The equilibrium constant, K c , for the reaction 2NOCl(g) ⇌ 2NO(g) + Cl 2 (g) is 6.0x10 −4 at a certain temperature. A mixture of [NOCl] = 0.20M, [NO] = 0.10M, and [Cl 2 ] = 0.40M was introduced into a container at this temperature. Which of the following is true?

The reaction would shift to form NOCl.

The reaction would shift to form NO and Cl 2 .

The reaction is at equilibrium and, therefore, no shifting will occur.

The reaction is NOT at equilibrium and, therefore, no shifting will occur.

Suppose the reaction A(aq) + 3 B(aq) ⇌ 2 C(aq) has a value of K = 10.0 at a certain temperature. If 0.5 moles of A, 0.5 moles of B and 0.5 moles of C are placed in a 5 L solution, which direction would the reaction initially proceed?

The reaction will shift to form reactants because Q > K.

The reaction will shift to form product because Q > K.

The reaction will shift to form product because Q < K.

The reaction will shift to form reactants because Q < K.

2 X(aq) ⇄ 3 Y(aq) + Z(aq) At room temperature, the equilibrium constant for the reaction shown is 5.0x10⁻ 82 . At 100°C, the equilibrium constant for the same reaction is 4x10⁶. As an equilibrium mixture at room temperature is heated to a warmer temperature, what will occur?

The concentrations of Y and Z will increase. Also written as "[Y] and [Z] will increase."

The concentration of X will increase. Also written as "[X] will increase."

The concentrations of all species will remain unchanged because Q > K.

The concentrations of all species will remain unchanged because Q < K.

2 X(aq) ⇄ 3 Y(aq) + Z(aq) At room temperature, the equilibrium constant for the reaction shown is 3.0x10 25 . At 100°C, the equilibrium constant for the same reaction is 8.6x10 -6 . As an equilibrium mixture at room temperature is heated to a warmer temperature, what will occur?

The concentration of X will increase. Also written as "[X] will increase."

The concentration of Z will increase. Also written as "[Z] will increase."

The concentrations of all species will remain unchanged because Q > K.

The concentrations of all species will remain unchanged because Q < K.

Fe 3+ (g) + SCN 1− (g) ⇌ Fe(SCN) 2+ (g) The synthesis of the complex Fe(SCN) 2+ ion is shown in the equilibrium above. A pure sample of Fe(SCN) 2+ is placed in a rigid, evacuated 1.00 L container. The initial pressure of the Fe(SCN) 2+ is 1.00 atm. The temperature is held constant until equilibrium is established. At equilibrium the partial pressure of the Fe 3+ (g), SCN 1− (g), and Fe(SCN) 2+ (g) is 0.20atm, 0.20atm, and 0.80atm respectively. What is the value of the equilibrium constant, Kp ?

It cannot be determined whether K p > 1, K p < 1, or K p = 1 without additional information.

Fe 3+ (g) + SCN 1− (g) ⇌ Fe(SCN) 2+ (g) The synthesis of the complex Fe(SCN) 2+ ion is shown in the equilibrium above. A pure sample of Fe(SCN) 2+ is placed in a rigid, evacuated 1.00 L container. The initial pressure of the Fe(SCN) 2+ is 1.00 atm. The temperature is held constant until equilibrium is established. At equilibrium the partial pressure of the Fe 3+ (g), SCN 1− (g), and Fe(SCN) 2+ (g) is 0.20atm, 0.20atm, and 0.80atm respectively. As the reaction progresses toward equilibrium, what happens to the rate of the forward reaction?

increases until it becomes the same as the reverse reaction rate at equilibrium.

decreases to become a constant nonzero rate at equilibrium.

stays constant before and after equilibrium is reached.

decreases to become zero at equilibrium.

Fe 3+ (g) + SCN 1− (g) ⇌ Fe(SCN) 2+ (g) The synthesis of the complex Fe(SCN) 2+ ion is shown in the equilibrium above. A pure sample of Fe(SCN) 2+ is placed in a rigid, evacuated 1.00 L container. The initial pressure of the Fe(SCN) 2+ is 1.00 atm. The temperature is held constant until equilibrium is established. At equilibrium the partial pressure of the Fe 3+ (g), SCN 1− (g), and Fe(SCN) 2+ (g) is 0.20atm, 0.20atm, and 0.80atm respectively. As the reaction progresses toward equilibrium, what happens to the rate of the reverse reaction?

decreases to become a constant nonzero rate at equilibrium.

stays constant before and after equilibrium is reached.

decreases to become zero at equilibrium.

increases until it becomes the same as the forward reaction rate at equilibrium.

AP Chem Unit 07 Days 01-02 Practice

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AP Chem Unit 07 Days 01-02 Practice

Quiz

•

Chemistry

•

11th Grade

•

Practice Problem

•

Easy

•

NGSS

HS-PS1-5, HS-PS1-7, HS-PS1-6

Standards-aligned

Patrick Boylan

Used 71+ times

FREE Resource

23 questions

Show all answers

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

Write the general equilibrium constant for
2NaBr(aq) + Pb(ClO₄)₂(aq) ⇄ PbBr₂(s) + 2NaClO₄(aq)

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

NO₂(g) + CO(g) ⇄ NO(g)+ CO₂(g) K = 1.2x10⁻⁷
Given the information above, how do the equilibrium concentrations of the reactants compare to the equilibrium concentrations of the products?

They are much smaller.

They are much bigger.

They are approximately the same.

They are identical.

NO₂(g) + CO(g) ⇄ NO(g)+ CO₂(g) K = 1.2x10⁷
Given the information above, how do the equilibrium concentrations of the reactants compare to the equilibrium concentrations of the products?

They are much smaller.

They are much bigger.

They are approximately the same.

They are identical.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Analyze the equilibrium mixture with its corresponding equation shown. Which K value correctly describes this mixture at equilibrium?

K = 0

K = 1

K > 1

K < 1

In which of the following cases will the LEAST time be required to arrive at equilibrium? The value of K below refers to the equilibrium constant.

K is a very small number.

K is a very large number.

K is equal to 1.

Cannot tell since the time to arrive at equilibrium does not depend on K.

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

In which of the following cases will the LEAST time be required to arrive at equilibrium?
Reaction I: A⇌B K = 4x10^-23
Reaction II: B⇌C K = 8x10^-2
Reaction III: C⇌D K = 5x10¹²

Reaction I

Reaction II

Reaction III

Cannot tell since the time to arrive at equilibrium does not depend on K.

MULTIPLE CHOICE QUESTION

2 mins • 1 pt

The equilibrium
A(aq) + B(aq) ⇌ 2C(aq)
exists in a closed container at 273K. If the molar concentrations of A, B, and C at equilibrium are [A] = 2.00M, [B] = 0.50M and [C] = 6.00M, respectively, what is value of the equilibrium constant at 273K?

0.030

6.0

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AP Chem Unit 07 Days 01-02 Practice

23 questions

Write the general equilibrium constant for
2NaBr(aq) + Pb(ClO₄)₂(aq) ⇄ PbBr₂(s) + 2NaClO₄(aq)

NO₂(g) + CO(g) ⇄ NO(g)+ CO₂(g) K = 1.2x10⁻⁷
Given the information above, how do the equilibrium concentrations of the reactants compare to the equilibrium concentrations of the products?

NO₂(g) + CO(g) ⇄ NO(g)+ CO₂(g) K = 1.2x10⁷
Given the information above, how do the equilibrium concentrations of the reactants compare to the equilibrium concentrations of the products?

Analyze the equilibrium mixture with its corresponding equation shown. Which K value correctly describes this mixture at equilibrium?

In which of the following cases will the LEAST time be required to arrive at equilibrium? The value of K below refers to the equilibrium constant.

In which of the following cases will the LEAST time be required to arrive at equilibrium?
Reaction I: A⇌B K = 4x10^-23
Reaction II: B⇌C K = 8x10^-2
Reaction III: C⇌D K = 5x10¹²

The equilibrium
A(aq) + B(aq) ⇌ 2C(aq)
exists in a closed container at 273K. If the molar concentrations of A, B, and C at equilibrium are [A] = 2.00M, [B] = 0.50M and [C] = 6.00M, respectively, what is value of the equilibrium constant at 273K?

The value of the equilibrium constant for the reaction
H₂(g) + I₂(g) ⇌ 2HI(g)
is 4.0×10⁻⁴ at a specified temperature. What would be the value of that constant for the reverse reaction under these same conditions?

Given the information
2 X(g) + Y(g) ⇌ 2 Z(g) K_c = 100
Determine the value of the equilibrium constant, K_c , for the following reaction at the same temperature and pressure.
Z(g) ⇌ X(g) + ½Y(g) K_c = ??

Given the equilibria and equilibrium constants shown, the correct expression for K₃ in terms of K₁ and K₂ is

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AP Chem Unit 07 Days 01-02 Practice

23 questions

Write the general equilibrium constant for2NaBr(aq) + Pb(ClO4)2(aq) ⇄ PbBr2(s) + 2NaClO4(aq)

NO2(g) + CO(g) ⇄ NO(g)+ CO2(g) K = 1.2x10−7Given the information above, how do the equilibrium concentrations of the reactants compare to the equilibrium concentrations of the products?

NO2(g) + CO(g) ⇄ NO(g)+ CO2(g) K = 1.2x107Given the information above, how do the equilibrium concentrations of the reactants compare to the equilibrium concentrations of the products?

Analyze the equilibrium mixture with its corresponding equation shown. Which K value correctly describes this mixture at equilibrium?

In which of the following cases will the LEAST time be required to arrive at equilibrium? The value of K below refers to the equilibrium constant.

In which of the following cases will the LEAST time be required to arrive at equilibrium?Reaction I: A⇌B K = 4x10-23Reaction II: B⇌C K = 8x10-2Reaction III: C⇌D K = 5x1012

The equilibrium A(aq) + B(aq) ⇌ 2C(aq)exists in a closed container at 273K. If the molar concentrations of A, B, and C at equilibrium are [A] = 2.00M, [B] = 0.50M and [C] = 6.00M, respectively, what is value of the equilibrium constant at 273K?

The value of the equilibrium constant for the reactionH2(g) + I2(g) ⇌ 2HI(g)is 4.0×10−4 at a specified temperature. What would be the value of that constant for the reverse reaction under these same conditions?

Given the information2 X(g) + Y(g) ⇌ 2 Z(g) Kc = 100Determine the value of the equilibrium constant, Kc , for the following reaction at the same temperature and pressure.Z(g) ⇌ X(g) + ½Y(g) Kc = ??

Given the equilibria and equilibrium constants shown, the correct expression for K3 in terms of K1 and K2 is

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Write the general equilibrium constant for
2NaBr(aq) + Pb(ClO₄)₂(aq) ⇄ PbBr₂(s) + 2NaClO₄(aq)

NO₂(g) + CO(g) ⇄ NO(g)+ CO₂(g) K = 1.2x10⁻⁷
Given the information above, how do the equilibrium concentrations of the reactants compare to the equilibrium concentrations of the products?

NO₂(g) + CO(g) ⇄ NO(g)+ CO₂(g) K = 1.2x10⁷
Given the information above, how do the equilibrium concentrations of the reactants compare to the equilibrium concentrations of the products?

In which of the following cases will the LEAST time be required to arrive at equilibrium?
Reaction I: A⇌B K = 4x10^-23
Reaction II: B⇌C K = 8x10^-2
Reaction III: C⇌D K = 5x10¹²

The equilibrium
A(aq) + B(aq) ⇌ 2C(aq)
exists in a closed container at 273K. If the molar concentrations of A, B, and C at equilibrium are [A] = 2.00M, [B] = 0.50M and [C] = 6.00M, respectively, what is value of the equilibrium constant at 273K?

The value of the equilibrium constant for the reaction
H₂(g) + I₂(g) ⇌ 2HI(g)
is 4.0×10⁻⁴ at a specified temperature. What would be the value of that constant for the reverse reaction under these same conditions?

Given the information
2 X(g) + Y(g) ⇌ 2 Z(g) K_c = 100
Determine the value of the equilibrium constant, K_c , for the following reaction at the same temperature and pressure.
Z(g) ⇌ X(g) + ½Y(g) K_c = ??

Given the equilibria and equilibrium constants shown, the correct expression for K₃ in terms of K₁ and K₂ is