Consider the following reaction:

Is the
forward reaction spontaneous when the concentrations of [N_{2}], [H_{2}],
and [NH_{3}] are 0.500 M, 0.750 M, and 1.25 M respectively at 375 K?

The change in free energy is related to the standard free energy as shown in the following equation

where R is the gas constant, T is the absolute temperature, and Q is the reaction quotient

Because ΔG is negative, the forward reaction is spontaneous.