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

How many mole of He gas occupy 22.4 litre at 30 C and one atmospheric pressure?

(1) 0.90

(2) 1.11

(3) 0.11

(4) 1.0

The rms speed of the molecules of a gas of density 4 kg$m^{-3} and pressure 1.2 \times {10}^5\times N{m}^{-2} is;$

$\left(a\right) 120 m{s}^{-1}$
$\left(b\right) 300 m{s}^{-1}$
$\left(c\right) 600 m{s}^{-1}$
$\left(d\right) 900 m{s}^{-1}$

4.0 g of argon gas pressure P and temperature T K in a vessel. On increasing the temperature by 50^o, 0.8 g of argon was given out to maintain the pressure P.

The original temperature was:

1. 73 K 

2. 100 K

3. 200 K 

4. 510 K 

Given below is the graphical representation of volumes occupied by several gases at STP  at Y axis and mass at X axis. find out which gas/gases is/are not placed at the correct position?

1. He, NH₃ 

2. CH₄, He

3. NH₃, H₂ 

4. NH₃, CH₄ 

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 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