A 334-mL cylinder for use in chemistry lectures contains 5.271 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?

Question

A 334-mL cylinder for use in chemistry lectures contains 5.271 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?

brittanyrolfe · Answer

I tried using the ideal gas equation. Here is my work.
So I first used the ideal gas law equation but modified it to isolate the number of moles:
$$n = \frac{ PV }{ RT }$$
Then I plugged in all the variables:
$$n= \frac{ 65(atm) \times .334(L) }{ 0.08206(R)\times296(K) }$$