Which of the following experiments would be consistent with this mechanism? slow Step 1: 2NO2(g) → NO3(g) + NO(g) Step 2: NO3(g) + CO(g) NO2(g) + CO2(g) fast Experiment I [CO] (M) Experiment II [CO] (M) time (s) time (s) 10 0.476 10 0.495 24 0.443 24 0.488 57 0.376 57 0.4715 98 0.306 98 0.451 150 0.236 150 0.425 300 0.112 300 0.35 Neither experiment Experiment II only O Experiment I and II O Experiment I only

The reaction of nitrogen dioxide and carbon monoxide in the gas state to form carbon dioxide and nitric oxide is represented by the equation: NO2(g)+CO(g)--->CO2(g)+NO(g) The following data were collected for the above reaction Experiment No [CO2] (M) [CO] (M) Initial Rate (M/s) 1 5.0*10-4 1.6*10-2 1.7*10-7 2 5.0*10-4 3.2*10-2 1.7*10-7 3 1.5*10-3 3.2*10-2 1.5*10-6 Determine the order of the reaction with respect to each reactant.

Given the following data, estimate the rate constant of A(g) + B(g) → AB(g) (do not write the units in your answer) Experiment [A] (M) [B] (M) Rate (M/s) 1 0.400 0.200 0.8 2 0.200 0.200 0.200 0.200 0.100 0.05

Determine the average rate of change of B from t :0 s to Time (s) Concentration of A (M) t = 252 s. 0.740 126 0.425 A → 2B 252 0.110 rateB = M/s

An experiment was carried out to investigate the effect of concentration on the reaction: BrO3(aq) + 5 Br (aq) + 6 H* (aq) = 3 Br₂ (1) + 3 H₂O (1) The following data was obtained: Initial [BrO3] Initial [Br] Initial [H*] Initial Rate Trial (mol/L) (mol/L) (mol/L) (mol/L's) 1 0.10 0.10 0.10 8.0 x 10-4 2 0.20 0.10 0.10 1.6 x 10-3 3 0.20 0.20 0.10 3.2 x 10-3 4 0.10 0.10 0.20 3.2 x 10-3 a) Deduce and state the rate law equation for this reaction. Show your process/reasoning. b) Calculate the value of k, the rate constant with correct units.

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Using the data in the table, calculate the rate constant of this reaction. k= A+B C+D Trial 1 2 3 Units [A] (M) 0.260 0.260 0.364 [B] (M) 0.350 0.945 0.350 Rate (M/s) 0.0167 0.122 0.0234

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Be sure to answer all parts. The rate law for 2 NO(g) + O2(g)→ 2 NO2(g) is rate = k[NO]°[O2l. %3D The following mechanisms have been proposed: I. 2 NO(g) + O2(g)→ 2 NO2(g) II. 2 NO(g) = N½O2(g) [fast] N,O2(g) + O2(g) → 2 NO,(g) [slow] III. 2 NO(g) = N,(g) + O2(g) [fast] N2(g) + 2 O2(g) → 2 NO2(g) [slow] (a) Which of these mechanisms is consistent with the rate law? Check all that apply. I. II. III. None of the above (b) Which of these mechanisms is most reasonable? I. II. III.

Use the data presented in the table to determine the rate equation for the hypothetical reaction shown. A(g) + 2B(g) + 3C(g) [Math Processing Error] D(g) + 2F(g) Exp {A} (M) {B} (M) {C} (M) initial rate (M/min) 0.0025 0.0025 0.0025 3.16x10-11 0.0025 0.0050 0.0025 1.27x10-10 3 0.0050 0.0050 0.0025 1.27x10-10 4 0.0100 0.0100 0.0050 4.06x10-9 What is the reaction order with respect to A? What is the reaction order with respect to B? What is the reaction order with respect to C? Enter each of your answers numerically as integers or fractions (ex: 0, 1/2, 1, 3/2, 2, 3, etc). Hint: Determining the order of one of the reactants will be difficult. Determine the order of the two easy reactants first, then use that information in determining the difficult one.