For the reaction C2H6 (g) → C2H4 (g) + H2 (g), ΔH° is 137 kJ/mol and ΔS° is 120 J/K·mol. This reaction is spontaneous: a) at all temperatures b) only at high temperature c) only at low temperature d) It is non-spontaneous at all temperatures
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For the reaction C2H6 (g) → C2H4 (g) + H2 (g), ΔH° is +137 kJ/mol and ΔS° is +120 J/K∙mol. This reaction is ________. a) Spontaneous only at high temperature b) Spontaneous at all temperatures c) Spontaneous only at low temperature d) Nonspontaneous at all temperatures
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For the reaction 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(g), ΔH is -125 kJ/mol and ΔS is +253 J/K*mol. This reaction is ____. a. Spontaneous at low temperature. b. Spontaneous at high temperature. c. Spontaneous at all temperatures. d. Nonspontaneous at all temperatures.
From the values of $\Delta H$ and $\Delta S$, predict which of the following reactions would be spontaneous at $25^{\circ} \mathrm{C}$ : reaction $\mathrm{A}$ : $\Delta H=10.5 \mathrm{kJ} / \mathrm{mol}, \Delta S=30 \mathrm{J} / \mathrm{K} \cdot \mathrm{mol} ;$ reaction $\mathrm{B}: \Delta H=$ $1.8 \mathrm{kJ} / \mathrm{mol}, \Delta S=-113 \mathrm{J} / \mathrm{K} \cdot$ mol. If either of the reactions is nonspontaneous at $25^{\circ} \mathrm{C},$ at what temperature might it become spontaneous?
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