Question : 51.              Consider the reaction and its equilibrium constant: S2Cl2(g) + Cl2(g) : 1335522

51.              Consider the reaction and its equilibrium constant:

S2Cl2(g) + Cl2(g) 2SCl2(g)  Keq = 4

Examine the figure, and determine if the system is at equilibrium. If it is not, in which direction will it proceed to reach equilibrium?

A)The reaction is at equilibrium.

B)The reaction is not at equilibrium, it will shift to the left.

C)The reaction is not at equilibrium, it will shift to the right.

D)It is not possible to tell if the reaction is at equilibrium.

E)To reach equilibrium, the value of Keq must change.

52.              Consider the reaction CO(g) + H2O(g) CO2(g) + H2(g), represented by the following diagram:

What is the composition of this system when the reaction reaches equilibrium?

A)3 CO, 3 H2O, 7 CO2, 7 H2D)8 CO, 8 H2O, 2 CO2, 2 H2

B)1 CO, 1 H2O, 4 CO2, 4 H2E)4 CO, 6 H2O, 4 CO2, 6 H2

C)2 CO, 2 H2O, 8 CO2, 8 H2

53.              The reaction S2Cl2(g) + Cl2(g) 2SCl2(g) has an equilibrium constant of K = 8.  The image shows a partially reacted system.  What is the composition of this system when the reaction reaches equilibrium?

A)1 S2Cl2, 3 Cl2, 10 SCl2D)4 S2Cl2, 6 Cl2, 4 SCl2

B)2 S2Cl2, 4 Cl2, 8 SCl2E)5 S2Cl2, 7 Cl2, 2 SCl2

C)3 S2Cl2, 5 Cl2, 6 SCl2

54.              The value of the equilibrium constant at a given temperature for the reaction:

2HI(g) H2(g) + I2(g)

is 0.200.  If [HI] = 0.200 M, [H2] = 0.200 M, and [I2] = 0.200 M, determine if the reaction is at equilibrium. If it is not, in which direction will it proceed to reach equilibrium?

A)The reaction is at equilibrium.

B)The reaction is not at equilibrium, it will shift to the left.

C)The reaction is not at equilibrium, it will shift to the right.

D)It is not possible to tell if the reaction is at equilibrium.

E)To reach equilibrium, the value of Keq must change.

55.              The value of the equilibrium constant at a given temperature for the reaction:

CO(g) + H2O(g) CO2(g) + H2(g)

is 16.  If [CO] = 4.0 M, [H2O] = 4.0 M, [CO2] = 4.0 M, and [H2] = 4.0 M, determine if the reaction is at equilibrium. If it is not, in which direction will it proceed to reach equilibrium?

A)The reaction is at equilibrium.

B)The reaction is not at equilibrium, it will shift to the left.

C)The reaction is not at equilibrium, it will shift to the right.

D)It is not possible to tell if the reaction is at equilibrium.

E)To reach equilibrium, the value of Keq must change.

56.              The value of the equilibrium constant at a given temperature for the reaction:

N2(g) + 3H2(g) 2NH3(g)

is 224.  If [N2] = 10.0 M, [H2] = 10.0 M, and [NH3] = 10.0 M, determine if the reaction is at equilibrium.  If it is not, in which direction will it proceed to reach equilibrium?

A)The reaction is at equilibrium.

B)The reaction is not at equilibrium, it will shift to the left.

C)The reaction is not at equilibrium, it will shift to the right.

D)It is not possible to tell if the reaction is at equilibrium>

E)To reach equilibrium, the value of Keq must change.

57.              Consider the following reaction at a specific temperature:

2HI(g) H2(g) + I2(g)

If [HI] = 0.447 M, [H2] = 0.200 M, and [I2] = 0.200 M at equilibrium, calculate the value of the equilibrium constant under these conditions.

A)  0.200    B)  0.0400    C)  0.0895    D)  0.407    E)  0.0447

58.              Consider the following reaction at a specific temperature:

CO2(g) + H2(g) CO(g) + H2O(g)

If [CO2] = 3.60 M, [H2] = 4.00 M, [CO] = 1.18 M, and [H2O] = 2.40 M at equilibrium, calculate the value of the equilibrium constant under these conditions.

A)  0.471    B)  0.197    C)  5.08    D)  2.12    E)  0.444

59.              Consider the following reaction at a specific temperature:

2HI(g) H2(g) + I2(g)

If [HI] = 1.17 M, [H2] = 1.37 M, and [I2] = 0.100 M at equilibrium, calculate the value of the equilibrium constant under these conditions.

A)  1.17    B)  1.26    C)  0.100    D)  10.0    E)  8.54

60.              Consider the following reaction at a specific temperature:

CO2(g) + H2(g) CO(g) + H2O(g)

If [CO2] = 1.80 M, [H2] = 2.00 M, [CO] = 0.590 M, and [H2O] = 1.20 M at equilibrium, calculate the value of the equilibrium constant under these conditions.

A)  0.471    B)  0.197    C)  5.08    D)  2.12    E)  0.444