Answer :
Answer:
-36.6 kJ·mol⁻¹
Explanation:
1. Calculate ΔG
[tex]\text{The relationship between $\Delta G^{\circ}$ and K is}\\\Delta G^{\circ} = -RT \ln K[/tex]
T = (250 + 273.15) K = 523.15 K
[tex]\begin{array}{rcl}\Delta G & = & -8.314 \text{ J}\cdot\text{K}^{-1} \text{mol}^{-1} \times \text{523.15 K} \ln (4.5 \times 10^{3}) \\& = & -4349\text{ J}\cdot \text{mol}^{-1} \times 8.412\\& = & \text{-36 590 J}\cdot \text{mol}^{-1}\\& = & \textbf{-36.6 kJ}\cdot \text{mol}^{-1}\\\end{array}[/tex]
2. Direction of spontaneity
ΔG is negative, so the reaction is spontaneous in the forward direction.