Consider the following reaction: CHCl3 (g) + Cl₂ (g) → CCL (g) + HCl(g) The initial rate of the reaction is measured at several different concentrations of the reactants with the following results: [CHC13] (M) [Cl₂] (M) Initial Rate (M/s) 0.010 0.010 0.0033 0.0066 0.0093 0.026 0.020 0.020 0.040 0.010 0.020 0.040 Submit Part B ✓ Correct Fractional-order reactions are not common but are occasionally observed. T show that the rate doubles when the concentration of CHCl3 is doubled, sm respect to CHCl3. However, comparing the second and third experiments of Cl2 is doubled, the rate increases by an approximate factor of 1.5. There respect to Cl₂ is fractional. From the data, determine the rate constant (k) for the reaction. Expres your answer using two significant figures. 5 ΑΣΦ k = Previous Answers Submit Provide Feedback Request Answer P Pearson ? Re M-1/2.s-1 Copyright © 2023 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissi

Consider the following reaction: CHCl3 (g) + Cl₂ (g) → CCL (g) + HCl(g) The initial rate of the reaction is measured at several different concentrations of the reactants with the following results: [CHC13] (M) [Cl₂] (M) Initial Rate (M/s) 0.010 0.010 0.0033 0.0066 0.0093 0.026 0.020 0.020 0.040 0.010 0.020 0.040 Submit Part B ✓ Correct Fractional-order reactions are not common but are occasionally observed. T show that the rate doubles when the concentration of CHCl3 is doubled, sm respect to CHCl3. However, comparing the second and third experiments of Cl2 is doubled, the rate increases by an approximate factor of 1.5. There respect to Cl₂ is fractional. From the data, determine the rate constant (k) for the reaction. Expres your answer using two significant figures. 5 ΑΣΦ k = Previous Answers Submit Provide Feedback Request Answer P Pearson ? Re M-1/2.s-1 Copyright © 2023 Pearson Education Inc. All rights reserved. | Terms of Use | Privacy Policy | Permissi

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...

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Given the reaction mechanism, write the overall reaction. Identify reaction intermediate(s) and catalyst(s). 2NO2 (g) à NO3 (g) + NO (g) (slow) ∆H = +kJ NO3(g) + CO(g) à NO2(g) + CO2(g) (fast) ∆H = - kJ ΔHtot = -100kJ Reaction Intermediate(s): List 4 ways that the reaction rate could be increased. 1. 2. 3. 4.
A chemistry graduate student is studying the rate of this reaction: 2SO3 (g) → 2SO₂(g) + 0₂ (8) She fills a reaction vessel with SO3 and measures its concentration as the reaction proceeds: time (seconds) [SO3] 0 0.0100M 10. 0.00385M 20. 0.00238M 30. 0.00172M 40. 0.00135M 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 2 200 Ar
26. Hydrogen reacts with nitrogen monoxide to form dinitrogen monoxide (laughing gas) according to the equation: H2(g)+2NO(g)⟶N2O(g)+H2O(g) Determine the rate law, the rate constant, and the orders with respect to each reactant from the following data: [NO] (M) 0.30 0.60 0.60 [H2] (M) 0.35 0.35 0.70 Rate (mol L−1 s−1) 2.835 × 10−3 1.134 × 10−2 2.268 × 10−2
State whether the followingis true or false. If true , explain your reason. if false, explain your reason and provide a correct statement. a) The rate of consumption of reactants and the rate of formation of products is always equal to the rate of reaction (True or false) b) In a reaction A + B ---> P, if the reaction is present in a much higher concentration than reactant A, you can determine the order of reaction with respect to B (True or false) c) In any chemicalreaction A + B ---> C, the concentration of A and B affect the rate of formation of C (True or false)
Consider the following reaction mechanism: Step 1: 2NO (g) + 1.50,(g) --> N,Og(s) Step 2: 2NO,(g) --> 2NO(g) + O2 (g) Write the overall reaction and identify any reaction intermediates.
For the reactionNO2 (g)+CO(g)NO(g)+CO2(g)calculate the order of the reaction with respect to the following reactants according to the following experimental data: Experiment [NO2]0(M) [CO]0(M) Initial Rate, –ΔΔ[NO2]/ΔΔt (M/s) 1 0.263 0.826 1.44 × 10–5 2 0.263 0.413 1.44 × 10–5 3 0.526 0.413 5.76 × 10–5 See Periodic Table Order of the reaction with respect to NO2: Order of the reaction with respect to CO:
The reaction H2 (g) + 2 NO (g) + H,O (g) is studied at a certain temperature by determining the rate of reaction at reactant concentrations. The results are as follows: N,0 (g) 2. Concentration (M) Rate [NO] (i) (ii) [H] (M/s) 0.25 0.10 0.126 0.50 0.10 0.504 (iii) 0.50 0.20 1.03 The rate law is written as Rate = k [NO]* [H]°. The exponents x and y represent the order with respect to NO and H2, respectively. Calculate the value of x and y from the data provided.
Consider the following general reaction for which gases A and B are mixed in a constant volume container: A(g) + B(g) -> C(g) + D(g) Match what happens to the rate of the reaction under the following changes: (consider each change separately) v all of gas B is removed from the container more gas A is added to the container the temperature of the container is increased there is no change to the reaction rate ya catalyst is added to the container I. the reaction proceeds at a faster rate v gas D is also added to the container the reaction proceeds at a slower rate II. some of gas B is removed from the container Iy the reaction does not proceed at all the volume of the container is increased
The reaction 2NO(g) + Cl2 (g) -----> 2NOCl (g) was studied at –10°C. The following results were obtained where Rate = - Delta [Cl2]/ delta t [NO]0 [Cl2]0 Initial Rate (mol/L) (mol/L) (mol/L·min) 0.11 0.11 0.24 0.11 0.22 0.48 0.22 0.22 1.92 a Question Content Area What is the rate law? ( Use k for the rate constant. ) Rate =
3. The following mechanism is proposed for the reaction of chlorine with chloroform: Cl, + CHCI, CCI, + HCI Cl, Step 1 fast equilibrium 2Cl CHCI, +CI » HCI +CCI, CCI, +Cl»cCI, Step 2 slow Step 3 fast a) Show that this mechanism gives the correct, overall balanced reaction equation. b) Write the rate law predicted by this mechanism.
The following mechanism has been proposed for the atmospheric decomposition of nitric oxide (NO). Step 1: 2 NO (g)  N2O Step 2: 2 (g)N2O2 (g) + H2 (g)  N2O(g) + H2O(g) Step : N2O(g) + H2 (g)  N2 (g) + H2O(g) Identify any intermediates in this reaction mechanism. Write the overall chemical reaction. Sketch the energy diagram for Step 1. E = - 4 kJ/mole. Include axes with labels. Label the reactants, product, and transition state on the energy diagram. Write the differential rate law for Step 1
Consider the reaction: A + B --> products. From the following data obtained at a certain temperature, determine the order of the reaction (rate law) and calculate the rate constant: [A] (M) [B] (M) Rate (M/s) 1.50 1.50 3.15 X 10-1 1.50 2.50 2.98 X 10 –1 3.00 1.50 5.50 X 10-1