A sample of oxygen gas was collected via water displacement. Since the oxygen was collected via water displacement, the sample i

Question

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A sample of oxygen gas was collected via water displacement. Since the oxygen was collected via water displacement, the sample i

s saturated with water vapor. If the total pressure of the mixture at 26.4 °C is 805 torr, what is the partial pressure of oxygen? The vapor pressure of water at 26.4 °C is 25.81 mm Hg.

Chemistry

1 answer:

lapo4ka [179] · Answer 1 · 2022-08-17T00:33:03+03:00

Answer : The partial pressure of oxygen is, 799.19 torr

Solution :

According to the Dalton's law, the total pressure of the gas is equal to the sum of the partial pressure of the mixture of gasses.

$P_T=p_{H_2O}+p_{O_2}$

where,

$P_T$ = total partial pressure = 805 torr

$P_{O_2}$ = partial pressure of oxygen gas = ?

$P_{H_2O}$ = partial pressure of water = 25.81 mm Hg = 25.81 torr

Now put all the given values is expression, we get the partial pressure of the oxygen gas.

$805\text{ torr}=25.81\text{ torr}+p_{O_2}$

$p_{O_2}=779.19\text{ torr}$

Therefore, the partial pressure of oxygen gas is, 799.19 torr