Assuming ideal gas behavior,what is the number of moles of $0.224 \ L$ of hydrogen gas at $STP$ $(273 \ K, 1 \ atm)$?

Pressure of $1 \ g$ ideal gas $X$ at $300 \ K$ is $2 \ atm$. When $2 \ g$ of another gas $Y$ is introduced in the same vessel at the same temperature,the total pressure becomes $3 \ atm$. The correct relationship between molar masses of $X$ and $Y$ is:

For one mole of an ideal gas, the slope of $V$ vs. $T$ curve at a constant pressure of $2 \ atm$ is $X \ L \ mol^{-1} \ K^{-1}$. The value of the ideal universal gas constant '$R$' in terms of $X$ is

Which of the following graphs is correct for an ideal gas?

$A$ 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?

If two moles of an ideal gas at $546 \ K$ occupy a volume of $44.8 \ L$,what is the pressure of the ideal gas at $546 \ K$ (in $atm$)? $(R = 0.0821 \ L \ atm \ mol^{-1} \ K^{-1})$