A mixture of ${\mathrm{N}}_2$ and Ar gases in a cylinder contains 7 g of ${\mathrm{N}}_2$ and 8 g of Ar. If the total pressure of the mixture of the gases in the cylinder is 27 bar, the partial pressure of ${\mathrm{N}}_2$ is:

[Use atomic masses (in g ${\mathrm{mol}}^{-1}$): N=14, Ar=40]

1. 12 bar

2. 15 bar

3. 18 bar

4. 9 bar

The molecular weight of a gas which diffuses through a porous plug of 1/6th of the speed of hydrogen under identical condition is:

(1) 27

(2) 72

(3) 36

(4) 48

If one mole of a monoatomic gas ($\gamma =5/3$) is mixed with one mole of a diatomic gas ($\gamma =7/5$), the value of $\gamma$ for the mixture is:

(1) 1.4

(2) 1.5

(3) 1.53

(4) 3.07

A gas is heated from $0°C to 100°C$ at 1.0 atm pressure. If the initial volume of the gas is 10 litre, its final volume would be:

(1) 7.32 litre

(2) 10.0 litre

(3) 13.66 litre

(4) 20.0 litre

The rates of diffusion of $O_2 and H_2$ at same P and T are in the ratio:

(1) 1:4

(2) 1:8

(3) 1:16

(4) 4:1

As the temperature is raised from $20°C to 40°C$, the average kinetic energy of neon atoms changes by a factor:

(1) 2

(2) $\sqrt{\frac{313}{293}}$

(3) $\frac{313}{293}$

(4) $\frac{1}{2}$

The rms speed of hydrogen is $\sqrt{7}$ times the rms speed of nitrogen. lf T is temperature of the gas, then:

 $\left(1\right) {T_H}_2=T_{N_2}$
${\left(2\right) T_H}_2>T_{N_2}$
$\left(3\right) {T_H}_2<T_{N_2}$
${\left(4\right) T_H}_2=\sqrt{7}{T}_{N_2}$

380 ml. of a gas at 27 C. 800 mm of Hg weights  0.455 g The mol. wt. of gas is:

(1) 27

(2) 28

(3) 29

(4) 30

The density of neon will be highest at:

(1) STP

(2) 0$°$ C,2 atm

(3) 273$°$ C, 1 atm 

(4) 273$°$ C,2 atm

At 27$°$ C, the ratio of root mean square speeds of ozone to oxygen is-

1.$\sqrt{(3/5)}$

2. $\sqrt{(4/3)}$

3. $\sqrt{(2/3)}$

4. 0.25