Question

A mixture of three gases has a total pressure at 298 K of 1560 mm Hg. the mixture is analyzed and is found to contain 1.50 mol Ne, 2.65 mol Ar, and 1.75 mol Xe. What is the partial pressure of Xe?

Answer 1

Answer:

the partial pressure of Xe is 452.4 mmHg

Explanation:

Dalton's law of partial pressures says that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of the individual gases.

The partial pressures can be calculated with the molar fraction of the gas, in this case, Xe.

Molar fraction of Xe is calculated as follows:

$x_{Xe}=\frac{n_{Xe} }{n_{t} }$

$x_{Xe}=1.75/5.9\\x_{Xe}=0.29$

Then, 0.29 is the molar fraction of Xe in the mixture of gases given.

To know the parcial pressure of Xe, we have to multiply the molar fraction by the total pressure:

Partial Pressure of Xe=1560mmHg*0.29

Partial Pressure of Xe=452.4mmHg