Values of `Delta H Delta S` for the given reaction are -95.4 kJ and -198.3 `J*K^(-1)` respectively:
`N_(2)(g)+3H_(2)(g) to 2NH_(3)(g)`
State whether the reaction will be spontaneous at 500 K or not. Consider `Delta H and DeltaS` are independent of temperature.

Explanation

We know, `DeltaG=DeltaH-TDeltaS`
Given, `DeltaH=-95.4kJ,DeltaS=-198.3J*K^(-1) and T=500K`.
`therefore DeltaG=[-95.4xx10^(3)-500xx(-198.3)]J=3750J=3.75kJ`
As the value of `DeltaG` is positive at constant pressure and 500 K temperature, it is not a spontaneous process.