Question

EXPERIMENT 3. Kinetic Study: The lodine Clock Reaction Prelaboratory Questions Name Fiza Chandning Laboratory Section 0000000000000000000000000000000000000000000000000000000000000000000000000000000 1. Consider the following reaction: 2 NO(g) + 4 NO, (g) + O2(g) The initial concentration of N, O, was 0.84 mol/L, and 35 minutes after initiating the reaction, all of the N,Os has been consumed. a) Calculate the average rate of the reaction over this 35-minute time interval. b) Is it correct to assume that the rate law is Rate = k[NO]? based on the balanced chemical equation? Briefly explain your answer. c) Suppose the reaction rate is determined by simultaneously measuring the rate of decrease of N,Os concentration (-A[N2O5]/At) and the rate of increase of NO, concentration (A[NO]/At). Which rate will be higher and by what factor? (continued on next page) 137

Answer 1

c * Pls - Plzt el I 0.320 o o os-x x x E (0-320-x) x x K= x² = 0.012 0-320-2 2 0-00384-0-0124 X-00122 -0.0038430 x = -bi 6²4ac 29 = toot2 I 0012 +uX000384 - 0-1246 +0.012 = 0-06825 (pus) - 0-320-0.0682520 25175 (23 -0.06825M puz} = 0.06825M Rate = K[Hz] {No] * 0 126 = K [025] [o to] 0 0.504 = K[0.503 [0:1039 - 0 1:03 = K [0.503 * {0 2039 - ② 2- (2) = 24 Rate = K[NO] ² [Hz]'