N2 Molecules in 500mL Container at 780mm Hg & 135°C

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To determine the number of N2 molecules in a 500mL container at 780mm Hg and 135°C, the ideal gas law (PV=nRT) can be applied. The volume of gas expands with temperature and decreases with pressure, which are crucial factors in this calculation. It's important to convert the conditions to appropriate units, such as converting pressure from mm Hg to atmospheres and temperature to Kelvin. Additionally, the forum emphasizes that users should demonstrate some initial effort before receiving assistance. Properly applying these principles will lead to the solution of the homework question.
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Can someone please get me started on this one homework question? How many molecules of N2 are in a 500mL container at 780mm Hg and 135 degress Celcius?


Thanks

David
 
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A mole of a gas at STP (0deg C and 1 atmosphere) always occupy the same volume, about 22.4litres.
The volume expands linearly with absolute temperature and decreases linearly with pressure.
Call back if you need more hints.
 
David:
1. Questions like this belong in the Homework & Coursework area (near the top of the forum main page);
2. We typically require you to first show some effort before we can help you.
 
with all the given variables that you are given, what formula should you use?
 
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