Calculate `DeltaG and E_(cell)` for the cell:
`AI//AI^(3+)(0.01M)||Fe^(2+)(0.02M)//Fe` given that `E^(@)(Al^(3+)//Al)=-1.66V and E^(@)(Fe^(2+)//Fe)=-0.44V`

Explanation

At anode, `2Al rarr 2Al^(3+) + 6e^(-)`
At cathode,
`ul(3Fe^(2+) +6e^(-) rarr 3Fe)`
`ul(2Al+ 3Fe^(2+) rarr 2Al^(3+) + 3Fe)`
`E= E^(@)- (0.059)/(2) "log" ([Al^(3-)]^(2))/([Fe^(2+)]^(3))`
`=1.22 - (0.059)/(2)"log" ((0.01)^(2))/((0.02)^(3))`
=1.209V
`Delta G^(@)= -nEF`
`=6(1.209) (065001)`
`=-700011J mol^(-1)`
`=-700.011k J mol^(-1)`