25. If increasing the concentration of either reactant increases the overall rate of reaction, which is the most likely rate law for the reaction shown below? CH₂CH₂Br(aq) + OH-(aq) → CH3CH₂OH(aq) + Br(aq) A) Rate = k[CH₂CH₂Br] [OH-] B) Rate = k[CH3CH₂Br][ OH-]0 C) Rate = k[CH3CH₂Br][OH-] D) Rate = K[CH3CH₂OH] [Br] E) Rate k[CH3CH₂OH][Br] =
25. If increasing the concentration of either reactant increases the overall rate of reaction, which is the most likely rate law for the reaction shown below? CH₂CH₂Br(aq) + OH-(aq) → CH3CH₂OH(aq) + Br(aq) A) Rate = k[CH₂CH₂Br] [OH-] B) Rate = k[CH3CH₂Br][ OH-]0 C) Rate = k[CH3CH₂Br][OH-] D) Rate = K[CH3CH₂OH] [Br] E) Rate k[CH3CH₂OH][Br] =
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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![### Chemistry Multiple-Choice Questions
#### Question 25
**If increasing the concentration of either reactant increases the overall rate of reaction, which is the most likely rate law for the reaction shown below?**
\[ \text{CH}_{3}\text{CH}_{2}\text{Br}(\text{aq}) + \text{OH}^- (\text{aq}) \rightarrow \text{CH}_{3}\text{CH}_{2}\text{OH} (\text{aq}) + \text{Br}^- (\text{aq}) \]
A) Rate = \( k[\text{CH}_{3}\text{CH}_{2}\text{Br}][\text{OH}^-]\)
B) Rate = \( k[\text{CH}_{3}\text{CH}_{2}\text{Br}]^2 [\text{OH}^-]\)
C) Rate = \( k[\text{CH}_{3}\text{Br}][\text{OH}^-]^2\)
D) Rate = \( k[\text{CH}_{3}\text{CH}_{2}\text{OH}] [\text{Br}^-]\)
### Question 26
**Why can the initial rate of reaction (the rate of the reaction during the time when the reaction first takes place) be used to determine the rate law of a reaction?**
A) At the beginning of the reaction, the reactants are at their highest concentration and monitoring the rate of the reaction when initial concentrations are changed provides information about how each reactant impacts the rate.
B) At the beginning of the reaction, the reaction is at its slowest point, and therefore this provides information about how the reactants are interacting with each other in the reaction.
C) At the beginning of the reaction, the reactants behave as catalysts and can lower the activation energy of the reaction.
D) All of the above.
E) A, B, and C are correct.
#### Question 28
**The decomposition of hydrogen peroxide is shown below. If the first order time-integrated rate constant for this reaction is 3.21 x 10^5 sec^-1, how long will it take for half of the initial hydrogen peroxide to decompose?**
\[ 2\text{H}_2\text{O}_2(l) \rightarrow 2\text{H}_2\text{O}(l) + \text{O}_](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F356d713b-7c6e-40b6-9a77-3224c6f78ffd%2Fd8e85d84-62f5-48c0-bcc8-534599642978%2Fy2be318_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Chemistry Multiple-Choice Questions
#### Question 25
**If increasing the concentration of either reactant increases the overall rate of reaction, which is the most likely rate law for the reaction shown below?**
\[ \text{CH}_{3}\text{CH}_{2}\text{Br}(\text{aq}) + \text{OH}^- (\text{aq}) \rightarrow \text{CH}_{3}\text{CH}_{2}\text{OH} (\text{aq}) + \text{Br}^- (\text{aq}) \]
A) Rate = \( k[\text{CH}_{3}\text{CH}_{2}\text{Br}][\text{OH}^-]\)
B) Rate = \( k[\text{CH}_{3}\text{CH}_{2}\text{Br}]^2 [\text{OH}^-]\)
C) Rate = \( k[\text{CH}_{3}\text{Br}][\text{OH}^-]^2\)
D) Rate = \( k[\text{CH}_{3}\text{CH}_{2}\text{OH}] [\text{Br}^-]\)
### Question 26
**Why can the initial rate of reaction (the rate of the reaction during the time when the reaction first takes place) be used to determine the rate law of a reaction?**
A) At the beginning of the reaction, the reactants are at their highest concentration and monitoring the rate of the reaction when initial concentrations are changed provides information about how each reactant impacts the rate.
B) At the beginning of the reaction, the reaction is at its slowest point, and therefore this provides information about how the reactants are interacting with each other in the reaction.
C) At the beginning of the reaction, the reactants behave as catalysts and can lower the activation energy of the reaction.
D) All of the above.
E) A, B, and C are correct.
#### Question 28
**The decomposition of hydrogen peroxide is shown below. If the first order time-integrated rate constant for this reaction is 3.21 x 10^5 sec^-1, how long will it take for half of the initial hydrogen peroxide to decompose?**
\[ 2\text{H}_2\text{O}_2(l) \rightarrow 2\text{H}_2\text{O}(l) + \text{O}_
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