Problem: When the oxide of generic metal M is heated at 25C, only a negligible amount of M is produced.MO2(s) ↔  M(s)+O2(g)delta G = 288.5 kJ/molWhen the reaction is coupled to the conversion of graphite to carbon dioxide, it becomes spontaneous.What is the chemical equation of this coupled process? Show that the reaction is in equilibrium, include physical states, and represent graphite as C(S).What is the thermodynamic equilibrium constant for the coupled reaction?K = ______

FREE Expert Solution

We are asked to determine the chemical equation involved in the given process. We are also asked to determine the equilibrium constant, K.

MO2(s) ↔  M(s)+O2(g)           ΔG˚rxn = 288.5 kJ/mol

C(s)O2(g)  ↔  CO2(g)  ΔG˚rxn = -394.4 kJ/mol

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MO2(s) + C(s ↔  M(s)+CO2(g)    ΔG˚rxn = -105.9 kJ/mol

Recall that ΔG˚rxn and K are related to each other:

$\overline{){\mathbf{\Delta G}}{{\mathbf{°}}}_{{\mathbf{rxn}}}{\mathbf{=}}{\mathbf{-}}{\mathbf{RTlnK}}}$

Solving for K:

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Problem Details

When the oxide of generic metal M is heated at 25C, only a negligible amount of M is produced.

MO2(s) ↔  M(s)+O2(g)

delta G = 288.5 kJ/mol

When the reaction is coupled to the conversion of graphite to carbon dioxide, it becomes spontaneous.

What is the chemical equation of this coupled process? Show that the reaction is in equilibrium, include physical states, and represent graphite as C(S).

What is the thermodynamic equilibrium constant for the coupled reaction?
K = ______