ion concentrations in the anode half-cell [tex](Fe^{2+}/Fe)[/tex] are increased by a factor of 10 from 1 M to 10 M.

The emf of the cell potential will be,

Using Nernst equation :

[tex]E_{cell}=E^o_{cell}-\frac{0.0592}{n}\log \frac{[Fe^{2+}]}{[Ag^{+}]^2}[/tex]

where,

n = number of electrons in oxidation-reduction reaction = 2

[tex]E_{cell}[/tex] = emf of the cell = ?

Now put all the given values in the above equation, we get:

[tex]E_{cell}=1.24-\frac{0.0592}{2}\log \frac{(10M)}{(1M)^2}[/tex]

[tex]E_{cell}=1.27V[/tex]

The change in cell voltage will be,

[tex]E_{cell}=1.27V-1.24V=0.03V[/tex]

Thus, the change in cell voltage is 0.03V

Learn more:

Spontaneity of reaction; https://brainly.com/question/13151873 (answer by Kobenhavn)

Standard reduction potential;  https://brainly.com/question/8739272 (answer by RomeliaThurston)

Keywords:

Nernst equation, standard reduction potential, spontaneity of the reaction.

The change in the cell voltage when the ion concentrations in the ANODE half-cell are increased by a factor of 10 is 0.030  V

What is the change in the cell voltage when the ion concentrations in the ANODE half-cell are increased by a factor of 10?

The Nernst equation

[tex]E=E^o - \frac{RT}{nF} lnQ[/tex]

The given electrochemical cell has both aqueous species Fe 2 +  and  Ag +  at  1  M  concentration

If the anode concentration is increased by a factor of  10 , the cell potential will change by the correction term:  

[tex]\Delta E = -\frac{RT}{nF} lnQ[/tex]

Now we determine the overall reaction

[tex]Fe(s) -> Fe^{2+}(aq)+2e [anode]\\2*(Ag^+(aq)+e -> Ag(s)) [cathode]\\Fe(s)+2Ag^+(aq)->Fe^{2+}(aq)+2Ag(s)  [overall][/tex]

n=2 electrons were transferred

[tex]Q=\frac{[Fe^{2+}]}{[Ag^+]^2}[/tex]

The change in cell potential is

[tex]\Delta E = - \frac{RT}{nF} ln \frac{[Fe^{2+}]}{[Ag^+]^2}[/tex]

Note that [tex][Fe^{2+}]=10M[/tex] and assume that T=298.15 K

[tex]\Delta E = - \frac{8.314J/molK*298.15K}{2*96485C/mol} ln \frac{10M}{1M^2}\\\Delta E = -0.030 V[/tex]

Therefore the cell potential will decrease by 0.030 V

Grade:        9

Subject:  chemistry

Chapter:   the ion concentrations

Keywords:  the cell voltage, the ion concentrations, the cathode half-cell,   the anode, factor

Answer:

Endothermic proceses

Exothermic proceses

Explanation:

By definition an exothermic processes are those in which the system releases energy to the enviroment, while endothermic processes are those in which the system absorbs energy from the environment.

That change in energy is generally measured as heat.

Then an exothermic process releases heat and and endothermic process absorbs heat.

From that, as a first consequence, in an exothermic process the final substances (products in the case of a chemical reaction) ends with lower energy and lower temperature than the initial substances (reactants in the case of a chemical reaction).

The heat content of the substances is usually measured as enthalpy, then, for a chemical reaction you can write th is equation for the enthalpy change:

Thus, for an exothermic reaction ΔH products  < ΔH reactants ⇒ ΔH < 0, whilced for an endothermic reaction ΔH products > ΔH reactants ⇒ ΔH > 0.

The difference in energy between the products and the reactants is a result of the chemical potential energy of the substances, which is the energy stored in the chemical bonds. Then, in an endothermic reaction more energy is needed to break the chemical bonds of the reactants than what is released from the formation of the chemical bonds of the products. Of course the opposite is true: in an exothermic reaction, energy is released because it is required less energy for the formation of the new bonds of the products than what is needed to break the bonds of the reactants.

Answer:

D: Increasing the amount of water.

Explanation:

Choice A: ­ increasing the pressure can force the liquid to stay a liquid  and affect the boiling point (decrease it).

Choice B and C: ­ both involve colligative properties, adding a solute to water will  increase the boiling point  of water.

Choice D: ­ just having more water does not change the boiling point of the water as this minimize the effect of any external factor.

So, the right choice is: D: Increasing the amount of water.

Answer:

[tex]\boxed{\text{10 mL}}[/tex]

Explanation:

1. Write the balanced chemical equation.

[tex]\text{2NaOH} + \text{H$_{2}$SO$_{4}$} \longrightarrow\ \text{Na$_{2}$SO$_{4}$} + 2\text{H{$_{2}$O}}[/tex]

2. Calculate the moles of NaOH

[tex]\text{Moles of NaOH} =\text{60.0 mL NaOH} \times \dfrac{\text{0.5 mmol NaOH}}{\text{1 mL NaOH}} = \text{30 mmol NaOH}[/tex]

3. Calculate the moles of H₂SO₄.

[tex]\text{Moles of H$_{2}$SO$_{4}$}=\text{30 mmol NaOH} \times \dfrac{\text{1 mmol H$_{2}$SO$_{4}$} }{\text{2 mmol NaOH}} = \text{30 mmol H$_{2}$SO$_{4}$}[/tex]

4. Calculate the volume of H₂SO₄

[tex]c = \text{30 mmol H$_{2}$SO$_{4}$} \times \dfrac{\text{1 mL H$_{2}$SO$_{4}$}}{\text{3.0 mmol H$_{2}$SO$_{4}$}} = \text{10 mL H$_{2}$SO$_{4}$}[/tex]

The titration will require [tex]\textbf{10 mL}[/tex] H₂SO₄.

Answer:

The pressure of the gas is 40atm

Explanation:

Given parameters:

P₁ = 2.0atm

V₁ = 0.2L

V₂ = 10.0mL = 10 x10⁻³L = 0.01L

P₂ =?

We apply Boyle's law to solve this kind of problem

Boyle's law states that "the volume of a fixed mass of a gas varies inversely as the pressure changes if the temperature is constant".

It is expressed as P₁V₁ = P₂V₂

Making P₂ the subject of the formula gives:

P₂ = P₁V₁/V₂

Inserting the values of the parameters:

P₂ = 2x0.2/0.01

P₂ = 40atm

Answer:

[tex]\boxed{\text{KNO}_{3}}[/tex]

Explanation:

The reaction is

KOH(aq) + HNO₃(aq) ⟶ KNO₃(aq) + H₂O(ℓ)

If you evaporate the water, the solid substance is the compound, potassium nitrate.

[tex]\boxed{\textbf{KNO}_{3}}[/tex]

KNO₃(aq) ⟶ KNO₃(s)

The balanced equation for the dissociation of chromium(III) nitrate in water is Cr(NO3)3 (s) → Cr3+ (aq) + 3 NO3- (aq), illustrating the separation into chromium(III) ions and nitrate ions.

The balanced equation that describes the dissociation of chromium(III) nitrate in water is as follows:

Cr(NO3)3 (s) → Cr3+ (aq) + 3 NO3− (aq)

When chromium(III) nitrate dissolves in water, it separates into chromium(III) ions and nitrate ions. Each formula unit of the solid compound yields one chromium(III) ion and three nitrate ions. The equation is balanced with respect to both mass and charge, fulfilling the law of conservation of mass and the principle of electroneutrality.

To describe the process, it is important to note that chromium(III) nitrate is a salt, and like most salts, it dissociates completely in water to give its constituent ions.

Specific heat capacity of a substance is the amount of heat required to raise the temperature by one degree Celsius of one gram of a substance. Therefore, the correct option is option A.

Enthalpy term is basically used in thermodynamics to show the overall energy that a matter have. Mathematically, Enthalpy is directly proportional to specific heat capacity of a substances.

Mathematically,

q = n ×ΔH

where

q = amount of heat

n = no of moles

ΔH = enthalpy

n = w / M.M

w = given mass

M.M = molar mass

A) C₆H₆

melting point =5.5° C

boiling point =80.1 ° C

Heat of fusion = 9.92 kJ/mol

Heat of vaporization =30.8kJ/mol

B) CH₃CH₂CH₂CH₂CH₂COH₆ is solid

C) NaCl is solid

D) NH₃

melting point = -77.73 °C

boiling point =  -33.34 °C

Therefore, the correct option is option A.

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1. Find the mole of each reactant present and determine the limiting reactant 2. determine the mole of product produced through the mole ratio of the equation 3. convert to grams if the 'amount' refers to grams

The partial pressure of oxygen in a mixture with a total pressure of 800.0 mm Hg, where oxygen makes up 40% of the mixture, is 320.0 mm Hg.

To find the partial pressure of oxygen in a mixture of gases, you can use the formula P = (Patm) X (percent content in mixture). Given that the total pressure of the mixture is 800.0 mm Hg and oxygen makes up 40% of this mixture by volume, the partial pressure of oxygen can be calculated as follows:

PO2 = (800.0 mm Hg) X (0.40)

PO2 = 320.0 mm Hg

Therefore, the partial pressure of oxygen in this mixture is 320.0 mm Hg.

Answer:

Conserved

Explanation:

In balancing nuclear reaction equations, there is conservation of mass numbers and atomic numbers, i.e the sum of the mass number on the product side must be equal to the sum of mass numbers on the reactant side.

Also, the sum of the atomic numbers on the product side must be equal to the sum of the atomic numbers on the reactant side.

Note: A nuclear reaction is a process in which a nucleus reacts with an elementary particle.

Answer:

where's the question... ?

Answer:

Explanation:

You can solve this question using just some chemical facts:

Hence, since you are asked to state the solution with the highest concentration of hydroxide ions, you just pick the highest pH. This is the option d, pH = 12.59.

These mathematical relations are used to find the exact concentrations of hydroxide ions:

Then, you can follow these calculations:

Solution    pH        pOH                            [OH⁻]

a.               3.21       14 - 3.21 = 10.79        antilogarithm of 10.79 = 1.6 × 10⁻¹¹

b.               7.00      14 - 7.00 = 7.00        antilogarithm of 7.00 = 10⁻⁷

c.                7.93      14 - 7.93 = 6.07        antilogarithm of 6.07 = 8.5 × 10⁻⁷

d.               12.59     14 - 12.59 = 1.41        antilogarithm of 1.41 = 0.039

e.               9.82      14 - 9.82 = 4.18        antilogarithm of 4.18 = 6.6 × 10⁻⁵

From which you see that the highest concentration of hydroxide ions is for pH = 12.59.

The pH with the highest hydroxide ion is 12.59

pH is the degree of acidity or alkalinity in a solution.

The lower the pH, the higher the acidity.The higher the pH the higher the basicity.

When the concentration is higher, it has more hydroxide ion.

Therefore, The pH with the highest hydroxide ion is 12.59 because the higher the pH the higher the concentration of the hydroxide ion.

Learn more about pH from the link below.

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Answer:

[tex]\boxed{\text{B. HC}}[/tex]

Explanation:

The blow-by gases that escape past the piston rings and get into the crankcase are mostly unburned fuel-air mixture.

The fuel is largely a mixture of hydrocarbons (HCs) .

The PCV system captures these gases and feeds them back to the cylinder for further combustion.

A. is wrong. Carbon dioxide exits through the exhaust.

C. is wrong. Most of the oxygen in the incoming air is used for combustion in the cylinders.

D is wrong. The NOx gases exit via the exhaust and are trapped by the catalytic converter.

4 carbon chain is butane.  With a triple bond it is butane.  Since the triple bond is on the first carbon it can be called 1-butyne, or but-1-yne.

the burning of ethanon is an exothermic reaction.

exothermic = releases heat.

knowing this, we can see that the atoms are released into the atmosphere, it then reacts with oxygen, producing cardon dioxide, water, and heat.

Answer:

Particle /                          mass number                atomic number

type of radiation

alpha / ⁴₂ He                              4                                     2

beta / e⁰                                     0                                   - 1

gamma / γ                                  0                                     0

neutron / n                                 1                                      0

Explanation:

These are the basic types of radiation: alpha (α), beta (β),  gamma (γ), and neutrons (n).

The radiation is emitted by unstable nuclei when undergo radiactive decay or by nuclei that are shooted by other particles.

Alpha radiation (⁴₂ He):

They are nuclei of helium-4 atoms: 2 protons and 2 neutrons.

Hence, the atomic number, which is the number of protons,  of these particles, is 2; and the mass number, which is the sum of protons and neutrons, is 2 + 2 = 4.

The symbol of this radiation is ⁴₂ He, where the superscript to the left of the chemical symbol is the mass number and the subscript to the left of the chemical symbol is the atomic number.

Beta (⁰₋ ₁ e)

These are electrons emiited from an unstable nucleus. The symbols used for this particle are either ⁰₋ ₁β or ⁰₋ ₁e.

The superscript 0 indicates that the relative mass of this particle is practically zero and the subscript -1 tells that the emission of electrons increases the atomic number of the nucleus that emits it.

Gamma (⁰₀γ)

The gamma rays are electromagnetic radiation of high (the highest) energy.

The both superscript and subscript are zero, meaning that this radiation does not change either the mass or atomic numbers of the nucleus.

Neutron (¹₀n):

Neutrons are also emiited from the nucleus and so they may be considered a radiation.

The atomic number of neutrons is 0 (since it does not have protons) and its mass number is 1.

Radioactive rays are divided into three, namely alpha rays, beta rays, and gamma rays.  

Check the picture below!

Types of Radioactive Rays

Based on the constituent particles, radioactive rays are divided into three, namely alpha rays, beta rays, and gamma rays.

Alfa ray (α ray)

Alpha rays are rays emitted by radioactive elements. This ray was discovered simultaneously with the discovery of the phenomenon of radioactivity, which is the decay of the nucleus which takes place spontaneously, uncontrolled, and produces radiation. Alpha rays consist of two protons and two neutrons. The following are the nature of alpha rays.

Beta Rays (β Rays)

Beta rays are high-energy electrons that originate from the nucleus. Here are some of the nature of beta rays.

Gamma Rays (Rays ˠ)

Gamma rays are radiation from electromagnetic waves that emanate from very high energy nuclei that have no mass or charge. Gamma rays also emit when a core emits alpha rays and beta rays. Gamma-ray decay does not cause changes in atomic number or atomic mass.

Gamma rays have the following natural properties:

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Detail

Class: High School

Subject: Chemistry

Keyword: Alpha, Beta, Gamma

Answer:

1.99 grams of methane

Explanation:

A combustion reaction always produces the product carbon dioxide and water. So the chemical equation for this reaction would be:

CH₄ + O₂ → CO₂ + H₂O

To answer this question, you need to first determine which is the excess reactant. First step is to balance the equation:

CH₄ + 2O₂ → CO₂ + 2H₂O

Next we get the number of moles of each reactant we actually have:

8.00 g of O₂ = ? moles of O₂

You can get the number of moles, by first computing how many grams of the molecule is present in 1 mole.

O = 15.999g/mole. Since there are 2 oxygens in one mole of O₂, all you need to do is add up the atomic mass of 2 oxygens. You will get:

O₂= 31.998 g/mole

You can use this then to determine how many moles of O₂ there are in 8.00g.

[tex]8.00g\times\dfrac{1mole}{31.998g}=0.250moles[/tex]

So there are 0.250 moles of O₂ in 8.00 g of O₂.

We do the same for CH₄

4.00g of CH₄=? moles of CH₄

            C           H₄

CH₄= 12.011 + 1.008(4) = 16.043 g/mole

[tex]4.00g\times\dfrac{1mole}{16.043g}=0.249moles[/tex]

So let's sum up our new given. We now have:

0.250 moles of O₂

0.249 moles of CH₄

Next we look at the molar ratio of reactants to produce products:

CH₄ + 2O₂ → CO₂ + 2H₂O

According to this equation we can assume the following:

We need 1 mole of CH₄ for every 2 moles of O₂ in this reaction. Using what we have, we will see how much of reactant of the other reactant we need to use up the other.

[tex]0.25molesofO_{2}\times\dfrac{1moleofCH_{4}}{2molesofO_{2}}=0.125molesofCH_{4}\\\\0.249molesofCH_{4}\times\dfrac{2molesofO_{2}}{1moleofCH_{4}}=0.498molesofO_{2}[/tex]

Compare the results with what we have:

What we have                   What we need

0.250 moles of O₂   <     0.498 moles of O₂

0.249 moles of CH₄ >     0.125 moles of CH₄

This means that since we have less O₂ that what we need to use up CH₄, then O₂ is the limiting reactant and CH₄ is the excess.

To compute how much we have in excess, we use the number of moles produced when we use up limiting reactant which we did earlier and convert it into grams to determine how much in grams we used up.

Earlier we solved that we need 0.125 moles of CH₄ to use up all the O₂. Now convert that value into grams:

[tex]0.125molesofCH_{4}\times\dfrac{16.043gofCH_{4}}{1moleofCH_{4}}=2.005g of CH_{4}[/tex]

This means that 2.005g of CH₄ will be used up.

Subtract that from the CH₄ we already have:

4.00 g - 2.005 g =1.99 g of CH₄

-59 kj/mol exothermic

The enthalpy change for the reaction of ethylene with hydrogen bromide to form ethyl bromide is -59 kJ/mol. This means that the reaction is exothermic, meaning that it releases heat.

The bond energies of the relevant bonds are as follows:

C-C bond energy: 347 kJ/mol

C-H bond energy: 413 kJ/mol

H-Br bond energy: 363 kJ/mol

C-Br bond energy: 276 kJ/mol

Reactants:

Ethylene: 2 C-H bonds + 1 C-C bond

Hydrogen bromide: 1 H-Br bond

Products:

Ethyl bromide: 3 C-H bonds + 1 C-C bond + 1 C-Br bond

Enthalpy change:

ΔH = Σ(bond energies broken in reactants) - Σ(bond energies formed in products)

ΔH = (2 × 413 kJ/mol + 1 × 347 kJ/mol) - (1 × 363 kJ/mol + 3 × 413 kJ/mol + 1 × 276 kJ/mol)

ΔH = -59 kJ/mol

Therefore, the enthalpy change for the reaction of ethylene with hydrogen bromide to form ethyl bromide is -59 kJ/mol. This means that the reaction is exothermic, meaning that it releases heat.

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Answer:

2.38

Explanation:

119 divided by 50 =2.38

i hope you get it right :)

A neutral atom of tin has 50 protons, 50 electrons, and 69 neutrons. The number of protons and electrons is determined by the atomic number, while the number of neutrons is calculated by subtracting the atomic number from the mass number.

An atom of tin (Sn) is described by its atomic number and its mass number. The atomic number refers to the number of protons in the nucleus of the atom, and in a neutral atom, it also equals the number of electrons. Therefore, a neutral tin atom has 50 protons and 50 electrons.

The mass number, on the other hand, is the sum of protons and neutrons in the nucleus. Therefore, to find out the number of neutrons, you have to subtract the atomic number from the mass number: 119 - 50 = 69. So, a neutral tin atom has 69 neutrons.

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Answer:

B. 92.4 g

Explanation:

the balanced equation for the reaction is as follows

CaCO₃ + 2HCl ---> CaCl₂ + CO₂ + H₂O

molar ratio of CaCO₃ to CaCl₂ is 1:1

number of CaCO₃ moles reacted - 104 g / 100 g/mol = 1.04 mol

therefore number of CaCl₂ moles reacted - 1.04 mol

mass of CaCl₂ expected to be formed = 1.04 mol x 111 g/mol = 115.44 g

percentage yield = actual yield / theoretical yield x 100 %

theoretical yield = 115.44 g

percentage yield = 80.15 %

substituting these values in the above equation

80.15 % = actual yield / 115.44 g x 100 %

actual yield = 92.5 g

therefore answer is B. 92.4 g

The answer is B.

ATP + Oxygen ---> ADP + P

cl2>F2>H2

we can do this by molar mass

Hydrogen - 1

clorine - 35 x2 = 70

flourine- 18 x 2 = 36

flourine - 18

Molar mass has a direct relationship with entropy. The order of decreasing molar entropy at 298K is F[tex]_2[/tex]> Cl[tex]_2[/tex] > H[tex]_2[/tex].

Entropy is a measurable physical characteristic and a scientific notion that is frequently connected to a condition of disorder, unpredictability, or uncertainty. It has several applications in physics and chemistry, as well as in biological systems as well as how they relate to life.

The phrase and the idea are employed in many different contexts, including information theory and classical thermodynamics. Molar mass has a direct relationship with entropy. The order of decreasing molar entropy at 298K is F[tex]_2[/tex]> Cl[tex]_2[/tex] > H[tex]_2[/tex].

Therefore, the order of decreasing molar entropy at 298K is F[tex]_2[/tex]> Cl[tex]_2[/tex] > H.

To know more about entropy, here:

https://brainly.com/question/13146879

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Answer:

1.0 x 10⁻¹².

Explanation:

Cu₂S(s) ⇌ 2Cu⁺(aq) + S²⁻(aq),

The equilibrium constant (Keq) = [Cu⁺]²[S²⁻]/[Cu₂S].

[Cu⁺] = 1.0 × 10⁻⁵ M, [S²⁻] = 1.0 × 10⁻² M.

[Cu₂S] = 1.0, since the concentration of solid is always can be considered = 1.0.

∴ Keq = [Cu⁺][S²⁻]/[Cu₂S] = (1.0 × 10⁻⁵)²(1.0 × 10⁻²)/(1.0) = 1.0 x 10⁻¹².

Answer: The equilibrium constant for the above reaction is [tex]1.0\times 10^{-12}[/tex]

Explanation:

Equilibrium constant in terms of concentration is defined as the ratio of concentration of products to the concentration of reactants each raised to the power their stoichiometric ratios. It is expressed as [tex]K_{c}[/tex]

For a general chemical reaction:

[tex]aA+bB\rightarrow cC+dD[/tex]

The expression for [tex]K_{c}[/tex] is written as:

[tex]K_{c}=\frac{[C]^c[D]^d}{[A]^a[B]^b}[/tex]

Concentration of solid and liquid substances in a chemical reaction is taken to be 1.

For the given chemical reaction:

[tex]Cu_2S(s)\rightarrow 2Cu^+(aq.)+S^{2-}(aq.)[/tex]

The expression for [tex]K_{c}[/tex] is written follows:

[tex]K_c=[Cu^+]^2\times [S^{2-}][/tex]

We are given:

[tex][Cu^+]=1.0\times 10^{-5}M[/tex]

[tex][S^{2-}]=1.0\times 10^{-2}M[/tex]

Putting values in above expression, we get:

[tex]K_c=(1.0\times 10^{-5})^2\times (1.0\times 10^{-2})\\\\K_c=1.0\times 10^{-12}[/tex]

Hence, the equilibrium constant for the above reaction is [tex]1.0\times 10^{-12}[/tex]

Answer:

A - NaCl is a product

D - Cl2 is a gas

Explanation:

Based on the chemical reaction;

2Na(s) + Cl2(g) → 2NaCl2

The true statements for the reaction 2Na(s) + Cl2(g) → 2NaCl(s) are that NaCl is a product and Cl2 is a gas. Sodium (Na) is a reactant, not a product, and a chemical reaction does occur in this equation.

The reaction given is 2Na (s) + Cl2(g) → 2NaCl (s). This chemical equation is balanced, indicating that the same number and types of atoms appear on both sides of the equation. The equation demonstrates the reaction of solid sodium (Na) with chlorine gas (Cl2) to form sodium chloride (NaCl), a solid.

For the statements provided:

Key Notes to Remember:

Chlorine is one of the seven elements that exist in nature as diatomic molecules, which include H2, N2, O2, Cl2, Br2, and I2—this is important for balancing chemical equations correctly.

Answer:

54.0 g.

Explanation:

2H₂ + O₂ → 2H₂O.

When 3.00 moles of hydrogen molecules and 1.50 moles of oxygen molecules react, they form 3.00 moles of water according to the balanced reaction.

∴ The no. of grams in 3.0 moles of water = no. of moles x molar mass = (3.0 mol)(18.0 g/mol) = 54.0 g.

Answer:

A) 54.0 g

Explanation:

Hello! The answer to your question is 54.0 grams.

2H2 + O2 --> 2H2O

Because of that, we know our result will possess 3 significant figures.

The only sensible answer here (without the calculations) would be 54.0, due to the decimal placement. Hope this helps you!

2.5 x 10^24 molecules of C4H10

Answer : The enthalpy change for this reaction is -193.8 kJ.

Solution :

The balanced chemical reaction is,

[tex]2SO_2(g)+O_2(g)\rightarrow 2SO_3(g)[/tex]

The expression for enthalpy change is,

[tex]\Delta H=\sum [n\times \Delta H_f(product)]-\sum [n\times \Delta H_f(reactant)][/tex]

[tex]\Delta H=[(n_{SO_3}\times \Delta H_{SO_3})]-[(n_{O_2}\times \Delta H_{O_2})+(n_{SO_2}\times \Delta H_{SO_2})][/tex]

where,

n = number of moles

[tex]\Delta H_{O_2}=0[/tex] (as heat of formation of substances in their standard state is zero

Now put all the given values in this expression, we get

[tex]\Delta H=[(2\times -395.7)]-[(1\times 0)+(2\times -298.8)][/tex]

[tex]Delta H=-193.8kJ[/tex]

Therefore, the enthalpy change for this reaction is, -193.8 KJ

Final answer:

The heat of reaction for the formation of sulfur trioxide from sulfur dioxide and oxygen, using the provided enthalpies of formation, is calculated to be -193.8 kJ.

Explanation:

The student has asked what the heat of reaction is when sulfur dioxide reacts with oxygen to form sulfur trioxide. The given balanced chemical equation is 2SO2(g) + O2(g) → 2SO3(g). The standard enthalpy of formation (ΔHf0) for SO2 is −298.8 kJ/mol, and for SO3 it's −395.7 kJ/mol.

Calculating the Heat of Reaction

To find the heat of reaction, we use the following formula:

ΔH = [∑ (ΔHf0 products)] - [∑ (ΔHf0 reactants)]

ΔH = [2 mol × (−395.7 kJ/mol SO3)] - [2 mol × (−298.8 kJ/mol SO2) + 1 mol × (0 kJ/mol O2)]

ΔH = [−2 × 395.7 kJ] - [−2 × 298.8 kJ]

ΔH = (−791.4 kJ) - (−597.6 kJ)

ΔH = −193.8 kJ

Therefore, the heat of reaction for the formation of sulfur trioxide from sulfur dioxide and oxygen is −193.8 kJ.