Estimate ΔG°rxn for the following reaction at 775 K. 2Hg(g) + O2(g) → 2HgO(s) ΔH°= -304.2 kJ; ΔS° = -414.2 J/K

Explanation:

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In this case, since the Gibbs free energy of any process is related with the enthalpy change, temperature and entropy change as shown below:

For a chemical reaction it is simply modified to:

Thus, since the enthalpy of reaction is given as -304.2 kJ and the entropy as -414.2 J/K (-0.4142 kJ/K), at 775 K the Gibbs free energy of reaction turns out:

Whose result means this is a nonspontaneous reaction.

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d: the voltage of the secondary coil is less than that of the primary coil.

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