Problem: 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.

FREE Expert Solution

Given:

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.

PV = nRT

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Problem Details

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.

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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 The Ideal Gas Law Derivations concept. You can view video lessons to learn The Ideal Gas Law Derivations. Or if you need more The Ideal Gas Law Derivations practice, you can also practice The Ideal Gas Law Derivations 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 Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.