{Equation: A+B – C + D Rate law: Rate = \[A[B]” Here, x is the order of the reaction wrtA y is the order of the reaction wrt B Experiment 1: 0.0112 M’s = $(0.390)*(0.300)” Experiment 2: 0.0645 M’s = Equation: A+B-C + D Rate law. Here, x is a measure of the reaction order wrtA. Experiment 1: 0.0112M’s = $(0.390),*(0.300),” Experiment 2 : 0.0645M’s = $ (0.390),*(0.720),” Experiment 3: 0.0190M’s = 0.0645M’s = 0.0390)*(0).720. Experiment 4 : 0.300) —-2 —-2 —-3 — — 2—-3 to determine the value of x. 0.0190 M’s (0.300), 0.0112 (0.390)* 0.300). 1.7 = (17.72 = (1.7), x = 1. 0.0645 M’s (0.390 (0.720) 0.0112 M/s K (03901″ (0.300) 5.8 = (2.4) 2.42 = (2.4) y = 2 Hence, the order of the reaction w.rt Bis 2 Therefore, the rate law is : Rate = k[A][B] Thus, order of the reaction = x + y = 2+1 = 3 Experiment 1:0.0112 M’s = (0.390)*(0.300) Rate law: Rate = k[A[B] Rate constant, k = [A][B] 0.0112 M/s (0.390 M) (0.300 M) = 0.319 M-:-|0.0645 Mis (0.720) 0.0112 K (03901″) 5.8 = (2.4), 2.42 = (2.4), y = 2, Experiment 1 :0.0112M’s = (0.390),*0.300) Rate law. Rate constant, Rate = [A][B] 0.0112M/s (0.300 M/s) 0.0390 M/s (0.300M) = 0.0319 M-:-}