Initial concentrations of 0.100 mol/L of H_2(g) and H_2(g) are mixed in a 1.00 L
ID: 979001 • Letter: I
Question
Initial concentrations of 0.100 mol/L of H_2(g) and H_2(g) are mixed in a 1.00 L container with excess solid sulfur, and the mixture is allowed to come to equilibrium at 390 K. For the reaction H_2S(g) rightarrow H_2(g) + S(g) the equilibrium constant, K_c, is 0.0700. As written, the reaction is endothermic. What is the concentration of H_2(g) at equilibrium Would the amount of hydrogen sulfide increase, decrees, or remain unchanged if more sulfur were added. fill the volume of the container were decreased. Mil the temperature were decreasedExplanation / Answer
(a) Kc = [H2]/[H2S]
0.07 = (0.1-x)/(0.1+x)
0.007 + 0.07x = 0.1 - x
1.07x = 0.1 - 0.007
x = 0.08692
Therefore [H2] = 0.1 - 0.08692 = 0.01308 M
(b)
(i) Addition of more sulphur doesnot alter the amount of H2S
(ii) Decrease in Volume of the container also does not alter the amount of H2S as eual number of gaseous moles are present at both sides.
(iii) Decrease in temperature decrease the amount of H2S as the reaction is endothermic.