Multiple Choice QuestionsWhich among the following gases can be liquified easily?
Chlorine
Nitrogen
Oxygen
Hydrogen
A.
Chlorine
A gas can be liquified when its temperature is below critical temperature, by cooling or compressing it. Gases which have high critical temperatures (such as Cl2, NH3, CO2, SO2 etc.,) can be liquified by applying a suitable pressure alone. Permanent gases (such as H2, N2, O2 etc.) cannot be liquified by the action of pressure and cooling.
If average velocity of a sample of gas molecules at 300 K is 5 cm s-1, what is RMS velocity of same sample of gas molecules at the same temperature? (Given, α: u: v = 1:1.224: 1.127)
6.112 cm/s
4.605 cm/s
4.085 cm/s
5.430 cm/s
Two closed bulbs of equal volume (V) containing an ideal gas initially at pressure pi and temperature T1 are connected through a narrow tube of negligible volume as shown in the figure below. The temperature of one of the bulbs is then raised to T2. The final pressure pf is:
The intermolecular interaction that is dependent on the inverse cube of the distance between the molecule is:
ion-ion interaction
ion-dipole interaction
London force
London force
If Z is a compressibility factor, Vander Waal's equation at low pressure can be written as
For the gaseous state, if most probable speed is denoted by C*, average speed by C and mean square speed by C, then for a large number of molecules the ratios of these speeds are:
'a' and 'b' are van der Waals constants for gases. Chlorine is more easily liquefied than ethane because :
a and b for Cl2 > a and b for C2H6
a and b for Cl2 < a and b for C2H6
a and Cl2 < a for C2H6 but b for Cl2 > b for C2H6
a and Cl2 < a for C2H6 but b for Cl2 > b for C2H6
If 10–4 dm3 of water is introduced into a 1.0 dm3 flask at 300 K, how many moles of water are in the vapour phase when equilibrium is established?(Given: Vapour pressure of H2O at 300 K is 3170 Pa; R = 8.314 J K–1 mol–1)
5.56 x 10-3 mol
1.53 x 10-2 mol
4.46 x 10-2 mol
4.46 x 10-2 mol
Assuming that water vapour is an ideal gas, the internal energy change(∆U) when 1 mol of water is vapourised at 1 bar pressure and 100°C, (Given: Molar enthalpy of vapourisation of water at 1 bar and 373 K = 41 kJ mol-1 and R = 8.3 J mol–1K–1 will be) –
4.100 kJ mol–1
3.7904 kJ mol–1
37.904 kJ mol–1
37.904 kJ mol–1
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