Question

For the reversible reaction $A_{(s)}+B_{(g)}\leftrightharpoons C_{(g)} +D_{(g)} \Delta G^\circ=-350kJ$ which one of the following statements is true?

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

Answer 1

Answer: (C)

Equilibrium constant is greater than one

Answer 2

$A(s)+B(g) \rightleftharpoons C(g)+D(g), \Delta G^{\circ}=-350\, kJ$

Relationship between $\Delta G^{\circ}$ and equilibrium constant is

$\Delta G^{\circ}=-2.303\, R T \log K_{p}$

When $K_{p} >1 ; \Delta G^{\circ}$ is negative.