a.) A 2.50 L flask was used to collect a 2.65 g sample of propane gas, . After the sample was collected, the gas pressure was found to be 743 mmHg. What was the temperature of the propane in the flask? ______°C
b.)Butane,C4H10 , is an easily liquefied gaseous fuel. Calculate the density of butane gas at 0.791 atm and 24°C. Give the answer in grams per liter.
Density = ______g/L
c.) A 0.488-g sample of a colorless liquid was vaporized in an evacuated 250.-mL flask at 121°C to give a pressure of 786 mmHg. What is the molecular weight of this substance?
Molecular weight = ______amu
d.)
You fill a balloon with helium gas to a volume of 4.68 L at 23°C and 789 mmHg. What would the volume of helium be if its pressure changed to 632 mmHg but the temperature was unchanged?
_______L
Solution a)
Mass of propane= 2.65 g
Pressure = 743 mm Hg
Let's convert pressure mm Hg into atm.
P = (743/760) atm
= 0.977 atm
Volume = 2.5 L
Mass of propane= 2.65 g
Molar Mass of Propane = C3H8 = 44 g/mol
So, Number of moles of Propane = ( 2.65g ÷ 44 g/mol )
= 0.06 mol
Now, According to the ideal gas,
PV = nRT
or, T = PV / nR
= (0.977 atm X 2.5 L) ÷ ( 0.06 mol X 0.0821 L atm mol-1 K-1)
= 495 K
= (495- 273) oC
= 222 oC
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