For the water gas reaction, C(s)+H2O(g)CO(g)+H2O(g) the standard Gibbs energy at 1000 K is -8.1 text kJ mol-1 . What is its equilibrium constant?

Question

For the water gas reaction, C(s)+H2O(g)CO(g)+H2O(g) the standard Gibbs energy at 1000 K is -8.1 text kJ mol-1 . What is its equilibrium constant? (A) 2.60 (B) 4.62 (C) 2.64 (D) None of these

Tardigrade Admin · Accepted Answer

Δ G° =-2.303 text RT text log text K or log K=(-Δ G° /2.303RT) log K=(-8.1/2.303× 8.314× 10-3× 1000) =0.423 or K=2.64

Q. For the water gas reaction, $C (s) + H_{2} O (g) CO (g) + H_{2} O (g)$ the standard Gibbs energy at 1000 K is $- 8.1 k J m o l^{- 1}$ . What is its equilibrium constant?

2.60

4.62

2.64

None of these

$Δ G^{\circ} = - 2.303 RT l o g K$ or $lo g K = \frac{- Δ G ^{\circ}}{2.303 RT}$ $lo g K = \frac{- 8.1}{2.303 \times 8.314 \times 10 ^{- 3} \times 1000}$ $= 0.423$ or $K = 2.64$

Q. For the water gas reaction, C(s)+H2​O(g)CO(g)+H2​O(g) the standard Gibbs energy at 1000 K is −8.1kJmol−1 . What is its equilibrium constant?