The volume versus temperature graph of $1 \ mole$ of an ideal gas is given below. The pressure of the gas (in $atm$) at $X, Y$ and $Z$,respectively,are

At $0\, ^\circ C$ and $1\, atm$ pressure,a gas occupies $100\, cc$. If the pressure is increased to $1.5$-times and temperature is increased by one-third of its absolute temperature,then the final volume of the gas will be .............. $cc$.

At constant temperature, a gas occupies a volume of $200 \text{ mL}$ at a pressure of $500 \text{ mm Hg}$. What will be its volume at $800 \text{ mm Hg}$ pressure (in $\text{ mL}$)?

The graph of $V$ versus $T$ for an ideal gas at constant pressures $P_1$ and $P_2$ is shown below. Which of the following is correct?

When $5 \, g$ of $XeF_4$ gas is filled in a $6 \, L$ container at $80 \, ^oC$,the pressure exerted by the gas will be ......... $atm$.

The isobars of one mole of an ideal gas were obtained at three different pressures ($p_1$, $p_2$ and $p_3$). The slopes of these isobars are $m_1$, $m_2$ and $m_3$ respectively. If $p_1 < p_2 < p_3$, then the correct relation of the slopes is