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A 34.0-litre cylinder contains 212g of oxygen at 27-degree Celcius.What mass of oxygen must be released to reduce the pressure to 2.463 atm?
Deat Ayush moles O2 = 212 g/32 g/mol=6.625p = 6.625 x 0.08206 x 300 K/ 34.0= 4.7968 = 4.8 atm 4.8 x 34.0 = 6.625 RT 2.463 x 34.0 = nRT 163.2 = 6.625 RT 83.742 = nRT 163.2/ 83.742 = 6.625 /n n = 3.399 = 3.46.625 - 3.4 =3.225 mass O2 that must be released = 3.225 mol x 32 g/mol=103.2 g Regards,Arun (AskIITians Forum Expert)
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