Some measurements of the initial rate of a certain reaction are given in the table below. [N-] H2 initial rate of reaction 2.47M 1.44M 46.0M/s 4.71M 1.44M 167.M/s 2.47M 5.08M 572. M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k k =

Some measurements of the initial rate of a certain reaction are given in the table below. [N-] H2 initial rate of reaction 2.47M 1.44M 46.0M/s 4.71M 1.44M 167.M/s 2.47M 5.08M 572. M/s Use this information to write a rate law for this reaction, and calculate the value of the rate constant Round your value for the rate constant to 3 significant digits. Also be sure your answer has the correct unit symbol. rate = k k =

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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k represents the rate constant when writing a rate law
The following reaction has rate law r = k[C4H6] 2 , where k = 0.014 M-1 s -1 What is the concentration of C4H6 (in M) after 3.0 hours, if [C4H6]o = 0.025 M? A. 0.0052 M B. 0.024 M C. 0.012 M D. 0.0060 M
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Some measurements of the initial rate of a certain reaction are given in the table below. [N₂] [H₂] initial rate of reaction 1.84M 2.20M 28.0M/s 0.689M 2.20M 3.93 M/s 1.84M 11.0M 700. M/s 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. rate = k ☐x10 k = 0 × ? Ś
D
Ⓒ Macmillan Learning Enter these data into the graphing tool and determine the value and units of the rate constant, k, for this reaction. Graphing Tool Add Row 10 total rows [A] [A] vs. t In[A] In[A] vs. t t (min) 0.0 2.0 4.0 6.0 1/[A] vs. t [A] (M) 1.00 0.66 0.43 0.28 1/[A] Clear All Data
Question 9 Which of the following statements is false? The average rate of a reaction decreases during a reaction. It is not possible to determine the rate of a reaction from its balanced equation. The rate of zero order reactions is not dependent on concentration. The half-life of a first order reaction is dependent on the initial concentration of reactant. None of the statements are false.
g.
Consider the following reaction performed at K and the given concentration and rate data: A products Experiment [A] Rate of reaction (M) (M/s) 1 0.78 0.0026988 2 1.56 0.0053976 3 3.12 0.0107952 First determine the rate law and rate constant. Based on this information; if you set up a new experiment where the [A]. (initial concentration of A) was 1.33 M, what would the concentration of A be after 144 s? [A](M) = number (rtol=0.01, atol=1e-08) ?
The rate of a certain reaction is given by the following rate law: rate =k| N,| H2 -k[N;][H+]° Use this information to answer the questions below. What is the reaction order in N,? What is the reaction order in H2? What is overall reaction order? At a certain concentration of N, and H2, the initial rate of reaction is 0.620 M / s. What would the initial rate of the reaction be if the concentration of N, were halved? Round M S your answer to 3 significant digits. The rate of the reaction is measured to be 24.0 M / s when [N2] = 1.5 M and [H2] = 0.16 M. Calculate the value of the k = |M -2 -1 •S rate constant. Round your answer to 2 significant digits.