In vanderwaal equation at const temperature 300 `K, a=14 atm "lt"^(2)"mole"^(2),v=100 ml, n=1` mole, what is pressure of gas:

In vanderwaal equation at const temperature 300K, a=1.4 atm "litre"^(2)"mole"^(2),v=100 ml, n=1 mole, what is pressure of gas:

In van der waals equation at temperature 300k, if a=1.4 atm*L^(-2)*mol^(-2),V=100mL,n=1 mole, then what is the pressure of the gas-

Volume of 1.5 mole of a gas at 1 atm. pressure and 273K is

How many moles of helium at temperature 300K and 1.00 atm pressure are needed to make the internal energy of the gas 100J?

How many moles of helium at temperature 300K and 1.00 atm pressure are needed to make the internal energy of the gas 100J?

How many moles of helium at temperature 300K and 1.00 atm pressure are needed to make the internal energy of the gas 100J?

Two moles of an ideal monoatomic gas occupy a volume 2V at temperature 300K, it expands to a volume 4V adiabatically, then the final temperature of gas is