When $16 \, g$ of $O_2$ at $37^\circ C$ is added to $22 \, g$ of $CO_2$ at $27^\circ C$,what will be the final temperature in $^\circ C$?

$A$ closed container contains a homogeneous mixture of two moles of an ideal monatomic gas $(\gamma=5/3)$ and one mole of an ideal diatomic gas $(\gamma=7/5)$. Here,$\gamma$ is the ratio of the specific heats at constant pressure and constant volume of an ideal gas. The gas mixture does a work of $66 \ J$ when heated at constant pressure. The change in its internal energy is . . . . . . $J$.

Considering the gases to be ideal,the value of $\gamma = \frac{C_P}{C_V}$ for a gaseous mixture consisting of $3$ moles of carbon dioxide and $2$ moles of oxygen will be $(\gamma_{O_2} = 1.4, \gamma_{CO_2} = 1.3)$.

$A$ cylindrical container of volume $4.0 \times 10^{-3} \, m^3$ contains one mole of hydrogen and two moles of carbon dioxide. Assume the temperature of the mixture is $400 \, K$. The pressure of the mixture of gases is:
[Take gas constant as $R = 8.3 \, J \, mol^{-1} \, K^{-1}$]

$A$ jar has a mixture of hydrogen and oxygen gas in the ratio of $1 : 5$. The ratio of mean kinetic energies of hydrogen and oxygen molecules is

$A$ gas mixture contains $2$ moles of $O_2$ and $4$ moles of $Ar$. Neglecting vibrational modes,what is the total internal energy of the system at temperature $T$ (in $, RT$)?