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).

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

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?

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 -

Consider one mole of a gas in a closed vessel fitted with a movable piston. At constant temperature $\left(\mathrm{T}\right)$, the pressure of the gas $\left(\mathrm{P}\right)$ is increased gradually and the volume $\left(\mathrm{V}\right)$ is noted. The resulting $P-V$ isotherm (not drawn to scale) is given below.

The correct plot (not drawn to scale) of the number of moles of the substance in gas phase $\left(n_{\mathrm{G}}\right)$ against $V$ or $P$ is:

Consider the chemical equilibrium $\mathrm{A}\left(\mathrm{s}\right)\rightleftharpoons \mathrm{B}\left(\mathrm{s}\right)+\mathrm{C}\left(\mathrm{g}\right)$inside a vessel fitted with a movable piston at temperature $\mathrm{T}$. The correct plot corresponding to volume change (assuming ideal gas behavior) is

A thermally insulated vessel is partitioned into two compartments by a fixed diathermal (heat conducting) wall and each compartment contains certain amount of ideal gas. The temperature, pressure, volume, number of moles, entropy of the gases in the first and second compartments are denoted by ${\mathrm{T}}_1,{\mathrm{P}}_1,{\mathrm{V}}_1,{\mathrm{n}}_1,{\mathrm{S}}_1$ and ${\mathrm{T}}_2,{\mathrm{P}}_2,{\mathrm{V}}_2$, ${\mathrm{n}}_2,{\mathrm{S}}_2$, respectively. Initially, ${\mathrm{T}}_1=400 \mathrm{K}$ and ${\mathrm{T}}_2=200 \mathrm{K},{\mathrm{n}}_1={\mathrm{n}}_2,{\mathrm{V}}_2={\mathrm{V}}_1$ and the system evolves in time till thermal equilibrium is reached. The correct figure(s) depicting this spontaneous process, can be described as

A certain gaseous reaction, carried out in an insulated sealed container results in an increase in temperature from $200 \mathrm{K}$ to $400 \mathrm{K}$, with the pressure remaining constant. The correct equation that describes the reaction is:

The temperature of a given mass of a gas is increased from $19°\mathrm{C}$ to $21°\mathrm{C}$ at constant pressure. The volume $\mathrm{V}$ of the gas is increased

A balloon filled with an air sample occupies $3 \mathrm{L}$ volume at $35°\mathrm{C}.$ On lowering the temperature to $\mathrm{T},$ the volume decreases to $2.5 \mathrm{L}.$ The temperature $\mathrm{T}$ is? [Assume P constant]

When a perfect gas at $27°\mathrm{C}$ is heated, at a constant pressure, to a final temperature of $327°\mathrm{C}$. then the volume of the gas increases to_________ times the original.

Pressure of $1 \mathrm{g}$ ideal gas $\mathrm{X}$ at $300 \mathrm{K}$ is $2 \mathrm{atm}.$ When $2\mathrm{g}$ of another gas $\mathrm{Y}$ is introduced in the same vessel at same temperature, the pressure become $1 \mathrm{atm}.$ The correct relationship between molar mass of $\mathrm{X}$ and $\mathrm{Y}$ is $\_\_\_$

For formation of $3.40 \mathrm{g}$ of ammonia gas, what volumes of hydrogen gas and nitrogen gas, respectively, are required at $\mathrm{NTP}$ conditions?

The graph between P and T according to Gay lussac's law is a