Measurable Properties of Gases

The temperature increases, the intermolecular forces of the gas molecules

$6$ atmosphere = $\mathrm{X}$ torr of $\mathrm{Hg}$. Here $\mathrm{X}$ is

A desiccator of internal volume of $1 \mathrm{L}$ and containing nitrogen at $1 \mathrm{atm}$ pressure is partially evacuated to a final pressure of $7.6 \mathrm{mmHg}$, while the temperature remains constant. What is the volume of the gas in litre at this stage?

The pressure exerted by the gas is due to

Kinetic energy of a gas

Which description fits best for a gas?

A sample of ${\mathrm{O}}_2$ gas is collected over water at $23 °\mathrm{C}$ at a barometric pressure of $751 \mathrm{mm} \mathrm{of} \mathrm{Hg}$ (vapour pressure of water at $23 °\mathrm{C}$ is $21 \mathrm{mm} \mathrm{of} \mathrm{Hg}$). The partial pressure of${\mathrm{O}}_2$  gas in the sample collected is

A 10 cm column of air is trapped by a column of Hg, 8 cm long, in a capillary tube horizontally fixed as shown below, at 1 atm pressure.

What is the pressure of air $\left(\mathrm{cm}\right)$ when the tube is held horizontally at ${45}^{°}$ with the open end up?

A 10 cm column of air is trapped by an 8 cm long column of Hg in a capillary tube horizontally fixed as shown in the figure at 1 atm pressure.The pressure of air measured when a tube is held vertically with the open end up is:

Air separated from the atmosphere by a column of mercury of length $h=15 \mathrm{cm}$ is present in a narrow cylindrical soldered at one end. When the tube is placed horizontally the air occupies a volume $V_1=250 {\mathrm{mm}}^3$. When it is set vertically with its open end upwards the volume of the air is $V_2=200 {\mathrm{mm}}^3$. The atmospheric pressure during the experiment is $x \mathrm{cm} \text{of} \mathrm{Hg}$. Find $x$.

What would be the height of a barometer column for one standard atmosphere, if water were used instead of mercury?

A bubble of gas released at the bottom of a lake increases to eight times its original volume when it reaches the surface. Assuming that atmospheric pressure is equivalent to the pressure exerted by a column of water, 10 m height, the depth of the lake is:

An air column closed in a tube sealed at one end by a $\mathrm{H}\mathrm{g}$ column having height $\mathrm{h}$. When the tube is placed with open ends down, the height of the air column is ${\mathcal{l}}_1$. If the tube is turned so that its open end is at the top, the height of the air column is ${\mathcal{l}}_2$. What is the atmospheric pressure $\left({\mathrm{P}}_0\right)$-

A gas is present in a cylinder fitted with movable piston. Above and below of the piston there is an equal number of moles of gas. The volume above is two times the volume below at a temperature of $300\mathrm{K}$. At what temperature will the volume above be four times the volume below-

At constant volume, for a fixed number of moles of a gas, the pressure of the gas increases with rise of temperature due to

When a capillary tube of diameter $0.8 \mathrm{mm}$ is dipped in a liquid having a density of $800 \mathrm{kg}$ ${\mathrm{m}}^{-3},$ then the height of the liquid in the capillary tube rises to $4 \mathrm{cm}$. The surface tension of the liquid is

A bulb of constant volume is attached to a manometer tube open at another end as shown in the figure. The manometer is filled with a liquid of density ${\left(\frac{1}{3}\right)}^{\text{rd}}$ that of mercury. Initially, $\mathrm{h}$ was $456 \mathrm{cm}$.



Through a small hole in the bulb, gas is leaked. Assuming, pressure decreases as $\frac{\text{dp}}{\text{dt}}=-\text{KP}$, if the value of $\mathrm{h}$ is $228 \mathrm{cm}$ after $28 \mathrm{minutes}$. What is the value of $\mathrm{K}$ $\left({\text{in hour}}^{-1}\right)$? $\left\{\text{Take log}\frac{57}{38}=\text{0.28 and density of Hg}={\text{13.6 g mL}}^{-1}\right\}$

A bulb that has constant volume is attached to a manometer tube open at the other end, as shown in the diagram. The manometer is filled with a liquid of density $(1/3{)}^{\mathrm{rd}}$ that of mercury. Initially, $\text{'h'}$ $228 \mathrm{cm}.$was 228 cm.


Through a small hole in the bulb, gas leaked assuming pressure decreases as $\frac{\text{dp}}{\text{dt}}=-\text{kP}$. If the value of $\text{'}\mathrm{h}\text{'}$ is $114 \mathrm{cm}$ after $14 \mathrm{minutes}$. What is the value of $\mathrm{k} (\mathrm{in} {\mathrm{hour}}^{-1})$ ?

[Use: ln$(4/3)=0.28$ and density of $\mathrm{Hg}=13.6 \mathrm{g} {\mathrm{mL}}^{-1}$].

An open manometer attached to a flask containing ammonia gas have no difference in mercury level initially as shown in diagram. After sparking into the flask, ammonia is partially dissociated as $2{\text{NH}}_3\left(\text{g}\right)⟶{\text{N}}_2\left(\text{g}\right)+3{\text{H}}_2\left(\text{g}\right)$. Now it have difference of $\text{18}\text{cm}$ in mercury level in two columns, what is partial pressure of ${\text{H}}_{\text{2}}\left(\text{g}\right)$ at equilibrium ?

The system shown in the diagram is at equilibrium at  $27^{\circ }c$And volume of the bulb is 150 mL.  At this temperature, the vapor pressure of water is 28 millimeters of mercury.  If,the bulb contains 0.001 mol of O₂ (g), volume of the liquid water is approximately.