On a humid day in summer, the mole fraction of gaseous H2 O (water vapor) in the air at 25^∘ C c

step 1 So in this question, we're told that the mole fraction of water vapor in the air is 0 .287 or ab

On a humid day in summer, the mole fraction of gaseous H2 O...

On a humid day in summer, the mole fraction of gaseous $\mathrm{H}_{2} \mathrm{O}$ (water vapor) in the air at $25^{\circ} \mathrm{C}$ can be as high as 0.0287 . Assuming a total pressure of 0.977 atm, what is the partial pressure in atmospheres of $\mathrm{H}_{2} \mathrm{O}$ in the air?

On a humid day in summer, the mole fraction of gaseous $\mathrm{H}_{2} \mathrm{O}$ (water vapor) in the air at $25^{\circ} \mathrm{C}$ can be as high as 0.0287 . Assuming a total pressure of 0.977 atm,
what is the partial pressure in atmospheres of $\mathrm{H}_{2} \mathrm{O}$ in the air?

Key Concepts

Dalton's Law of Partial Pressures

Dalton's Law of Partial Pressures is a fundamental principle in gas mixtures which states that the total pressure exerted by a mixture of non-reacting gases is equal to the sum of the pressures that each gas would exert if it occupied the volume alone. This concept is critical in determining the behavior of each individual gas component in a mixture and allows for the calculation of a gas's partial pressure using its fraction of the total quantity in the mixture.

Mole Fraction

The mole fraction is a dimensionless quantity that represents the ratio of the number of moles of a particular gas to the total number of moles present in a mixture. It is an essential concept when calculating the contribution of each gas to the total pressure in a mixture, as it directly relates to how much pressure each gas exerts under the conditions of the system.

Total Pressure

Total pressure refers to the overall pressure exerted by all gases in a mixture combined. It is the sum of the partial pressures of each individual gas present in the system. This concept serves as a baseline value for calculating the partial pressures of individual gases using their respective mole fractions.

Partial Pressure

Partial pressure is the hypothetical pressure that a single component of a gas mixture would exert if it were alone in the container at the same temperature. It is calculated by multiplying the mole fraction of the component by the total pressure. This concept is crucial for understanding the behavior of gases in various processes, including chemical reactions and physical phenomena involving gas mixtures.

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