The reaction between nitric oxide and chlorine gas obeys an overall third-order rate law with a rate constant of 3.00 M^–2•s^–1: 

2 NO(g) + Cl₂(g) → 2 NOCl(g)      rate = k[NO]²[Cl2]

When [NO] = [Cl₂], the integrated rate law is: 

1/[Cl₂]_t² = 2 kt +1/([Cl₂]₀)²

If the initial concentrations of NO and Cl₂ are 0.300 M and 0.150 M, respectively, calculate the concentrations of NO, Cl₂, and NOCl after 50.0 s.