Calculate the standard enthalpy of formation | vedclass

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(C) The formation reaction for $ICl_{(g)}$ is: $\frac{1}{2}I_{2(s)} + \frac{1}{2}Cl_{2(g)} 	o ICl_{(g)}$,$\Delta H_f = ?$From the given equations:$(i

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$+16.8$

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(C) The formation reaction for $ICl_{(g)}$ is: $\frac{1}{2}I_{2(s)} + \frac{1}{2}Cl_{2(g)} 	o ICl_{(g)}$,$\Delta H_f = ?$From the given equations:$(i) \frac{1}{2}Cl_{2(g)} 	o Cl_{(g)}$,$\Delta H = \frac{242.3}{2} = 121.15 	ext{ kJ mol}^{-1}$$(ii) \frac{1}{2}I_{2(g)} 	o I_{(g)}$,$\Delta H = \frac{151.0}{2} = 75.5 	ext{ kJ mol}^{-1}$$(iii) I_{(g)} + Cl_{(g)} 	o ICl_{(g)}$,$\Delta H = -211.3 	ext{ kJ mol}^{-1}$$(iv) \frac{1}{2}I_{2(s)} 	o \frac{1}{2}I_{2(g)}$,$\Delta H = \frac{62.76}{2} = 31.38 	ext{ kJ mol}^{-1}$Adding these equations:$\Delta H_f = 121.15 + 75.5 - 211.3 + 31.38 = 16.73 \approx 16.8 	ext{ kJ mol}^{-1}$.

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