Question
- Using the data given below, calculate the value of equilibrium constant for the reaction at 298K.
- Based on your calculated value, comment whether this process can be recommended as a practical method for making benzene.
✓
Answer
- $\Delta\text{G}^\circ=\Delta_\text{f}\text{G}^\circ[\text{C}_6\text{H}_6(\text{g})]-3\Delta_\text{f}\text{G}^\circ[\text{CH}\equiv\text{CH(g)}]$
$=1.24\times10^5\text{J mol}^{-1}-6.27\times10^5\text{J mol}^{-1}$
$=-5.03\times10^5\text{J mol}^{-1}$
$-5.03\times10^5=-2.303\times8.314\times298\log\text{K}$
$\Rightarrow\log\text{K}=\frac{5.03\times10^5\text{J}}{5705.8\text{J}}=+88.1559$
$\Rightarrow\text{K}=1.432\times10^{88}$
- Yes, this process can be recommended as a practical method for making benzene as value of K is very high.
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