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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![Data in the table were collected at 540 K for the following reaction:
\[ \text{CO(g)} + \text{NO}_2\text{(g)} \rightarrow \text{CO}_2\text{(g)} + \text{NO(g)} \]
**Initial Concentrations (mol/L):**
\[
\begin{array}{ccc}
\hline
[\text{CO}] & [\text{NO}_2] & \text{Initial Rate (mol/L \cdot h)} \\
\hline
5.1 \times 10^{-4} & 0.35 \times 10^{-4} & 5.0 \times 10^{-8} \\
5.1 \times 10^{-4} & 0.70 \times 10^{-4} & 1.0 \times 10^{-7} \\
5.1 \times 10^{-4} & 0.18 \times 10^{-4} & 2.6 \times 10^{-8} \\
1.0 \times 10^{-3} & 0.35 \times 10^{-4} & 9.8 \times 10^{-8} \\
1.5 \times 10^{-3} & 0.35 \times 10^{-4} & 1.5 \times 10^{-7} \\
\hline
\end{array}
\]
**Explanation:**
This table presents the initial concentrations of carbon monoxide (CO) and nitrogen dioxide (NO₂) along with the corresponding initial reaction rates for the formation of carbon dioxide (CO₂) and nitric oxide (NO) at a temperature of 540 K. Each row represents a different experimental condition with varying concentrations of the reactants. The unit of the initial rate is moles per liter per hour (mol/L·h).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd32c0099-d35b-45af-b7af-24c06e9e82b9%2Fa164345c-7010-4eea-b5a4-fc587ae47c7e%2F1zmz5be_processed.png&w=3840&q=75)
Transcribed Image Text:Data in the table were collected at 540 K for the following reaction:
\[ \text{CO(g)} + \text{NO}_2\text{(g)} \rightarrow \text{CO}_2\text{(g)} + \text{NO(g)} \]
**Initial Concentrations (mol/L):**
\[
\begin{array}{ccc}
\hline
[\text{CO}] & [\text{NO}_2] & \text{Initial Rate (mol/L \cdot h)} \\
\hline
5.1 \times 10^{-4} & 0.35 \times 10^{-4} & 5.0 \times 10^{-8} \\
5.1 \times 10^{-4} & 0.70 \times 10^{-4} & 1.0 \times 10^{-7} \\
5.1 \times 10^{-4} & 0.18 \times 10^{-4} & 2.6 \times 10^{-8} \\
1.0 \times 10^{-3} & 0.35 \times 10^{-4} & 9.8 \times 10^{-8} \\
1.5 \times 10^{-3} & 0.35 \times 10^{-4} & 1.5 \times 10^{-7} \\
\hline
\end{array}
\]
**Explanation:**
This table presents the initial concentrations of carbon monoxide (CO) and nitrogen dioxide (NO₂) along with the corresponding initial reaction rates for the formation of carbon dioxide (CO₂) and nitric oxide (NO) at a temperature of 540 K. Each row represents a different experimental condition with varying concentrations of the reactants. The unit of the initial rate is moles per liter per hour (mol/L·h).
![**Calculate the Rate Constant**
To determine the rate constant for a reaction, use the formula provided:
**Rate constant = [blank] L/(mol · h)**
Fill in the required value to complete the calculation. This formula is used to calculate the rate constant, which is a critical parameter in the rate equation of a chemical reaction. The units, liters per mole per hour (L/(mol · h)), indicate how the rate constant relates to concentrations and time.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd32c0099-d35b-45af-b7af-24c06e9e82b9%2Fa164345c-7010-4eea-b5a4-fc587ae47c7e%2Fytflepp_processed.png&w=3840&q=75)
Transcribed Image Text:**Calculate the Rate Constant**
To determine the rate constant for a reaction, use the formula provided:
**Rate constant = [blank] L/(mol · h)**
Fill in the required value to complete the calculation. This formula is used to calculate the rate constant, which is a critical parameter in the rate equation of a chemical reaction. The units, liters per mole per hour (L/(mol · h)), indicate how the rate constant relates to concentrations and time.
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