The free energy change of the reaction a(g) ⟺ b(g) is –32.5 kj under nonstandard conditions. the standard free energy change of the reaction is –42.5 kj. is the reaction at the nonstandard conditions more spontaneous or nonspontaneous? the reaction is more spontaneous at nonstandard conditions. the reaction is less spontaneous at nonstandard conditions. the reaction is at equilibrium.

The reaction is less spontaneous at nonstandard condition.

Explanation:

Thermodynamically, for a spontaneous reaction, change in free energy should be negative.

More negative the free energy change, more will be the spontaneity of reaction. This is due to - (1) either decrease in enthalpy change during reaction which indicates that product of the reaction is more stable (2) and/or due to increase in change in entropy during reaction which indicates increase in randomness in system.

Here nonstandard free energy change is lesser negative (-32.5 kJ) than standard free energy change (-42.5 kJ).

Therefore the reaction is less spontaneous at nonstandard condition.

? you expect us to answer this? ? this is your schoolwork, i don't think we can with this, i think it would considering being

m=9

step-by-step explanation: