At $0\, ^\circ C$,$4\, g$ of $O_2$ and $2\, g$ of $H_2$ are filled in a $1\, L$ bulb. What will be the total pressure of the mixture (in $, atm$)?

The mathematical form of Charles's law is given by $V_{t} = V_{0} \left( \frac{273.15 + t}{273.15} \right)$. Using this equation,explain the relationship between volume $(V)$ and temperature $(T)$ in Kelvin.

What is the temperature of $4$ moles of a gas occupying $5 \ L$ volume at $3.32 \ bar$ (in $K$)? $\left(R=0.083 \ bar \ L \ K^{-1} \ mol^{-1}\right)$

At a given temperature,the density of gas $x$ is twice that of gas $y$. The molar mass of $x$ is one-third of the molar mass of $y$. What is the ratio of their pressures $(P_x / P_y)$?

If $4 \ g$ of $O_2$ and $2 \ g$ of $H_2$ are filled in a $1 \ L$ bulb at $0 \ ^oC$,the total pressure of the mixture will be...... (in $atm$)

What is the density of carbon monoxide at $STP$ in $g \, L^{-1}$?