ΔG⁰ equals +20.00 KJ for the reaction below at 298 K and 1atm of pressure;
CuS(s) +H₂(g) -> Cu(s) +H₂S(g)
a. Calculate the equilibrium constant for the reaction.
b. At 298 K, does the equilibrium lie largely in the direction reactants or products? Why?

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08-08-2024
Chemistry

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ΔG⁰ equals +20.00 KJ for the reaction below at 298 K and 1atm of pressure;
CuS(s) +H₂(g) -> Cu(s) +H₂S(g)
a. Calculate the equilibrium constant for the reaction.
b. At 298 K, does the equilibrium lie largely in the direction reactants or products? Why?

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