Combined Gas Law: volume of gas at STP from -247.7°C and 380 torr

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Can someone explain how to solve the following problem using the Combined Gas Law step by step?

What volume will gas occupy if 60.0 mL at -247.7°C and 380 torr pressure are adjusted to STP?

Thank you.
 
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You are going to want to use the ideal gas equation. There is no doubt more complicated/precise ways of solving the problem, but this is how i was taught and is probably how you are expected to do so.

the equation is:

pv = nrt

where p is pressure, v is volume, n is moles, r is the ideal gas constant, and t is temperature.

the ideal gas is constant for all gasses that are assumed to behave ideally. That is, for your first condition (60.0 mL at -247.7°C and 380 torr) r will be the same as r for your second condition (stand temp and pressure).

This means that if you solve the equation for r (pv = nrt ::: r =pv / nt) you can set up a proportion of r = r, so that: p(1) * v(1) / n(1) * t(1) = p (2) * v(2) / n(2) * t(2).

With this equation you can plug in what you have (standard temp/pressure on one side, your original conditions on the other --- you will have to set up a proportion with your original data to solve for the number of moles) and solve for v(2).

You're going to have to assume that the number of moles will not change, and make sure that you keep the conditions isolated to a single side of the proportion.

-anonymous

edit: answer my question if you know it! (https://www.physicsforums.com/showthread.php?t=443314)
 
I'm sorry but I didn't understand a thing you said. Can you please explain with the combined gas law formula?
 
He did.

anonymity said:
the equation is:

pv = nrt
 
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