The standard free energies of formation of H₂S(g) and CdS(s) at 1000°C are -49.0 kJ/mol and -127.2 kJ/mol respectively. Use these data to predict whether H₂(g) will reduce CdS(s) to metallic Cd at this temperature.

A) ΔG = -78.2 kJ/mol and H₂ reduces CdS B) ΔG = -39.1 kJ/mol and H₂ reduces CdS C) ΔG = 0 kJ/mol and the reaction is at equilibrium D) ΔG = 78.2 kJ/mol and the reaction is not feasible

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Correct Answer: Option D

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The standard free energies of formation of H2S(g) and CdS(s) at...

The standard free energies of formation of H2S(g) and CdS(s) at 1000°C are -49.0 kJ/mol and -127.2 kJ/mol respectively. Use these data to predict whether H2(g) will reduce CdS(s) to metallic Cd at this temperature.

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Related Questions on Chemical Thermodynamics

The standard free energies of formation of H₂S(g) and CdS(s) at 1000°C are -49.0 kJ/mol and -127.2 kJ/mol respectively. Use these data to predict whether H₂(g) will reduce CdS(s) to metallic Cd at this temperature.