With 100% increase in temperature, the average velocity of a gaseous molecule increases by -

1. 2.8 times

2. 4.0 times

3. 1.4 times

4. 2.0 times

What volume of oxygen gas (O₂) measured at 0°C and 1 atm, is needed to burn completely 1 L of propane gas (C₃H₈) measured under the same conditions?

(1) 7L

(2) 6L

(3) 5L

(4) 10L

Maximum deviation from ideal gas is shown by-

1. H_2(g)   

2. N_2(g)

3. CH_4(g)

4. NH_3(g)

Equal masses of H₂, O₂ and methane have been taken in a container of volume V at temperature 27°C in identical conditions. The ratio of the volumes of gases H₂: O₂ : CH₄ would be-

1. 8:16:1

2. 16:8:1

3. 16:1:2

4. 8:1:2

A gas such as carbon monoxide would be most likely to obey the ideal gas law at-

1. High temperature and low pressure

2. Low temperature and high pressure

3. High temperature and high pressure

4. Low temperature and low pressure

Equal moles of hydrogen and oxygen gases are placed in container with a pin-hole through which both can escape. What fraction of the oxygen escapes in the time required for one-half of the hydrogen to escape?

1. 1/4         

2. 3/8         

3. 1/2           

4. 1/8

The temperature of an ideal gas is reduced from 927°C to 27°C. The rms velocity of the molecules becomes

(1) Double the initial value

(2) Half of the initial value

(3) Four times the initial value

(4) Ten times the initial value

If the average velocity of N₂ molecules is 0.3 m/s at 27°C, then the velocity of 0.6 m/s will take place at 

(1) 273 K

(2) 927 K

(3) 1000 K

(4) 1200 K

The rms velocity of hydrogen is $\sqrt{7}$times the rms velocity of nitrogen. If T is the temperature of the gas [IIT 2000]

(1) $T\left(H_2\right)=T\left(N_2\right)$

(2) $T\left(H_2\right)>T\left(N_2\right)$

(3) $T\left(H_2\right)<T\left(N_2\right)$

(4) $T\left(H_2\right)=\sqrt{7}T\left(N_2\right)$

The rms velocity of an ideal gas at 27°C is 0.3 ms^–1. Its rms velocity at 927°C (in ms^–1) is [IIT 1996; EAMCET 1991]

(1) 3.0

(2) 2.4

(3) 0.9

(4) 0.6