10. What is the atmospheric pressure if the partial pressures of nitrogen, oxygen, and

argon are 604.5 mm Hg, 162.8 mm Hg, and 0.500 mm Hg, respectively?

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Chemistry

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27 December, 16:02

10. What is the atmospheric pressure if the partial pressures of nitrogen, oxygen, and

argon are 604.5 mm Hg, 162.8 mm Hg, and 0.500 mm Hg, respectively?

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Answers (1)

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Gina Walker · Answer 1

1.009 atm is the total pressure for the mixture

Explanation:

To determine the total pressure in atm, of the three gases (N₂, O₂ and Ar) we have to sum all the values.

Sum of partial pressures in a mixture = Total pressure

First of all, we need to convert the values from mmHg to atm

604.5 mmHg. 1atm / 760 mmHg = 0.795 atm

162.8 mmHg. 1atm / 760 mmHg = 0.213 atm

0.500 mmHg. 1atm / 760 mmHg = 6.58*10⁻⁴ atm

Partial pressure N₂ + Partial pressure O₂ + Partial pressure Ar = Total P

0.795 atm + 0.213 atm + 6.58*10⁻⁴ atm = 1.009 atm

10. What is the atmospheric pressure if the partial pressures of nitrogen, oxygen, andargon are 604.5 mm Hg, 162.8 mm Hg, and 0.500 mm Hg, respectively?

10. What is the atmospheric pressure if the partial pressures of nitrogen, oxygen, and

argon are 604.5 mm Hg, 162.8 mm Hg, and 0.500 mm Hg, respectively?