Find the temperature in $^\circ C$ for a $6.4 \ g$ $O_2$ gas filled in a $200 \ mL$ vessel having pressure $50 \ bar$. $[R = 8.314 \times 10^{-2} \ bar \ L \ K^{-1} \ mol^{-1}]$ (in $^\circ C$)

In a closed vessel,an ideal gas at $1 \, atm$ is heated from $27^{\circ} C$ to $327^{\circ} C$. The final pressure of the gas will approximately be $..... \, atm$

Pressure of $1 \, g$ of an ideal gas $A$ at $27^{\circ} C$ is found to be $2 \, bar$. When $2 \, g$ of another ideal gas $B$ is introduced in the same flask at the same temperature,the pressure becomes $3 \, bar$. Find a relationship between their molecular masses.

For $0.09 \, \text{mol}$ of $CO_2$ at $300 \, K$,the volume is $112.0 \times 10^{-3} \, m^3$ at a pressure of $2.0 \times 10^4 \, Pa$. What will be the volume at a pressure of $4.0 \times 10^4 \, Pa$?

At $27^{\circ} C$,$1 \ L$ of $H_2$ with a pressure of $1 \ bar$ is mixed with $2 \ L$ of $O_2$ with a pressure of $2 \ bar$ in a $10 \ L$ flask. What is the pressure exerted by the gaseous mixture in $bar$? (Assume $H_2$ and $O_2$ as ideal gases)

Calculate the new pressure of a gas enclosed in a cylinder when it is compressed from $5 \text{ L}$ to $2 \text{ L}$ at an initial pressure of $1 \text{ atm}$ and temperature of $300 \text{ K}$. The final temperature in this process is $500 \text{ K}$. (in $\text{ atm}$)