At 298K the standard free energy of formation of `H_(2)O(l)` is `-256.5 kJ..mol`, while that of its ionisation to `H^(+)` & `OH^(-)` is `80 kJ//mol`. What will be emf at 298 K of the cell.
`H_(2)(g,1 bar) |H^(+)(1M) || O_(2)(g,1bar)`
Fill your answer by multiplying it with 10.

At 298 K the standard free energy of formation of H_(2)O (l) is -237.20 kJ/"mole" while DeltaG^(@) of its ionisation into H^(+) ion and hydroxyl ionosis 80kJ//"mole" , then the emf of the following cell at 298 K will be: H-92)(g,1bar)| H^(+)(1 M) || OH^(-)(1M) | O_(2)(g,1bar)

At 298 K the standard free energy of formation of H_(2)O(l) is -237.20 kJ/"mole" while that of its ionisation into H^(+) ions and hydroxyl ions is 80kJ/"mole" , then the emf of the following cell at 298 K will be : [Take 1F = 96500 C] H_(2)O(g, 1 bar)|H^(+)(1M)||OH^(-)(1M) |O_92)(g, 1bar)

At 298K, the standard free energy of formation of H_(2)O(l)=-237.13kJ*mol^(-1) . Calcualte the value of equilibrium constant at that temperature for the following reaction: 2H_(2)O(l)to2H_(2)(g)+O_(2)(g) .

The standard free energy of formation of NO(g) is 86.6 kJ/ mol at 298 K what is the standard free energy of formation of NO_(2) g at 298 k? K _(p)= 1.6 xx 10^(12)

The internal energy change (Delta U) for reaction CH_(4)(g) + (20_(2)(g) to CO_(2) (g) + 2H_(2) O(l) is -885.5 kj/mol at 298K. What is Delta H at 298 K?

The enthaply at 298K of the reaction H_(2)O_(2)(l)rarr+(1)/(2)O_(2)(g) is -23.5Kcal mol^(-1) and the enthaply of formation of H_(2)O_(2)(l) is -44.8Kcal mol^(-1) . The enthaply of formatiom of H_(2)O(l) is

The enthalpy of the reaction : H_(2)O_(2)(l) rarr H_(2)O(l) + (1)/(2)O_(2)(g) is -98.3 KJ mol^(-1) and the enthalpy of formation of H_(2)O(l) is -285.6 kJ mol^(-1) . The enthalpy of formation of H_(2)O_(2)(l) is :

If Delta G_(298K) for the reaction 2H_(2(g. 1atm)) + O_(2(g. 1atm)) rarr 2H_(2)O_((g.1atm)) is -240kJ , what will be Delta G_(298K) for the reaction H_(2)O_((g.0.2 atm)) rarr H_(2(g.4atm)) + (1)/(2) O_(2(g.0.26atm))

The standard enthalpy of formation (Delta H^(0)) at 298K for methane, CH_(4(g)) is 74.8 kJ mol^(1) . The additional information required to determine the average energy for C-H bond formation would be