The initial concentration for the compounds involved in the reaction shown were determined to be [CS2(g)] = 1.075 mol/L, [H2(g)] = 1.436 mol/L, [CH4(g)] = 0.6740 mol/L, [H2S(g)] = 0.3120 mol/L. Calculate the value of the equilibrium constant (Kc) at 1175 K if the equilibrium concentration of CH4(g) was 0.7910 mol/L.

Question

The initial concentration for the compounds involved in the reaction shown were determined to be [CS2(g)] = 1.075 mol/L, [H2(g)] = 1.436 mol/L, [CH4(g)] = 0.6740 mol/L, [H2S(g)] = 0.3120 mol/L. Calculate the value of the equilibrium constant (Kc) at 1175 K if the equilibrium concentration of CH4(g)  was 0.7910 mol/L.

CS2(g)+4H2(g) = CH4(g)+2H2S(g)
CH4 is increased by .117
H2S is increased by 2x.117
H2 is decreased by 4x.117
CS2 is decreased by .117

final:
CH4=.791
HS2=.546
H2=.968
CS2=.958

(.791)(.546)^2/(.958)(.968)^4

DrBob222 · Answer

That looks good to me.