Question

For real gases, how does a change in pressure affect the ratio of pv to nrt?

Answer 1

At constant temperature and volume the pressure of a gas is directly proportional to the number of moles of the gas. PV =n RT, where R is the universal gas constant. A change in pressure depends with the number of moles of the gas, such that if the number of moles increases then there are many vibrations and collision of the gas molecules with the walls of a container thus increasing the pressure and vice versa.

Answer 2

Explanation :

From real gas equation

PV = nRT

where,

P is the pressure of the gas

V is the volume of gas

n is the number of moles

R is the gas constant

T is the temperature

According to Gay-Lussac’s law, at constant volume pressure of the gas is directly proportional to the temperature on the Kelvin scale.

so, as pressure increases keeping volume constant then the temperature will also increase.

Hence, on increasing P the ratio of PV to nRT also increases.