0.149 mol/L of A₂(g) and 0.149 B₂(g) are initially present in a flask. The A₂ and B2 react according to the balanced equation

Question

0.149 mol/L of A₂(g) and 0.149 B₂(g) are initially present in a flask. The A₂ and B2 react according to
the balanced equation below.
A₂(g) + B₂(g) = 2 AB(g)
When equilibrium is reached, the concentration of B₂(g) has decreased to 0.036 mol/L. What is the
equilibrium constant, Kc, for the reaction?

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