QUESTION 7 The number of moles should have remained similar since you did not pump more molecules in. What variable, besides volume, changed to counteract the increase in Volume? A. Temperature B. Pressure
QUESTION 7 The number of moles should have remained similar since you did not pump more molecules in. What variable, besides volume, changed to counteract the increase in Volume? A. Temperature B. 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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![To conduct the first experiment, pump the gas pump to introduce gas into the chamber. Use between 3 and 7 pumps. Set the temperature between 100 K and 500 K using the fire/ice bucket at the bottom. Keep the chamber width at 10.0 nm (adjust with handle on the left of the chamber). Do not open the chamber to release gas molecules (use handle on top of the chamber).
**Calculating Moles Using the Ideal Gas Law:**
\[ PV = nRT, \]
where \( R = 0.0821 \).
Once everything is set, calculate the moles of gas in the chamber using the Ideal Gas Law, which requires units: atm, L, moles, and Kelvin.
**Pressure:**
This is indicated by the circular instrument on the top right of the chamber, measured in atmospheres.
**Volume:**
Determine the volume in nm\(^3\) by multiplying the width, height, and depth of the chamber. The depth is always 1.00 nm, and the height is always 10.0 nm. Adjust the width to 10.0 nm or 15.0 nm depending on the experiment. The volume calculation is width x 10.0 nm x 1.00 nm, resulting in units of nm\(^3\). Assume your volume in nm\(^3\) converts to liters when using the Ideal Gas Law.
**Temperature:**
The thermometer shows the temperature in Kelvin.
**Quantity:**
For these experiments, you will calculate the number of moles of gas under each scenario using the Ideal Gas Law, \( PV = nRT \), solving for \( n \) (moles). \( R = 0.0821 \).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6f1e8666-0358-4f82-8394-bfae4d254ad0%2F667643b1-ba90-49a0-a3e2-ee5c3fe6210e%2Fvt49na_processed.jpeg&w=3840&q=75)
Transcribed Image Text:To conduct the first experiment, pump the gas pump to introduce gas into the chamber. Use between 3 and 7 pumps. Set the temperature between 100 K and 500 K using the fire/ice bucket at the bottom. Keep the chamber width at 10.0 nm (adjust with handle on the left of the chamber). Do not open the chamber to release gas molecules (use handle on top of the chamber).
**Calculating Moles Using the Ideal Gas Law:**
\[ PV = nRT, \]
where \( R = 0.0821 \).
Once everything is set, calculate the moles of gas in the chamber using the Ideal Gas Law, which requires units: atm, L, moles, and Kelvin.
**Pressure:**
This is indicated by the circular instrument on the top right of the chamber, measured in atmospheres.
**Volume:**
Determine the volume in nm\(^3\) by multiplying the width, height, and depth of the chamber. The depth is always 1.00 nm, and the height is always 10.0 nm. Adjust the width to 10.0 nm or 15.0 nm depending on the experiment. The volume calculation is width x 10.0 nm x 1.00 nm, resulting in units of nm\(^3\). Assume your volume in nm\(^3\) converts to liters when using the Ideal Gas Law.
**Temperature:**
The thermometer shows the temperature in Kelvin.
**Quantity:**
For these experiments, you will calculate the number of moles of gas under each scenario using the Ideal Gas Law, \( PV = nRT \), solving for \( n \) (moles). \( R = 0.0821 \).
Transcribed Image Text:**QUESTION 7**
The number of moles should have remained similar since you did not pump more molecules in. What variable, besides volume, changed to counteract the increase in Volume?
A. Temperature
B. Pressure
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