Question

Kinetic theory of gases proves:
A.Only Boyle’s law
B.Only Charles’s law
C.Only Avogadro’s law
D.All of these

Answer 1

Hint: For this we must know the statements of all these laws and the ideal gas equation given by kinetic theory of gas. Then we need to check whether each of them satisfy the kinetic equation or not.
Formula used: \[{\text{PV = nRT}}\]
Where \[{\text{P}}\] is pressure, \[{\text{V}}\] is volume, \[{\text{n}}\] is number of moles, \[{\text{R}}\] is universal gas constant and \[{\text{T}}\] is temperature.

Complete step by step answer:
Let us start the equation by defining each of the equation:
Boyle’s law: it states that pressure of gas is inversely proportional to the volume occupied by the gas requires temperature and number of moles remains constant. The expression is:
\[P \propto \dfrac{1}{V}\] Where \[{\text{T}}\] and \[{\text{n}}\] are constant.
Charles’s law: it states that volume of gas is directly proportional to the temperature of gas required pressure and number of moles remains constant. The expression is:
\[V \propto T\] where \[{\text{P}}\] and \[{\text{n}}\] are constant.
Avogadro’s law: it states that equal volume of all gases contain equal number of moles, under similar condition of temperature and pressure.
Now let us check weather each of them follow the ideal gas equation or not:
\[{\text{PV = nRT}}\]
Moving \[{\text{V}}\] to the denominator side we will get \[{\text{P = }}\dfrac{{{\text{nRT}}}}{{\text{V}}}\]. Clearly pressure and volume are inversely proportional to each other and hence Boyle’s law is verified.
In the ideal gas equation, we can see that volume and temperature are directly proportional to each other. Hence Charles’s law is also verified.
Now coming to Avogadro law, it is obvious that when pressure, temperature and volume are equal for two gases , as given in the definition of law then obviously no. of moles of gases will be the same .

Hence, all laws are proved. So, option D is the correct option.

Note:
The ideal gas equation does not imply in real life, because the conditions on which the ideal gas equation works is not found to obey in practical life. It assumes that volume of a molecule of gas is negligible in comparison to the total volume of gas and the interaction between two gas molecules is zero. For that we study real gases.