Two perfect monoatomic gases at absolute temperature `T_(1)` and `T_(2)` are mixed. There is no loss of energy. Find the temperature of the mixture if the number of moles in the gases are` n_(1)` and `n_(2)`.

Two perfect gases at absolute temperature T_(1) and T_(2) are mixed. There is no loss of energy. The masses of the molecules are m_(1) and m_(2) . The number of molecules in the gases are n_(1) and n_(2) . The temperature of the mixture is

Two perifect gases at absolute temperatures T_(1) and T_(2) are mixed. The absolute temperature of the mixture is T. there is no loss of energy.If m_(1) and m_(2) are masses of molecules and n_(1) and n_(2) are number of molecules, then

Three perfect gases at absolute temperature T_(1), T_(2) and T_(3) are mixed. The masses f molecules are m_(1), m_(2) and m_(3) and the number of molecules are n_(1), n_(2) and n_(3) respectively. Assuming no loss of energy, the final temperature of the mixture is

Three perfect gases at absolute temperature T_1,T_2, and T_3 are mixed. The masses of molecules are n_1,n_2 and n_3 respectively. Assuming to loss of energy, the final temperature of the mixture is:

Two monoatomic gases are at absolute temperatures 300 K and 350 K respectively. Ratio of average kinetic energy of their molecules is

n_(1) and n_(2) moles of two ideal gases (mo1 wt m_(1) and m_(2)) respectively at temperature T_(1)K and T_(2)K are mixed Assuming that no loss of energy the temperature of mixture becomes .

Two ideal polyatomic gases at temperature T_(1) and T_(2) are mixed so that there is no loss of energy . If F_(1) and F_(2), m_(1) and m_(2) ,n_(1) and n_(2) be the degrees of freedom, masses, number of molecules of the firest and second gas respectively, the temperature of mixture of these two gases is :