Question

if within a mixture of gases, hydrogen exerts a partial pressure of 200 torr, and hydrogen has a mole fraction of 0.25, what is the total pressure of the mixture of gases?

Answer 1

Using Dalton's Law of Partial Pressures and the given mole fraction, the total pressure of the gas mixture where hydrogen has a partial pressure of 200 torr and a mole fraction of 0.25 is calculated to be 800 torr.

Step-by-step explanation:

To find the total pressure of a mixture of gases when the partial pressure of hydrogen is given as 200 torr and its mole fraction is 0.25, we can use Dalton's Law of Partial Pressures.

This law states that the total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of individual gases. The partial pressure of a gas is the pressure it would exert if it occupied the whole volume on its own.

Since we know the partial pressure of hydrogen and its mole fraction, we can calculate the total pressure of the gas mixture by dividing the partial pressure of hydrogen by its mole fraction.

The formula to calculate the total pressure (PTotal) is given by:

PHydrogen = XHydrogen × PTotal

Isolating for PTotal we get:

PTotal = PHydrogen / XHydrogen

By substituting the given values, we find:

PTotal = 200 torr / 0.25

= 800 torr

The total pressure of the gas mixture is therefore 800 torr.