This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Here are the solutions to the questions: 1. (d) (i) Determine the overall order of the reaction 2NO(g) + Cl_2(g) 2NOCl(g) showing all the steps. The general rate law for this reaction can be written as: Rate = k[NO]^x[Cl_2]^y where x is the order with respect to NO, y is the order with respect to Cl_2, and k is the rate constant. Step 1: Determine the order with respect to [Cl_2] (y). Compare Experiment 1 and Experiment 2, where [NO] is kept constant. From Experiment 1: Rate_1 = k(0.10)^x(0.10)^y = 0.17 From Experiment 2: Rate_2 = k(0.10)^x(0.20)^y = 0.35 Divide Rate_2 by Rate_1: Rate_2Rate_1 = (k(0.10)^x(0.20)^y)/(k(0.10)^x(0.10)^y) = (0.35)/(0.17) ((0.20)/(0.10))^y = 2.0588 (2)^y ≈ 2 Therefore, y = 1. The reaction is first order with respect to [Cl_2]. Step 2: Determine the order with respect to [NO] (x). Compare Experiment 2 and Experiment 3, where [Cl_2] is kept constant. From Experiment 2: Rate_2 = k(0.10)^x(0.20)^y = 0.35 From Experiment 3: Rate_3 = k(0.20)^x(0.20)^y = 1.45 Divide Rate_3 by Rate_2: Rate_3Rate_2 = (k(0.20)^x(0.20)^y)/(k(0.10)^x(0.20)^y) = (1.45)/(0.35)