Deduce Dalton's from kinetic gas equation.

Explanation

Dalton's law of partial pressure: Consider a given mass of gas (l) in a container volume V.
Let number of molecules in the gas =`n_1`,
Mass of each molecule= `m_1`,
RMS velocity =`c_1`
Then according to kinetic gas equation,
`Pressure(P_1)=1/3(m_1n_1c_1^2)/V`
Now, replace gas (1) by gas (2).
Let number of molecules in the gas =`n_2`
Mass of each molecule=`m_2`,
`RMS velocity=c_2`
Then according to kinetic gas equation ,
`Pressure(P_2)=1/3(m_1n_1c_1^2)/V`
Suppose, the two gases are mixed in the same container. Let the total pressure of the gas be P.
Then, `=1/3(m_1n_1c_1^2)/V+1/3(m_1n_1c_2^2)/V`
`therefore P=P_1+P_2` This is Dalton's law of partial pressures.
(i.e.,) At constant termperature , the total pressure exerted by a mixture of gases which do not react chemically with each other is equal to the sum of partial pressures of the individual gases. This is Dalton's law of partial pressures.