Question

The equilibrium constant expression for a gas reaction is, $K_C=\frac{\left[N{H}_3{]}^4\right[O_2{]}^5}{\left[NO{]}^4\right[H_{2}O{]}^6}$
The balanced chemical equation corresponding to this expression is.

• A. $4NO\left(g\right)+6H_{2}O\left(g\right)\rightleftharpoons 4N{H}_3\left(g\right)+5O_2\left(g\right)$
• B. $4N{H}_3\left(g\right)+5O_2\left(g\right)\rightleftharpoons 4NO\left(g\right)+6H_{2}O\left(g\right)$
• C. both of above
• D. none of these

Answer 1

The correct option is A $4NO\left(g\right)+6H_{2}O\left(g\right)\rightleftharpoons 4N{H}_3\left(g\right)+5O_2\left(g\right)$

The equilibrium constant expression is $K_C=\frac{\left[N{H}_3{]}^4\right[O_2{]}^5}{\left[NO{]}^4\right[H_{2}O{]}^6}$
The terms in the numerator indicates the concentrations of products raised to appropriate stoichiometric coefficients. Thus the products are ammonia and oxygen. Their stoichiometric coefficients are 4 and 5 respectively.
The terms in the denominator indicates the concentrations of reactants raised to appropriate stoichiometric coefficients. Thus the reactants are nitric oxide and water. Their stoichiometric coefficients are 4 and 6 respectively.
The balanced chemical equation is$4NO\left(g\right)+6H_{2}O\left(g\right)\rightleftharpoons 4N{H}_3\left(g\right)+5O_2\left(g\right)$