When heated, hydrogen sulfide gas decomposes according to the equation above. A 3.40 g sample of H2S(g) is introduced into an evacuated rigid 1.25 L container. The sealed container is heated to 483 K and 3.7 x 10^(-2) mol of S2(g) is present at equilibrium.
PART B : Calculate the equilibrium concentration, in mol-L, of the following gases in the container at 483 K a) H2 b) H2S
PART C : Calculate the value of the equilibrium constant, Kc, for the decomposition reaction at 483 K
PART D : Calculate the partial pressure of S2(g) in the container at equilibrium at 483 K.