For the reaction Cl _ 2( ~g ) +2 NO _ ( g ) 2 NOCl _ ( g ) , the following data was obtained: Experiment No. Initial concentration of Cl₂ (M) Initial concentration of NO (M) Initial reaction rate (M/min) I 0.15 0.15 0.60 II 0.30 0.15 1.20 III 0.15 0.30 2.40 IV 0.25 0.25 2.78 Identify the order of the reaction with respect to Cl ₂, NO and the value of Rate constant.

Step-by-step solution

The rate law for the reaction is given by Rate = k[Cl₂]^x [NO]^y . Using data from Experiment I and II: 0.60 = k(0.15)^x (0.15)^y 1.20 = k(0.30)^x (0.15)^y Dividing the two equations: 1.20 0.60 = ( 0.30 0.15 )^x 2 = 2^x x = 1 . Using data from Experiment I and III: 0.60 = k(0.15)^1 (0.15)^y 2.40 = k(0.15)^1 (0.30)^y Dividing the two equations: 2.40 0.60 = ( 0.30 0.15 )^y 4 = 2^y y = 2 . The rate law is Rate = k[Cl₂]^1 [NO]^2 . Calculating the rate constant k using Experiment I: 0.60 = k(0.15)(0.15)^2 0.60 = k(0.15)