For the given reaction:
`H_(2)(g)+Cl_(2)(g) to2H^(+)(aq)+2Cl^(-)(aq)`
`DeltaG^(@)=-262.4kJ`
The value of Gibbs free energy of formation `(DeltaG_(r)^(@))` for the ion `Cl^(-)(aq)` is:

Options

A. `-131 .2` kJ/mol
B. `+132 .2` KJ/mol
C. `-262 .4` KJ/mol
D. `+262 .4 ` KJ/mol

Answer

A

Explanation

`Delta_(r) G^(@) = Delta_(r)G^(@) "( Products)" -Delta_(f)G^(@)` (Reactants )
` [2Delta_(f) G^(@) + (H^(+))+ 2Delta_(f) G^(@) (CI^(-))]`
`- [Delta_(f)G^(@)(H_(2))+ Delta_(f) G^(@) (CI_(2))]`
` [ 0 + 2Delta_(f) G^(@))] - [ 0 + 0]`
` or (-262.4)/2 = Delta_(f) G^(@) (CI^(-))`
` or Delta G^(@) (CI^(-)) - 131.2 ` KJ/mol