A mixture of oxygen, hydrogen and eater vapor has a total pressure of 684 mm Hg. The partial pressure of oxygen is 380 mm Hg and that of hydrogen is 0.100 atm. That is the partial pressure of the water vapor?

A mixture of oxygen, hydrogen and water vapor has a total pressure of 684 mm Hg, then the partial pressure of water vapor is 228 mmHg.

What is Dalton's Law?

Dalton's law of gases states that total pressure of the mixture of gases is equal to the sum of the partial pressure of each gases present there, i.e.

P = p₁ + p₂ + p₃, where

P = total pressure of gas = 684 mmHg

p₁ = partial pressure of oxygen = 380 mmHg

p₂ = partial pressure of hydrogen = 0.100 atm = 76 mmHg

p₃ = partial pressure of water vapor = ?

On putting values, we get

p₃ = 684 - (380 + 76)

p₃ = 228 mmHg

Hence required partial pressure of water vapor is 228 mmHg.

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