For the reaction `N_(2)(g)+3H_(2)(g)to2NH_(3)(g),DeltaH and DeltaS` are `-95.4kJa nd -198.3J*K^(-1)` respectively. Assuming reaction be spontaneous at 500K ? Explain.

Explanation

We know, `DeltaG=DeltaH-TDeltaS`
Given that `DeltaH=-95.4kJ and DeltaS=-198.3J*K^(-1)`
`therefore DeltaG=-95.4kJ-500K(-198.3xx10^(-3)kJ*K^(-1))`
`=3.75kJ`
As `DeltaG gt0` at 500K, the reaction will not be spontaneous at 500K.