For the reaction, N_(2)(g) + 3H_(2)(g) rarr 2NH_(3)(g), Delta H = -95.2 kJ and Delta S = -198.1 JK^(-1). Calculate the temperature at which Gibb's energy change of the reaction (Delta G) becomes equal to zero.

For the reaction, N_(2)(g) + 3H_(2)(g) rarr 2NH_(3)(g), Delta H = -95.

1.	For the reaction, N_(2)(g) + 3H_(2)(g) rarr 2NH_(3)(g), Delta H = -95.2 kJ and Delta S = -198.1 JK^(-1). Calculate the temperature at which Gibb's energy change of the reaction (Delta G) becomes equal to zero.
Answer» Solution :`DELTA G = Delta H - T Delta S`. When `Delta G = 0, Delta H = T Delta S` or `T = (Delta H)/(Delta S) ""T = (-95.2 xx 10^(3)J)/(-198.1 JK^(-1)) = 480.6 K`.