According to kinetic molecular theory of gases, PV=mnc^2+3 where c=rms velocity of the gas. Now if we create a condition where the rms velocity gets converted to the speed of light then what would happen to this gas? (assumed condition:we can create very high temperatures in laboratory i.e.upto 1,85,25,727k)

Dear Student,

As according to kinetic theorey of gases,
In a gas, which consists of multiple no. of atoms and it would be nearly impossible to know all their speeds,Apart from Average speed, There is another way of determining average speed, as defined by the kinetic theory of gases

μrms = (3RT/M)½
          = (3PV/M)½

μrms = root mean square velocity in m/sec
R = ideal gas constant = 8.3145 (kg·m2/sec2)/K·mol
T = absolute temperature in Kelvin
M = mass of a mole of the gas in kilograms.

If value of rms speed become near to speed of light,then we will replace v(rms) in formula's by c(speed of light),
Although it would be very difficult to achieve this,it will lead to extremely high temperature and also the Pressure*Volume product will become very high.

{A gas could be converted to a plasma state by exposing it to extremely high temperatures.
Heating matter to high temperatures causes electrons to leave the atoms, resulting in the presence of free electrons. At very high temperatures, such as those present in stars, it is assumed that essentially all electrons are "free", and that a very high-energy plasma is essentially bare nuclei swimming in a sea of electrons.

It could happen at temperature range,mentioned by you}

Hope this information will clear your doubts about topic.

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in this question the kinetic gas eq is PV=mnc^2/3....
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