For a particular reaction, ah = 81.95 kj/mol and as = 27.0 j/(mol-k) calculate ag for this reaction at 298 k. ag = kj/mol what can be said about the spontaneity of the reaction at 298 k? the system is spontaneous in the reverse direction o the system is at equilibrium o the system is spontaneous as written o o

The system is spontaneous in the reverse direction

Explanation:

According the equation of Gibb's free energy -

∆G = ∆H -T∆S  

∆G = is the change in gibb's free energy

∆H = is the change in enthalpy

T = temperature  

∆S = is the change in entropy .

And , the sign of the  ΔG , determines whether the reaction is Spontaneous or non Spontaneous or at equilibrium ,  

i.e. ,  

if  

ΔG < 0 , the reaction is Spontaneous

ΔG > 0 , the reaction is non Spontaneous

ΔG = 0 , the reaction is at equilibrium

from the question ,

∆H = 81.95 kJ/mol

( since , 1 KJ = 1000 J )

∆H = 81950 J/mol

∆S =  27.0 J/(mol-K)

The ∆G is calculated from the above formula -

∆G = ∆H -T∆S  

∆G = (81950 J/mol) - [(298 K) x ( 27.0 J/(mol·K))]

∆G = (81950 J/mol) - (8046 J/mol)

∆G = 73904 J/mol

∆G = 73.904 kJ/mol

Since ΔG > 0 , the system is non spontaneous in the forward direction and hence it will be spontaneous in the reverse direction .