For the reaction: 2N2O5(g) -->4NO(g) + O2(g)(a) write the mathematical rate expression in terms of(1) the disappearance of N½O5 (Reactant);(ii) the formation of NO (Product);(ii) the formation of O2 (Product).(b) What are the stoichiometric relationships (rationalization) of the various rates for this reaction? (e.g. Product C formation is 2x faster than Reactant Adisappearance/decomposition.)

Answered: Image /qna-images/answer/6629580a-aea9-4133-b979-2b83921fce9e.jpg

Answered: For the reaction: 2N½O5(g) -->4NO(g) +…

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...

See similar textbooks

Similar questions

The reaction of nitric oxide with hydrogen at 1280oC is 2NO(g) + 2H2(g) -- N2(g) + 2H2O(g) From the following data collected at this temperature, determine (a) the rate law, (b) the rate constant, and (c) the rate of the reaction when [NO] = 12.0 x 10-3 M and [H2] = 6.0 x 10-3 M. Experiment [NO] (M) [H2] (M) Initial Rate (M/s) 1 5.0 x 10-3 2.0 x 10-3 1.3 x 10-5 2 10.0 x 10-3 2.0 x 10-3 5.0 x 10-5 3 10.0 x 10-3 4.0 x 10-3 10.0 x 10-5
Consider the following reaction: 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) (a) The rate law for this reaction is second order in NO(g) and first-order in H2(g). What is the rate law for this reaction? (b) If the rate constant for this reaction at a certain temperature is 9.70e+04, what is the reaction rate when [NO(g)] = 0.0560 M and [H2(g)] = 0.119 M?Rate = M/s.(c) What is the reaction rate when the concentration of NO(g) is doubled, to 0.112 M while the concentration of H2(g) is 0.119 M?Rate = M/s
Suppose the formation of nitrosyl chloride proceeds by the following mechanism: step elementary reaction rate constant NO(g) + Cl2(g) NOCI2(g) k1 1 2 |NOCI2(g) + N0(g) → 2 NOC1(g) k2 Suppose also k,»k,. That is, the first step is much faster than the second. Write the balanced chemical equation for the overall chemical reaction: Write the ? experimentally- observable rate law for the overall chemical reaction. rate = k | Note: your answer should not contain the concentrations of any intermediates. Express the rate constant k for the overall chemical reaction in terms of k1, k2, and (if necessary) the rate constants k-1 and k = 0 k-2 for the reverse of the two elementary reactions in the mechanism. Dlo X
15.For the reaction, 2H,S(g) + 0,(g) 2S(s) + 2H,0(1), which one of the following statements is absolutely true? (a) The reaction is first order with respect to H,S and second order with respect to O (b) The reaction is fourth order overall. (c) The rate law is: rate = k[H,S][0,]. %3D (d) The rate law is: rate = k[H,S][O,]. %3D (e) The rate law cannot be determined from the information given.
The isomerization reaction CH3NC → CH3CN obeys the first-order rate law, rate = k[CH3NC], in the presence of an excess of argon. Measurement at 500. K reveals that in 485 seconds, the concentration of CH3NC has decreased to 73% of its original value. Calculate the rate constant (k) of the reaction at 500. K. s−1 (The integrated form for the first-order rate law can be written in the general terms ln[A]t − ln[A]0 = −kt, where [A]0 is the initial concentration of reactant A, [A]t is the concentration of A at time t, and k is the rate constant.)
1. The initial rate of the reaction A + B C + D is determined for different initial conditions, with the results listed in the table. (a) What is the order of reaction with respect to A and to B? (b) What is the overall reaction order? (c) What is the value of the rate constant, K? Expt [A], M [B], M Initial Rate, M s-1 3.35 x 104 1 0.185 0.133 2 0.185 0.266 1.35 x 10-3 3 0.370 0.133 6.75 x 107 4 0.370 0.266 2.70 × 10-³
(4) Use the following experimental data to write the rate law and the rate constant for the reaction 2 NO (g) + O2 (g) = 2 NO2 (g) Experiment [NO] (M) [O2] (M) Initial rate (M/s) 1 0.0100 0.0100 0.711 x 10-2 2 0.0100 0.0400 2.84 x 10-2 3 0.0200 0.0100 2.84 x 10-2
The reaction O₂(g) + 2 NO(g) → 2 NO₂(g) was studied at a certain temperature with the following results: (a) What is the rate law for this reaction? O Ratek [0₂(9)] [NO(g)] O Ratek [0₂(9)]² [NO(g)] O Rate = k [0₂(9)] [NO(g)]² O Ratek [0₂(9)]² [NO(g)]² O Ratek [0₂(9)] [NO(g)]³ O Rate = k [O₂(g)]* [NO(g)] (b) What is the value of the rate constant? Experiment [0₂(9)] (M) 0.0235 0.0235 0.0470 0.0470 [NO(g)] (M) 0.0235 0.0470 0.0235 0.0470 Rate (M/S) 0.158 0.633 0.317 1.27 (c) What is the reaction rate when the concentration of O₂(g) is 0.0318 M and that of NO(g) is 0.0649 M if the temperature is the same as that used to obtain the data shown above?
The half-life for the above reaction is 9 hours. Using 12 mol of AB3, calculate the moles of B2 formed and its volume under normal conditions (half-life is independent of the amount of the starting substance.
2. The reaction of peroxydisulfate ion (S₂O) with iodide ion (I) is |S₂O²¯(aq) + 31¯(aq) →→→ 2SO¾¯(aq) + Iz (aq) From the following data collected at a certain temperature, determine the (a) rate law, (b) overall order of the reaction and (c) calculate the rate constant (Show your complete solution and use the data from Experiment I) Experiment [S₂0²¯] (M) [I] (M) Initial Rate (M/s) 1 0.080 0.034 2.2 × 10-4 2 0.080 0.017 1.1 x 10-4 3 0.16 0.017 2.2 x 10-4 Answers: b). overall order of the reaction: second-order Note: answer for letter a will be provided by the student. c.) 8.1 x 102 /M.s
(i) What is the order of the reaction whose rate constant has same units as the rate of reaction?(ii) For a reaction A + H2O → B; Rate ∝ [A],What is the order of this reaction?
The enzyme urease catalyzes the reaction of urea, 1NH2CONH22, with water to produce carbon dioxide and ammonia. In water, without the enzyme, the reaction proceeds with a first-order rate constant of 4.15 * 10-5 s-1 at 100 °C. In the presence of the enzyme in water, the reaction proceeds with a rate constant of 3.4 * 104 s-1 at 21 °C. (a) Write out the balanced equation for the reaction catalyzed by urease.

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS