The product gas is then passed through a concentrated solution of koh to remove the co2. after passage through the koh solution, the gas contains n2 and is saturated with water vapor. in a given experiment a 0.253-g sample of a compound produced 31.8 ml n2 saturated with water vapor at 258c and 726 torr. what is the mass percent of nitrogen in the compound

The mass percent of nitrogen gas in the compound is 13.3 %

Explanation:

Assuming the chemical equation of the compound forming product gases is:

Now, the product gases are treated with KOH to remove carbon dioxide.

We are given:

So, pressure of nitrogen gas will be =

To calculate the number of moles of nitrogen, we use the equation given by ideal gas which follows:

where,

P = pressure of nitrogen gas = 702.2 torr = 0.924 atm    (Conversion factor: 1 atm = 760 torr)

V = Volume of nitrogen gas = 31.8 mL = 0.0318 L   (Conversion factor:  1 L = 1000 mL)

T = Temperature of nitrogen gas =

R = Gas constant =

n = number of moles of nitrogen gas = ?

Putting values in above equation, we get:

Molar mass of nitrogen gas = 28 g/mol

Moles of nitrogen gas = 0.0012 moles

Putting values in above equation, we get:

Mass of compound = 0.253 g

Mass of nitrogen gas = 0.0336 g

Putting values in above equation, we get:

Hence, the mass percent of nitrogen gas in the compound is 13.3 %

c. heat could easily travel through the molecules in the air and escape/enter the flask. removing the air slows down the heat transfer.  

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