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 Questions and Explanations
**Question 54: How and why do chemical reaction rates depend on temperature?**
**Answer:**
Chemical reaction rates typically increase with temperature. This is because higher temperatures provide more energy to the reactant molecules, increasing their kinetic energy. As a result, the molecules move faster, collide more frequently, and with greater energy, which increases the chances of overcoming the activation energy barrier for the reaction to occur. This relationship is often quantified by the Arrhenius equation, which shows that the rate constant of a reaction increases exponentially with an increase in temperature.
**Question 55: Define the partial pressure of a vapor. Use air in this classroom as an example.**
**Answer:**
The partial pressure of a vapor is the pressure exerted by a single type of gas in a mixture of gases. It is the hypothetical pressure of that gas if it alone occupied the entire volume of the mixture at the same temperature. The total pressure of the gas mixture is the sum of the partial pressures of all the individual gases present.
For example, air in this classroom is a mixture of several gases, primarily nitrogen (N₂), oxygen (O₂), and small amounts of other gases such as argon (Ar) and carbon dioxide (CO₂). The partial pressure of oxygen is the pressure that oxygen would exert if it occupied the entire volume alone at the same temperature. Similarly, the partial pressure of nitrogen is the pressure that nitrogen would exert under the same conditions, and so on for each gas in the mixture.
Total classroom air pressure (P_total) can be expressed as the sum of the partial pressures of nitrogen (P_N₂), oxygen (P_O₂), argon (P_Ar), and carbon dioxide (P_CO₂), as follows:
\[ P_{total} = P_{N_2} + P_{O_2} + P_{Ar} + P_{CO_2} \]
This concept is fundamental in understanding gas behavior and is important in various scientific and industrial applications, including respiratory physiology, chemical engineering, and environmental science.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F03b7918c-d94c-4943-a460-522394a4ae27%2F066e5077-f07f-45fc-8344-10c09d1de40b%2Fy40kza4_processed.png&w=3840&q=75)
Transcribed Image Text:### Chemistry Questions and Explanations
**Question 54: How and why do chemical reaction rates depend on temperature?**
**Answer:**
Chemical reaction rates typically increase with temperature. This is because higher temperatures provide more energy to the reactant molecules, increasing their kinetic energy. As a result, the molecules move faster, collide more frequently, and with greater energy, which increases the chances of overcoming the activation energy barrier for the reaction to occur. This relationship is often quantified by the Arrhenius equation, which shows that the rate constant of a reaction increases exponentially with an increase in temperature.
**Question 55: Define the partial pressure of a vapor. Use air in this classroom as an example.**
**Answer:**
The partial pressure of a vapor is the pressure exerted by a single type of gas in a mixture of gases. It is the hypothetical pressure of that gas if it alone occupied the entire volume of the mixture at the same temperature. The total pressure of the gas mixture is the sum of the partial pressures of all the individual gases present.
For example, air in this classroom is a mixture of several gases, primarily nitrogen (N₂), oxygen (O₂), and small amounts of other gases such as argon (Ar) and carbon dioxide (CO₂). The partial pressure of oxygen is the pressure that oxygen would exert if it occupied the entire volume alone at the same temperature. Similarly, the partial pressure of nitrogen is the pressure that nitrogen would exert under the same conditions, and so on for each gas in the mixture.
Total classroom air pressure (P_total) can be expressed as the sum of the partial pressures of nitrogen (P_N₂), oxygen (P_O₂), argon (P_Ar), and carbon dioxide (P_CO₂), as follows:
\[ P_{total} = P_{N_2} + P_{O_2} + P_{Ar} + P_{CO_2} \]
This concept is fundamental in understanding gas behavior and is important in various scientific and industrial applications, including respiratory physiology, chemical engineering, and environmental science.
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