Question

Write relation between partial pressure and mole fraction rainly.In

Answer 1

The partial pressure of each gas in a mixture is proportional to its mole fraction. ... Consequently, the total pressure exerted by a mixture of gases is the sum of the partial pressures of the components (Dalton's law of partial pressures).


The total pressure of a mixture of gases can be defined as the sum of the pressures of each individual gas: Ptotal=P1+P2+…+Pn. ... The partial pressure of an individual gas is equal to the total pressure multiplied by the mole fraction of that gas.

Answer 2

Answer: Mole fraction is equal to the ratio of partial pressure to that of total pressure.

Explanation:

The molecules that make up ideal gases are constantly moving in random directions. Because of the molecular collisions with the walls of containers pressure is exerted.

The ratio of the partial pressure of a particular gas to the overall pressure exerted by the gaseous mixture is the mole fraction $(x)$ of that particular gas in a mixture of gases.

$x = \frac{P}{P_{total} }$

Using ideal gas equation for a particular gas:

$PV = nRT$             .....$(1)$

Using Ideal gas equation for a mixture of gases:

$P_{total} V = n_{total} RT$        ....$(2)$

On dividing equation $(1)$ by $(2)$

$\frac{P}{P_{total} } = \frac{n}{n_{total} }$                 .....$(3)$

$x = \frac{n}{n_{total} }$                       .....$(4)$

Now as the mole fraction of a gas is the ratio of number of moles that gas to the total number of moles.

Therefore from equations $(3)$ and $(4)$;

$x = \frac{P}{P_{total} }$

This is the relation between partial pressure and mole fraction.

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