What is the average kinetic energy per atom of He in a gas mixture at 448 K?

AI Thread Summary
The discussion focuses on calculating the average kinetic energy per atom of helium (He) in a gas mixture at 448 K, which includes both helium and neon (Ne). The formula KE(bar) = (3/2)kT is highlighted as the method to find this average kinetic energy, where k is Boltzmann's constant. A participant expresses confusion about calculating kinetic energy due to difficulties with typing small values in an online format. The conversation also touches on calculating the average kinetic energy for neon and the total kinetic energy for helium by multiplying the average energy per atom by the number of helium atoms. The calculations emphasize the importance of understanding the relationship between temperature, kinetic energy, and the number of particles in a gas mixture.
Punjabi.Sher
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A gas contains a mixture of He and Ne.
The gas is at a temperature of 448 K, with
0.85 mole of He and 2 mole of Ne.
Avogadro’s number is 6.02 × 1023 mol−1,
and Boltzmann’s constant is 1.38×10−23 J/K.
What is the average kinetic energy per
molecule of He? Answer in units of J.



2. KE(bar) = (1/2)mv² = (3/2)kT



3. The middle equation above gives you the average kinetic energy, but I don't have any velocity. Can someone please guide me with this problem?
 
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What's wrong with using KE(bar) = (3/2)kT?
 
wow, it was just a matter of typing it in correctly. I can't believe this, because I am doing these online, so I didn't know how to type in very small values like with exponents.
 
Ok there's part 2 to this question. It looks so similar to this, but the same method doesn't give me the right answer.

Part 2: What is the average kinetic energy per
molecule of Ne?

Part 3: What is the average total kinetic energy of
He? Answer in units of J.
 
For part 3 it sounds like the want average kinetic energy per atom of He * number of atoms of He.
 

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