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Answer to Question #20527 in Physical Chemistry for Cody

Question #20527
A scientist wishes to compress 50.0 ml of ammonia gas at normal atmospheric pressure to a volume of 1.0 ml. What pressure in atmospheres is necessary
Expert's answer
Using Law: PV = nRT we can calculate P (pressure)

But this law becomes P1V1/T1 = P2V2/T2 for one compound under different conditions

T1 = T2 = const, so P1V1 = P2V2

P1 = 1 atm (STP), so P2 = P1V1/V2 = 1*50.0/1.0 = 50 atm

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Assignment Expert
16.05.18, 09:07

Dear Aaditya if the volume is 2.0 ml
P1 = 1 atm (STP), so P2 = P1V1/V2 = 1*50.0/2.0 = 25 atm

15.05.18, 01:35

what if the volume is 2.0 ml

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