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In this lesson, we will learn how to use the ideal gas law to calculate the molar mass of an ideal gas from its density, temperature, and pressure.
The density of a certain gaseous fluoride of phosphorus is 3.88 g/L at standard temperature and pressure (
, 1.00 bar).
What is the molar mass of this fluoride?
What is the molecular formula of this fluoride?
What is the molar mass of an ideal gas if 0.281 g of the gas occupies a volume of 125 mL at a temperature
and a pressure of 777 torr?
The approximate molar mass of a volatile liquid can be determined by:
What of the following assumptions is not necessary in order to calculate a good estimate of the molar mass from the mass of the vapor?
Using this procedure a sample of chloroform gas weighing
0.494 g is collected in a flask with a
volume of 129 cm3 at
when the atmospheric pressure is 742.1 mmHg.
What is the approximate molar mass of chloroform?
At a temperature of
and a pressure of 0.932 bar, sulfur vapor has a density of 3.71 g/dm3. What molecular formula for sulfur is compatible with this set of conditions?
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