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Suppose there is a gaseous mixture of nitrogen and oxygen. If the total pressure of the mixture is 470 mmHg , and the partial pressure of nitrogen is 280 mmHg , calculate the partial pressure of oxygen in the mixture using Dalton's law.

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Answer:

190 mmHg

Explanation:

According to Dalton's law, in a mixture of ideal gases, each gas behaves independently of the other. Also, the total pressure is equal to the sum of the individual partial pressures.

The total pressure of the mixture is 470 mmHg , and the partial pressure of nitrogen is 280 mmHg. Then,

P = pO₂ + pN₂

pO₂ = P - pN₂

pO₂ = 470 mmHg - 280 mmHg

pO₂ = 190 mmHg

The partial pressure of the oxygen in the mixture is 190mmHg.

Given that,

  • The total pressure of the mixture is 470 mmHg, and the partial pressure of nitrogen is 280 mmHg.

Based on the above information, the calculation is as follows:

= Total pressure of the mixture - partial pressure of nitrogen

= 470 - 280

= 190 mmHg

Therefore we can conclude that the partial pressure of the oxygen in the mixture is 190mmHg.

Learn more: brainly.com/question/13145357

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