1. Given the experimental information in the following table, answer the questions given.A > productsTime (minutes)[A] (M)0.000.15631.000.14692.000.1431a. Calculate the average rate of reaction during the first minute and the second minute.b. Why are the rates calculated not equal?

1. Given the experimental information in the following table, answer the questions given. A → products Time (minutes) 0.00 1.00 2.00 (A] (M) 0.1563 0.1469 0.1431 a. Calculate the average rate of reaction during the first minute and the second minute. b. Why are the rates calculated not equal?

1. Given the experimental information in the following table, answer the questions given. A → products Time (minutes) 0.00 1.00 2.00 (A] (M) 0.1563 0.1469 0.1431 a. Calculate the average rate of reaction during the first minute and the second minute. b. Why are the rates calculated not equal?

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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3. Let us consider a decomposition reaction with a reactant ‘B’ and the rate of reaction is absolutely depended on B’s concentration. From different batches of the same experiment it was found that, with varying concentration of ‘B’ the rate of reaction remains fairly constant. What was the order of the reaction? Show the calculation steps.
74. Experiments were conducted to study the rate of the reaction represented by this equation. 2 2NO(g) + 2H2(g) · N2(g) + 2H2O(g) Initial concentrations and rates of reaction are given here. Experiment Initial Concentration Initial Concentration, [H2] Initial Rate of Formation of [NO] (mol L-1) (mol L-1 min-1) N2 (mol L-1 min¬1) 1 0.0060 0.0010 1.8 × 10-4 2 0.0060 0.0020 3.6 x 10-4 3 0.0010 0.0060 0.30 × 10-4 4 0.0020 0.0060 1.2 x 10-4 Consider the following questions: (a) Determine the order for each of the reactants, NO and H2, from the data given and show your reasoning. (b) Write the overall rate law for the reaction. (c) Calculate the value of the rate constant, k, for the reaction. Include units. (d) For experiment 2, calculate the concentration of NO remaining when exactly one-half of the original amount of H, had been consumed. (e) The following sequence of elementary steps is a proposed mechanism for the reaction. Step 1: NO + NO = N,02 Step 2: N,02 + H, = H20+N,0 Step 3:…
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Consider the reaction A → products. Which of the following plots is consistent with a zero-order reaction? a. In [A] plotted against time gives a straight line of negative slope. b. 1/[A] plotted against time gives a straight line of positive slope. c. [A] plotted against time gives a curved line of negative slope, decreasing in magnitude as time increases d. [A] plotted against time gives a horizontal, straight line. e. [A] plotted against time gives a straight line of negative slope.
For the reaction: 4NH3 (g) + 7O2 (g) → 4NO2 (g) + 6H2 (g), if H2 is produced at a rate of 3.5 x 10-3 M/s, O2 is consumed at a rate of... A. -2.5 x 10-2 M/s B. -4.1 x 10-3 M/s C. -2.1 x 10-2 M/s D. -3.0 x 10-3 M/s E. -5.8 x 10-4 M/s
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