nattycat1105
Answered

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?​

Answer :

anfabba15

Answer:

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

The 1.009 atm should be considered as the total pressure for the mixture.

Calculation of the atmospheric pressure:

here we know that

Sum of partial pressures in a mixture = Total pressure

So,

we need to convert the values from mmHg to atm

So,

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

Now

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

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