The Gas Laws

The molecular weight of ${\text{O}}_2$ and ${\text{S}\text{O}}_2$  are $32$ and $64$ respectively. At $15^o\text{C}$ and $150$ mm of Hg pressure, one litre of ${\text{O}}_2$ contains ‘N’ molecules. The number of molecules in two litres of ${\text{S}\text{O}}_2$ under the same conditions of temperature and pressure will be :

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?

The correct value of the gas constant is close to:

A gaseous mixture of $2$ moles of $\text{A}$, $3$ moles of $\text{B}$, $5$ moles of $\text{C}$ and $10$ moles of $\text{D}$ is contained in a vessel. Assuming that gases are ideal and the partial pressure of $\text{C}$ is $1.5$ atm, total pressure is

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 -

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.

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

Choose the correct option for graphical representation of Boyle's law, which shows a graph of pressure vs. volume of a gas at different temperatures:

$10 {\mathrm{dm}}^3 \mathrm{of} {\mathrm{N}}_2$ gas and $10 {\mathrm{dm}}^3$of gas $\mathrm{X}$ at the same temperature contains the same number of molecules. The gas $\mathrm{X}$ is

The density of air at sea level is more than that of air at high altitudes. Which of the following laws can explain this practical application?

If $200 {\mathrm{cm}}^3$ of gas at $1 \mathrm{atm}$ is compressed to $50 {\mathrm{cm}}^3$ at constant temperature, what will be the resultant pressure?

What should be the percentage increase in pressure for a $5\%$ decrease in volume of a gas at constant temperature? 

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

For comparing the same substance under different sets of conditions, Avogadro's law can be expressed as:

Explain why the number of atoms in a certain volume of hydrogen is twice the number of atoms in the same volume of helium at the same temperature and pressure.

A vessel of volume $24.6 \mathrm{L}$ contains $1.5$ $\mathrm{moles}$ of ${\mathrm{H}}_2$ and $2.5$ $\mathrm{moles}$ of ${\mathrm{N}}_2$ at $300 \mathrm{K}$. Calculate the partial pressure of ${\mathrm{N}}_2$ in the vessel.

A gas is heated from $273 \mathrm{K}$ to $373 \mathrm{K}$ at $1 \mathrm{atm}$ pressure. If the initial volume of the gas is $10 \mathrm{L}$, its final volume would be