If 3.37 m3 of a gas initially at STP is placed under a pressure of 2.30 atm , the temperature of the gas rises to 33.0 ?C. What is the volume?
Using PV = nRT
The gas is going to retain the same number of molecules, and the
constant R remains the same, so:
=
n and R cancel out for the previously explain reason; so you have P1V1/T1 = P2V2/T2
STP is defined as 273K (0 C) and 100kPa (or 10^5 Pa)
1 atm = 1.013 x 10^5 Pa
No conversion necessary for m^3
Substituting: (100,000)(3.37)/ 273 = (2.30 x 101,300)(V2) / (273 + 33)
(V2) = 1234.43 / 761.40
(V2) = 1.621 m3
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