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:
V = 334 mL
T = 23° C + 273.15 K = 296.15 K
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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