[dillonchester21]

You have .500 mol of He 2.50 mol of Neon, and enough volume to have a partial pressure of 2.00 atm for Argon. The volume(constant) is 8.20 L and the temperature(constant) is 127 degrees CELSIUS.

1) Total  Pressure?
thought it you would use PV=NRT for Helium and Neon to find each pressure then add each pressure to 2.00 atm.



2) mols of Argon? No idea

[dillonchester21]

Also this you have to describe the situation using kinetic energy.

1) Double the volume, the temperature is constant.
I thought it would decrease since it talks about kinetic energy not average kinetic energy and because there would be less collision with particles.

2) Increase Temperature
Said the kinetic energy would increase because of more collisions.

3) Absolute Zero
Said that the particles are still in constant motion but at minimal KE.

[Borek]

thought it you would use PV=NRT for Helium and Neon to find each pressure then add each pressure to 2.00 atm.

Soudns oK

2) mols of Argon? No idea

P? V? T? What more do you need?