A flask contains argon and chlorine in the ratio 2:1 by mass. The temperature of the mixture is `27^(@)C`. Obtain the ratio of
`(i)` average kinetic energy per molecule, and
`(ii)` root mean square speed of the molecules of two gases.
Atomic mass of argon = 39.9 u, Molecular mass of chlorine = 70.9 u.

A flask contains argon and chlorine in the ratio 2:1 by mass. The temperature of the mixture is 27^(@) . Obtain the ratio of (i) average kinetic energy per molecule, and (ii) root mean square speed of the molecules of two gases. Atomic mass of argon = 39.9 u, Molecular mass of chlorine = 70.9 u.

The temperature of a gas is -68^(@)C . To what temperature should it be heated so that (i) the average kinetic energy of the molecules be doubled and (ii) the root-mean-square velocity of the molecules be doubled ?

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When two gases having volumes 1 litres and 2 liters are at the same temperature, then the ratio of the average kinetic energy of the molecules in the two gases

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The temperature at which oxygen molecules have the same root mean square speed as helium atoms have at 300 K is: Atomic masses: He=4 u, 0 = 16u)

A vessel A contains hydrogen and another vessel B whose volume is twice that of A contains same mass of hydrogen at same temperature. Compare (i) average KE of hydrogen and oxygen molecule. (ii) root mean square speeds of molecules (iii) pressure of gases in A and B. Molecular weight of hydrogen and oxygen are 2 and 32 respectively.

In a container, two gases neon and argon are filled. Find the ratio of the root mean square of the molecules of the two gases. M_(Ne) = 20.0 mu and M_(Ar) = 39.9 mu. The temperature of the system is 30^(@)C.