Which one of the following statements is wrong about gases?

Gases do not have a definite shape and volume

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Volume of the gas is equal to the volume of the container confining the gas

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Confined gas exerts uniform pressure on the walls of its container in all directions

No worries! We‘ve got your back. Try BYJU‘S free classes today!

Mass of the gas cannot be determined by weighing a container in which it is enclosed

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Open in App

Solution

The correct option is D
Mass of the gas cannot be determined by weighing a container in which it is enclosed

The mass of gas can be determined by weighing the container, filled with gas and again weighing this container after removing the gas. The difference between the two weights gives the mass of the gas.

Suggest Corrections

Similar questions

Q. The temperature of a gas is raised while its volume remains constant, the pressure exerted by a gas on the walls of the container increases because its molecules

Q. Consider two containers A and B containing gases at the same pressure, volume and temperature. The gas in container A is compressed to half of its original volume isothermally while the gas in container B is compressed to half of its original volume adiabatically. The ratio of final pressure of gas in B to that of gas in A is

According to Avogadro's Law, "Equal volumes of gases at the same temperature and pressure contain equal numbers of molecules". But how is this statement correct? How do we know that equal number of molecules are present in two gases taken in equal volumes?

Even if we consider equal volumes of any two gases(let's consider two gases for example) contain equal number of molecules, if we have the two gases in two containers of same volumes, we can add more gas to any one container and increase the density of the gas inside the container. In that case, the volume of the gas remains equal to the volume of the container but the number of gas molecules inside the container has increased and there is no chage to the number of molecules of the other gas we took inside a similar container. So now we have equal volumes of two gases but we have increased the number of molecules of one gas so now how can we say that the equal volumes of these two gases contain equal number of molecules?

If we take equal number of molecules of two gases and contain one of the gas in a container of some volume and the other gas in a container of a different volume, we will have unequal volumes of two gases having equal number of particles.

So how is Avogadro's Law explained?

Q. Consider two containers

A

and

B

containing identical gases at the same pressure, volume and temperature. The gas in container

A

is compressed to half of its original volume isothermally while the gas in container

B

is compressed to half of its original value adiabatically. The ratio of final pressure of gas in

B

to that of gas in

A

Give reason -. A gas fills completely in the vessel in which it is kept.

2. A gas exerts pressure on the walls of the container.

Join BYJU'S Learning Program