A chemistry graduate student is studying the rate of this reaction: H2CO, (aq)- H,O (aq)+ CO, (aq) 3 He fills a reaction vessel with H,CO, and measures its concentration as the reaction proceeds: [H,CO,] time (seconds) 0 0.500 M 0.321 M 1.0 0.206 M 2.0 0.132 M 3.0 0.0849 M 4.0 Use this data to answer the following questions. = k న్ Write the rate law for this reaction. rate xt0 Calculate the value of the rate constant k. k = 0 ? Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol.

A chemistry graduate student is studying the rate of this reaction: H2CO, (aq)- H,O (aq)+ CO, (aq) 3 He fills a reaction vessel with H,CO, and measures its concentration as the reaction proceeds: [H,CO,] time (seconds) 0 0.500 M 0.321 M 1.0 0.206 M 2.0 0.132 M 3.0 0.0849 M 4.0 Use this data to answer the following questions. = k న్ Write the rate law for this reaction. rate xt0 Calculate the value of the rate constant k. k = 0 ? Round your answer to 2 significant digits. Also be sure your answer has the correct unit symbol.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 5ALQ: Consider the following statements: In general, the rate of a chemical reaction increases a bit at...

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Consider the hypothetical reaction A+B+2C2D+3E In a study of this reaction three experiments were run at the same temperature. The rate is defined as [B]/t. Experiment 1: [A]0 = 2.0 M [B]0 = 1.0 103 M [C]0 = 1.0 M [B] (mol/L) Time(s) 2.7 104 1.0 105 1.6 104 2.0 105 1.1 104 3.0 105 8.5 105 4.0 105 6.9 105 5.0 105 5.8 105 6.0 105 Experiment 2: [A]0 = 1.0 102M [B]0 = 3.0 M [C]0 = 1.0 M [A] (mol/L) Time(s) 8.9 103 1.0 7.1 103 3.0 5.5 103 5.0 3.8 103 8.0 2.9 103 10.0 2.0 103 13.0 Experiment 3: [A]0 = 10.0 M [B]0 = 5.0 M [C]0 = 5.0 101M [C] (mol/L) Time(s) 0.43 1.0 102 0.36 2.0 102 0.29 3.0 102 0.22 4.0 102 0.15 5.0 102 0.08 6.0 102 Write the rate law for this reaction, and calculate the value of the rate constant.
If a textbook defined a catalyst as "a substance that increases the rate of a reaction," would that definition be adequate?
Consider the decomposition reaction 2X2Y+ZThe following graph shows the change in concentration with respect to time for the reaction. What does each of the curves labeled 1, 2, and 3 represent?
The following statements relate to the reaction for the formation of HI: H2(g) + I2(g) -* 2 HI(g) Rate = it[HJ [I2J Determine which of the following statements are true. If a statement is false, indicate why it is incorrect. The reaction must occur in a single step. This is a second-order reaction overall. Raising the temperature will cause the value of k to decrease. Raising the temperature lowers the activation energy' for this reaction. If the concentrations of both reactants are doubled, the rate will double. Adding a catalyst in the reaction will cause the initial rate to increase.
Why awe elementary reactions involving three or more reactants very uncommon?
Experimental data are listed here for the reaction B: Time (s) IB] (mol/L) 0.00 0.000 10.0 0.326 20.0 0.572 30.0 0.750 40.0 0.890 Prepare a graph from these data, connect the points with a smooth line, and calculate the rate of change of [B] for each 10-s interval from 0.0 to 40.0 s. Does the rate of change decrease from one time interval to the next? Suggest a reason for this result. How is the rate of change of [AJ related to the rate of change of [B] in each time interval? Calculate the rate of change of [AJ for the time interval from 10.0 to 20.0 s. What is the instantaneous rate, A[B]/Ar, when [BI = 0.750 mol/L?
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 [NO] (mol/L) Initial Concentration, [H2] (mol/L) Initial Rate of Formation of N2 (mol/L min) 1 0.0060 0.0010 1.8104 2 0.0060 0.0020 3.6104 3 0.0010 0.0060 0.30104 4 0.0020 0.0060 1.2104 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+NON2O2 Step 2: N2O2+H2H2O+N2O Step 3: N2O+H2N2+H2O 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.
Based on the diagram in Exercise 12.83, which of the reactions has the fastest rate? Which has the slowest rate?
Experimental data are listed here for the reaction A 2 B. (a) Prepare a graph from these data; connect the points with a smooth line; and calculate the rate of change of [B] for each 10-second interval from 0.0 to 40.0 seconds. Does the rate of change decrease from one time interval to the next? Suggest a reason for this result. (b) How is the rate of change of [A] related to the rate of change of [B] in each time interval? Calculate the rate of change of [A] for the time interval from 10.0 to 20.0 seconds.
At 40C, H2O2 (aq) will decompose according to the following reaction: 2H2O2(aq)2H2O(l)+O2(g) The following data were collected for the concentration of H2O2 at various times. Times(s) [H2O2](mol/L) 0 1.000 2.16 104 0.500 4.32 104 0.250 a. Calculate the average rate of decomposition of H2O2 between 0 and 2.16 104 s. Use this rate to calculate the average rate of production of O2(g) over the same time period. b. What are these rates for the time period 2.16 104 s to 4.32 104 s?
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