The Ideal Gas Law and Calculating Volume at Different Temperatures

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Homework Help Overview

The discussion revolves around the application of the Ideal Gas Law to determine the volume of an air bubble as it rises from the bottom of a lake to the surface, considering changes in temperature and pressure.

Discussion Character

  • Exploratory, Assumption checking, Mathematical reasoning

Approaches and Questions Raised

  • Participants discuss the setup of the Ideal Gas Law equation, questioning the relationships between pressure and temperature at different depths. There is an exploration of how to correctly apply the formula p1v1/T1 = p2v2/T2, with some participants seeking clarification on the variables involved.

Discussion Status

The discussion includes attempts to set up the equation correctly, with one participant expressing uncertainty about their calculations. Another participant has indicated they have solved the problem, suggesting some progress has been made, though no consensus on the method has been reached.

Contextual Notes

Participants are working under the constraints of a homework assignment, which may limit the information they can use or the methods they can apply. There is a focus on ensuring the correct application of temperature conversions and pressure relationships.

Forceflow
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An air bubble of volume 18 cm3 is at the bottom of a lake 40 m deep where the temperature is 3.0°C. The bubble rises to the surface, which is at a temperature of 30°C. Take the temperature of the bubble to be the same as that of the surrounding water. What is the volume of the bubble just as it reaches the surface?

So, my teacher told me to use p1v1/T1 = p2v2/T2 p1=pgh+p0

however, when i did the work, the answer i got was 19.7608
So, could someone set up the equation for me in case I'm doing it wrong?
 
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How is p2 related to p1 and p0? What did you use for T1 and T2? Show us how you did the calculation.
 
the only parts that i understand is the first equation which i set up like this..

18/(3+273)=x/(30+273)
 
i solved it..thank you though
 

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