Question

1) The equilibrium constant, Kc, for the reaction below is 0.10 at 25°C. Find the equilibrium concentration of chlorine gas, Cl2(g), if the equilibrium concentrations of ICl(g) and I2(g) are known to be 0.50 M and 0.40 M respectively. 2 ICl(g) ? Cl2(g) + I2(g) 2) The equilibrium constant, Kp, is 7.6 x 10?¹? at 1000°C for the reaction represented below. 2 H?O(g) ? 2 H?(g) + O?(g) a. Write the equilibrium expression, Kp, for the reaction. b. Suppose you start out with only H?O(g) in a rigid container, and its initial partial pressure is recorded to be 1.27 atm. What are the partial pressures of each species when the system reaches equilibrium? 3) The equilibrium constant, Kp, is 4.8 x 10?³¹ at 25°C for the reaction represented below. N?(g) + O?(g) ? 2 NO(g) a. Write the equilibrium expression, Kp, for the reaction. b. Suppose you start out with only reactants in a rigid container. The initial partial pressure of N?(g) is 0.675 atm and that of O?(g) is 0.472 atm. What are the partial pressures of each gas when the system reaches equilibrium? 4) The equilibrium constant, Kc, is 3.2 x 10?³? at 25 °C for the reaction represented below. 2 HCl(g) ? H?(g) + Cl?(g) a. Write the equilibrium expression, Kc, for the reaction. b. Suppose you start out with only reactants in a rigid container at 25°C. The initial concentration of HCl(g) is measured to be 0.375 M. What are the concentrations of each gas when the system reaches equilibrium? 5) The equilibrium constant, Kp, is 4.51x10?? at 450°C for the reaction represented below. N?(g) + 3 H?(g) ? 2 NH?(g) a. Write the equilibrium expression, Kp, for the reaction. b. Suppose you start out with only reactants in a rigid container. The initial partial pressure of N?(g) is 1.0 atm and that of H?(g) is 1.4 atm. What are the partial pressures of each species when the system reaches equilibrium?

          1) The equilibrium constant, Kc, for the reaction below is 0.10 at 25°C. Find the equilibrium concentration of chlorine gas, Cl2(g), if the equilibrium concentrations of ICl(g) and I2(g) are known to be 0.50 M and 0.40 M respectively.

2 ICl(g) ? Cl2(g) + I2(g)

2) The equilibrium constant, Kp, is 7.6 x 10?¹? at 1000°C for the reaction represented below.

2 H?O(g) ? 2 H?(g) + O?(g)

a. Write the equilibrium expression, Kp, for the reaction.
b. Suppose you start out with only H?O(g) in a rigid container, and its initial partial pressure is recorded to be 1.27 atm. What are the partial pressures of each species when the system reaches equilibrium?

3) The equilibrium constant, Kp, is 4.8 x 10?³¹ at 25°C for the reaction represented below.

N?(g) + O?(g) ? 2 NO(g)

a. Write the equilibrium expression, Kp, for the reaction.
b. Suppose you start out with only reactants in a rigid container. The initial partial pressure of N?(g) is 0.675 atm and that of O?(g) is 0.472 atm. What are the partial pressures of each gas when the system reaches equilibrium?

4) The equilibrium constant, Kc, is 3.2 x 10?³? at 25 °C for the reaction represented below.

2 HCl(g) ? H?(g) + Cl?(g)

a. Write the equilibrium expression, Kc, for the reaction.
b. Suppose you start out with only reactants in a rigid container at 25°C. The initial concentration of HCl(g) is measured to be 0.375 M. What are the concentrations of each gas when the system reaches equilibrium?

5) The equilibrium constant, Kp, is 4.51x10?? at 450°C for the reaction represented below.

N?(g) + 3 H?(g) ? 2 NH?(g)

a. Write the equilibrium expression, Kp, for the reaction.
b. Suppose you start out with only reactants in a rigid container. The initial partial pressure of N?(g) is 1.0 atm and that of H?(g) is 1.4 atm. What are the partial pressures of each species when the system reaches equilibrium?

1) The equilibrium constant, Kc, for the reaction below is 0.10 at 25°C. Find the equilibrium concentration of chlorine gas, Cl2(g), if the equilibrium concentrations of ICl(g) and I2(g) are known to be 0.50 M and 0.40 M respectively.

2 ICl(g) ? Cl2(g) + I2(g)

2) The equilibrium constant, Kp, is 7.6 x 10?¹? at 1000°C for the reaction represented below.

2 H?O(g) ? 2 H?(g) + O?(g)

a. Write the equilibrium expression, Kp, for the reaction.
b. Suppose you start out with only H?O(g) in a rigid container, and its initial partial pressure is recorded to be 1.27 atm. What are the partial pressures of each species when the system reaches equilibrium?

3) The equilibrium constant, Kp, is 4.8 x 10?³¹ at 25°C for the reaction represented below.

N?(g) + O?(g) ? 2 NO(g)

a. Write the equilibrium expression, Kp, for the reaction.
b. Suppose you start out with only reactants in a rigid container. The initial partial pressure of N?(g) is 0.675 atm and that of O?(g) is 0.472 atm. What are the partial pressures of each gas when the system reaches equilibrium?

4) The equilibrium constant, Kc, is 3.2 x 10?³? at 25 °C for the reaction represented below.

2 HCl(g) ? H?(g) + Cl?(g)

a. Write the equilibrium expression, Kc, for the reaction.
b. Suppose you start out with only reactants in a rigid container at 25°C. The initial concentration of HCl(g) is measured to be 0.375 M. What are the concentrations of each gas when the system reaches equilibrium?

5) The equilibrium constant, Kp, is 4.51x10?? at 450°C for the reaction represented below.

N?(g) + 3 H?(g) ? 2 NH?(g)

a. Write the equilibrium expression, Kp, for the reaction.
b. Suppose you start out with only reactants in a rigid container. The initial partial pressure of N?(g) is 1.0 atm and that of H?(g) is 1.4 atm. What are the partial pressures of each species when the system reaches equilibrium?

Added by Jordan C.

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