At a constant temperature,by what percentage $(\%)$ must the pressure of a given mass of gas be increased so that its volume decreases by $10\%$ (in $.1$)?

At $0\,^{\circ}\text{C}$,the value of the density of a fixed mass of an ideal gas divided by its pressure is $x$. At $100\,^{\circ}\text{C}$,this value will be

The number of molecules in a gas at pressure $1.64 \times 10^{-3} \text{ atm}$ and temperature $200 \text{ K}$ having the volume $1 \text{ cc}$ is:

$A$ sample of an ideal gas occupies a volume $V$ at a pressure $P$ and absolute temperature $T,$ the mass of each molecule is $m.$ The expression for the density of gas is ($k =$ Boltzmann's constant)

An ideal gas is initially at temperature $T$ and volume $V.$ Its volume is increased by $\Delta V$ due to an increase in temperature $\Delta T,$ pressure remaining constant. The quantity $\delta = \Delta V / (V \Delta T)$ varies with temperature as

We have a jar filled with gas characterized by parameters $P, V, T$ and another jar $B$ filled with gas having parameters $2P, V/4, 2T$,where symbols have their usual meaning. The ratio of the number of molecules in jar $A$ to those in jar $B$ is