1. The problem statement, all variables and given/known data The Reaction; 2NO(g) + Cl2 (g) → 2NOCl (g) Is second order in NO and first order in Cl2. Five moles of nitric oxide and two moles of Cl2 were brought together in a volume of 2dm3 and initial rate was 2.4x10-3 moldm-3sec-1. What will be the rate when one half of the chlorine has reacted? 2. Relevant equations Rate = k [NO]2 [Cl2] 3. The attempt at a solution Initial Rate= 2.4x10-3 moldm-3sec-1 2.4x10-3 = k [NO]2 [Cl2] 5mols of NO in 2dm3 = 5mols in 2L ∴ 1L contains 2.5mols [NO] = 2.5M 2mols of Cl2 in 2dm3 = 2mols in 2L ∴ 1L contains 1mol [Cl2] = 1M 2.4x10-3 = k (2.5)2 (1) k = 2.4x10-3/6.25 = 0.000384 When half of the chorine is used (1mol), molarity = 0.5M ∴ Rate = (0.000384) (2.5)2 (0.5) Rate = 0.0012moldm-3sec-1 Am I going about this the right way or this completely wrong?