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What will be the volume of the gas when it is released from the tanks?

Chemistry
Tutor: None Selected Time limit: 1 Day

Atmospheric pressure on the peak of Mt. Everest can be as low as 148 mm Hg, which is why climbers need to bring oxygen tanks for the last part of the climb. If the climbers carry 10.0 liter tanks with an internal gas pressure of 3.04 x 10^4 mm Hg, what will be the volume of the gas when it is released from the tanks?

Apr 1st, 2015

Ideal Gas law states that,

PV=nRT (p=Pressure,V=volume,n=number of moles,R=constant,T=temperature)

Let 1 be initial state and 2 be stage at mt everest height

1V1/nRT1= P­2V2/nRT2

since T,R,n are same for both the times, we are left with

1V1= P­2V2

148*V1=10*3.04 x 10^4

thus V1= 10*3.04 x 10^4 / 148 = 2.054 * 10^3 liter (ANSWER)


Apr 1st, 2015

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