1.

For a cell reaction2H_(2(g)) + O_(2(g))to 2H_2O_((l)) DeltaS_(298)^(@) = - 0.32 kJ // K . What is the value Delta_(i) H_(298)^(@) (H_2O, l) ? Given : O_(2(g)) + 4H_((aq))^(+) + 4e^(-) to 2H_2O_((l)) , E^(@) = 1.23 V

Answer»

`-285. 07 kJ// mol `
`-570.14 kJ // mol `
`285. 07 kJ//mol`
None of these

SOLUTION :`DeltaG = DeltaH -TDeltaS^(0) - NFE^(0) = DeltaH-TDeltaS - 4 XX 1.23 xx 96,500 = DeltaH - 298 xx (-0.32)`
`DeltaH_("for2 moles") = -(4 xx 1.23 xx 96,500) - (298 xx 0.32)`
`DeltaH_(H_2O)` for 1 mole `=(1)/(2) [(-4 xx 1.23 xx 96,500) - (298 xx 0.32)] = -285.07 "KJ/mole"`


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