Equilibrium constant problems worksheet answers

This equilibrium practice problem set includes questions on writing the equilibrium constant of given chemical reactions, determining the value of the equilibrium constant based on the concentrations and partial pressures of gases, deriving a new expression for an equilibrium constant from separate reactions, converting between K_c and K_p, calculating the quotient and determining the course of the reaction, calculations of concentrations based on the quotient and equilibrium constant, as well as working on equilibrium reactions based on the Le Châtelier’s principle.

The links to the corresponding articles are provided herein:

• Chemical Equilibrium
• Equilibrium Constant
• K_pand Partial Pressure
• K_pandK_cRelationship
• KChanges with Chemical Equation
• Equilibrium Constant K from Two Reactions
• Reaction Quotient – Q
• ICE Table – Calculating Equilibrium Concentrations
• ICE Table Practice Problems
• Le Châtelier’s principle
• Le Châtelier’s principle Practice Problems
• Chemical Equilibrium Practice Problems

Practice

Write the equilibrium expression (K) for each of the following reactions.

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Tree different reactions are represented in the diagram below. The reaction equations can be written as A + X ⇆ AX (X = B, C, or D).

(a) Which reaction has the largest equilibrium constant? (b) Which reaction has the smallest equilibrium constant?

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The following graph represents an initial mixture of N₂ and H₂ at high temperature and pressure:

The gases react to form ammonia gas (NH₃) as represented by the following concentration profile:

a) Label each plot on the graph as H₂, N₂, or NH₃, and explain your answers.

b) What information do the relative shapes of the plots tell us?

c) At what time is equilibrium reached?

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At a particular temperature, it is determined for the reaction

that at equilibrium, the concentrations are as follows: [NO(g)] = 3.2 x 10 -3 M, [H₂(g)] = 6.7 x 10 -6 M, [N₂(g)] = 4.8 x 10 -2 M, and [H₂O(g)] = 2.4 x 10 -2 M. What is the value of the equilibrium constant K for the reaction at this temperature?

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Given the equilibrium concentrations, calculate the value of the equilibrium constant K for the reaction between CO₂ and H₂ that produces methanol and water at high temperature.

[CO₂] = 0.061 M, [H₂] = 0.079 M, [CH₃OH] = 4.7 x 10 2 M, and [H₂O] = 5.7 x 10 4 M Calculate the value of K for the reaction.

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The reaction for converting methane to acetylene has an equilibrium constant of K = 0.154 at 2000 K.

Calculate the equilibrium constant for this process if the reaction is represented as follows:

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The following reaction has an equilibrium constant of K_p = 4.42 x 10 -5 at 298 K:

Calculate the equilibrium constant for this process if the reaction is represented as follows:

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The equilibrium constant values for the reactions below were determined at a certain temperature:

Using these data, determine the equilibrium constant Kc for the following reaction:

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The equilibrium constant values for the reactions below were determined at a certain temperature:

Using these data, determine the equilibrium constant Kc for the following reaction:

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The following equilibrium pressures were observed at a certain temperature for the Haber process

Calculate the value for the equilibrium constant Kp at this temperature.

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Consider the following reactions:

In which reaction are the K and Kp equal?

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At 300 K, the equilibrium concentrations for the following reaction are [CH₃OH] = 0.240 M, [CO] = 0.350 M, and [H₂] = 1.65 M for the reaction

Calculate Kp at this temperature.

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Given the equilibrium constant, calculate Kp for each of the following reactions at 298 K.

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Calculate the K_c for each reaction at 298 K.

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Consider the reaction between nitrogen and hydrogen gases:

Using the data given in the table, complete the missing numbers assuming that all concentrations are measured at equilibrium.

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