Need Help... in molar volume, mass, and perent error...?

Question

Hi, I am in 8th grade taking chemistry and need some help and direction on how to start the question below. Your help is really appreaciated.

Question.

A student denteremiend the molar volume of CO2 gas with following data.

Mass of flask, stopper, and air, g (108.812)

Mass of flask, stopper, and CO2, g (180.892)

Volume of flask, L (.144)

Barometric pressure, in. Hg (29.72)

Temperature, C (24)

Density of air at 24.0 C and 29.72 in. Hg, g/ml (1.189 x 10-3)



How do I....

1. calculate the volume, L, of the CO2 sample at STP?
2. calculate the mass of air in the flask?
3. calculate the mass of CO2 in the flask?
4. calculate the molar volume of CO2 at STP?
5. calculate the precent error in answer based on the accepted molar volume of CO2 22.4 L/mol?

Answer 1

PV = nRT

P = pressure
V= volume
n= mass/molar mass of molecule.
R = 0.0821 (Liters.atm/mol.Kelvin)

Also Density = mass/volume

Density is also = [P(MM) / RT]

where MM = molar mass
R the value that I gave you above 0.0821 (Liters.atm/mol.Kelvin)
T is the temperature in Kelvins

Answer 2

Your flask volume or one of your weights seems awful screwed up. Replacing air with CO2 and getting 80 additional grams requires a much larger flask than 0.144 L, being that the difference in weight between CO2 and air is about 15 g/mole, and each mole occupies about 25 liters at 24 deg C.

Answer 3

Your flask quantity or one in each of your weights seems undesirable screwed up. changing air with CO2 and getting 80 extra grams demands a lots extra beneficial flask than 0.a hundred and forty four L, being that the version in weight between CO2 and air is approximately 15 g/mole, and each mole occupies approximately 25 liters at 24 deg C.