QuestionJuly 27, 2025

From the values of Delta H Delta S predict which of the following reactions would be spontaneous at 21^circ C Part: 0/4 Part 1 of 4 reaction A: Delta H=10.5(kJ)/(mol),Delta S=30.0(J)/(Kcdot mol) Select the single best answer. spontaneous nonspontaneous impossible to tell

From the values of Delta H Delta S predict which of the following reactions would be spontaneous at 21^circ C Part: 0/4 Part 1 of 4 reaction A: Delta H=10.5(kJ)/(mol),Delta S=30.0(J)/(Kcdot mol) Select the single best answer. spontaneous nonspontaneous impossible to tell
From the values of Delta H Delta S predict which of the following reactions would be spontaneous at 21^circ C Part: 0/4 Part 1 of 4 reaction A: Delta H=10.5(kJ)/(mol),Delta S=30.0(J)/(Kcdot mol) Select the single best answer. spontaneous nonspontaneous impossible to tell

Solution
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Answer

nonspontaneous Explanation 1. Convert Units Convert \Delta S from \frac{J}{K \cdot mol} to \frac{kJ}{K \cdot mol}: \Delta S = 30.0 \frac{J}{K \cdot mol} = 0.030 \frac{kJ}{K \cdot mol}. 2. Calculate Gibbs Free Energy Change Use the formula **\Delta G = \Delta H - T\Delta S**. Convert temperature to Kelvin: T = 21 + 273.15 = 294.15 \, K. Then calculate \Delta G: \Delta G = 10.5 - (294.15 \times 0.030) = 10.5 - 8.8245 = 1.6755 \, kJ/mol. 3. Determine Spontaneity If \Delta G 0, so the reaction is nonspontaneous.

Explanation

1. Convert Units<br /> Convert $\Delta S$ from $\frac{J}{K \cdot mol}$ to $\frac{kJ}{K \cdot mol}$: $\Delta S = 30.0 \frac{J}{K \cdot mol} = 0.030 \frac{kJ}{K \cdot mol}$.<br />2. Calculate Gibbs Free Energy Change<br /> Use the formula **$\Delta G = \Delta H - T\Delta S$**. Convert temperature to Kelvin: $T = 21 + 273.15 = 294.15 \, K$. Then calculate $\Delta G$: <br />$$\Delta G = 10.5 - (294.15 \times 0.030) = 10.5 - 8.8245 = 1.6755 \, kJ/mol.$$<br />3. Determine Spontaneity<br /> If $\Delta G < 0$, the reaction is spontaneous. Here, $\Delta G > 0$, so the reaction is nonspontaneous.
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