For the Reaction CuS(s) + H₂(g) $\leftrightharpoons$ H₂S(g) + Cu(s) $\Delta$ G ^$\circ$

Multiple Choice

For the reaction CuS(s) + H₂(g) $\leftrightharpoons$ H₂S(g) + Cu(s) ,
$\Delta$ G ^$\circ$ _f (CuS) = -53.6 kJ/mol
$\Delta$ G ^$\circ$ _f (H₂S) = -33.6 kJ/mol
$\Delta$ H ^$\circ$ _f (CuS) = -53.1 kJ/mol
$\Delta$ H ^$\circ$ _f (H₂S) = - 20.6 kJ/mol
Calculate the value of the equilibrium constant (K_p) for this reaction at 298 K.

A) 2.71 * 10^-4
B) 2.91 * 10^-4
C) 3.11 * 10^-4
D) 3.31 * 10^-4
E) None of the above