How Many Moles of NO2 and SO2 Are in the Mixture?

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Discussion Overview

The discussion revolves around a homework problem involving the calculation of moles of NO2 and SO2 in a gas mixture based on given pressures and conditions. Participants explore the application of the ideal gas law to determine the number of moles present in the sample.

Discussion Character

  • Homework-related, Mathematical reasoning

Main Points Raised

  • The initial poster attempted to use the ideal gas law (PV = nRT) to calculate the moles of NO2 and reported a value of 3.1 x 10-3 moles.
  • Some participants suggest that the initial poster may have made an arithmetic mistake or a mistake in units.
  • One participant asserts that the book's answer of 1.9 x 10-3 moles for NO2 is correct.
  • The initial poster later acknowledges an error in manipulating the equations, indicating a resolution to their confusion.
  • Another participant expresses curiosity about the correct calculations and requests to see the work leading to the correct answer.

Areas of Agreement / Disagreement

The discussion indicates that there was initial disagreement regarding the correctness of the initial poster's calculations, but the initial poster later agrees with the book's answer after recognizing their error. However, the specific details of the correct calculations remain unresolved as one participant seeks clarification.

Contextual Notes

Participants did not provide detailed calculations or clarify the specific arithmetic or unit errors made by the initial poster, leaving some aspects of the problem unresolved.

RedemistiDeus
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Homework Statement


A sample containing only NO2 and SO2 has a total pressure of 120 torr. Measurements show that the partial pressure of NO2 is 43 torr. If the vessel has a volume of 800.0 ml and the temperature is 22.0°C, how many moles of each gas are present?

Homework Equations



PV = nRT

The Attempt at a Solution


I tried to solve it using the equation above by solving for n for each gas (using their given pressure).
For the n of NO2, I had the answer 3.1 x 10-3 (using n = PV/RT).
But the book provides a different answer for it which is 1.9 x 10-3.

My question is I would like to know how my answer turned to be incorrect. I don't know any other possible methods of solving this than the ideal gas law.
Thank you.
 
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I suspect you have either an arithmetic mistake and/or a mistake in units.

Please post the details of your calculations.
 
Book answer is correct.
 
Okay guys, I got it. I had an error in manipulating the equations. Thank you PF for helping me resolve the problem!
 
RedemistiDeus said:
Okay guys, I got it. I had an error in manipulating the equations. Thank you PF for helping me resolve the problem!

I'm curious as to how you arrived at the correct answer. Could you show your work?
 

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