For the reversible reaction :
`A_(s) + B_(g) hArr C_(g) + D_(g) : Delta G^(@) = - 350 kJ`
Which one of the following statements is true ?

Options

A. The reaction is thermodynamically nonfeasible
B. The entropy change us neative.
C. Equilibrium constant is greater than one.
D. The reaction should be instantaneous.

Answer

C

Explanation

For a reversible reaction,
`A_(s)+B_(g)hArrC_(g)+D_(g)+D_(g),DeltaG^(@)`=-350KJ
Standard free energy change can be thermodynamically calculated as,
When `DeltaG^(@)lt0,` i.e,-ve,then `K_(c)gt1`.In this case forward reaction is feasible .The reaction is spontaneous reaction.