A 2.5l flask at 15°c contains a mixture of n2, he and ne at partial pressure of 0.32 atm for n2, 0.15 atm for he and 0.42 atm for ne. calculate the volume in liter at stp occupied by he and ne if the n2 is removed selectively. how to solve this problem?

Question

Chemistry

Annie

11 November, 01:02

A 2.5l flask at 15°c contains a mixture of n2, he and ne at partial pressure of 0.32 atm for n2, 0.15 atm for he and 0.42 atm for ne. calculate the volume in liter at stp occupied by he and ne if the n2 is removed selectively. how to solve this problem?

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Beatrice Calhoun · Answer 1

Below are supposed to be the question:

a) what is the total pressure of the mixture?

b) calculate the volume in Liters at STP occupied by He and Ne if the N2 is removed selectively.

Below is the answers:

a. Dalton's law says that you just add 'em all together and you will get the total pressures. So it's. 89 atm at 15 degrees.

b. Use the partial pressure given and ignore the other gasses. Convert to STP ...32+.42=.74 atm.

This is at 15 degrees C and with a volume of 2.5. We need to change the volume, by the same factor of the gas we just removed. Then we can convert this number to STP. 15/.74=.2. Our gas volume just went down by 20% (by taking out the N2). 2.5-20%=2. The gas is now occupying 2 liters at 15 C and. 74 atm.

Let's convert the temperature to K. 15+273=288. When we chill the gas to 0 degrees, we lose some volume, represented by 273/288. So, 2 liters (273/288) = 1.9 liters at 0 degrees C and. 74 atm.

Now, we need to compress our gas until it reaches 1 atm. This will further reduce the volume. 1.9 * (.74/1) = 1.4 atm. This is your final answer.