The equilibrium constant for the reaction $2SO_2(g)+O_2(g) \to 2SO_3(g)$ would be :

Question

$\begin{array}{1 1} (a)\; K= 2[SO_3]/2[SO_2][O_2] \\ (b)\; K= 2[SO_2]/[O_2][SO_3] \\ (c) \;[SO_3]^2[SO_2]^2[O_2] \\ (d)\; [SO_2]^2[O_2]/[SO_3]^2 \end{array} $

Answer 1

Solution :

Using the chemical reaction given above, we can rewrite the Equilibrium constant expression to reflect concentration. The concentration is molarity, written as moles per liter (M=mol/L).

$K_c=[C]^c[D]^d/[A]^a[B]^b$

The products are in the numerator and those of the reactants are in the denominator. The equation is a function of the concentrations, the upper case letters are the molar concentrations of the reactants and products (A, B etc.).

The lowercase letters are the stoichiometric coefficients that balance the equation.

Hence Answer is $K = [SO_3]^2/[SO_2]^2[O_2]$