NEET | 2017Chemical BondingHard

Question

For a given reaction, ∆H = 35.5 kJ mol-1 and ∆S = 83.6 JK-1mol-1. The reaction is spontaneous at : (Assume that ∆H and ∆Sdo not vary with tempearature)

Options

A.

T > 425 K

B.

All temperatures

C.

T > 298 K

D.

T < 425 K

Solution

∆G=∆H-T∆G
for equilibrium ∆G=0
∆H=T∆S
Teq.=∆H∆S=35.5×100083.6=425 K
Since the reaction is endothemic it will be spontaneous at T > 425K. Option (1)

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