Question:
The mole fraction of dioxygen in a neon-dioxygen mixture is $0.18$. If the total pressure of the mixture is $25$ bar, the partial pressure of neon in the mixture would be
The mole fraction of dioxygen in a neon-dioxygen mixture is $0.18$. If the total pressure of the mixture is $25$ bar, the partial pressure of neon in the mixture would be
Updated On: May 12, 2024
- $25.18\, bar$
- $25.82\, bar$
- $4.5\, bar$
- $20.5\, bar$
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The Correct Option is D
Solution and Explanation
Given $P_{total}$ = 25 bar,
$ x_{O_2} = 0.18 $
$\therefore \:\:\: x_{Ne} = 1 - 0.18 = 0.82$
$ p_{Ne} = x_{Ne} \times P_{total} = 0.82 \times 25 = 20.5 bar$
$ x_{O_2} = 0.18 $
$\therefore \:\:\: x_{Ne} = 1 - 0.18 = 0.82$
$ p_{Ne} = x_{Ne} \times P_{total} = 0.82 \times 25 = 20.5 bar$
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Concepts Used:
Partial Pressure
Partial Pressure is defined as if a container filled with more than one gas, each gas exerts pressure. The pressure of anyone gas within the container is called its partial pressure.
Dalton’s Law of Partial Pressure:
According to Dalton’s law of partial pressures, the total pressure exerted by the mixture of gases is the sum of the partial pressure of every existing individual gas, and every gas is assumed to be an Ideal gas.
Ptotal = P1 + P2 + P3 …
Where P1, P2, P3 are the partial pressures of gas 1, gas 2, and gas 3. Since every gas has an independent behavior, the ideal gas law is used to find the pressure of that gas if its number of moles, the volume of container and temperature is known.