Question 1

At an elevated temperature,K_p = 0.19 for the reaction 2 NOCl(g)⇌ 2 NO(g)+ Cl₂(g).If the initial partial pressures of NOCl,NO,and Cl₂ are 0.50 atm,0.25 atm,and 0.45 atm,respectively,a net ________ (forward,reverse)reaction must occur in order to achieve equilibrium.

Accepted Answer

The answer of At an elevated temperature,K_p = 0.19 for...

Question 2

For the reaction shown below the value of K_p is ________ than the value of K_c,because Δn = ________. N₂O₄(g)⇌ 2 NO₂(g)

Accepted Answer

The answer of For the reaction shown below the value...

Question 3

K_c = 57.0at 700 K for the reaction shown below. H₂(g)+ I₂(g)⇌ 2 HI(g) If [H₂(g)] = [I₂(g)] = 0.200 M at equilibrium,the molar concentration [HI((g)] = ________ at equilibrium.

Accepted Answer

The answer of K_c = 57.0at 700 K for...

Question 4

For the reaction shown below the equilibrium constant expression for K_c= ________. HF(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ F^-(aq)

Accepted Answer

The answer of For the reaction shown below the equilibrium...

Question 5

Which of the following changes in reaction conditions will not alter the composition of a homogeneous equilibrium mixture of gases in a reaction having unequal moles of gaseous products and reactants?

Accepted Answer

Addition of a catalyst does not affect the equilibrium composition of a homogeneous mixture of gases as it only speeds up the reaction rate without altering the position of the equilibrium.

Options B, C, and D would impact the equilibrium composition:
B) Addition of reactants would shift the equilibrium towards the product side to counteract the increase in concentration on the reactant side.
C) Decreasing the temperature would shift the equilibrium to the side with the higher enthalpy (heat) of reaction to compensate for the lost energy, which will depend on the specific reaction.
D) Increasing the volume would shift the equilibrium to the side with more moles of gas to counteract the increase in space.

Question 6

In a reversible reaction,when the rate of the forward reaction equals the rate of the reverse reaction,the reaction is at ________.

Accepted Answer

The answer of In a reversible reaction,when the rate of...

Question 7

At 298 K,K_c = 1.7 × 10^-56 for the reaction 3 O₂(g)⇌ 2 O₃(g).What is the value of K_p at this temperature?

Accepted Answer

The answer of At 298 K,K_c = 1.7 × 10^-56...

Question 8

For the reaction shown below,N₂O₄ and NO₂ have equilibrium concentrations,[N₂O₄]_eq = 2.160 × 10^-⁴ and [NO₂]_eq = 1.001 × 10^-³,respectively.The equilibrium constant,K_c,for this reaction equals ________. N₂O₄(g)⇌ 2 NO₂(g)

Accepted Answer

The answer of For the reaction shown below,N₂O₄ and NO₂...

Question 9

For the reaction CaCO₃(s)⇌ CaO(s)+ O₂(g)the equilibrium expression is K_p = ________.

Accepted Answer

The answer of For the reaction CaCO₃(s)⇌ CaO(s)+ O₂(g)the equilibrium...

Question 10

Which will alter the composition of an equilibrium mixture?

Accepted Answer

All of the given factors - increasing volume, temperature and pressure - can alter the composition of an equilibrium mixture.

Increasing volume will shift the equilibrium towards the side with more moles of gas, in order to occupy the increased volume.

Increasing temperature will shift the equilibrium in the endothermic direction (if the reaction is exothermic) and in the exothermic direction (if the reaction is endothermic) to counteract the added heat.

Increasing pressure will shift the equilibrium in the direction with fewer moles of gas, in order to reduce the total pressure.

Question 11

For the reaction H₂(g)+ S(s)⇌ H₂S(g),if the rate constant for the forward reaction is greater than the rate constant for the reverse reaction,the value of K_c must be ________ (equal to,greater than,less than)1.

Accepted Answer

The answer of For the reaction H₂(g)+ S(s)⇌ H₂S(g),if the...

Question 12

Which of the following statements about a catalyst is true?

Accepted Answer

A catalyst provides an alternate lower energy pathway for a reaction, which allows the reaction to proceed more easily and quickly without being consumed in the reaction. Options A and B are incorrect as they do not describe the role of a catalyst accurately. Option C is also incorrect as a catalyst is not consumed in a reaction.

Question 13

At 1000 K,K_p = 19.9 for the reaction Fe₂O₃(s)+ 3 CO(g)⇌ 2 Fe(s)+ 3 CO₂(g).What is the value of K_p for the reaction 2 Fe₂O₃(s)+ 6 CO(g)⇌ 4 Fe(s)+ 6 CO₂(g)?

Accepted Answer

The answer of At 1000 K,K_p = 19.9 for the...

Question 14

At 1000 K,K_p = 19.9 for the reaction Fe₂O₃(s)+ 3 CO(g)⇌ 2 Fe(s)+ 3 CO₂(g).What is the value of K_p for the reaction 8 Fe(s)+ 12 CO₂(g)⇌ 4 Fe₂O₃(s)+ 12 CO(g)?

Accepted Answer

The answer of At 1000 K,K_p = 19.9 for the...

Question 15

The overall reaction for photosynthesis can be represented by the following equation: 6 CO₂(g)+ 6 H₂O(l)⇌ C₆H₁₂O₆(s)+ 6 O₂(g) The enthalpy change for this reaction is 2802 kJ.Which of the following changes in condition will shift the equilibrium to the right?

Accepted Answer

According to Le Chatelier's principle, if a stress is applied to a system in equilibrium, the system will shift in the direction that counteracts the stress. In this case, increasing the temperature will increase the kinetic energy of the molecules in the system leading to an increase in the rate of the forward reaction, which will shift the equilibrium to the right. Increasing the pressure of gas or adding water or solid product will not affect the equilibrium as they are not part of the gaseous reactant or product. Adding more solid product will shift the equilibrium to the left according to Le Chatelier's principle.

Question 16

A reaction in which reactants form products in the forward reaction and products simultaneously form reactants in the reverse reaction is said to be ________.

Accepted Answer

The answer of A reaction in which reactants form products...

Question 17

For the reaction shown below,which change in conditions made to the system at equilibrium will result in a net reaction to the right to form more product? C(s)+ 2 H₂(g)⇌ CH₄(g)ΔH° = -74.8 kJ

Accepted Answer

According to Le Chatelier's principle, increasing the concentration of one of the reactants will shift the equilibrium towards the side of the reaction with fewer moles of gas. In this case, increasing the concentration of H₂ will shift the equilibrium to the right to form more product, CH₄.

Question 18

At 298 K,K_p = 2.1 × 10⁴ for the reaction CO(g)+ 2 H₂(g)⇌ CH₃OH(g).What is the value of K_c at this temperature?

Accepted Answer

The answer of At 298 K,K_p = 2.1 × 10⁴...

Question 19

K_c = 1.2 × 10^-42at 500 K for the reaction shown below. H₂(g)⇌ 2 H(g) If [H₂] = 1 × 10^-2 M and [H] = 1.2 × 10^-22 M,in order to achieve equilibrium a net reaction must occur from ________ to ________ until Q_c = ________.

Accepted Answer

The answer of K_c = 1.2 × 10^-42at 500...

Question 20

The decomposition of nitrosyl bromide is exothermic: 2 NOBr(g)⇌ 2 NO(g)+ Br₂(g).Which of the following changes in reaction condition will shift the reaction to the left?

Accepted Answer

The answer of The decomposition of nitrosyl bromide is exothermic:...

Quiz 14: Chemical Equilibrium

At an elevated temperature,K_p = 0.19 for the reaction 2 NOCl(g)⇌ 2 NO(g)+ Cl₂(g).If the initial partial pressures of NOCl,NO,and Cl₂ are 0.50 atm,0.25 atm,and 0.45 atm,respectively,a net ________ (forward,reverse)reaction must occur in order to achieve equilibrium.

For the reaction shown below the value of K_p is ________ than the value of K_c,because Δn = ________. N₂O₄(g)⇌ 2 NO₂(g)

K_c = 57.0at 700 K for the reaction shown below. H₂(g)+ I₂(g)⇌ 2 HI(g) If [H₂(g)] = [I₂(g)] = 0.200 M at equilibrium,the molar concentration [HI((g)] = ________ at equilibrium.

For the reaction shown below the equilibrium constant expression for K_c= ________. HF(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ F^-(aq)

Which of the following changes in reaction conditions will not alter the composition of a homogeneous equilibrium mixture of gases in a reaction having unequal moles of gaseous products and reactants?

In a reversible reaction,when the rate of the forward reaction equals the rate of the reverse reaction,the reaction is at ________.

At 298 K,K_c = 1.7 × 10^-56 for the reaction 3 O₂(g)⇌ 2 O₃(g).What is the value of K_p at this temperature?

For the reaction shown below,N₂O₄ and NO₂ have equilibrium concentrations,[N₂O₄]_eq = 2.160 × 10^-⁴ and [NO₂]_eq = 1.001 × 10^-³,respectively.The equilibrium constant,K_c,for this reaction equals ________. N₂O₄(g)⇌ 2 NO₂(g)

For the reaction CaCO₃(s)⇌ CaO(s)+ O₂(g)the equilibrium expression is K_p = ________.

Which will alter the composition of an equilibrium mixture?

For the reaction H₂(g)+ S(s)⇌ H₂S(g),if the rate constant for the forward reaction is greater than the rate constant for the reverse reaction,the value of K_c must be ________ (equal to,greater than,less than)1.

Which of the following statements about a catalyst is true?

At 1000 K,K_p = 19.9 for the reaction Fe₂O₃(s)+ 3 CO(g)⇌ 2 Fe(s)+ 3 CO₂(g).What is the value of K_p for the reaction 2 Fe₂O₃(s)+ 6 CO(g)⇌ 4 Fe(s)+ 6 CO₂(g)?

At 1000 K,K_p = 19.9 for the reaction Fe₂O₃(s)+ 3 CO(g)⇌ 2 Fe(s)+ 3 CO₂(g).What is the value of K_p for the reaction 8 Fe(s)+ 12 CO₂(g)⇌ 4 Fe₂O₃(s)+ 12 CO(g)?

The overall reaction for photosynthesis can be represented by the following equation: 6 CO₂(g) + 6 H₂O(l) ⇌ C₆H₁₂O₆(s) + 6 O₂(g) The enthalpy change for this reaction is 2802 kJ.Which of the following changes in condition will shift the equilibrium to the right?

A reaction in which reactants form products in the forward reaction and products simultaneously form reactants in the reverse reaction is said to be ________.

For the reaction shown below,which change in conditions made to the system at equilibrium will result in a net reaction to the right to form more product? C(s) + 2 H₂(g) ⇌ CH₄(g) ΔH° = -74.8 kJ

At 298 K,K_p = 2.1 × 10⁴ for the reaction CO(g)+ 2 H₂(g)⇌ CH₃OH(g).What is the value of K_c at this temperature?

K_c = 1.2 × 10^-42at 500 K for the reaction shown below. H₂(g)⇌ 2 H(g) If [H₂] = 1 × 10^-2 M and [H] = 1.2 × 10^-22 M,in order to achieve equilibrium a net reaction must occur from to until Q_c = ________.

The decomposition of nitrosyl bromide is exothermic: 2 NOBr(g) ⇌ 2 NO(g) + Br₂(g) .Which of the following changes in reaction condition will shift the reaction to the left?

Quiz 14: Chemical Equilibrium

At an elevated temperature,Kp = 0.19 for the reaction 2 NOCl(g)⇌ 2 NO(g)+ Cl2(g).If the initial partial pressures of NOCl,NO,and Cl2 are 0.50 atm,0.25 atm,and 0.45 atm,respectively,a net ________ (forward,reverse)reaction must occur in order to achieve equilibrium.

For the reaction shown below the value of Kp is ________ than the value of Kc,because Δn = ________. N2O4(g)⇌ 2 NO2(g)

Kc = 57.0 at 700 K for the reaction shown below. H2(g)+ I2(g)⇌ 2 HI(g) If [H2(g)] = [I2(g)] = 0.200 M at equilibrium,the molar concentration [HI((g)] = ________ at equilibrium.

For the reaction shown below the equilibrium constant expression for Kc = ________. HF(aq)+ H2O(l)⇌ H3O+(aq)+ F-(aq)

Which of the following changes in reaction conditions will not alter the composition of a homogeneous equilibrium mixture of gases in a reaction having unequal moles of gaseous products and reactants?

In a reversible reaction,when the rate of the forward reaction equals the rate of the reverse reaction,the reaction is at ________.

At 298 K,Kc = 1.7 × 10-56 for the reaction 3 O2(g)⇌ 2 O3(g).What is the value of Kp at this temperature?

For the reaction shown below,N2O4 and NO2 have equilibrium concentrations,[N2O4]eq = 2.160 × 10-4 and [NO2]eq = 1.001 × 10-3,respectively.The equilibrium constant,Kc,for this reaction equals ________. N2O4(g)⇌ 2 NO2(g)

For the reaction CaCO3(s)⇌ CaO(s)+ O2(g)the equilibrium expression is Kp = ________.

Which will alter the composition of an equilibrium mixture?

For the reaction H2(g)+ S(s)⇌ H2S(g),if the rate constant for the forward reaction is greater than the rate constant for the reverse reaction,the value of Kc must be ________ (equal to,greater than,less than)1.

Which of the following statements about a catalyst is true?

At 1000 K,Kp = 19.9 for the reaction Fe2O3(s)+ 3 CO(g)⇌ 2 Fe(s)+ 3 CO2(g).What is the value of Kp for the reaction 2 Fe2O3(s)+ 6 CO(g)⇌ 4 Fe(s)+ 6 CO2(g)?

At 1000 K,Kp = 19.9 for the reaction Fe2O3(s)+ 3 CO(g)⇌ 2 Fe(s)+ 3 CO2(g).What is the value of Kp for the reaction 8 Fe(s)+ 12 CO2(g)⇌ 4 Fe2O3(s)+ 12 CO(g)?

The overall reaction for photosynthesis can be represented by the following equation: 6 CO2(g) + 6 H2O(l) ⇌ C6H12O6(s) + 6 O2(g) The enthalpy change for this reaction is 2802 kJ.Which of the following changes in condition will shift the equilibrium to the right?

A reaction in which reactants form products in the forward reaction and products simultaneously form reactants in the reverse reaction is said to be ________.

For the reaction shown below,which change in conditions made to the system at equilibrium will result in a net reaction to the right to form more product? C(s) + 2 H2(g) ⇌ CH4(g) ΔH° = -74.8 kJ

At 298 K,Kp = 2.1 × 104 for the reaction CO(g)+ 2 H2(g)⇌ CH3OH(g).What is the value of Kc at this temperature?

Kc = 1.2 × 10-42 at 500 K for the reaction shown below. H2(g)⇌ 2 H(g) If [H2] = 1 × 10-2 M and [H] = 1.2 × 10-22 M,in order to achieve equilibrium a net reaction must occur from ________ to ________ until Qc = ________.

The decomposition of nitrosyl bromide is exothermic: 2 NOBr(g) ⇌ 2 NO(g) + Br2(g) .Which of the following changes in reaction condition will shift the reaction to the left?

At an elevated temperature,K_p = 0.19 for the reaction 2 NOCl(g)⇌ 2 NO(g)+ Cl₂(g).If the initial partial pressures of NOCl,NO,and Cl₂ are 0.50 atm,0.25 atm,and 0.45 atm,respectively,a net ________ (forward,reverse)reaction must occur in order to achieve equilibrium.

For the reaction shown below the value of K_p is ________ than the value of K_c,because Δn = ________. N₂O₄(g)⇌ 2 NO₂(g)

K_c = 57.0at 700 K for the reaction shown below. H₂(g)+ I₂(g)⇌ 2 HI(g) If [H₂(g)] = [I₂(g)] = 0.200 M at equilibrium,the molar concentration [HI((g)] = ________ at equilibrium.

For the reaction shown below the equilibrium constant expression for K_c= ________. HF(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ F^-(aq)

At 298 K,K_c = 1.7 × 10^-56 for the reaction 3 O₂(g)⇌ 2 O₃(g).What is the value of K_p at this temperature?

For the reaction shown below,N₂O₄ and NO₂ have equilibrium concentrations,[N₂O₄]_eq = 2.160 × 10^-⁴ and [NO₂]_eq = 1.001 × 10^-³,respectively.The equilibrium constant,K_c,for this reaction equals ________. N₂O₄(g)⇌ 2 NO₂(g)

For the reaction CaCO₃(s)⇌ CaO(s)+ O₂(g)the equilibrium expression is K_p = ________.

For the reaction H₂(g)+ S(s)⇌ H₂S(g),if the rate constant for the forward reaction is greater than the rate constant for the reverse reaction,the value of K_c must be ________ (equal to,greater than,less than)1.

At 1000 K,K_p = 19.9 for the reaction Fe₂O₃(s)+ 3 CO(g)⇌ 2 Fe(s)+ 3 CO₂(g).What is the value of K_p for the reaction 2 Fe₂O₃(s)+ 6 CO(g)⇌ 4 Fe(s)+ 6 CO₂(g)?

At 1000 K,K_p = 19.9 for the reaction Fe₂O₃(s)+ 3 CO(g)⇌ 2 Fe(s)+ 3 CO₂(g).What is the value of K_p for the reaction 8 Fe(s)+ 12 CO₂(g)⇌ 4 Fe₂O₃(s)+ 12 CO(g)?

The overall reaction for photosynthesis can be represented by the following equation: 6 CO₂(g) + 6 H₂O(l) ⇌ C₆H₁₂O₆(s) + 6 O₂(g) The enthalpy change for this reaction is 2802 kJ.Which of the following changes in condition will shift the equilibrium to the right?

For the reaction shown below,which change in conditions made to the system at equilibrium will result in a net reaction to the right to form more product? C(s) + 2 H₂(g) ⇌ CH₄(g) ΔH° = -74.8 kJ

At 298 K,K_p = 2.1 × 10⁴ for the reaction CO(g)+ 2 H₂(g)⇌ CH₃OH(g).What is the value of K_c at this temperature?

K_c = 1.2 × 10^-42at 500 K for the reaction shown below. H₂(g)⇌ 2 H(g) If [H₂] = 1 × 10^-2 M and [H] = 1.2 × 10^-22 M,in order to achieve equilibrium a net reaction must occur from to until Q_c = ________.

The decomposition of nitrosyl bromide is exothermic: 2 NOBr(g) ⇌ 2 NO(g) + Br₂(g) .Which of the following changes in reaction condition will shift the reaction to the left?