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a container holds 6.4 moles of gas. hydrogen gas makes up 25% of the total moles in the container. if the total pressure is 1.24 atm. what is the partial pressure of hydrogen?

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The total pressure of the mixture of gases is equal to the sum of the pressure of each gas as if it is alone in the container. The partial pressure of a component of the mixture is said to be equal to the product of the total pressure and the mole fraction of the component in the mixture.

Partial pressure of hydrogen gas = 1.24 atm x .25 = 0.31 atm
Partial pressure of the remaining = 1.24 atm x (1-.25) = 0.93 atm 

Answer:

0.31 atm

Explanation:

According to the Dalton's law of partial pressure, the total pressure of the gaseous mixture is equal to the sum of the pressure of the individual gases.

Also, the partial pressure of the gas is equal to the product of the mole fraction and total pressure.

Given, for hydrogen gas, it is 25% of the total moles.

So, Mole fraction = 0.25

Total pressure = 1.24 atm

Partial pressure of hydrogen = 0.25 * 1.24 atm = 0.31 atm

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