A balloon is filled with helium gas with a partial pressure of 1.00 atm and neon gas with a partial pressure of 0.50 atm. For each of the following changes (a to e) of the initial balloon, select the diagram (A, B, or C) that shows the final volume of the balloon:
c. All of the neon gas is removed (T and P do not change).

Question

A balloon is filled with helium gas with a partial pressure of 1.00 atm and neon gas with a partial pressure of 0.50 atm. For each of the following changes (a to e) of the initial balloon, select the diagram (A, B, or C) that shows the final volume of the balloon:
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c. All of the neon gas is removed (T and P do not change).

c. All of the neon gas is removed (T and P do not change).

Accepted Answer

Hello. In this problem, we are told a cylinder with a movable piston contains a mixture of Argon and Xenon gas with the partial pressures of 0.80 atmospheres and 1.20 atmospheres. Respectfully, we are asked to choose the diagram that represents the change in volume when Argon gas is removed from the cylinder at constant temperature and pressure we are given then our initial state and then three possible answers. Answer A B and CC has the same volume as our initial state. B has a lower volume than our initial state. And A has a higher volume than our initial state. We can begin with the ideal gas equation PV equals N RT. And we can move everything to the right hand side that is constant and everything to the left hand side that is variable. We will begin by moving the pressure to the right hand side. So we'll divide both sides by the pressure. We then get our volume is equal to the moles times the gas, constant times temperature divided by pressure. We will now move our moles of gas to the left hand side. So we'll divide both sides by the moles, we then get our volume divided by the moles of gas is equal to the gas constant times the temperature divided by pressure R is a constant. We are told the temperature and pressure remain constant. So that means then everything on the right hand side is constant. So we have the volume divided by the moles is equal to a constant. We call that this is Avogadro's Law. And so we can write the general form of a gas law or under two different conditions, we have our initial volume divide by our initial moles is equal to our volume. Under a second set of conditions divided by the moles. Under this second set of conditions, we're trying to find the change of volume. So we'll solve for V two, our volume two then is equal to the moles under our final condition times our initial volume divided by our initial number of moles. So as our moles decreases, so N two being less than M one and that's because argon gas is removed, then we find that B two will be less than V one looking at the diagrams that were provided, the one that has a volume less than our initial volume is image B. So B then is our correct answer. Thanks for watching. Hope this helped.

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Key Concepts

Partial Pressure

Gas Laws

Volume Change in Gases