Problem: If the pressure in a helium-filled balloon is 4.4 atm when filled to 5.0 × 10  2 L, what volume is occupied by the helium-filled balloon when the pressure is reduced to 1.1 atm?(a) 2.0 × 102 L(b) 2.5 × 102 L(c) 2.2 × 102 L(d) 2.0 × 103 L(e) 3.0 × 102 L

🤓 Based on our data, we think this question is relevant for Professor Gulde's class at UB.

FREE Expert Solution

Helium inside a balloon was initially at 4.4 atm when filled to 5.0 × 10  2 L then the pressure was reduced to  1.1 atm at a constant temperature. We’re being asked to determine the volume of the gas after decreasing the pressure.


Recall that the ideal gas law is:


PV=nRT


The pressure and volume of a gas are related to the number of moles, gas constant and temperatureThe value nRT is constant


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Problem Details

If the pressure in a helium-filled balloon is 4.4 atm when filled to 5.0 × 10  2 L, what volume is occupied by the helium-filled balloon when the pressure is reduced to 1.1 atm?

(a) 2.0 × 102 L

(b) 2.5 × 102 L

(c) 2.2 × 102 L

(d) 2.0 × 103 L

(e) 3.0 × 102 L

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 Gulde's class at UB.