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

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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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From the given information, calculate enthalpy of formation of 2 moles of C6H6C_6H_6C6​H6​(l) at 25°C. Given: CH(C6H6CH(C_6H_6CH(C6​H6​(l)) = –3264.6 kJ/mol CH(C(s))CH(C(s))CH(C(s)) = –393.5 kJ/mol fH(H2O(l))fH(H_2O(l))fH(H2​O(l)) = –285.83 kJ/mol

The Correct Option is C

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Questions Asked in JEE Main exam

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