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Calculate the standard free energy change for the reaction,4NH3 (g) + 5O2 (g) 4NO (g) + 6H2O (l)Given that the standard free energies of formation (ΔfG°) for NH3 (g), NO (g) and H2O (l) are – 16.8, + 86.7 and – 237.2 kJ mol–1 respectively. Predict the feasibility of the above reaction at the standard state. |
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Answer» Here, we are given Δf G° (NH3 ) = – 16.8 kJ mol–1 Δf G° (NO) = + 86.7 kJ mol–1 Δf G° (H2O) = – 237.2 kJ mol–1 ∴ Δf G° = ∑f G° (Products) ∑ Δf G° (Reactants) =[14 × Δf G° (NO) + 6 × Δf G°(H2O)] – [4 × Δf G° (NH3 ) + 5 × Δf G° (O2 )] = [4 × (86.7) + 6 × (–237.2)] – [4 × (– 16.8) + 5 × 0] = – 1009.2 kJ Since Δf G° is negative, the process is feasible. |
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