🤓 Based on our data, we think this question is relevant for Professor Atwood's class at UB.
V1 = 15.0 L
P1 = 2.00x102 atm
V2 = ?
P2 = 1 atm
Remember the ideal gas law: PV = nRT
Assuming the amount of He will remain constant, T is constant and R is also a constant.
A 15.0-L tank is filled with He to a pressure of 2.00 x 102 atm. How many balloons (each 2.00 L) can be inflated to a pressure of 1.00 atm from the tank? Assume that there is no temperature change and that the tank cannot be emptied below 1.00 atm pressure.
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Chemistry Gas Laws concept. If you need more Chemistry Gas Laws practice, you can also practice Chemistry Gas Laws practice problems.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Atwood's class at UB.
What textbook is this problem found in?
Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl 2nd Edition practice problems.