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Deep-sea divers use a breathing mixture of helium, oxygen, and carbon dioxide. What is the partial pressure of oxygen if the total pressure of the mixture is 760 mm Hg, the pressure exerted by the helium is 609 mm Hg, and the pressure exerted by the carbon dioxide is 1 mm Hg?
A
760 mm Hg

B
500 mm Hg

C
150 mm Hg

D
609 mm Hg

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dsdrajlin

A gaseous mixture (760 mmHg) containing helium (609 mmHg), carbon dioxide (1 mmHg) and oxygen (C. 150 mmHg).

What does Dalton's law of partial pressures state?

Dalton's law of partial pressures states that the total pressure of a mixture of gases is equal to the sum of the partial pressures of the component gases.

A gaseous mixture with a total pressure of 760 mmHg contains Helium (609 mmHg), carbon dioxide (1 mmHg) and oxygen. We can calculate the partial pressure of oxygen using Dalton's law.

P = pHe + pCO₂ + pO₂

pO₂ = P - pHe - pCO₂

pO₂ = 760 mmHg - 609 mmHg - 1 mmHg = 150 mmHg

where,

  • P is the total pressure.
  • pHe is the partial pressure of helium.
  • pCO₂ is the partial pressure of carbon dioxide.
  • pO₂ is the partial pressure of oxygen.

A gaseous mixture (760 mmHg) containing helium (609 mmHg), carbon dioxide (1 mmHg) and oxygen (C. 150 mmHg).

Learn more about Dalton's law here: https://brainly.com/question/14119417

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