For the Reaction CuS(s)+ H 2 (g) H 2 S(g)+ Cu(s)$\Delta$ G° f (CuS)= -53

The Answer of For the Reaction CuS(s)+ H 2 (g) H 2 S(g)+ Cu(s)$\Delta$ G° f (CuS)= -53

For the Reaction CuS(s)+ H 2 (g) H 2 S(g)+ Cu(s)$\Delta$ G° f (CuS)= -53

The Answer of For the Reaction CuS(s)+ H 2 (g) H 2 S(g)+ Cu(s)$\Delta$ G° f (CuS)= -53

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For the Reaction CuS(s)+ H₂(g) H₂S(g)+ Cu(s) $\Delta$ G°_f (CuS)= -53

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For the reaction CuS(s)+ H₂(g) $For the reaction CuS(s)+ H2(g) H2S(g)+ Cu(s), \Delta G°f (CuS)= -53.6 kJ/mol \Delta G°f (H2S)= -33.6 kJ/mol \Delta H°f (CuS)= -53.1 kJ/mol \Delta H°f (H2S)= -20.6 kJ/mol Calculate the value of the equilibrium constant (Kp)at 798 K and 1 atm pressure.$ H₂S(g)+ Cu(s),
$\Delta$ G°_f (CuS)= -53.6 kJ/mol
$\Delta$ G°_f (H₂S)= -33.6 kJ/mol
$\Delta$ H°_f (CuS)= -53.1 kJ/mol
$\Delta$ H°_f (H₂S)= -20.6 kJ/mol
Calculate the value of the equilibrium constant (K_p)at 798 K and 1 atm pressure.

For the Reaction CuS(s)+ H2(g) H2S(g)+ Cu(s) Δ\DeltaΔ G°f (CuS)= -53

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For the Reaction CuS(s)+ H₂(g) H₂S(g)+ Cu(s) $\Delta$ G°_f (CuS)= -53

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