QuestionJuly 5, 2025

30 Consider the following reaction at 25^circ C 3Ni(s)+N_(2)(g)+3H_(2)O(g)arrow 3NiO(s)+2NH_(3)(g)

30 Consider the following reaction at 25^circ C 3Ni(s)+N_(2)(g)+3H_(2)O(g)arrow 3NiO(s)+2NH_(3)(g)
30 Consider the following reaction at 25^circ C 3Ni(s)+N_(2)(g)+3H_(2)O(g)arrow 3NiO(s)+2NH_(3)(g)

Solution
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Answer

The reaction is spontaneous at 25^{\circ}C if \Delta G < 0. Explanation 1. Identify the type of reaction This is a redox reaction involving nickel oxidation and nitrogen reduction. 2. Calculate moles of reactants and products Use stoichiometry to determine moles. For every 3 moles of Ni, 1 mole of N_2, and 3 moles of H_2O, you get 3 moles of NiO and 2 moles of NH_3. 3. Determine enthalpy change Use standard enthalpies of formation: \Delta H = \sum (\Delta H_f \text{products}) - \sum (\Delta H_f \text{reactants}). Look up values for NiO, NH_3, N_2, and H_2O. 4. Calculate Gibbs free energy change Use \Delta G = \Delta H - T\Delta S. Find entropy values for each substance and calculate \Delta S similarly to \Delta H. 5. Assess spontaneity If \Delta G < 0, the reaction is spontaneous at 25^{\circ}C.

Explanation

1. Identify the type of reaction<br /> This is a redox reaction involving nickel oxidation and nitrogen reduction.<br /><br />2. Calculate moles of reactants and products<br /> Use stoichiometry to determine moles. For every 3 moles of Ni, 1 mole of $N_2$, and 3 moles of $H_2O$, you get 3 moles of $NiO$ and 2 moles of $NH_3$.<br /><br />3. Determine enthalpy change<br /> Use standard enthalpies of formation: $\Delta H = \sum (\Delta H_f \text{products}) - \sum (\Delta H_f \text{reactants})$. Look up values for $NiO$, $NH_3$, $N_2$, and $H_2O$.<br /><br />4. Calculate Gibbs free energy change<br /> Use $\Delta G = \Delta H - T\Delta S$. Find entropy values for each substance and calculate $\Delta S$ similarly to $\Delta H$.<br /><br />5. Assess spontaneity<br /> If $\Delta G < 0$, the reaction is spontaneous at $25^{\circ}C$.
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