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Answer:
The total pressure is 890.8 mm Hg
Explanation:
Let's assume all three gases and their mixture behaves ideally.
Hence, according to Dalton's law-
Total pressure = (pressure of Ar) + (pressure of He) + (pressure of nitrogen)
= 0.33 atm + 330 mm Hg + 310 torr
[tex]=(0.33\times 760)mm Hg+330 mmHg+310 mmHg[/tex]
= 890.8 mm Hg
So, the total pressure is 890.8 mm Hg
Considering the Dalton's law, the total pressure of the gas mixture is 890.8 mmHg.
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 exerted by a gaseous mixture is equal to the sum of the pressures that would be exerted by the gases if each were present and occupied the total volume.
In other words, each gas in the mixture acts as if it were alone, so the pressures of each gas that make up a mixture add up:
PT = P₁ + P₂ + ... + Pₙ
In this case, the total pressure will be:
Total pressure = Pressure of Argon + Pressure of Helium + Pressure of Nitrogen
You know that:
- Pressure of Argon= 0.33 atm= 250.8 mmHg (being 1 atm= 760 mmHg)
- Pressure of Helium= 330 mmHg
- Pressure of Nitrogen= 310 torr= 310 torr(being 1 torr= 1 mmHg)
Then, replacing:
Total pressure= 250.8 mmHg + 330 mmHg + 310 mmHg
Solving:
Total pressure= 890.8 mmHg
Finally, the total pressure of the gas mixture is 890.8 mmHg.
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