A rate is equal to 0.0200 M/s. If [A] = 0.100M and rate = k[A]<, what is the new rate if the concentration of [A] is increased to 0.200 M?

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...
icon
Related questions
Question
100%
**Understanding Reaction Rates: Example Problem**

**Problem Statement:**
A rate is equal to 0.0200 M/s. If [A] = 0.100 M and the rate equation is given by rate = k[A]^2, what is the new rate if the concentration of [A] is increased to 0.200 M?

**Possible Answers:**
- ☐ 0.0200 M/s
- ☐ 0.100 M/s
- ☐ 0.0400 M/s
- ☐ 0.0600 M/s
- ☐ 0.0800 M/s

**Explanation:**
To solve this problem, you need to understand how the rate of a reaction changes with the concentration of a reactant. The given rate law is rate = k[A]^2, indicating that the rate of reaction is directly proportional to the square of the concentration of [A].

Given:
- Initial rate = 0.0200 M/s
- Initial concentration, [A] = 0.100 M
- Rate = k[A]^2

Firstly, determine the rate constant (k) using the provided data:
\[ 0.0200 \text{ M/s} = k \times (0.100 \text{ M})^2 \]
\[
0.0200 \text{ M/s} = k \times 0.0100 \text{ M}^2
\]
\[ 
k = \frac{0.0200 \text{ M/s}}{0.0100 \text{ M}^2} 
\]
\[ 
k = 2 \text{ M}^{-1}\text{s}^{-1} 
\]

Now, use this rate constant to find the new rate when [A] = 0.200 M:
\[ 
\text{New rate} = k \times (0.200 \text{ M})^2 
\]
\[ 
\text{New rate} = 2 \text{ M}^{-1}\text{s}^{-1} \times (0.200 \text{ M})^2 
\]
\[ 
\text{New rate} = 2 \text{ M}^{-1}\text{s}^{-1} \times 0.0400 \text{ M}^2 
\] 
\[ 
\text{New rate} = 0.080
Transcribed Image Text:**Understanding Reaction Rates: Example Problem** **Problem Statement:** A rate is equal to 0.0200 M/s. If [A] = 0.100 M and the rate equation is given by rate = k[A]^2, what is the new rate if the concentration of [A] is increased to 0.200 M? **Possible Answers:** - ☐ 0.0200 M/s - ☐ 0.100 M/s - ☐ 0.0400 M/s - ☐ 0.0600 M/s - ☐ 0.0800 M/s **Explanation:** To solve this problem, you need to understand how the rate of a reaction changes with the concentration of a reactant. The given rate law is rate = k[A]^2, indicating that the rate of reaction is directly proportional to the square of the concentration of [A]. Given: - Initial rate = 0.0200 M/s - Initial concentration, [A] = 0.100 M - Rate = k[A]^2 Firstly, determine the rate constant (k) using the provided data: \[ 0.0200 \text{ M/s} = k \times (0.100 \text{ M})^2 \] \[ 0.0200 \text{ M/s} = k \times 0.0100 \text{ M}^2 \] \[ k = \frac{0.0200 \text{ M/s}}{0.0100 \text{ M}^2} \] \[ k = 2 \text{ M}^{-1}\text{s}^{-1} \] Now, use this rate constant to find the new rate when [A] = 0.200 M: \[ \text{New rate} = k \times (0.200 \text{ M})^2 \] \[ \text{New rate} = 2 \text{ M}^{-1}\text{s}^{-1} \times (0.200 \text{ M})^2 \] \[ \text{New rate} = 2 \text{ M}^{-1}\text{s}^{-1} \times 0.0400 \text{ M}^2 \] \[ \text{New rate} = 0.080
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps with 2 images

Blurred answer
Knowledge Booster
Rate Laws
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.
Similar questions
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY