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

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

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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1 Consider the reaction and the following experimental data: C4H9CI(aq) + H2O1)→ C4H9OH(aqg) + HCl(aq). Time/sec [C4H9CI] 0.1000 50 0.0905 100 0.0820 150 0.0741 200 0.0671 300 0.0549 400 0.0448 500 0.0368 800 0.0200 Differentiate between the "average rate of a reaction" and the "instantaneous rate of a reaction". a Determine the average rate of the reaction between 100 seconds and 500 seconds. Ensure your answer is given with the correct units. b By graphing the above data, determine the instantaneous rate of the reaction at 300 seconds.
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A+B → Products Run 1 2 3 [A]o [B] (M) (M) 1 1 2 1 2 1 Initial Rate (M/sec) 1 2 4 Rate = k [A]² [B]. What is k (don't forget the units) = [k]?
plz answer all in detail if u plan to do only 1 then plz skip do all
Consider the gas-phase reaction: H2(g) + 12(g) → 2 HI(g) The reaction was experimentally determined to be first order in H₂ and first order in 12. Consider the proposed mechanisms. Mechanism 1: H2(g) + 2(g) 2 HI(g) single step k₁ Mechanism 2: 12(g) k_1 21(g) fast H2 212 HI(g) slow K2 *Draw energy diagrams for the mechanisms shown: Show that both of the proposed mechanisms are valid.
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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