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from the given information calculate enthalpy of f
Question:
From the given information, calculate enthalpy of formation of 2 moles of $C_6H_6$(l) at 25°C. Given: $CH(C_6H_6$(l)) = –3264.6 kJ/mol $CH(C(s))$ = –393.5 kJ/mol $fH(H_2O(l))$ = –285.83 kJ/mol
JEE Main
Updated On:
Sep 17, 2024
–124.5 kJ/mol
–46.11 kJ/mol
46.11 kJ/mol
124.5 kJ/mol
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The Correct Option is
C
Solution and Explanation
The Correct answer is option is (C) : 46.11 kJ/mol
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Consider the following cases of standard enthalpy of reaction (\( \Delta H_f^\circ \) in kJ mol\(^{-1}\)):
\[ \text{C}_2\text{H}_6(g) + 7 \text{O}_2(g) \rightarrow 2 \text{CO}_2(g) + 3 \text{H}_2\text{O}(l) \quad \Delta H_1^\circ = -1550 \] \[ \text{C(graphite)} + \text{O}_2(g) \rightarrow \text{CO}_2(g) \quad \Delta H_2^\circ = -393.5 \] \[ \text{H}_2(g) + \frac{1}{2} \text{O}_2(g) \rightarrow \text{H}_2\text{O}(g) \quad \Delta H_3^\circ = -286 \]
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