Log in
Chemistry
2
answers
0
watching
14
views
13 Dec 2019

A 38.0 L gas tank at 35 c has nitrogen at a pressure of 4.65 atm. The contents of the tank are transferred without loss to an evacuated 55.0 L tank in a cold room where the temperature is 4 c. What is the pressure in the tank?

Watch
2
answers
0
watching
14
views

For unlimited access to Homework Help, a Homework+ subscription is required.

Unlock all answers

Get 1 free homework help answer.
Get unlimited access
Already have an account? Log in
Share
Jamar Ferry
Jamar FerryLv2
17 Dec 2019
Get unlimited access
Already have an account? Log in
Share
discord banner image
Join us on Discord
Chemistry Study Group
Join now

Related textbook solutions

Basic Chemistry
5 Edition,
Timberlake
ISBN: 9780134138046
Principles of Chemistry Molecular Approach
4th Edition,
Tro
ISBN: 9780134112831
Chemistry: Structure and Properties
2nd Edition,
Tro
ISBN: 9780134293936
Principles of Chemistry Molecular Approach
3rd Edition, 2014
Tro
ISBN: 9780321971944
Chemistry: A Molecular Approach
3rd Edition,
Tro
ISBN: 9780321809247
Chemistry: A Molecular Approach
5th Edition,
Tro
ISBN: 9780134874371
Principles of Chemistry: A Molecular Approach
4th Edition,
Tro
ISBN: 9780134895741
Chemistry: The Central Science
14th Edition, 2017
Brown
ISBN: 9780134414232

Related questions

The volume of a large, irregularly shaped, closed tank is determined as follows. The tank is first evacuated, and then it is connected to a 50.0 L cylinder of compressed nitrogen gas. The gas pressure in the cylinder, originally at 21.5 atm, falls to 1.55 atm without a change in temperature. What is the volume of the tank?

Many gases are shipped in high-pressure containers. Consider a steel tank whose volume is 55.0 gallons that contains O2 gas at a pressure of 16,500 kPa at 23 °C. (a) What mass of O2 does the tank contain? (b) What volume would the gas occupy at STP? (c) At what temperature would the pressure in the tank equal 150.0 atm? (d) What would be the pressure of the gas, in kPa, if it were transferred to a container at 24 °C whose volume is 55.0 L?

Part #1:

Which of the following would DECREASE the amount of gas dissolved in your tank?

A) Increase the air pressure above the tank

B) Decrease the Temperature

C) Increase the Temperature

Part #2:

At a particular temperature, you determine that in 50.4 L of water, 0.703 grams of N2 gas are dissolved. You measure the pressure above the tank to be 0.771 atm. Assuming the maximum amount of gas has been dissolved, calculate the Henry's Law constant in the units of mol/(L*atm). Assume that there is ONLY nitrogen in the air above the tank.

Part #3:

You determine that at room temperature (25 oC) the Henry’s Law constant of O2 gas is 1.3 * 10-3 mol/(L*atm). If you have a 50.4 L of water in your fish tank, and the air pressure is 0.771 atm in the room, how many grams of O2 gas could be dissolved? (enter the number only, without units)

Weekly leaderboard

Home
Homework Help 3,900,000
Chemistry 830,000
Start filling in the gaps now
Log in