An unopened can of soda pop explodes if left in the hot sun. Which two properties change while it is in the sun? A. Temperature B. Volume C. Pressure D. Quantity of gas molecules

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
icon
Concept explainers
Question
**Experimental Procedure for Calculating Gas Moles Using the Ideal Gas Law**

1. **Gas Pumping Instructions**: 
   - Use the gas pump to insert gas into the chamber.
   - Limit the pumping to 3-7 pumps.
   - Adjust the temperature between 100 K and 500 K using the available fire/ice bucket below the chamber.
   - Keep the chamber width constant at 10.0 nm. The handle to adjust is located on the left.
   - Ensure the chamber remains closed (via the handle on top) to prevent gas molecules from escaping.

2. **Ideal Gas Law Formula**:
   - Use the equation \( PV = nRT \), where \( R = 0.0821 \).

3. **Components to Measure**:

   - **Pressure**: 
     - Indicated by the circular instrument at the top right of the chamber.
     - Measured in atmospheres (atm).

   - **Volume**:
     - Calculated in nm³ by multiplying the width, height, and depth.
     - Depth is fixed at 1.00 nm, and height is fixed at 10.0 nm.
     - Width can be adjusted to 10.0 nm or 15.0 nm.
     - Volume simplifies to the width selected x 10.0 nm, with everything in nm³.
     - For calculations, assume nm³ is equivalent to liters (L).

   - **Temperature**:
     - Indicated by the thermometer.
     - Measured in Kelvin (K).

   - **Quantity (Moles)**:
     - Calculate the number of moles using the Ideal Gas Law equation.
     - Solve for \( n \) using \( PV = nRT \).

By following these steps and utilizing the Ideal Gas Law, you can determine the number of moles of gas in various experimental scenarios.
Transcribed Image Text:**Experimental Procedure for Calculating Gas Moles Using the Ideal Gas Law** 1. **Gas Pumping Instructions**: - Use the gas pump to insert gas into the chamber. - Limit the pumping to 3-7 pumps. - Adjust the temperature between 100 K and 500 K using the available fire/ice bucket below the chamber. - Keep the chamber width constant at 10.0 nm. The handle to adjust is located on the left. - Ensure the chamber remains closed (via the handle on top) to prevent gas molecules from escaping. 2. **Ideal Gas Law Formula**: - Use the equation \( PV = nRT \), where \( R = 0.0821 \). 3. **Components to Measure**: - **Pressure**: - Indicated by the circular instrument at the top right of the chamber. - Measured in atmospheres (atm). - **Volume**: - Calculated in nm³ by multiplying the width, height, and depth. - Depth is fixed at 1.00 nm, and height is fixed at 10.0 nm. - Width can be adjusted to 10.0 nm or 15.0 nm. - Volume simplifies to the width selected x 10.0 nm, with everything in nm³. - For calculations, assume nm³ is equivalent to liters (L). - **Temperature**: - Indicated by the thermometer. - Measured in Kelvin (K). - **Quantity (Moles)**: - Calculate the number of moles using the Ideal Gas Law equation. - Solve for \( n \) using \( PV = nRT \). By following these steps and utilizing the Ideal Gas Law, you can determine the number of moles of gas in various experimental scenarios.
**Question 11**

An unopened can of soda pop explodes if left in the hot sun. Which two properties change while it is in the sun?

A. Temperature  
B. Volume  
C. Pressure  
D. Quantity of gas molecules
Transcribed Image Text:**Question 11** An unopened can of soda pop explodes if left in the hot sun. Which two properties change while it is in the sun? A. Temperature B. Volume C. Pressure D. Quantity of gas molecules
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 2 steps

Blurred answer
Knowledge Booster
Ideal and Real Gases
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