Question

# Answer the following questions: (a) The equilibrium constant for the following reaction is 2.90×10-2 at 1150K....

(a) The equilibrium constant for the following reaction is 2.90×10-2 at 1150K.

2SO3(g) --> 2SO2(g) + O2(g)

If an equilibrium mixture of the three gases at 1150K contains 2.33×10^-2 M SO3(g) and 1.73×10^-2 M SO2, what is the equilibrium concentration of O2? ________ M

(b) Consider the equilibrium system at 881 K.

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

If an equilibrium mixture of the three gases at 881 K contains 6.06 x10^-5 M NH3, and 1.37 x 10^-2 M N2, and 3.15 x 10^-2 M H2, what is the value of the equilibrium constant K? K = ____________

(c) The equilibrium constant for the following reaction is 4.50×10-2 at 648K.

SO2Cl2 (g) --> SO2 (g) + Cl2 (g)

If an equilibrium mixture of the three gases at 648K contains 2.72×10-2 M SO2Cl2(g) and 1.94×10-2 M SO2, what is the equilibrium concentration of Cl2? ______ M

Part a

Equilibrium constant expression of the reaction

K = [O2] [SO2]2/ [SO3]2

2.90 x 10^-2 = [O2] [1.73*10^-2]2 / [2.33*10^-2]2

(2.90 x 10^-2) x [( 2.33*10^-2)/(1.73*10^-2)]2 = [O2]

[O2] = 0.0526 M

Part b

Equilibrium constant expression of the reaction

K = [N2] [H2]3/ [NH3]2

K = (1.37*10^-2)(3.15*10^-2)3 / (6.06*10^-5)2

= 116.6

Part C

Equilibrium constant expression of the reaction

K = [Cl2] [SO2] / [SO2Cl2]

4.50*10^-2 = [Cl2] [1.94*10^-2] / [2.72*10^-2]

[Cl2] = 0.063 M