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The E^(@) at 25^(@)C for the following r...

The `E^(@)` at `25^(@)`C for the following reaction is 0.55 V. Calculate the `DeltaG^(@)` in kJ`//`mol :
`4BiO^(+)(aq)+3N_(2)H_(5)^(+)to4Bi(s)+3N_(2)(g)+4H_(2)O(l)+7H^(+)`

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Use the following standard electrode potentials, calculate DeltaG^(@) in kJ // mol for the indicated reaction : 5Ce^(4+)(aq)+Mn^(2+)(aq)+4H_(2)O(l)to5Ce^(3+)(aq)+ MnO_(4)^(-)(aq)+8H^(+)(aq) MnO_(4)^(-)(aq)+8H^(+)(aq)+5e^(-)toMn^(2+)(aq)+4H_(2)O(l), E^(@)=+1.51 V Ce^(4+)(aq)+e^(=)toCe^(3+)(aq)" "E^(@)=+1.61 V

Use the following standard electrode potentials, calculate DeltaG^(@) in kJ // mol for the indicated reaction : 5Ce^(4+)(aq)+Mn^(2+)(aq)+4H_(2)O(l)to5Ce^(3+)(aq)+MnO_(4)^(-)(aq)+8H^(+)(aq) MnO_(4)^(-)(aq)+8H^(+)(aq)+5e^(-)toMn^(2+)(aq)+4H_(2)O(l), E^(@)=+1.51 V Ce^(4+)(aq)+e^(=)toCe^(3+)(aq)" "E^(@)=+1.61 V

Use the following standard electrode potentials, calculate DeltaG^(@) in kJ // mol for the indicated reaction : 5Ce^(4+)(aq)+Mn^(2+)(aq)+4H_(2)O(l)to5Ce^(3+)(aq)+MnO_(4)^(-)(aq)+8H^(+)(aq) MnO_(4)^(-)(aq)+8H^(+)(aq)+5e^(-)toMn^(2+)(aq)+4H_(2)O(l), E^(@)=+1.51 V Ce^(4+)(aq)+e^(=)toCe^(3+)(aq)" "E^(@)=+1.61 V

Using the following E^(@) values for electrode potentials, calculate triangle G^(@) in kJ for the indicated reaction: 5Ce^(4+) (aq) + Mn^(2+) (aq) + 4H_(2)O(l) rarr 5Ce^(3+) (aq) + MnO_(4)^(-) (aq) +8H^(+) (aq) MnO_(4)^(-) (aq) +8H^(+) (aq) +5e^(-) rarr Mn^(2+) (aq) + 4H_(2) O(l), E^(@) = +1.51V Ce^(4+) (aq) + e^(-)rarr Ce^(3+)(aq), E^(@) = +1.61V

The heat of reaction for the following reaction (DeltaH^(0)) at 25^(@)C temperatue is -1368 kJ: C_(2)H_(5)OH(l)+3O_(2)(g) to 2CO_(2)(g)+3H_(2)O(l) If the enthalpy of formation of CO_(2)(g) and H_(2)O(l) at 25^(@)C are -393.5 and -285.8 kJ*mol^(-1) respectively, then what will be the value of the standard enthalpy of formation of C_(2)H_(5)OH(l) ?