Asked by Nick

I am not quite sure how to do this problem, it doesn't seem to fit into any of my given equations:

A gas has a volume of 35.5L and a pressure of 765mmHg at standard temperature. If the same sample is placed in a 56.0L container and the pressure is measured at 0.92atm, calculate the temperature of the sample in this new container.

I have already converted the .92atm to 699.2mmHg but i don't know where else to go from here. PLEASE HELP!!!
Answered by GK
P1V1/T1 = P2V2/T2
(765mmHg)(35.5L)/273K = (699.2mmHg)(56.0L)/T2

Solve for T2 to get the final temperature in degrees Kelvin. If you need degrees Celsius, use:
C = K - 273
Answered by Nick
How did you find that value for K?
Answered by DrBob222
Standard T is 273 Kelvin (0 degrees C).
Standard pressure is 1 atmosphere or 760 mm Hg.
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