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

question 74

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

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