**Question 1:** Assuming constant volume and moles, how would the pressure of an ideal gas change if the temperature, in degrees Kelvin, tripled? **Question 2:** Assuming constant moles and temperature, how would the pressure of an ideal gas change if volume was doubled? **Explanation:** These questions relate to the Ideal Gas Law, expressed as \( PV = nRT \) where: - \( P \) is pressure - \( V \) is volume - \( n \) is the number of moles - \( R \) is the ideal gas constant - \( T \) is the temperature in Kelvin **For Question 1:** - With constant volume and moles, pressure is directly proportional to temperature. Tripling the temperature will also triple the pressure. **For Question 2:** - With constant moles and temperature, pressure is inversely proportional to volume. Doubling the volume will halve the pressure.

Question 1: Assuming constant volume and moles, how would the pressure of an ideal gas change if the temperature, in degrees Kelvin, tripled? Question 2: Assuming constant moles and temperature, how would the pressure of an ideal gas change if volume was doubled? Explanation: These questions relate to the Ideal Gas Law, expressed as \( PV = nRT \) where: - \( P \) is pressure - \( V \) is volume - \( n \) is the number of moles - \( R \) is the ideal gas constant - \( T \) is the temperature in Kelvin For Question 1: - With constant volume and moles, pressure is directly proportional to temperature. Tripling the temperature will also triple the pressure. For Question 2: - With constant moles and temperature, pressure is inversely proportional to volume. Doubling the volume will halve the pressure.

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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