Using a zero order integrated rate law to find concentration change-1Under 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 H₂H2(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 noother reaction is important.Be sure your answer has a unit symbol, if necessary, and round it to 2 significant digits.M☐ x10ك?00018ArNew Chrome available :

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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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Under certain conditions the rate of this reaction is zero order in dinitrogen monoxide with a rate constant of 0.0028 M.s¯¹: 2N₂O(g) 2N2(g) + O2(g) Suppose a 350. mL 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 2 significant digits. X ☐ x10
: Nitrosyl chloride, NOCI, decomposes to NO and Cl2. 2NOCI(g) → 2NO(g) + Cl2(g) Determine the rate equation, the rate constant, and the overall order for this reaction from the following data: [NOCI] (M) 0.10 0.30 0.20 Rate (mol/L/h) 8.0 x 10-10 3.2 x 10-9 7.2 x 10-9
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
13.102 Chlorine oxide (CIO), which plays an important role in the depletion of ozone (see Problem 13.101), decays rapidly at room temperature according to the equation 2C10(g) Cl₂(g) + O₂(g) From the following data, determine the reaction order and calculate the rate constant of the reaction. Time (s) 0.12 x 10-³ 0.96 x 10-³ 2.24 x 10-³ 3.20 x 10-³ 4.00 x 10-³ [CIO] (M) 8.49 x 10-6 7.10 x 10-6 5.79 x 10-6 5.20 x 10-6 4.77 x 10-6
A chemistry graduate student is studying the rate of this reaction: 2C1₂O5 (g) → 2Cl₂ (g) +50₂ (g) He fills a reaction vessel with C1₂05 and measures its concentration as the reaction proceeds: time (seconds) 0 0.10 [C₁₂05] 0.600M 0.215M 0.20 00. 0.131M 0.30 0.0941 M 0.40 0.0734M 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 X Ś
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.
In a study to determine the rate of the following reaction: 2NO(g) +0,(g) 2NO, (g) the concentration of NO was 0.0650 Mat t= 5.0 s and 0.0225 Mat t= 650.0 s. What is the average rate of the reaction during this time period? M/s
You have a reaction: A + B --> C The reaction is first order with respect to A and 2nd order with respect to B. If 1.3 mol of A is mixed with 2.3 mol of B to make a 1.000 L solution and the rate of the reaction is 1.6 M/s, what is the rate constant (k)?
4 At a certain temperature the rate of this reaction is first order in CICH₂CH₂Cl with a rate constant of 6.83 × 10 CICH₂CH₂Cl (g) → CH₂CHC1 (g) + HC1 (g) S Suppose a vessel contains CICH₂CH₂Cl at a concentration of 0.890M. Calculate the concentration of CICH₂CH₂Cl in the vessel 880. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.
2 3 4 =5 #1 6 7 Under certain conditions the rate of this reaction is zero order in hydrogen iodide with a rate constant of 0.0040 M-s¹: 2 HI (g) → H₂(g) + 1₂ (g) Suppose a 5.0 L flask is charged under these conditions with 300. mmol of hydrogen iodide. How much is left 4.0 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. S A S ? Continue Submit 00 X
Consider this reaction: 2C1₂05 (g) → 2Cl₂ (g) +50₂ (g) At a certain temperature it obeys this rate law. rate = (8.98 × 10-4 ')[c,os] -1 S Suppose a vessel contains Cl₂05 at a concentration of 1.40M. Calculate the concentration of Cl₂O5 in the vessel 690. seconds later. You may assume no other reaction is important. Round your answer to 2 significant digits.
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

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