Gaseous Laws and Ideal Gas Equation

In a closed flask of 5 litres, 1.0 g of  ${\mathrm{H}}_2$ is heated from 300 K to 600 K. Which statement is not correct?

A bubble of air is underwater at temperature  ${15}^{o}C$ and the pressure 1.5 bar. If the bubble rises to the surface where the temperature is  $\mathrm{}\mathrm{}25°C$ and the pressure is 1.0 bar, what will happen to the volume of the bubble?

Cyclopropane and oxygen at partial pressures $170$ torr and $570$ torr respectively are mixed in a gas cylinder. What is the ratio of the number of moles of cyclopropane to the number of moles of oxygen  $\left(\frac{{\mathrm{nC}}_3{\mathrm{H}}_6}{{\mathrm{nO}}_2}\right)?$ (Assume no reaction).

Under what conditions will a pure sample of an ideal gas not only exhibit a pressure of $1 \mathrm{atm}$ but also a concentration of $1 \mathrm{mole} {\mathrm{L}}^{-1}$?

$(\mathrm{R}=0.082 \mathrm{L}\mathrm{atm}{\mathrm{mol}}^{-1}{\mathrm{deg}}^{-1})$

The correct value of the gas constant is close to:

If $\mathrm{P}, \mathrm{V}, \mathrm{M}, \mathrm{T} \mathrm{and} \mathrm{R}$ are pressure, volume, molar mass, temperature and gas constant respectively, then for an ideal gas, the density is given by

If $P,V,M, T \mathrm{and} R$ are pressure, volume, molar mass, temperature and gas constant respectively, then for an ideal gas, the density is given by

Calculate the number of molecules in one litre of an ideal gas at $136.5°\mathrm{C}$ temperature and $3 \mathrm{atm}$ pressure.

A vertical hollow cylinder of height $152 \mathrm{cm}$ is fitted with a weightless piston. The lower half is filled with an ideal gas and the upper half with mercury. The cylinder is now heated at $300 \mathrm{K}$ , so that $1/4^{\mathrm{th}}$ of the mercury comes out. Find the temperature at which it will happen assuming thermal expansion of $\mathrm{Hg}$ to be negligible. (Give your answer up to two decimal)

Which one of these graphs for an ideal gas, the arrow indication is incorrectly marked? 

A balloon contains $400 {\mathrm{m}}^3$ of hydrogen. If the mass of the balloon without hydrogen is $34 \mathrm{kg}$, its net lifting ability is (density of hydrogen $=0.09{\mathrm{kgm}}^{-3}$, density of air =$1.3{\mathrm{kgm}}^{-3}$)

A mixture of ${\mathrm{H}}_2\mathrm{O} ,{\mathrm{CO}}_2$​ and ${\mathrm{N}}_2$​ are trapped in a glass apparatus with a volume of $0.731 \mathrm{mL}$. The pressure of total mixture was $1.74\mathrm{mm}$ of Hg at $23°\mathrm{C}$. The sample was transferred to a bulb in contact with dry ice($-75°\mathrm{C}$) so that $\mathrm{H}2\mathrm{O}\left(\mathrm{v}\right)$ are frozen out. When the sample returned to the normal value of temperature, the pressure was $1.32\mathrm{mm}$ of Hg. The sample was then transferred to bulb in contact with liquid ${\mathrm{N}}_2(-75°\mathrm{C})$ to freeze out ${\mathrm{CO}}_2$​. In the measured volume, the pressure was $0.53\mathrm{mm}$ of Hg at original temperature. Mole of ${\mathrm{N}}_2$​ in mixture are $2.1\times {10}^{-\mathrm{y}}$.
So, the value of $\mathrm{y}$ is......(as nearest integer)

The density of air at $25°\mathrm{C} \mathrm{and} 1 \mathrm{atm} \mathrm{is} 1·3 \mathrm{g}/\mathrm{L}$. Calculate the partial presser of ${\mathrm{N}}_2$ gas assuming that air contains only ${\mathrm{N}}_2 \mathrm{and} {\mathrm{O}}_2$ gases.

The density of the gaseous mixture in a vessel $\left({\mathrm{N}}_2\mathrm{ }\mathrm{and}\mathrm{ }\mathrm{He}\right)$ at 2.1 atmosphere and 310 K is 1.35 g/litre. If a small pin-hole is made on the wall of the vessel, through which gases effuse, then which of the following is the correct composition of the gases He and ${\mathrm{N}}_2$   effusing out initially?

A $10.0 \mathrm{L}$ flask contains $64 \mathrm{g}$ of oxygen at $27°\mathrm{C}$. (Assume ${\mathrm{O}}_2$ gas is behaving ideally). The pressure inside the flask in bar is

(Given $\mathrm{R}=0.0831 \mathrm{L} \mathrm{bar} {\mathrm{K}}^{-1}{ \mathrm{mol}}^{-1}$)

A bulb of constant Volume is attached to a very thin manometer tube as shown in the figure. Gas starts leaking through a small hole in the bulb causing change in pressure as $\frac{\mathrm{dp}}{\mathrm{dt}}=-{\mathrm{kP}}^2$:

Where $\mathrm{k}$ is constant and $P$ is pressure at any instant.

Initial height difference '$\mathrm{h}$' was $76 \mathrm{cm}$ and after $10{ \min }^{\text{'}}{\mathrm{h}}^{\text{'}}$ was $38 \mathrm{cm}$. Then the value of $\mathrm{k}$ in ${\mathrm{atm}}^{-1} {\mathrm{hr}}^{-1}$

Select the incorrect statement(s):

Internal energy of $n_1$ mol of hydrogen of temperature $T$ is equal to the internal energy of $n_2$ mol of helium at temperature $2T$. The value of $\frac{10n_1}{n_2}$ is

At STP, $5.6$ litre of a gas weighs $60\mathrm{ }\mathrm{g}$. The vapour density of gas is -

Calculate the number of hours (up to the nearest integer) of service that can be derived at $1 \mathrm{atm}$, $\mathrm{300 }\mathrm{K}$ from an acetylene lamp containing $640\mathrm{ }\mathrm{g}$ calcium carbide. Given that the lamp requires $50\mathrm{ }\mathrm{L}$ acetylene gas at $1 \mathrm{atm}$, $\mathrm{300 }\mathrm{K}$ for one hour. [Take $0.0821\mathrm{ }\times \mathrm{ }300=\mathrm{25]}$