A mixture of 2 moles of helium gas (`(atomic mass)=4a.m.u`) and 1 mole of argon gas (`(atomic mass)=40a.m.u`) is kept at 300K in a container. The ratio of the rms speeds `((v_(rms)(helium))/((v_(rms)(argon))` isA. `0.32`B. `0.45`C. `2.24`D. `3.16`

A mixture of 2 moles of helium gas (`(atomic mass)=4a.m.u`) and 1 mole

1.	A mixture of 2 moles of helium gas (`(atomic mass)=4a.m.u`) and 1 mole of argon gas (`(atomic mass)=40a.m.u`) is kept at 300K in a container. The ratio of the rms speeds `((v_(rms)(helium))/((v_(rms)(argon))` isA. `0.32`B. `0.45`C. `2.24`D. `3.16`
Answer» Correct Answer - D `((v_(rms))_(He))/((v_(rms))_(Ar)) = sqrt(((M_(0))_(Ar))/((M_(0))_(He)))=sqrt(40/4)=sqrt(10)=3.16`

Discussion

No Comment Found

Related InterviewSolutions

To what temperature in `.^(@)C` a gas has to be heated to produce 10% change in volume at constant pressure, if the initloa temperature of the gas is at `0^(@)C`?A. 17.3B. 27.3C. 33.3D. 13.15
If the pressure of an ideal gas is decreased by 10% isothermally, then its volume willA. decrease by 9%B. increase by 10%C. increase by 11.6%D. increase by 9%
By what percentage should the pressure of a given mass of a gas be increased so as to decrease its volume by 10% at a constant temperature?A. `8.1%`B. `10.1%`C. `9.1%`D. `11.1%`
A certain volume of dry air at `20^(@)C` is expanded to three thimes its volume (i) Slowly, (ii) suddenly. Calculate the final pressure and temperature in each case. Atmosperic pressure `= 10^(5) Nm^(-2), gamma` of air = 1.4
The volume of a gas at `20^(@)C` is 100 cm 3 at normal pressure. If it is heated to `100^(@)C` , its volume becomes 125 cm 3 at the same pressure, then volume coefficient of the gas at normal pressure isA. `0.0033//.^(@)C`B. 0.0030/`.^(@)C`C. 0.0025/`.^(@)C`D. 0.0021/`.^(@)C`
One litre of helium gas at a pressure `76 cm`. Of Hg and temperature `27^(@)C` is heated till its pressure and volume are double. The final temperature attained by the gas is:A. `327^(@)C`B. `927^(@)C`C. `1027^(@)C`D. `827^(@)C`
An ideal gas has volume`V_(0)` at . `27^(@)C` It is heated at constant pressure so that its volume becomes . `2V_(0).`The final temperature isA. `327K`B. `327^(@)C`C. `54^(@)C`D. `150^(@)C`
`250 litre` of an ideal gas is heated at constant pressure from `27^(@)C` such that its volume becomes `500 litre`. The final temperature isA. `54^(@)C`B. `300^(@)C`C. `327^(@)C`D. `600^(@)C`
A gas at pressure P is abiabatically compressed so that its density becomes twice that of initial value. Given that `gamma=C_(p)//C_(v)=(7//5)` , What will be the final pressure of the gas ?A. `2p`B. `(7)/(5)`C. 2.63 pD. p
To what temperature should the oxygem at `27^(@)C` be heated at constant pressure, so that the root mean square velocity of its molecules becomes thrice of its previous value.A. `2700^(@)C`B. `2700K`C. `2327^(@)C`D. 270K

A mixture of 2 moles of helium gas (`(atomic mass)=4a.m.u`) and 1 mole of argon gas (`(atomic mass)=40a.m.u`) is kept at 300K in a container. The ratio of the rms speeds `((v_(rms)(helium))/((v_(rms)(argon))` isA. `0.32`B. `0.45`C. `2.24`D. `3.16`

Discussion

No Comment Found

Related InterviewSolutions

Reply to Comment