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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![**Rate Law Calculation Example**
**Question 19 of 36:**
*A reaction has a rate law of Rate = (1.25 M⁻¹s⁻¹)[A][B]. What is the rate of the reaction if [A] = 0.301 M and [B] = 0.280 M?*
**Calculation:**
**Step 1: Understand the Rate Law**
The rate law is given by:
\[ \text{Rate} = k[A][B] \]
Where:
- \( k \) is the rate constant, which is \( 1.25 \, \text{M}^{-1}\text{s}^{-1} \) in this problem.
- \([A]\) and \([B]\) are the concentrations of the reactants.
**Step 2: Plug in the Given Values**
Given:
\[ [A] = 0.301 \, \text{M} \]
\[ [B] = 0.280 \, \text{M} \]
\[ k = 1.25 \, \text{M}^{-1}\text{s}^{-1} \]
The rate is:
\[ \text{Rate} = (1.25 \, \text{M}^{-1}\text{s}^{-1})(0.301 \, \text{M})(0.280 \, \text{M}) \]
**Step 3: Perform the Calculation**
\[ \text{Rate} = 1.25 \times 0.301 \times 0.280 \]
\[ \text{Rate} = 0.10535 \, \text{M/s} \]
**Answer:**
The rate of the reaction is \( 0.10535 \, \text{M/s} \).
**Interactive Elements:**
The screenshot includes a numeric keypad for entering the calculated rate, with buttons for each digit (1-9, 0), a decimal point ".", a plus/minus sign "+/-", a backspace "←", a clear "C" button, and an exponential notation button "x 10".
This educational example guides students step-by-step through the process of calculating reaction rates using the given rate law and demonstrates where to input their final answer.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F17050110-9897-4bd6-b477-110f723d877a%2F651be67a-0a81-4fc8-b568-62df1ff08c7e%2Fh32idz8_processed.png&w=3840&q=75)
Transcribed Image Text:**Rate Law Calculation Example**
**Question 19 of 36:**
*A reaction has a rate law of Rate = (1.25 M⁻¹s⁻¹)[A][B]. What is the rate of the reaction if [A] = 0.301 M and [B] = 0.280 M?*
**Calculation:**
**Step 1: Understand the Rate Law**
The rate law is given by:
\[ \text{Rate} = k[A][B] \]
Where:
- \( k \) is the rate constant, which is \( 1.25 \, \text{M}^{-1}\text{s}^{-1} \) in this problem.
- \([A]\) and \([B]\) are the concentrations of the reactants.
**Step 2: Plug in the Given Values**
Given:
\[ [A] = 0.301 \, \text{M} \]
\[ [B] = 0.280 \, \text{M} \]
\[ k = 1.25 \, \text{M}^{-1}\text{s}^{-1} \]
The rate is:
\[ \text{Rate} = (1.25 \, \text{M}^{-1}\text{s}^{-1})(0.301 \, \text{M})(0.280 \, \text{M}) \]
**Step 3: Perform the Calculation**
\[ \text{Rate} = 1.25 \times 0.301 \times 0.280 \]
\[ \text{Rate} = 0.10535 \, \text{M/s} \]
**Answer:**
The rate of the reaction is \( 0.10535 \, \text{M/s} \).
**Interactive Elements:**
The screenshot includes a numeric keypad for entering the calculated rate, with buttons for each digit (1-9, 0), a decimal point ".", a plus/minus sign "+/-", a backspace "←", a clear "C" button, and an exponential notation button "x 10".
This educational example guides students step-by-step through the process of calculating reaction rates using the given rate law and demonstrates where to input their final answer.
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