The standard oxidation potential for `Mn^(3+)` ion acid solution are `Mn^(2+)overset(-1.5V)rarrMn^(3+) overset(-1.0V)rarr MnO_(2)`. Is the reaction `2Mn^(3+)+2H_(2)O rarr Mn^(2+)+MnO_(2)+4H^(+)` spontaneous under conditions of unit activity ? What is the change in free energy ?

Options

A. spontaneous ,`-48250J`
B. nonspontaneous, `+48250J`
C. no change in free energy
D. spontaneous , `-96500J`

Answer

1

Explanation

`DeltaG=DeltaG^(@)+2.303RTlogQ`
`Q=1("activity"=1)`
`DeltaG=DeltaG^(@)`
`Mn^(+3)+e^(-)rarrMn^(+2)" "DeltaG_(1)^(@)=-1xxFxx1.5`
`Mn^(+3)+2H_(2)OrarrMnO_(2)+4H^(+)+e^(-)" "DeltaG_(2)^(@)=-1xxF(-1)`
`bar(2Mn^(3+)+2H_(2)Orarr Mn^(2+)+MnO_(2))+4H^(+)" "DeltaG^(@)=DeltaG_(2)^(@)=-48250J(DeltaGlt0)`