What is the pressure of nitrogen when cooled to -5oC?

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SUMMARY

The pressure of nitrogen in a cylinder initially pressurized to 200 BAR at 25°C decreases to approximately 180 BAR when cooled to -5°C. This calculation is based on the ideal gas law, specifically the equation P1/T1 = P2/T2. The temperatures were converted to Kelvin, resulting in T1 as 298 K and T2 as 268 K. The correct application of the equation confirms the final pressure after cooling.

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Homework Statement



A cylinder of nitrogen is pressurised to 200 BAR at 25oC
The cylinder is left to cool outside on a winters day to –5oC

What is the pressure of the Nitrogen once it has cooled?



Homework Equations



P1/T1=P2/T2 ?


The Attempt at a Solution



25+273 = 298 Kelvin. 273-5=268 Kelvin.

200/298=0.6711409396

0.6711409396 x 268 = 179 BAR ?

Have i used the relevant equation? Going through some practice questions but can't find the solutions. doh.

cheers
 
Physics news on Phys.org
You would normally just do
200 * 268/298 = 180Bar

Yes you are correct.
 

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