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A mixture of `N_2 ` and `O_2` gases are in a 2.0L container at 23 degrees C and at a...
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From Dalton's law of partial pressures we know,
Where P is the total pressure, `P_i` is the partial pressure of the ith component, and `x_i` , its mole-fraction.
Applying the concept of mole-fraction for a binary gas mixture,
Agan, assuming ideal behaviour, total number of moles of gaseous species `(n_(O_2)+n_(N_2))`
Putting the value of `n_(O_2)` ,
Mass of `N_2` = number of moles of `N_2` * molar mass of `N_2`
Therefore, mass of `N_2` present in the gas mixture was 2.14 g.
Posted by llltkl on August 10, 2013 at 6:26 PM (Answer #1)
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