Posted by **april** on Sunday, October 17, 2010 at 8:20pm.

At 16°C a sample of ammonia gas exerts a pressure of 11.7 atm. What is the pressure when the volume of the gas is reduced to one-fourth of the original value at the same temperature

so the inital Temp=16 C

initial Pressure. 11.7

final pressure-unknown

temperature-same

what next?

- chemistry -
**DrBob222**, Sunday, October 17, 2010 at 9:32pm
You omitted some of the problem.

initial T = 16 C

p = 11.7 atm

final pressure = ??, the unknown.

final T = 16 (apparently doesn't change).

initial volume = ?

final volume = 1/4 the original volume.

What I usually do is to assume a value for V1 (a convenient number of 4), that makes the final volume 1 (1/4 of 4 = 1).

Then use P1V1 = P2V2 and solve for P2.

- chemistry -
**april**, Sunday, October 17, 2010 at 10:36pm
okay thank you

With your information I did

p1v1=p2v2

(11.7)( 4)= P2(1)

my final answer 46.8 atm

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