At 298 K, pure helium gas has a volume of 160.0 L and a pressure of 1860 psi inside a tank.
We’re being asked to determine how many 3.5-L helium balloons can be filled from pure helium in the tank assuming an atmospheric pressure of 1.0 atm and a temperature of 298 K.
Recall that the ideal gas law is:
The pressure and volume of a gas are related to the number of moles, gas constant and temperature. The value nRT is constant.
A 160.0 -L helium tank contains pure helium at a pressure of 1860 psi and a temperature of 298 K.
How many 3.5-L helium balloons can be filled from the helium in the tank? (Assume an atmospheric pressure of 1.0 atm and a temperature of 298 K.)
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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 Chemistry Gas Laws concept. If you need more Chemistry Gas Laws practice, you can also practice Chemistry Gas Laws practice problems.
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