The standard free energy of formation of at , representing the reaction , is . What is for ? — Chemical Equilibrium Chemistry Question
Question
The standard free energy of formation of $NH_3(g)$ at $298\text{ K}$, representing the reaction $\frac{1}{2}N_2(g) + \frac{3}{2}H_2(g) \rightleftharpoons NH_3(g)$, is $-16.5\text{ kJ mol}^{-1}$. What is $\Delta G^\circ$ for $N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g)$?
Answer: C
💡 Solution & Explanation
Standard free energy is an extensive property. The target reaction is obtained by multiplying the given formation reaction by 2. Therefore, its standard free energy change $\Delta G^\circ = 2 \times (-16.5) = -33.0\text{ kJ mol}^{-1}$.
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