74. Experiments were conducted to study the rate of the reaction represented by this equation.21 2NO(g) + 2H2(g) → N2(8) + 2H20(g) Initial concentrations and rates of reaction are given here. Experiment Initial Concentration Initial Concentration, [H2] Initial Rate of Formation of [NO] (mol L-) (mol L-1 min ) N2 (mol L-1 min ) 1 0.0060 0.0010 1.8 x 10-4 2 0.0060 0.0020 3.6 x 10-4 3 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,0, Step 2: N202 + H, = H20+N,0 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.

74. Experiments were conducted to study the rate of the reaction represented by this equation.21 2NO(g) + 2H2(g) → N2(8) + 2H20(g) Initial concentrations and rates of reaction are given here. Experiment Initial Concentration Initial Concentration, [H2] Initial Rate of Formation of [NO] (mol L-) (mol L-1 min ) N2 (mol L-1 min ) 1 0.0060 0.0010 1.8 x 10-4 2 0.0060 0.0020 3.6 x 10-4 3 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,0, Step 2: N202 + H, = H20+N,0 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.

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

The iodate ion reacts with sulfite ions in the reaction: 103 + 3SO3²1+ 3SO4². At what rate are the iodide and sulfate ions being produced if the sulfite ion is disappearing at a rate of 8.7 x 10.4 mol L ¹ s ¹? Rate of the iodide ion production is i Rate of the sulfate ion production is i Save for Later x 10-4 mol L ¹ s1. x 104 mol L-¹ s-1. Attempts: 0 of 10 used Submit Answer
Kinetic data are normally presented as graphs. The following questions test your knowledge about labeling and interpreting graphs correctly. [B] is used to represent the concentration of a reactant B in a reaction. y y LLLE 44 X X B с Decide if each of the following statements is True or False. y A y Consider graph D: if y = 1/[B] and x = time, the graph could represent a first order reaction. Consider graph A: if y = [B] and x = time, the graph could represent a first order reaction. ✓Consider graph C: if y = In[B] and x = time, the graph could represent a second order reaction. ✓Consider graph C: if y = [B] and x = time, the graph could represent a zero order reaction. ✓Consider graph D: if y = 1/[B] and = time, the slope is equal to -k. ✓ Consider graph B: if y = [B] and x = time, the graph could represent a second order reaction. X D
Time, s C3H8], M 0.0 0.26 10.0 0.18 20.0 0.14 30.0 0.10 . 40.0 0.064 .50.0 0.052 M
A chemistry graduate student is studying the rate of this reaction: 2SO3 (g) → 2SO₂(g) + O₂(g) He fills a reaction vessel with SO3 and measures its concentration as the reaction proceeds: time (minutes) 0 10. 20. 30. [so,] 0.0500M 0.0190M 0.0117 M 0.00847 M 40. 0.00663 M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k. Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. rate = k k = 0 x10 ロ・ロ X
Units of M s-1 please
8 OKONETICS AND EQUILIBRIUM Deducing a rate law from the change in concentration over time A chemistry graduate student is studying the rate of this reaction: 2N₂O, (g) → 2N₂O, (g) + O₂(g) He fills a reaction vessel with N₂O, and measures its concentration as the reaction proceeds: time (minutes) 0 10. [N₂O,] Explanation 0.300M 0.121 M 20. 0.0762 M 30. 0.0555 M 40. 0.0436M Use this data to answer the following questions. Write the rate law for this reaction. Calculate the value of the rate constant k Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol. Check rate & D www-awa.aleks.com k= D.D X
In the reaction 2H2O2(aq) +> 2H2O(l) + O2(g), the initial concentration of H2O2 is 0.745 M and, 1min. 25 seconds later, the concentration of H2O2 is 0.218 M. What is the average rate of reaction in MH2O2/s over this time interval? a. 0.003100. b. 00620 c. 0.124 d. 0.0422
Q4. Consider the reaction (at 20 °C). 2 NO(g) + Cl2(g) 2 NOC1 Look at to the below-given table. INITIAL INITIAL RATE OF Experiment No CONCENTRATIONS FORMATION NOCI NO Cl2 (mol/L. min) 1 0.10 0.10 0.18 0.10 0.20 0.36 3 0.20 0.20 1.45 Calculate the order of reaction with respect of NO and Cl2
The data for the reaction given NOCI (g) The following experimental data was measured for the reaction. Use the Method of Initial Rates to determine the rate law equation for this reaction 1 2 3 NO (g) + 1/2 Cl2₂ (g) [NO] [Cl₂] Initial Rate Experiment (mol.L-¹) (mol.L-¹) (mol.L-¹ s¯¹) 1.4x10-6 2.8x10-6 5.6x10-6 0.250 0.250 0.500 0.250 0.500 0.250 → 1. Determine the order of the reaction with respect to NO oxide 2. Determine the order of the reaction with respect to Cl₂ 3. What is the overall order of this reaction? 5. Calculate the value of the rate constant, k → 4. Select the correct rate law (rate equation) for this reaction: Rate =
A chemistry graduate student is studying the rate of this reaction: →H2CO3aq+H2OaqCO2aq She fills a reaction vessel with H2CO3 and measures its concentration as the reaction proceeds time(seconds) H2CO3 0 0.500M 10. 0.101M 20. 0.0563M 30. 0.0390M 40. 0.0298M 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 2 significant digits. Also be sure your answer has the correct unit symbol. =k
Consider the following fictitious reaction and the measured initial rates at different reaction conditions. Determine the rate law for this reaction. X (g) + y (g) XY (g) Trial 1 2 3 Initial Rate (M/h) 0.05069 [X] M [Y] M 0.1383 0.1860 0.1383 0.6783 0.18476 0.3804 0.1860 0.05079
A chemistry graduate student is studying the rate of this reaction: H,CO, (aq) →+ H,O(aq) + CO, (ag) She fills a reaction vessel with H₂CO, and measures its concentration as the reaction proceeds: time (seconds) [H₂CO,] 0.100M 0 1.0 2.0 0.0262M 3,0 0.0151 M 0.0106M 4.0 0.00816M Use this data to answer the following questions. write the rate law for this reaction. Calculate the value of the rete constant k Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol rate & 0 C+D Da 7.