Answer:
As we know that the equilibrium constant, Kc, is defined as the product of the equilibrium concentrations of products over the equilibrium concentrations of reactants, each raised to the power of the stoichiometric coefficients of the reactants and products.
The given reaction in the question is,
Therefore, the equilibrium constant for the reaction,
![\mathrm{K}_{\mathrm{C}}=\left(\left[\mathrm{H}_{2}\right]\left[\mathrm{CO}_{2}] \mathrm{~J}\right) /\left(\left[\mathrm{H}_{2} \mathrm{O}\right][\mathrm{CO}]\right)=\left(0.4 \times 0.4\right) /(0.6 \times 0.6)=0.444\right.](https://www.learnatnoon.com/s/wp-content/ql-cache/quicklatex.com-9c3ec30ba0b51282ce22d45525e36956_l3.png "Rendered by QuickLaTeX.com")
