a) A sample of carbon dioxide gas collected at a pressure of 1.22 atm and a temp

Question

a) A sample of carbon dioxide gas collected at a pressure of 1.22 atm and a temperature of 9.00 °C is found to occupy a volume of 29.2 liters. How many moles of CO2 gas are in the sample?

_____ mol

b) A 4.69 gram sample of an unknown gas is found to occupy a volume of 2.43 L at a pressure of 907 mm Hg and a temperature of 30°C. The molecular weight of the unknown gas is

_______ g/mol

c) A sample of oxygen gas has a density of __________ g/L at a pressure of 0.644 atm and a temperature of58 °C. Assume ideal behavior.

Explanation / Answer

Assuming ideal gas behavior,

PV = nRT

1.22 x 29.2 = n x 0.082 x 282

n = 1.54 moles ( since volume is L, the R value in L is used)

b). PV = nRT

907 mm Hg 1.19342 atm

n = 0.116 mol

molar mass = weight /number of moles = 4.69 / 0.116 = 40.43 g/mol

c). PV = nRT

PV = (mass/molar mass) RT

density = mass/V = Px molar mass/RT = 0.644 x 32 /0.082x331 = 20.608/27.142 = 0.759 g/L

molar mass of oxygen molecule = 32 g/mole

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