QuestionJune 1, 2025

Use standard enthalpy and entropy data from Appendix G to calculate the standard free energy change for the reaction shown here (298 k). What does the computed value for Delta G^circ say about the spontaneity of this process? C_(2)H_(6)(g)arrow H_(2)(g)+C_(2)H_(4)(g) Delta G^circ =-102.0kJ/mol ; the reaction is spontaneous at 25^circ C Delta G^circ =-102.0kJ/mol : the reaction is nonspontaneou s at 25 {}^circ C Delta G^circ =102.0kJ/mol ; the reaction is nonspontaneous at 25 {}^circ C Delta G^circ =102.0kJ/mol ; the reaction is spontaneous at 25^circ C

Use standard enthalpy and entropy data from Appendix G to calculate the standard free energy change for the reaction shown here (298 k). What does the computed value for Delta G^circ say about the spontaneity of this process? C_(2)H_(6)(g)arrow H_(2)(g)+C_(2)H_(4)(g) Delta G^circ =-102.0kJ/mol ; the reaction is spontaneous at 25^circ C Delta G^circ =-102.0kJ/mol : the reaction is nonspontaneou s at 25 {}^circ C Delta G^circ =102.0kJ/mol ; the reaction is nonspontaneous at 25 {}^circ C Delta G^circ =102.0kJ/mol ; the reaction is spontaneous at 25^circ C
Use standard enthalpy and entropy data from Appendix G to calculate the standard free energy change for the reaction shown here (298 k). What does the computed value for Delta G^circ say about the spontaneity of this process? C_(2)H_(6)(g)arrow H_(2)(g)+C_(2)H_(4)(g) Delta G^circ =-102.0kJ/mol ; the reaction is spontaneous at 25^circ C Delta G^circ =-102.0kJ/mol : the reaction is nonspontaneou s at 25 {}^circ C Delta G^circ =102.0kJ/mol ; the reaction is nonspontaneous at 25 {}^circ C Delta G^circ =102.0kJ/mol ; the reaction is spontaneous at 25^circ C

Solution
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Answer

\Delta G^{\circ} = 102.0 \text{ kJ/mol}; the reaction is nonspontaneous at 25^{\circ}C Explanation 1. Identify the formula for Gibbs free energy Use the formula \Delta G^{\circ} = \Delta H^{\circ} - T\Delta S^{\circ} to calculate the standard Gibbs free energy change. 2. Determine spontaneity If \Delta G^{\circ} 0, it is nonspontaneous.

Explanation

1. Identify the formula for Gibbs free energy<br /> Use the formula $\Delta G^{\circ} = \Delta H^{\circ} - T\Delta S^{\circ}$ to calculate the standard Gibbs free energy change.<br />2. Determine spontaneity<br /> If $\Delta G^{\circ} < 0$, the reaction is spontaneous. If $\Delta G^{\circ} > 0$, it is nonspontaneous.
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