How to Calculate the Pressure of Each Element in a Compound Mixture?

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Discussion Overview

The discussion revolves around calculating the pressure of each component in a mixture of ether and chloroform under specific conditions, including temperature and volume. Participants explore the relevant formulas and concepts necessary for solving the problem, including the ideal gas law and partial pressures.

Discussion Character

  • Homework-related
  • Technical explanation
  • Conceptual clarification

Main Points Raised

  • One participant expresses uncertainty about which formula for ether to use, noting the presence of multiple formulas and indicating a need for clarity on the number of moles.
  • Another participant suggests assuming the problem refers to diethyl ether, commonly known as "ether," but does not provide a definitive direction on how to proceed.
  • A participant questions whether the concept of partial pressure has been studied, implying its relevance to the problem at hand.
  • Another participant advises treating each substance separately, as gases behave independently in terms of partial pressures.

Areas of Agreement / Disagreement

Participants do not reach a consensus on how to proceed with the calculations. There are multiple viewpoints regarding the approach to take, particularly concerning the use of formulas and the application of the concept of partial pressures.

Contextual Notes

Participants express uncertainty about the specific formulas for ether and the application of the ideal gas law in this context. The discussion lacks clarity on the definitions and assumptions necessary for solving the problem.

MaiteB
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Homework Statement


A compound of ether (0.287 g) and chloroform (0.568 g) evaporates in the temperature 373 K in an empty container with volume 0.0001m3. Find the pressure of each element. I don't know which formula of ether should I use since there are many. However even if I knew the n of moles for example n I would do these actions: pV=nRT. Since the T is the same: T=p1V1/n1R=p2V2/n2R=> 373=p1x/n1=p2(0.0001-x)/n2. What should I do next?

Homework Equations


pV=nRT

The Attempt at a Solution


I don't know which formula of ether should I use since there are many. However even if I knew the n of moles for example n I would do these actions: pV=nRT. Since the T is the same: T=p1V1/n1R=p2V2/n2R=> 373=p1x/n1=p2(0.0001-x)/n2. What should I do next?
 
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MaiteB said:

Homework Statement


A compound of ether (0.287 g) and chloroform (0.568 g) evaporates in the temperature 373 K in an empty container with volume 0.0001m3. Find the pressure of each element. I don't know which formula of ether should I use since there are many. However even if I knew the n of moles for example n I would do these actions: pV=nRT. Since the T is the same: T=p1V1/n1R=p2V2/n2R=> 373=p1x/n1=p2(0.0001-x)/n2. What should I do next?

Homework Equations


pV=nRT

The Attempt at a Solution


I don't know which formula of ether should I use since there are many. However even if I knew the n of moles for example n I would do these actions: pV=nRT. Since the T is the same: T=p1V1/n1R=p2V2/n2R=> 373=p1x/n1=p2(0.0001-x)/n2. What should I do next?
You can roll the dice and assume the problem is talking about diethyl ether, which is the compound commonly referred to when talking about "ether":

http://en.wikipedia.org/wiki/Diethyl_ether

Like chloroform, ether was once used as an anesthetic.
 
SteamKing said:
You can roll the dice and assume the problem is talking about diethyl ether, which is the compound commonly referred to when talking about "ether":

http://en.wikipedia.org/wiki/Diethyl_ether

Like chloroform, ether was once used as an anesthetic.
ok, but what should I do next?
 
Just treat each substance separately, as if there were no other present. That's how gases behave (and that's what partial pressures are about).
 

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