Experiments were conducted to study the rate of the reaction represented by this equation.21 2NO(g) + 2H2(g) – N2(g) + 2H2O(g) Initial concentrations and rates of reaction are given here. Initial Concentration, [H] (mol/L) Experiment Initial Concentration Initial Rate of Formation of [NO] (mol/L) N2 (mol/L min) 0.0060 0.0010 1.8 x 10-4 0.0060 0.0020 3.6 x 10-4 0.0010 0.0060 0.30 x 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 H2 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: N202+ H2 = H20+N20 Step 3: N20+H2 = N2+ H20 Based on the data presented, which of these is the rate determining step? Show that the mechanism is consistent with the observed rate law for the reaction and the overall stoichiometry of the reaction. 2. 3.

Experiments were conducted to study the rate of the reaction represented by this equation.21 2NO(g) + 2H2(g) – N2(g) + 2H2O(g) Initial concentrations and rates of reaction are given here. Initial Concentration, [H] (mol/L) Experiment Initial Concentration Initial Rate of Formation of [NO] (mol/L) N2 (mol/L min) 0.0060 0.0010 1.8 x 10-4 0.0060 0.0020 3.6 x 10-4 0.0010 0.0060 0.30 x 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 H2 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: N202+ H2 = H20+N20 Step 3: N20+H2 = N2+ H20 Based on the data presented, which of these is the rate determining step? Show that the mechanism is consistent with the observed rate law for the reaction and the overall stoichiometry of the reaction. 2. 3.

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...

See similar textbooks

Similar questions

A chemistry graduate student is studying the rate of this reaction: NH4OHaq→NH3aq+H2Oaq She fills a reaction vessel with NH4OH and measures its concentration as the reaction proceeds time(seconds) NH4OH 0 0.0700M 10. 0.0370M 20. 0.0196M 30. 0.0103M 40. 0.00547M Use this data to answer the following questions. Write the rate law for this reaction. rate =k Calculate the value of the rate constant k.Round your answer to 2significant digits. Also be sure your answer has the correct unit symbol. =k
Cn.
Very confused with this rate law
None
7. A study of the hypothetical reaction 2A + B C+D gave these results: Initial Rate (emol Ls) Initial Concentration (mal/) Experiment 181 1. 0.10 0.050 6.0 x 10 2. 0.20 0.050 1.2 x 10 3 0.30 0.050 1.8 x 10 2 4. 0.20 0.150 1.1 x 10-1 a) What is the rate law for this reaction? b) Calculate the rate constant k and express it in appropriate units.
8. Smelling salt decomposes spontaneously at room temperature by the equation below. A student places a 10.00-g sample into a 1-liter sealed rigid vessel. What measurements should the student make to determine the rate of this reaction?(NH4)2CO3(s)→2NH3(g)+H2O(g)+CO2(g) a. change in mass and temperature b. temperature and time c. change in mass and time d. change in pressure and time
Deducing a rate law from initial reaction rate data Some measurements of the initial rate of a certain reaction are given in the table below. N2| H2 initial rate of reaction 圖 2.26M0.562M 9.00 × 10°M/s 2.26 M 0.108M 3.32 x 10ʻM/s 8.45 M 0.562M 3.37 x 10°M/s olo Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k| k = 1
Consider the given reaction : 2HgC2(ag) + C204²(ag) – 2CH(ag) + 2CO2(g) + Hg2Cl2(s) Experiment [HgCl2] [C2O42] Initial rate 1 0.0836 M 0.202 M 5.2 x10-5 0.0836 M 0.404 M 2.08 x10-4 0.0418 M 0.404 M 1.04 x104 4 0.0627 M 0.606 M ? Calculate the initial rate for experiment 4. 3.50 x 10-4 M min-1 8.75 x 103 M min-1 1.20 x 10-4 M min-1 O 6.00 x 104 M min 1
O KINETICS AND EQUILIBRIUM Deducing a rate law from initial reaction rate data Some measurements of the initial rate of a certain reaction are given in the table below. H, I, initial rate of reaction 0.735 M 0.260 M 78.0M/s 0.735 M 0.341 M 102. M/s 0.354 M 0.260 M 37.6M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. Do rate = k| x10 k = Explanation Check © 2021 McGraw-Hill Educat II
2. Consider the reaction: NH4 (aq) + 2NO2 (aq) → N2(g) + 2H2O[g) Rate = k[NH4*][NO2] Which of the following reaction conditions will generally result in a longer reaction time? O Adding a catalyst to the reaction mixture. O Placing the reaction mixture in a hot water bath. O Increasing the concentration of any reactants. O Adding distilled water to the mixture.
Draw the order of reaction graphs (reaction rate vs the concentration) for [NO] and [H2]. Explain the difference between the two graphs
Consider the reaction: NO2 + 03 → NO3 + 02 [NO,], M [03], M Rate, M/s 6.30 x 10-3 Experiment 1 0.21 0.70 1.89 x 10-2 3.15 x 10-3 0.63 0.65 3 0.21 0.35 4 0.42 0.35 6.30 x 10-3 Calculate the rate of [NO3] production at 0.84 M [NO2]and 1.4 M [03]. Final answer must be rounded off to 2 decimal places, and shall NOT have any units.