Using a zero order integrated rate law to find concentration changeUnder certain conditions the rate of this reaction is zero order in dinitrogen monoxide with a rate constant of 0.0087 M.s¯ 1:2N2O (g) → 2N2 (g) + O2(g)Suppose a 5.0 L flask is charged under these conditions with 150. mmol of dinitrogen monoxide. How much is left 0.9 s later? You mayassume no other reaction is important.Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.x10

The integrated rate law (concentration vs. time) equation for a zero order reaction is given by: [A]…

Answered: Using a zero order integrated rate law…

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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The reaction in aqueous acidic solution occurs as shown by the balanced chemical equation below: H2O2(aq) + 3 I (aq) + 2 H* (aq) 13 (aq) + 2 H20(I) In the first 40.0 seconds of the reaction, the concentration of I' changes from 1.000 M to 0.868 M. Use the information to determine the average rate of the reaction within the first 40.0 seconds of the reaction. O 3.20x103 M/s O 1.10x10-3 M/s O 4.40x10-3 M/s O 2.20x10-3 M/s
For the reaction:A(g) + B(g) →AB(g) the rate is 0.30 mol/L.s, when [A]0 = [B]0 = 1.0 mol/L. If the reaction is first order in B and second order in A, what is the rate when [A]0 = 1.9 mol/L and [B]0 = 4.3 mol/L?
For the reaction AB(g) —>A(g) + B(g) the rate law is determined to be rate =k[AB]^2 and k=0.255 L/mol-min. If the initial concentration of AB is 1.00M, how long will it take for the concentration of AB to fall to 0.40M?
Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0041 M's : 2 HI(g) → H2(g)+I,(g) Suppose a 4.0 L flask is charged under these conditions with 300. mmol of hydrogen iodide. After how much time is there only 150. mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. x10
Under certain conditions the rate of this reaction is zero order in dinitrogen monoxide with a rate constant of 0.0039 M²s¯¹: 2N₂O(g) 2 N₂(g) + O₂(g) Suppose a 4.0 L flask is charged under these conditions with 400. mmol of dinitrogen monoxide. How much is left 6.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. 0 00 X 3
Using a zero order integrated rate law to find concentration change -1 Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0068 M.s¹: 2 NH3 (g) → N₂ (g) +3 H₂ H2(g) Suppose a 300. mL flask is charged under these conditions with 450. mmol of ammonia. How much is left 60. s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. M ☐ x10 ك ? 000 18 Ar New Chrome available :
Under certain conditions the rate of this reaction is zero order in dinitrogen monoxide with a rate constant of 0.0037 M's : 2 N,0(g) 2 N2(g)+O,(g) Suppose a 5.0L flask is charged under these conditions with 400. mmol of dinitrogen monoxide. After how much time is there only 200. mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits.
The exponents in a rate law describe the effects of the reactant concentrations on the reaction rate and define the reaction order. Consider a reaction for which the rate law is: rate = k[A]m[B]n If m is 1, the reaction is first order with respect to A. If the exponent is 2, the reaction is second order with respect to A. If n is 1, the reaction is first order in B. If m or n is zero, the reaction is zero order in A or B. If m = 1 and n = 1, the overall order of the reaction is second. (m + n = 1 + 1 = 2). 1. What is the difference between a reaction rate and a reaction's rate constant? 2. What does it mean if a reaction is zero order with respect to a reactant? 3. Doubling the concentration of a reactant increases the rate of a reaction four times. What is the order of the reaction with respect to that reactant? 4. Doubling the concentration of a reactant increases the rate of a reaction four times. Tripling the concentration of a different reactant increases the rate of a reaction…
The rate of a certain reaction is given by the following rate law: =k[N₂]²[H₂]² Use this information to answer the questions below. rate What is the reaction order in N₂? What is the reaction order in H₂? What is overall reaction order? At a certain concentration of N₂ and H₂, the initial rate of reaction is 71.0 M/s. What would the initial rate of the reaction be if the concentration of N₂ were halved? Be sure your answer has the correct number of significant digits. The rate of the reaction is measured to be 0.930 M/s when [N₂] = 0.79 M and [H₂] = 0.88 M. Calculate the value of the rate constant. Be sure your answer has the correct number of significant digits. M 04/1 S -3 1 k = M ²³.5²¹ S
- 1 Under certain conditions the rate of this reaction is zero order in ammonia with a rate constant of 0.0080 M's : 2 NH3 (g) → N, (g)+3 H, (g) Suppose a 5.0 L flask is charged under these conditions with 300. mmol of ammonia. How much is left 2.0 s later? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits. x10 ?
23. Consider the following reaction: 2 NO2(g) + O3(g) N2O5(g) + O2(g) (a) The rate law for this reaction is first order in NO2(g) and first order in O3(g). What is the rate law for this reaction? Rate = k [NO2(g)] [O3(g)] Rate = k [NO2(g)]2 [O3(g)] Rate = k [NO2(g)] [O3(g)]2 Rate = k [NO2(g)]2 [O3(g)]2 Rate = k [NO2(g)] [O3(g)]3 Rate = k [NO2(g)]4 [O3(g)] (b) If the rate constant for this reaction at a certain temperature is 62500, what is the reaction rate when [NO2(g)] = 0.530 M and [O3(g)] = 1.08 M?Rate =_____ M/s.(c) What is the reaction rate when the concentration of NO2(g) is doubled, to 1.06 M while the concentration of O3(g) is 1.08 M?Rate =____ M/s
- 1 Under certain conditions the rate of this reaction is zero order in dinitrogen monoxide with a rate constant of 0.0056 M's : 2 N,0 (g) → 2 N, (g) + O2 (g) Suppose a 400. mL flask is charged under these conditions with 500. mmol of dinitrogen monoxide. After how much time is there only 250. mmol left? You may assume no other reaction is important. Be sure your answer has a unit symbol, if necessary, and round it to the correct number of significant digits. |x10

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