Chemistry

Chemistry

Problem

The following elementary reactions occur under standard conditions: 1. P+Q→RΔG∘=+15.0 kJ⋅mol−1P + Q \to R \quad \Delta G^\circ = +15.0\,\text{kJ}\cdot\text{mol}^{-1} 2. R→S+TΔG∘=+20.0 kJ⋅mol−1R \to S + T \quad \Delta G^\circ = +20.0\,\text{kJ}\cdot\text{mol}^{-1} 3. 2T→QΔG∘=−90.0 kJ⋅mol−12T \to Q \quad \Delta G^\circ = -90.0\,\text{kJ}\cdot\text{mol}^{-1} Determine the standard Gibbs free energy change, in kJ⋅mol−1\text{kJ}\cdot\text{mol}^{-1}, for the overall reaction that results when these three reactions are combined so that no intermediates remain. Indicate whether the overall reaction is spontaneous under standard conditions.

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