O KINETICS AND EQUILIBRIUMDeducing a rate law from the change in concentration over timeA chemistry graduate student is studying the rate of this reaction:H,CO, (aq)- H,0 (aq)+CO, (aq)He fills a reaction vessel with H,CO, and measures its concentration as the reaction proceeds:time[H,CO,](seconds)1.00 M0.100.527 M0.200.278 M0.300.146 M0.400.0771 MUse this data to answer the following questions.ato - H CO TVArite therate l for thir ronctinExplanationCheck U.146 M0.400.0771 MUse this data to answer the following questions.Write the rate law for this reaction.rate = * [H,Co,TCalculate the value of the rate constant k.k = 0Round your answer to 2 significant digits. Also besure your answer has the correct unit symbol.ExplanationCheckO 2021 McGraw-Hill EducCation, Ali RType here to searchChp

Rate law for the reaction is rate = K[H2CO3], Where K is rate constant

A chemistry graduate student is studying the rate of this reaction: H,CO, (aq) → H,0 (aq)+CO, (aq) He fills a reaction vessel with H,CO, and measures its concentration as the reaction proceeds: [H,CO,] time (seconds) 1.00 M 0.10 0.527 M 0.20 0.278 M 0.30 0.146 M 0.40 0.0771 M Use this data to answer the following questions.

A chemistry graduate student is studying the rate of this reaction: H,CO, (aq) → H,0 (aq)+CO, (aq) He fills a reaction vessel with H,CO, and measures its concentration as the reaction proceeds: [H,CO,] time (seconds) 1.00 M 0.10 0.527 M 0.20 0.278 M 0.30 0.146 M 0.40 0.0771 M Use this data to answer the following questions.

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter8: Reaction Rates And Equilibrium

Section: Chapter Questions

Problem 8.64E

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Consider the following statements: In general, the rate of a chemical reaction increases a bit at first because it takes a while for the reaction to get warmed up. After that, however, the rate of the reaction decreases because its rate is dependent on the concentrations of the reactants, and these are decreasing. Indicate everything that is correct in these statements, and indicate everything that is incorrect. Correct the incorrect statements and explain.
If a textbook defined a catalyst as "a substance that increases the rate of a reaction," would that definition be adequate?
The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in automobile engines. Suppose that a series of experiments measured the rate of this reaction at 500 K and produced the following data; [NO] (mol L ’) [OJ (mol L 1) Rate = -A[NO]/Af (mol L_1 s-1) 0.002 0.005 8.0 X 10"'7 0.002 0.010 1.6 X 10-'6 0.006 0.005 2.4 X IO-'6 Derive a rate law for the reaction and determine the value of the rate constant.
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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?
A friend of yours states, A balanced equation tells us how chemicals interact. Therefore, we can determine the rate law directly from the balanced equations. What do you tell your friend?
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.
. Account for the increase in reaction rate brought about by a catalyst.
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.
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.
Consider a hypothetical reaction between A and B: A + B products Use the following initial rate data to calculate the rate constant for this reaction. [A] (mol/L) [B] (mol/L) Initial Rate (mol/L s) 0.20 1.0 3.0 0.50 1.0 11.8 2.0 2.0 189.5
Consider the following hypothetical data collected in two studies of the reaction 2A+2BC+2D Time(s) Experiment 1 [A] (mol/L) Experiment 2 [A] (mol/L) 0 1.0 102 1.0 102 10. 8.4 103 5.0 103 20. 7.1 103 2.5 103 30. ? 1.3 103 40. 5.0 103 6.3 104 In Experiment 1, [B]0 = 10.0 M. In Experiment 2, [B]0 = 20.0 M. Rate=[A]t a. Use the concentration versus time data to determine the rate law for the reaction. b. Solve for the value of the rate constant (k) for the reaction. Include units. c. Calculate the concentration of A in Experiment 1 at t =30.s