If δh = -70.0 kj and δs = -0.300 kj/k , the reaction is spontaneous below a certain temperature. calculate that temperature.

The reaction is spontaneous below a temperature of 233.3 K.

Explanation:

Using Gibbs Helmholtz equation:

= Gibbs free energy  

= enthalpy change  = -70 kJ

= entropy change  = -0.300 kJ/K

T = temperature in Kelvin

= +ve, reaction is non spontaneous

= -ve, reaction is spontaneous

= 0, reaction is in equilibrium

At equilibrium :

Thus the reaction is spontaneous below a temperature of 233.3 K.