Question

Be sure to answer all parts. At 1130°C, the equilibrium constant (K) for the reaction 2H,S(g) =2H2(g) +S2(8) is 2.25 x 104. If [H,8] = 4.50 x 10-2 Mand [H2] = 1.50 10-M, calculate [S2]. * 10 M (Enter your answer in scientific notation.)

Answer 1

The balanced equilibrium reaction is as follows:

2H₂S(g) $\rightleftharpoons$ 2H₂(g) + S₂(g)

K_c = 2.25 x 10^-4

[H₂S] = 4.50 x 10^-3 M

[H₂] = 1.50 x 10^-3 M

The K_c expression from the balanced equilibrium reaction is as follows:

K_c = [H₂]² [S₂] / [H₂S]²

Substitute the known values and solve for [S₂] as follows:

2.25 x 10^-4 = [1.50 x 10^-3]² [S₂] / [4.50 x 10^-3]²

2.25 x 10^-4 = [2.25 x 10^-6] [S₂] / [2.025 x 10^-5]

[S₂] = 2.025 x 10^-3 M

Thus, [S₂] = 2.02 x 10^-3 M [3 S.F]