0. 820 mole of hydrogen gas has a volume of 2. 00 l at a certain temperature and pressure. What is the volume of 0. 125 mol of t
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<u>Answer:</u> The mass percent of nitrogen gas in the compound is 13.3 %
<u>Explanation:</u>
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:
- To calculate the mass of nitrogen gas, we use the equation:
Molar mass of nitrogen gas = 28 g/mol
Moles of nitrogen gas = 0.0012 moles
Putting values in above equation, we get:
- To calculate the mass percent of nitrogen gas in compound, we use the equation:
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 %