Let's assume the volume of the box was 2.00 L when we started and the initial pressure of the gas was 3.58 atm. If we decreased the volume to 1.40 L, what would be the new pressure of the gas (assuming the temperature and moles of gas remained constant)? Show your work and don't forget units.
Let's assume the volume of the box was 2.00 L when we started and the initial pressure of the gas was 3.58 atm. If we decreased the volume to 1.40 L, what would be the new pressure of the gas (assuming the temperature and moles of gas remained constant)? Show your work and don't forget units.
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...
Related questions
Question
using Boyle's Law to complete the question
Transcribed Image Text:Instructions
Click on the link for the gas laws simulation in the Chapter 8 "Lab" Assignment on
Canvas or copy/paste this link: https://phet.colorado.edu/sims/html/gases-
intro/latest/gases-intro en.html
You will see two boxes: "Intro" on the left and "Laws" on the right. Click on the "Laws"
box. Play around with the simulation to see what everything does. Hint: move the
pump up and down to get some gas particles into the box to start.
Activity 1: Pressure and Volume (Boyle's Law)
Click the yellow button in the bottom right corner of the simulation to reset the
simulation. Pump some blue gas molecules into the box.
Record the Pressure of the gas:
Now grab the handle on the left side of the box (with your mouse) and pull it to the right.
What happened to the pressure of the gas when you decreased the volume?
atm
New Pressure:
atm
When you decreased the size of the box (volume), how did this affect the frequency with
which the gas molecules are colliding with the container walls?
Let's assume the volume of the box was 2.00L when we started and the initial pressure
of the gas was 3.58 atm. If we decreased the volume to 1.40 L, what would be the new
pressure of the gas (assuming the temperature and moles of gas remained constant)?
Show your work and don't forget units.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 3 steps
Knowledge Booster
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.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY