Given the concentrations, calculate the equilibrium constant for this reaction: 2SO2(g) +O2(g)⇌2SO3(g) At equilibrium, the molar concentrations for reactants and products are found to be [SO2]=0.48 M, [O2]=0.40 M, and [SO3]=1.12 M. What is the equilibrium constant (Kc) for this reaction?

The equilibrium constant for this reactions is 13.61

Explanation:

Step 1: Data given

Concentrations at the equilibrium are:

[SO2]=0.48 M

[O2]=0.40 M

[SO3]=1.12 M.

Step 2: The balanced equation

2SO2(g) +O2(g) ⇌ 2SO3(g)

Step 3: Calculate Kc

Kc = [SO3]²/[O2]*[SO2]²

Kc = (1.12²) / (0.40 * 0.48²)

Kc = 13.61

The equilibrium constant for this reactions is 13.61

neutrons are in the middle of the atom and the electrons, which are much smaller.