Problem: A 334-mL cylinder for use in chemistry lectures contains 5.257 g of helium at 23˚C.How many grams of helium must be released to reduce the pressure to 65 atm assuming ideal gas behavior?

🤓 Based on our data, we think this question is relevant for Professor Briggs' class at ASU.

FREE Expert Solution

Since the gas behaves ideally, the ideal gas equation can be used to solve this problem:

Calculate the number of moles of gas required for P = 65 atm:

Given:

V = 334 mL

T = 23° C + 273.15 K = 296.15 K

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Problem Details

A 334-mL cylinder for use in chemistry lectures contains 5.257 g of helium at 23˚C.

How many grams of helium must be released to reduce the pressure to 65 atm assuming ideal gas behavior?

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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 concept. You can view video lessons to learn The Ideal Gas Law. Or if you need more The Ideal Gas Law practice, you can also practice The Ideal Gas Law practice problems.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Briggs' class at ASU.