Solve Gas Law Problem: Find Average Kinetic Energies of CH4 & N2

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Discussion Overview

The discussion revolves around solving a gas law problem related to calculating the average kinetic energies of methane (CH4) and nitrogen (N2) molecules at two different temperatures, 294 K and 574 K. Participants explore various equations and methods to arrive at the correct solution.

Discussion Character

  • Homework-related

Main Points Raised

  • One participant expresses frustration over not being able to find the correct answers despite trying multiple approaches.
  • Another participant asks what equations have been attempted to assist in troubleshooting the problem.
  • A participant lists several equations they have used, including KE = 3/2 RT, sqrt[3RT/M], and KE = (3/2)RT/Avogadro's number.
  • A later post indicates that the original poster has resolved the issue independently.
  • Another participant acknowledges missing a previous response, indicating ongoing engagement in the discussion.

Areas of Agreement / Disagreement

The discussion does not reach a consensus on the correct approach or solution, as the original poster ultimately finds the answer independently.

Contextual Notes

Participants do not clarify which specific equations were successful or what assumptions were made in their calculations, leaving some uncertainty regarding the methods used.

ironizer
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Gas Law problem... please help

Calculate the average kinetic energies of the CH4 and N2 molecules at 294 K and 574 K.

I've tried every possible way I could think of. I can't get the right answer. I don't know what equation to use anymore, I've done it all and nothing works.

I got all these answers:

676
4.06e-21
4333.34
J/molecule 3 sig figs
And none of them are good. I'm getting annoyied, someone give me a hint please. Thanks
 
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What equations have you tried to use?
 


KE= 3/2 RT

sqrt[3RT/M]

and KE=(3/2)RT/avo's number
 


Thank-you all for the help.


I figured it out myself.
 


Sorry, somehow I missed your previous answer :frown:
 

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