$A$ gas obeys Charles's law in the temperature range $0-500 \ K$ at a given pressure. Its volume changes to zero at a temperature of:

Dalton's law of partial pressure will not apply to which of the following mixtures of gases?

$A$ plot of volume $(V)$ of the gas versus temperature ($T$ in $K$) is shown below. Which of the following options is correct for the plot?

Which of the following gases of the same mass exerts the highest pressure at a constant temperature?

Two separate identical containers contain Gas $A$ $(Mw = 40 \ g \ mol^{-1})$ and gas $B$ $(Mw = x \ g \ mol^{-1})$ in the mass ratio $5 : 8$ under similar conditions of temperature and pressure. The value of $x$ is $:-$

At a temperature of $300 \ K$,if the pressure of $0.09 \ mol$ of a gas is halved,what will be its volume?