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InterviewSolution
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Calculate the enthalpy of formation of `Delta_(f)H` for `C_(2)H_(5)OH` from tabulated data and its heat of combustion as represented by the following equaitons: i. `H_(2)(g) +(1)/(2)O_(2)(g) rarr H_(2)O(g), DeltaH^(Theta) =- 241.8 kJ mol^(-1)` ii. `C(s) +O_(2)(g) rarr CO_(2)(g),DeltaH^(Theta) =- 393.5kJ mol^(-1)` iii. `C_(2)H_(5)OH (l) +3O_(2)(g) rarr 3H_(2)O(g) + 2CO_(2)(g), DeltaH^(Theta) =- 1234.7kJ mol^(-1)` a. `-2747.1 kJ mol^(-1)` b. `-277.7 kJ mol^(-1)` c. `277.7 kJ mol^(-1)` d. `2747.1 kJ mol^(-1)`A. `+ x_(1) kJ mol^(-1)`B. `- x_(2) kJ mol^(-1)`C. `+ x_(3) kJ mol^(-1)`D. `x_(4) kJ mol^(-1)` |
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Answer» Correct Answer - B By definition, the enthalpy of formation of `H_(2) O (1)` is the enthalpy change when one mole of `H_(2) O (1)` is synthesized from its elements in their standard state: `H_(2) (g) + (1)/(2) O_(2) (g) = H_(2) O (1)`, `Delta_(f) H^(@) = - x_(2) kJ mol^(-1)` |
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