TIA A chemistry graduate student is studying the rate of this reaction:2H₂PO4 (aq) → P₂O, (aq) + 3H₂O (aq)He fills a reaction vessel with H₂PO4 and measures its concentration as the reaction proceeds:time(seconds)00.100.30[H₂PO4]0.400.900M0.20 0.225M0.450M0.113 M0.0564MUse 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 besure your answer has the correct unit symbol.rate = kk = 0x10XŚ?

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A chemistry graduate student is studying the rate of this reaction: 2H₂PO4 (aq) → P₂O5, (aq) + 3H₂O (aq) He fills a reaction vessel with H₂PO4 and measures its concentration as the reaction proceeds: time (seconds) 0 0.10 [H₂PO4] 0.900M 0.40 0.450M 0.20 0.225M 0.30 0.113M 0.0564M 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 0 x10 ロ・ロ X 2 5 S

A chemistry graduate student is studying the rate of this reaction: 2H₂PO4 (aq) → P₂O5, (aq) + 3H₂O (aq) He fills a reaction vessel with H₂PO4 and measures its concentration as the reaction proceeds: time (seconds) 0 0.10 [H₂PO4] 0.900M 0.40 0.450M 0.20 0.225M 0.30 0.113M 0.0564M 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 0 x10 ロ・ロ X 2 5 S

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

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 100AE: Consider a hypothetical reaction between A and B: A + B products Use the following initial rate...

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The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table were collected. (a) Determine the order of the reaction for each reactant. (b) Write the rate equation for the reaction. (c) Calculate the rate constant for the reaction. (d) Find the rate of appearance of N2 at the instant when [NO] = 0.350 mol/L and [H] = 0.205 mol/L.
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
Give at least two physical properties that might be used to determine the rate of a reaction.
Nitrosyl bromide, NOBr, is formed from NO and Br2: 2 NO(g) + Br2(g) 2 NOBr(g) Experiments show that this reaction is second-order in NO and first-order in Br2. (a) Write the rate equation for the reaction. (b) How does the initial reaction rate change if the concentration of Br2 is changed from 0.0022 mol/L to 0.0066 mol/L? (c) What is the change in the initial rate if the concentration of NO is changed from 0.0024 mol/L to 0.0012 mol/L?
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.
You are running the reaction 2A+BC+3D. Your lab partner has conducted the first two experiments to determine the rate law for the reaction by the method of initial rates. Experiment Number Concentration of A (M) Concentration of B(M) 1 0.0250 0.0330 2 0.0500 0.0330 3 Presuming that you can measure the initial rate of each experiment, which of the following concentrations for Experiment 3 would help you determine the rate law easily? a [A] = 0.0330 M, [B] = 0.0330 M b [A] = 0.0125 M, [B] = 0.0500 M c [A] = 0.0250 M, [B] = 0.0400 M d [A] = 0.0250 M, [B] = 0.0330 M e [A] = 0.0500 M, [B] = 0.0330 M
Ozone, O3, in the Earths upper atmosphere decomposes according to the equation 2 O3(g) 3 O2(g) The mechanism of the reaction is thought to proceed through an initial fast, reversible step followed by a slow, second step. Step 1: Fast, reversible O3(g) O2(g) + O(g) Step 2: Slow O3(g) + O(g) 2 O2(g) (a) Which of the steps is rate-determining? (b) Write the rate equation for the rate-determining step
The reaction of water with CH3Cl in acetone as a solvent is represented by the equation CH3Cl+H2OCH3OH+HCl The rate of the reaction doubles when the concentration of CH3Cl is doubled and it quadruples when the concentration of H2O is doubled. a What is the unit for k? b Calculate k if CH3OH is formed at a rate of 1.50 M/s when [CH3Cl] = [H2O] = 0.40 M.
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.
Kinetics II You and a friend are working together in order to obtain as much kinetic information as possible about the reaction A(g)B(g)+C(g). One thing you know before performing the experiments is that the reaction is zero order, first order, or second order with respect to A. Your friend goes off, runs the experiment, and brings back the following graph. a After studying the curve of the graph, she declares that the reaction is second order, with a corresponding rate law of Rate = k[A]2. Judging solely on the basis of the information presented in this plot, is she correct in her statement that the reaction must be second order? Here are some data collected from her experiment: Time (s) [A] 0.0 1.0 1.0 0.14 3.0 2.5 103 5.0 4.5 105 7.0 8.3 107 b The half-life of the reaction is 0.35 s. Do these data support the reaction being second order, or is it something else? Try to reach a conclusive answer without graphing the data. c What is the rate constant for the reaction? d The mechanism for this reaction is found to be a two-step process, with intermediates X and Y. The first step of the reaction is the rate-determining step. Write a possible mechanism for the reaction. e You perform additional experiments and find that the rate constant doubles in value when you increase the temperature by 10oC. Your lab partner doesnt understand why the rate constant changes in this manner. What could you say to your partner to help her understand? Feel free to use figures and pictures as part of your explanation.