Question

explain the deviation of ideal gas equation​

Answer 1

Answer:

The causes of deviations from ideal behaviour may be due to the following two assumptions of kinetic theory of gases. The volume occupied by gas molecules is negligibly small as compared to the volume occupied by the gas. The forces of attraction between gas molecules are negligible.The two condition at which the gases deviate from ideal behaviour are low temperature and high pressure.

please mark as brainliest!! :) <3

Answer 2

Answer:

Explanation:Answer:

Explanation:From Boyle's law,

V is indirectly proportional to pressure at constant temperature - eqn 1

From Charles law

V is directly proportional to temperature T at constant pressure - eqn 2

From eqn 1 and 2

V=k.T/P

Where k= Proportionality constant

PV=KT- equation 3

In equation 3 "k" is replaced by by another constant known as universal gas constant or molar gas constant. And is denoted by R.

For 1 mole of gas,

PV=RT eqn 4

Where R is universal gas constant or molar gas constant

For n moles of gas,

PV=nRT is called ideal gas eqn.

Where n is number of moles of gas

R is universal gas constant

P is pressure of gas

V is volume of gas

T is temperature of gas in Kelvin scale