A 334-mL cylinder for use in chemistry lectures contains 5.399 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?

Note that pressure is given in units of atm. This means the gas constant we use must include units of atm in its units. The gas constant R=0.08206 (L x atm) / (mol x K) should be used in your calculation.