Question 1

Calculate K for the following reaction, provided the concentration versus time graph shown below. 2A 2B + 3C

Accepted Answer

The answer of Calculate K for the following reaction, provided...

Question 2

An equilibrium that strongly favors products has ________

Accepted Answer

The equilibrium constant expression for a chemical reaction is given by the ratio of the concentration of products to the concentration of reactants, each raised to their respective stoichiometric coefficients. Therefore, an equilibrium that strongly favors products will have a large value of this equilibrium constant, which means the concentration of products is much larger than the concentration of reactants in the equilibrium mixture. Option B has a value of KF1F1F1S1F1F1F101, which indicates that the equilibrium strongly favors the products.

Question 3

A decrease in the number of moles of gas as the reaction goes from reactants to products in a gas-phase equilibrium results in ________

Accepted Answer

According to Le Chatelier's principle, a decrease in the number of moles of gas will shift the equilibrium toward the side with more gas molecules in order to minimize the effect of the change. Therefore, in this case, the equilibrium will shift toward the reactants side to compensate for the decrease in the number of gas molecules. This means that the concentration of reactants will increase and the concentration of products will decrease, resulting in a net reverse reaction. As a result, the value of Kp (equilibrium constant in terms of partial pressures) will decrease. Therefore, option B is correct as it states that Kp will become less than the initial equilibrium constant.

Question 4

Under what conditions are the values of K_c and K_p for a given gas-phase equilibrium the same?

Accepted Answer

Kc and Kp are equal when there is no change in the number of moles of gas in the reaction, as the relationship between Kc and Kp involves the change in moles of gas (Δn).

Question 5

Two students measured an equilibrium constant for the same chemical reaction. Ken obtained a value of 130 for the equilibrium constant, but Barbie obtained a value of 11.4. The instructor checked their results and said they were both correct. How can that be?

Accepted Answer

The answer of Two students measured an equilibrium constant for...

Question 6

The equilibrium constant for the formation of hydrogen iodide from hydrogen and iodine is 45.0 at a certain temperature. H₂(g) + I₂(s) 2 HI(g) Which of the following is true regarding this equilibrium? I.The reaction is product-favored. II.The reaction is reactant-favored. III.Equilibrium lies to the right. IV.Equilibrium lies to the left.

Accepted Answer

The equilibrium constant, K = [HI]2/([H2]*[I2]), is 45.0, which means at equilibrium, [HI] is larger compared to [H2] and [I2]. This also means that the numerator is much larger than the denominator, indicating that the reaction is product-favored. Therefore, choices (I) and (III) are correct. Choices (II) and (IV) are incorrect. Hence, the answer is (A).

Question 7

For the following reaction, K_c = 0.500 at 300K. What is the value of K_p? 2A(g) + B(g) 2C(g) + D(g)

Accepted Answer

The answer of For the following reaction, K_c = 0.500...

Question 8

Water can decompose at an elevated temperature to give hydrogen and oxygen according to the equation below. At a particular temperature, the partial pressures of H₂O, H₂, and O₂ are 0.055 atm, 0.0065 atm, and 0.0045 atm, respectively, at equilibrium. What is the value of the equilibrium constant, K_P, for this reaction at this temperature? 2H₂O(g) 2H₂(g) + O₂(g)

Accepted Answer

The equilibrium constant expression for the given reaction is as follows: K_P = ([H₂]2[O₂])/([H₂]2[₂]) Substituting the given partial pressure values, we get: K_P = ((0.055)2(0.0045))/((0.0065)2) = 6.31 ≈ 6.3 Therefore, the correct answer is C.

Question 9

Sulfur dioxide, gaseous water, and oxygen gas react to prepare sulfuric acid in the following unbalanced equation. Under equilibrium conditions, the partial pressures of the components are P_SO2 = 0.1 atm, P_H2O = 0.05 atm, P_O2 = 0.25 atm, P_H2SO4 = 2.75 atm. What is the value of the equilibrium constant, K_p, for the reaction?

Accepted Answer

The answer of Sulfur dioxide, gaseous water, and oxygen gas...

Question 10

For the following hypothetical equilibrium, what is the value of the equilibrium constant if the concentrations at equilibrium are as shown? A + 2B C [A] = 4.5 $\times$ 10^-5M [B] = 2.2 $\times$ 10^-2M [C] = 9.4 $\times$ 10^-3M

Accepted Answer

The equilibrium constant can be calculated as: Kc = ([B]^2/[_{]^2) * ([]^2 * [F1F1F10]) / ([^{3]^2 * [F1F1F1S1]^4.5)

Plugging in the given equilibrium concentrations, we get:

Kc = (2.2^2/4.5^2) * (0.1^2 * 9.4) / (0.12^2 * 2.2^4.5) ≈ 4.3

Therefore, the answer is C.}}

Question 11

Equilibrium constants can be expressed in terms of molar concentration, K_c, or partial pressure, K_P. To relate these two equilibrium constants to each other, ________

Accepted Answer

To relate equilibrium constants expressed in terms of molar concentration to those expressed in terms of partial pressure, each concentration must be multiplied by the factor RT. This is because the ideal gas law relates pressure, volume, number of moles, and temperature, and R is the gas constant. By multiplying each concentration by RT, we can convert it to the equivalent partial pressure, and the two equilibrium constants can be compared.

Question 12

Coal (C) can be heated with steam (H₂O) at high temperatures to produce a mixture of hydrogen and carbon monoxide gases. Methanol, which is a useful fuel, can be produced from these gases by the reaction below. At a particular high temperature, the equilibrium concentrations are the following: [H₂] = 0.095 mol/L, [CO] = 0.035 mol/L, and [CH₃OH] = 0.065 mol/L. What is the value of the equilibrium constant, K_c, for this reaction at this temperature? 2H₂(g) + CO(g) CH₃OH(g)

Accepted Answer

The answer of Coal (C) can be heated with steam...

Question 13

Calculate K for the following reaction, provided the concentration versus time graph shown below. 3A  B + 2C

Accepted Answer

The answer of Calculate K for the following reaction, provided...

Question 14

Equilibrium constants for gases can be expressed in terms of concentrations, K_c, or in terms of partial pressures, K_p. Which one of the following statements regarding K_c and K_p is correct?

Accepted Answer

The equilibrium constant expression for gases in terms of concentrations is KC = [C]^c[D]^d/[A]^a[B]^b and in terms of partial pressures is KP = (PC)^c(PD)^d/(PA)^a(PB)^b. Both expressions are equal when the sum of the stoichiometric coefficients for the products equals the sum of the stoichiometric coefficients for the reactants (i.e. when the balanced reaction equation is balanced). Therefore, choice C is the correct answer.

Question 15

Which expression corresponds to the equilibrium constant K_c for the reaction written as 2NH₃(g) + 2O₂(g) N₂O(g) + 3H₂O₂(g)

Accepted Answer

The answer of Which expression corresponds to the equilibrium constant...

Question 16

The chemical equilibrium constant for the following reaction is 2.15 $\times$ 10². 2NO₂(g) N₂O₄(g) What is the value of the equilibrium constant for the following reaction? 6NO₂(g) 3N₂O₄(g)

Accepted Answer

The answer of The chemical equilibrium constant for the following...

Question 17

An increase in the number of moles of gas as the reaction goes from reactants to products in a gas-phase equilibrium results in ________

Accepted Answer

The answer of An increase in the number of moles...

Question 18

The equilibrium constant for the acid ionization of mercaptoethanol (HSCH₂CH₂OH ) is 1.91 $\times$ 10^-10_. HSCH₂CH₂OH(aq) H^-(aq) + SCH₂CH₂OH^-(aq) Which of the following is true regarding this equilibrium? I.The reaction is product-favored. II.The reaction is reactant-favored. III.Equilibrium lies far to the right. IV.Equilibrium lies far to the left.

Accepted Answer

The answer of The equilibrium constant for the acid ionization...

Question 19

The equilibrium constant for the formation of calcium carbonate from the ions in solution is 2.2 $\times$ 10⁸ according to the reaction: What is the value of the equilibrium constant for the reverse of this reaction?

Accepted Answer

The answer of The equilibrium constant for the formation of...

Question 20

For the following reaction, K_p = 137 at 3.50 $\times$10²K. What is the value of K_c? 2C₄H₁₀(l) + 3O₂(g) 8CO₂(g) + 10H₂O(g)

Accepted Answer

Using the equation K_p = 137 and the stoichiometric coefficients given in the balanced chemical equation, we can set up an ICE (initial, change, equilibrium) table for the reaction: | | 2C₄H₁₀(l) | F1F1F1S1F1F1F10 | 3O₂(g) | 8CO₂(g) | 10H₂O(g) | |----------|--------------------------------|------------------|-------------------|---------------------|---------------------| | Initial | 0.01 | 0.01 | 0.01 | 0.01 | 0.01 | | Change | -x | -2x | 3x | 8x | 10x | | Equilibrium | 0.01 - x | 0.01 - 2x | 0.01 + 3x | 0.01 + 8x | 0.01 + 10x | where x is the change in concentration or pressure for each species. We can plug the equilibrium concentrations or pressures into the equilibrium expression for the reaction: K_c = [F1F1F1S1] / ([C₄]2[H₁₀][O₂]3/[CO₂]8/[H₂O]10) K_c = (0.01 - 2x) / (0.01)2(0.01 + 3x)3 / (0.01 + 8x)8 / (0.01 + 10x)10 Using algebra, we can simplify and solve for x: 137 = K_p = K_c 137 = (0.01 - 2x) / (0.01)2(0.01 + 3x)3 / (0.01 + 8x)8 / (0.01 + 10x)10 x = 7.03x10-9 Substituting x back into the equilibrium concentrations or pressures gives us: [C₄] = 0.01 - x = 0.01 - 7.03x10-9 = 0.01 [F1F1F1S1] = 0.01 - 2x = 0.01 - 2(7.03x10-9) = 0.00999998594 [H₁₀] = 0.01 [O₂] = 0.01 + 3x = 0.01000002109 [CO₂] = 0.01 + 8x = 0.01000005626 [H₂O] = 0.01 + 10x = 0.01000007029 Therefore, the equilibrium constant K_c is approximately 7.03x1010, which corresponds to choice A.

Quiz 14: Chemical Equilibrium: How Much Product Does a Reaction Really Make

Calculate K for the following reaction, provided the concentration versus time graph shown below. 2A 2B + 3C

An equilibrium that strongly favors products has ________

A decrease in the number of moles of gas as the reaction goes from reactants to products in a gas-phase equilibrium results in ________

Under what conditions are the values of Kc and Kp for a given gas-phase equilibrium the same?

Two students measured an equilibrium constant for the same chemical reaction. Ken obtained a value of 130 for the equilibrium constant, but Barbie obtained a value of 11.4. The instructor checked their results and said they were both correct. How can that be?

For the following reaction, Kc = 0.500 at 300K. What is the value of Kp? 2A(g) + B(g) 2C(g) + D(g)

For the following hypothetical equilibrium, what is the value of the equilibrium constant if the concentrations at equilibrium are as shown? A + 2 B C [A] = 4.5 ×\times× 10-5 M [B] = 2.2 ×\times× 10-2 M [C] = 9.4 ×\times× 10-3 M

Equilibrium constants can be expressed in terms of molar concentration, Kc, or partial pressure, KP. To relate these two equilibrium constants to each other, ________

Calculate K for the following reaction, provided the concentration versus time graph shown below. 3A B + 2C

Equilibrium constants for gases can be expressed in terms of concentrations, Kc, or in terms of partial pressures, Kp. Which one of the following statements regarding Kc and Kp is correct?

Which expression corresponds to the equilibrium constant Kc for the reaction written as 2NH3(g) + 2O2(g) N2O(g) + 3H2O2(g)

The chemical equilibrium constant for the following reaction is 2.15 ×\times× 102. 2NO2(g) N2O4(g) What is the value of the equilibrium constant for the following reaction? 6NO2(g) 3N2O4(g)

An increase in the number of moles of gas as the reaction goes from reactants to products in a gas-phase equilibrium results in ________

The equilibrium constant for the formation of calcium carbonate from the ions in solution is 2.2 ×\times× 108 according to the reaction: What is the value of the equilibrium constant for the reverse of this reaction?

For the following reaction, Kp = 137 at 3.50 ×\times× 102K. What is the value of Kc? 2C4H10(l) + 3O2(g) 8CO2(g) + 10H2O(g)

Under what conditions are the values of K_c and K_p for a given gas-phase equilibrium the same?

Equilibrium constants can be expressed in terms of molar concentration, K_c, or partial pressure, K_P. To relate these two equilibrium constants to each other, ________

Equilibrium constants for gases can be expressed in terms of concentrations, K_c, or in terms of partial pressures, K_p. Which one of the following statements regarding K_c and K_p is correct?

Which expression corresponds to the equilibrium constant K_c for the reaction written as 2NH₃(g) + 2O₂(g) N₂O(g) + 3H₂O₂(g)