`2` moles of a monoatomic gas are expanded to double its initial volume, through a process `(P)//(V) =` constant. If its initial temperature is `300 K`, then which of the following is not true.

I mole of an ideal monoatomic gas is expanded till the temperature of the gas is doubled under the process V^(2)T=contant . The initial temperature of the gas is 400K . In terms of R find total work done in the process.

What is the change in enthalapy (kcal) when 1 mole of ideal monoatomic gas is expended reversibly and adibatically from initial volume of 1 L and initial temperature 300 K to final volume of 8 L :

A monoatomic gas is compressed adiabatically to 8/27 of its initial volume, if initial temperature is 27^° C, then increase in temperature

An ideal gas undergoes an adiabatic process obeying the relation PV^(4//3) = constant. If its initial temperature is 300 K and then its pressure is increased upto four times its initial value, then the final temperature (in Kelvin):

A gas enclosed in a cylinder is expanded to double its initial volume at a constant pressure of one atmosphere . How much work is done in this process ?

2 mole of an ideal monoatomic gas undergoes a reversible process for which PV^(2)=C . The gas is expanded from initial volume of 1 L to final volume of 3 L starting from initial temperature of 300 K. Find DeltaH for the process :

2 mole of an ideal monoatomic gas undergoes a reversible process for which PV^(2)=C . The gas is expanded from initial volume of 1 L to final volume of 3 L starting from initial temperature of 300 K. Find DeltaH for the process :

2 mole of an ideal monoatomic gas undergoes a reversible process for which PV^(2)=C . The gas is expanded from initial volume of 1 L to final volume of 3 L starting from initial temperature of 300 K. Find DeltaH for the process :

A monoatomic gas is compressed adiabatically to (8)/(27) of its initial volume if initial temperature is 27^@C , find increase in temperature