Question

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.

Answer 1

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