21440.What are the conditions under which the relation between volume (V) and number of moles (n) of gas plotted? (P = pressure; T = temperature)
Constant P and T
Constant T and V
Constant P and V
Constant n and V
21441.What is the dominant inter–molecular force or bond that must be overcome in converting liquid CH3OH to a gas?
London dispersion force
Hydrogen bonding
Dipole–dipole interaction
Covalent bonds
21442.A certain mass of a gas occupies a volume of 2 litres at STP. To what temperature the gas must be heated to double its volume, keeping the pressure constant?
100 K
273 K
273°C
546°C
21443.When r, P and M represent rate of diffusion, pressure and molecular mass, respectively, then the ratio of the rates of diffusion (rA/rB) of two gases A and B, is given as
(PA/PB)(MA/MB)1/2
(PA/PB)1/2(MA/MB)
(PA/PB)(MB/MA)1/2
(PA/PB)1/2(MB/MA)
21444.At 400 K, the root mean square (rms) speed of a gas X (molecular weight = 40) is equal to the most probable speed of gas Y at 60 K. The molecular weight of the gas Y is
4
6
8
10
21445.In the equation of state of an ideal gas PV = nRT, the value of the universal gas constant would depend only on
the nature of the gas
the pressure of the gas
the units of the measurement
None of the above
21446.If a gas expands at constant temperature, it indicates that:
Number of the molecules of gas increases
Kinetic energy of molecules decreases
Pressure of the gas increases
Kinetic energy of molecules remains the same
21447.A and B are ideal. The molecular weights of A and B are in the ratio of 1 : 4. The pressure of a gas mixture containing equal weights of A and B is P atm. What is the partial pressure (in atm) of B in the mixture?
P/2.5
P/2
P/5
3P/4
21448.Which of the given sets of temperature and pressure will cause a gas to exhibit the greatest deviation from ideal gas behaviour?
100°C and 4 atm
100°C and 2 atm
–100°C and 4 atm
0°C and 2 atm