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A sample of ammonia gas at 75°c and 445 mm hg has a volume of 16.0 l. what volume will it occupy if the pressure rises to 1225 mm hg at constant temperature? 1 atm = 760 mm hg.
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A sample of ammonia gas at 75°c and 445 mm hg has a volume of 16.0 l. what volume will it occupy if the pressure rises to 1225 mm hg at constant temperature? 1 atm = 760 mm hg.

User Blease
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1 Answer

4 votes
In this kind of exercises, you should use the "ideal gas" rules: PV = nRT
P should be in Pascal:
445mmHg = 59328Pa
1225mmHg = 163319Pa

V should be in cubic meter:
16L = 0.016 m3

R =
(PV)/(nT) = constant

(P1 V1)/(n T) =
(P2 V2)/(n T)
==> P1 * V1 = P2 * V2
V2 =
(P1 V1)/(P2) =
(445 0.016)/(1225)
V2 = 0.00581 m3 = 5.81 L


User RD Florida
by
6.5k points
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