Chemistry

Chemistry

Problem

Reaction 1: X→YX \to Y  ΔG∘=+35.0 kJ⋅mol−1\Delta G^\circ = +35.0\,\text{kJ}\cdot\text{mol}^{-1} Reaction 2: Z→XZ \to X  ΔG∘=−50.0 kJ⋅mol−1\Delta G^\circ = -50.0\,\text{kJ}\cdot\text{mol}^{-1} Calculate the standard Gibbs free energy change, ΔG∘\Delta G^\circ, for the net reaction Z→YZ \to Y and state whether the overall process is spontaneous under standard conditions.

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