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
This reaction proceeds spontaneously at 298 K and 1 atm pressure.

Question

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
This reaction proceeds spontaneously at 298 K and 1 atm pressure.

Quizplus · Accepted Answer

The Answer of 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 This reaction proceeds spontaneously at 298 K and 1 atm pressure.

For the Reaction CuS(s) + H2(g) ⇋\leftrightharpoons⇋ H2S(g) + Cu(s) Δ\DeltaΔ G ∘\circ∘

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