When the rate for the reaction2 NO + O22 NO2was studied, the rate was found to double when the O, concentration was doubled whilethe NO concentration was unchanged. It was also found that the rate quadruples whenthe NO concentration is doubled while the Oz concentration is unchanged.a. What is the rate law expression for this reaction? Place this answer clearly labeledwithin the answer box in the quiz.Two mechanisms were proposed for this reaction as shown below.PROPOSAL IStep 1:NO + O2NO3(fast)Step 2:NO + NO:NO, + NO: (slow, RDS)PROPOSAL IIStep 1Step 2Step 3NO + NONO2O2 +N204NO2(slow, RDS)(fast)NO2 (fast)N20,NO2 +b. Write a predicted rate law for each proposed mechanism. In your predicted rate law,make sure no intermediates are present in the overall expression. Show your work or nocredit will be awarded. Show your answer for this question on the scratch paper clearlylabeled.c. Which proposed mechanism I or II agrees with the rate law expression that youdetermined above? You must also explain your reasoning or no credit will be qiven. Placeyour answer on the scratch paper clearly labeled.

The given equation for which the rate law to be determined is: 2NO + O2 -----> 2NO2

When the rate for the reaction 2 NO + 02 2 NO2 was studied, the rate was found to double when the O, concentration was doubled while the NO concentration was unchanged. It was also found that the rate quadruples when the NO concentration is doubled while the Oz concentration is unchanged. a. What is the rate law expression for this reaction? Place this answer clearly labeled within the answer box in the quiz. Two mechanisms were proposed for this reaction as shown below. PROPOSAL I Step 1: NO + O2 NO, (fast) Step 2: NO + NO: NO2 + NO, (slow, RDS) PROPOSAL II Step 1 Step 2 Step 3 NO + NO Oz + NO2 NO, NO2 N0. NO2 + NO2 (fast) (slow, RDS) (fast) b. Write a predicted rate law for each proposed mechanism. In your predicted rate law, make sure no intermediates are present in the overall expression. Show your work or no credit will be awarded. Show your answer for this question on the scratch paper clearly labeled. c. Which proposed mechanism I or II agrees with the rate law expression that you determined above? You must also explain your reasoning or no credit will be given. Place your answer on the scratch paper clearly labeled.

When the rate for the reaction 2 NO + 02 2 NO2 was studied, the rate was found to double when the O, concentration was doubled while the NO concentration was unchanged. It was also found that the rate quadruples when the NO concentration is doubled while the Oz concentration is unchanged. a. What is the rate law expression for this reaction? Place this answer clearly labeled within the answer box in the quiz. Two mechanisms were proposed for this reaction as shown below. PROPOSAL I Step 1: NO + O2 NO, (fast) Step 2: NO + NO: NO2 + NO, (slow, RDS) PROPOSAL II Step 1 Step 2 Step 3 NO + NO Oz + NO2 NO, NO2 N0. NO2 + NO2 (fast) (slow, RDS) (fast) b. Write a predicted rate law for each proposed mechanism. In your predicted rate law, make sure no intermediates are present in the overall expression. Show your work or no credit will be awarded. Show your answer for this question on the scratch paper clearly labeled. c. Which proposed mechanism I or II agrees with the rate law expression that you determined above? You must also explain your reasoning or no credit will be given. Place your answer on the scratch paper clearly labeled.

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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4. The reaction 2NO (g) + 2H2 (g) - N2 (g) + 2H2O (g) is found experimentally to be second order in NO (g) and first-order in H2 (g). a. Write the rate law for the reaction. b. What is the overall order of the reaction? c. What are the units for the rate constant k? d. If [NO] is doubled (while keeping [H2] constant), by what factor will the reaction rate increase? e. If [H2] is doubled (while keeping [NO] constant), by what factor will the reaction rate increase?
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Based on the provide elementary steps below, determine the net reaction. NO,CI (g) – NO2 (g) + CI (g) Elementary Step 1 NO,CI (g) + CI (g) > NO2 (g) + Cl2 (g) Elementary Step 2 O 2 NO2CI (g) 2 NO2 (g) + Cl2 (g) O 2 NO2CI (g) 2 NO2 (g) 2 NO2CI (g) + CI (g) 2 NO2 (g) + Cl2 (g) + CI (g) O NO2CI (g) + CI (g) - NO2 (g) + Cl2 (g) + CI (g)
Some measurements of the initial rate of a certain reaction are given in the table below. Use this information to write a rate law for this reaction, and calculate the value of the rate constant k. Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol.
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16. The reaction between A and B is as follows: * A + 2B → 2C The rate of reaction with variation of concentration of A and B at the same temperature is shown in Table 2. Table 2 Rate of reaction /mol dm³s' 1.20 × 10² 9.00 × 103 1.35 × 102 Experiment [A]/mol dm³³ | [B]/mol dm³³ I 1.00 2.00 II 1.00 1.50 III 1.50 1.00 IV 2.00 0.50 What is the value of x ? A. 3.00 × 103 В. 6.00 х 103 C. 1.20 × 10² D. 2.40 × 102
EXAMPLE 1: Use this mechanism, to derive an expression for the rate law. Express the rate constant in terms of k1, k–1, k2, and k3 (not all of these terms will necessarily appear in the expression for the rate constant). The rate law should only include concentrations of the reactants involved in the overall reaction – intermediates should not appear.
3. The following reaction: CH;CH2B + H2O CH;CH2OH + HBr is first order with respect to CH;CH,Br and first order with respect to H,0. The initial concentration of both reactants is 0.100 M. a. What is the overall rate equation for the reaction? b. What is the value and units for the rate constant, k, if the rate of the reaction is 2.50 M/s?
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3 Explain why the following mechanism is not plausible for this reaction. NO(g) + Cl2 → ← NOCl(g) + Cl fast NO(g) + Cl(g) → NOCl(g) slow experiment rate law: Rate = k[NO]2[Cl2]. Select one: a. the experiment rate law is incorrect b. does not match the experiment rate law c. it match the experiment rate law d. sufficient data is needed to answer the problem