Quote:
Originally Posted by WDE46
I don't know where you got this number. Did you assume a 1 atm starting point at 25C for this and calculate the change in pressure given the same volume but higher temperature?
I mean did you do: P1/T1 = P2/T2

I used ideal gas law: PV=nRT. V is the volume, n is the amount of air that occupies the V. R is the gas constant, and T is temperature. Air is an ideal gas.
One also needs to know that 1 mole of gas occupies 22.4 L of space. No need to assume a starting point. Just plug in the numbers and solve for P.
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