An ideal gas has an initial pressure of 1216 mmhg at T=-23 degrees celsius and occupies a volume of 400 mL.
What is the final temperature of the gas (in degrees Kelvin) if it occupies 1.20 liters at P=0.80 ATM?
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Initial pressure , P1 = 1216 mmHg = 1.6 atm
Initial tepmerature, T1 = -23 C = 250 K
Initial volume, V1 = 0.4 litres
Final pressure , P1 = 0.8 atm
Final tepmerature, T1 = ???
Final volume, V1 = 1.2 litres
For an ideal gas, PV = nRT
nR = PV/T
for two cases,
nR = P1V1/T1 = P2V2/T2
(1.6 x 0.4 / 250) = (0.8 x 1.2/T2)
Here, you dont need to worry about the units because they will cancel out.
T2 = 375 K.
The final temperature of gas is 375 K
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