Answer:
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Explanation:
Answer:
The partial pressure of oxygen in the mixture is 296 mmHg.
Explanation:
The pressure exerted by a particular gas in a mixture is known as its partial pressure. So, Dalton's law states that the total pressure of a gas mixture is equal to the sum of the pressures that each gas would exert if it were alone.
This relationship is due to the assumption that there are no attractive forces between the gases.
So, in this case, the total pressure is:
PT=Phelium + Pnitrogen + Poxygen
You know:
- PT= 756 mmHg
- Phelium= 122 mmHg
- Pnitrogen= 338 mmHg
- Poxygen= ?
Replacing:
756 mmHg= 122 mmHg + 338 mmHg + Poxygen
Solving:
756 mmHg - 122 mmHg - 338 mmHg = Poxygen
Poxygen= 296 mmHg
<u><em>The partial pressure of oxygen in the mixture is 296 mmHg.</em></u>
Answer:
Explanation:
Graham’s Law applies to the diffusion of gases:
The rate of diffusion (r) of a gas is inversely proportional to the square root of its molar mass (M).
If you have two gases, the ratio of their rates of diffusion is
The time for diffusion is inversely proportional to the rate.
Data:
t₂ = 222 s
t₁ = 175 s
M₁ = 28.01
Calculation
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