Partial Pressure of Kr in a N2/Kr Mixture (0.505 atm)

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Discussion Overview

The discussion revolves around calculating the partial pressure of krypton (Kr) in a mixture of nitrogen (N2) and krypton, given a total pressure of 0.505 atm. The context includes aspects of gas laws and the application of the ideal gas equation.

Discussion Character

  • Homework-related, Mathematical reasoning

Main Points Raised

  • One participant presents a problem involving a mixture of N2 and Kr and asks for the partial pressure of Kr.
  • Another participant requests that the original poster share their attempts at solving the problem to facilitate assistance.
  • A participant expresses confusion regarding the assumptions of constant volume and temperature, questioning whether they should use arbitrary values for these variables in the ideal gas equation.
  • One participant claims to have found the solution by calculating the mole fraction of Kr and multiplying it by the total pressure.
  • A later reply confirms the previous participant's method, emphasizing the importance of starting from the definitions related to partial pressure.

Areas of Agreement / Disagreement

The discussion includes some agreement on the method of calculating the partial pressure using mole fractions, but there is uncertainty regarding the assumptions about volume and temperature, and the initial problem-solving approach is not fully resolved.

Contextual Notes

There are unresolved assumptions regarding the conditions of the gas mixture, such as whether volume and temperature are constant, which may affect the application of the ideal gas law.

parwana
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A mixture of 5.40 g of N2 and 10.2 g of Kr exerts a pressure of 0.505 atm.
What is the partial pressure, in atm, of Kr?
 
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parwana, please show what you've tried, when you need help with a problem.
 
I just don't get the problem at all, i mean does this mean volume and temperature are constant and if so do i make up any numbers for the temp and volume and substitute in the equation pv=nrt??

pleASE help
 
i got it, i got the mole fraction of Ke and then times thta by total pressure.
 
parwana said:
i got it, i got the mole fraction of Ke and then times thta by total pressure.

If you meant "Kr", then yes, that's correct. With any such problem, you want to start from the definitions. In this case, the definition of 'partial pressure' is all you need.
 

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