Please reference your Chem 101 textbook for the Ideal Gas Law:
pV = nRT
From there you can derive the proper Isobaric Process calculation:
V2 =V1(T2/T1)
Your given are:
V1 = 6.8 L
T2 = 20 ºC
T1 = 0 ºC
But since you cannot divide by Zero, you'd leave it at multiplying 6.8 by 20.
V2 = 136 L
A. 3.15
Chlorine gas occupies a volume of 25 mL at 300K What volume it occupy at 600k
1 mole occupies 22.4 liters. 0.5 moles occupies 11.2 liters at STP.
Standard molar volume of the substance.
A thousand liters Kiloliter A cubic meter occupies the volume of a kiloliter.
1.0 liters
A gas occupies 40.0 L at -123 Celsius. It occupies 80 L of volume at 27 degrees Celsius.
Assuming standard temperature and pressure: 1 mole (64.1 g) of SO2 occupies 22.4 liters 72.0 g SO2 occupies (72.0/64.1) x 22.4 liters
1 mole of gas at STP occupies 22.4 liters.
This is the molar volume of an ideal gas at a given temperature and pressure.
1mol of a gas occupies 24 dm3 at STP, so 2.2mol X 24 mol/dm3 =52.8dm3 or 5280cm3
At STP, 1 mol or 6.02x10^23 representative particles, of any gas occupies a volume of 22.4 Liters. (chemistry)