Predict whether it is possible or not to reduce magnesium oxide using carbon at `298K` according to the reaction.
`MgO(s) +C(s) rarr Mg(s) +CO(g)`
`Delta_(r)H^(Theta) = +491.18 kJ mol^(-1)` and `Delta_(r)S^(Theta) = 197.67 J K^(-1) mol^(-1)`
If not at what temperature, the reaction becomes spontaneous.

Explanation

`MgO_((s))+C_((s))toMg_((s))+CO_((g))`
`DeltaG^(@)=DeltaH^(@)-TDeltaS^(@)`
`=491.18-298xx[197.67xx10^(-3)]`
`=432.27 kJ`
Thus reaction is non-spontaneous at `298 K`. For spontaneous nature
`DeltaG^(@)=-ve i.,e TDeltaS^(@)gtDeltaH^(@)`
or `Txx[197.67xx10^(-3)]gt491.18`
or `Tgt491.18/(197.67xx10^(-3))gt2484.8 K`