A mixture of `N_2 ` and `O_2` gases are in a 2.0L container at 23 degrees C and at a total pressure of 1.00 atm. The partial pressure of O2 was .0722 atm. How many grams of `N_2 ` were in the gas mixture?
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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.
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