1. Tardigrade
  2. Question
  3. Chemistry
  4. For the water gas reaction C(s)+H2O(g)rightharpoons CO(g)+H2(g) At 1000 K, the standard Gibbs free energy change of the reaction is -8.314 kJ/mol. Therefore, at 1000 K the equilibrium constant of the above water gas reaction is

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Q. For the water gas reaction
$C\left(s\right)+H_{2}O\left(g\right)\leftrightharpoons CO\left(g\right)+H_{2}\left(g\right)$
$At 1000 K,$ the standard Gibbs free energy change of the reaction is $-8.314\, kJ/mol$. Therefore, at $1000\, K$ the equilibrium constant of the above water gas reaction is

Thermodynamics

Solution:

$\Delta_{r}G^{\circ}=-8.314\times10^{3}$
$\therefore -\Delta_{r}G^{\circ}=8.314\times10^{3}=RT ln K_{eq}$
or $8.314 \times 10^3 = 8.314 \times10^3 ln K_{eq}$
or $ln \,K_{eq}= 1 = ln \,e$
or $K_{eq}= e = 2.718$