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If enthalpies of formation of C(2)H(4)(g...

If enthalpies of formation of `C_(2)H_(4)(g),CO_(2)(g)` and `H_(2)O(l)` at `25^(@)C` and 1 atm pressure are 52, -394 and -286 KJ/mol , the enthalpy of combustion of ethane is equal to

A

`- 141 .2 kJ// mol`

B

`-1412 kJ// mol`

C

`14.2 kJ// mol`

D

`+14.12 kJ// mol`

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If enthalpies of formation of C_(2)H_(4)(g)1 ,CO_(2) and H_(2)O(l) at 25(@)C and 1 atm pressure be 52,-394 and -286kJmol^(-1) respectively ,the enthalpy of combustion of C_(2)H_(4)(g) will be

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Standard enthalpy of formation of C_(3)H_(7)NO_(2)(s),CO_(2)(g) and H_(2)O(l) are 133.57,-94.05 and -68.32kcal mo1^(-1) respectively Standard enthalpy combustion of CH_(4) at 25^(@)C is -212.8 kcal mo1^(-1) Calculate DeltaH^(Theta) for the reaction: 2CH_(4)+CO_(2)+1//2N_(2)rarrC_(3)H_(7)NO_(2)(s)+1//2H_(2) Calculate DeltaU for combustion of C_(3)H_(7)NO_(2)(s) .

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In a fuel cell methanol is used as fuel and oxygen gas is used as an oxidizer. The reaction is : CH_(3)OH_((l))+(3)/(2)O_(2(g))rarr CO_2((g))+2H_(2)O_((l)) At 298K standard Gibb's energies of formation for CH_(3)OH(l), H_(2)O(l) and CO_(2)(g) are -166.2,-237.2 and -394.4kJ mol^(-1) respectively. If standard enthalpy of combustion of methanol is -726kJ mol^(-1) , efficiency of the fuel cell will be :

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