Question

given the following equation and equilibrium constant, 2h_2(g)+s_2(g)⇌2h_2s(g) kc=1.08x10^7 determine kc for the following reaction. 1/2h_2s(g)⇌1/2h_2(g)+1/4s_2(g)

Answer 1

To find the new equilibrium constant for the reaction with halved stoichiometric coefficients, take the square root of the original Kc, which is √1.08x10^7.

Step-by-step explanation:

When calculating the equilibrium constant Kc for a modified reaction where the stoichiometric coefficients are divided or multiplied, the original equilibrium constant must be raised to the power of the factor by which the coefficients are changed. In the given equation 2H2(g) + S2(g) ⇌ 2H2S(g) with Kc=1.08x107, the stoichiometric coefficients are halved to get the new reaction 1/2H2S(g) ⇌ 1/2H2(g) + 1/4S2(g). To find the new equilibrium constant, we should take the original Kc and raise it to the power of 1/2 (since all coefficients are divided by 2).

The calculation is as follows: (Kc') = (Kc)1/2 = (1.08x107)1/2. Therefore, Kc for the second reaction is the square root of 1.08x107, which can be calculated using a calculator.