Question

The equilibrium constant for the reaction $3A+2B$ $\rightleftharpoons$ $C$ will be:

• A. $\frac{\left[3A\right]\left[2B\right]}{\left[C\right]}$
• B. $\frac{{\left[A\right]}^3\left[B\right]}{\left[C\right]}$
• C. $\frac{\left[C\right]}{{\left[A\right]}^3{\left[B\right]}^2}$
• D. $\frac{\left[C\right]}{\left[3A\right]\left[2B\right]}$

Answer 1

Answer: (C)

$\frac{\left[C\right]}{{\left[A\right]}^3{\left[B\right]}^2}$

The equilibrium constant of a reaction is the ratio of the equilibrium concentration of products to the equilibrium concentration of reactants. The concentration terms are raised to appropriate powers which are equal to stoichiometric coefficients.

The reaction is $3A+2B\rightleftharpoons C$.

The expression for the equilibrium constant will be $K_c=\frac{\left[C\right]}{{\left[A\right]}^3{\left[B\right]}^2}$.