- All the three states i.e. water, ice and vapour exist simultaneously at
- 4.58 mm & 0.00980 C
- 3.67 mm & 0.08910C
- c. S.T.P conditions
- 250 C & 1 atm.
- A certain sample of gas has a volume of 0.2 L measured at 1 atm. Pressure at 00 C at the same pressure but 273 0C it’s vol. will be
- 0.4 L
- 0.8 L
- 27.8L
- 55.6 L
- Which is the correct value of vibrational degree of freedom of C6H6
a. 2
b. 3
c. 15
d. 30
- Triple point of water is
- 273 K
- 373 K
- 203 K
- 193 K
- Equal masses of methane and hydrogen are mixed in an empty container at 250C. the fraction of the total pressure exerted by hydrogen is
- ½
- 8/9
- 1/9
- 16/17
- Dalton’s law of partial pressure will not applicable to which of the following gaseous mixtures
- Nitric oxide & oxygen
- Nitrogen & oxygen
- CO & H2
- N2 & H2
- The densities of 2 gases are in the ratio of 1:16. the ratio of their rates of diffusion is
- 16:1
- 4:1
- 1:4
- 1:16
- A football bladder contains equimolar proportion of H2 and O2. the composition by mass of the mixture effusing out of punctured football is in the ratio (H2:O2)
- 1:4
- 2√2:1
- 1:2√2
- 4:1
- If vapour density of O2 &H2 are 16 and 1,then the ratio of rate of diffusion of H2 to that of diffusion of O2 is
- 16
- 1/16
- 4
- ¼
10. At constant volume and temperature conditions the rates of diffusion DA and DB of gases A & B having densities ρA and ρB are related by the expression
- DA=[DB ρA/ρB]1/2
- DA=[DB ρB/ρA]1/2
- DA=DB [ρA/ρB]1/2
- DA=DB [ρB/ρA]1/2
- A constant volume for a fixed no. of moles of a gas ,the pressure of the gas increases with the rise in temp. due to
- increase in average molecular speed
- increase in rate of collisions
- increase in molecular attraction
- increase in mean free path
- When an ideal gas undergoes unrestricted expansion, no cooling occurs because the molecules
- exert no attractive force on each other
- collide with loss of energy
- do work equal to K.E. loss
- Exert attractive forces.
- The K.E. of 4 moles of nitrogen gas 1270C is (R=2 cal mol-1 K-1)
- 4400 cals
- 3200 cals
- 4800 C
- 1524 cals
- The temp. at which real gases obey the ideal gas laws over a wide range of pressure is called
- Critical temp.
- Boiling temp.
- inversion temp.
- reduced temp.
- The volume of 2.8g of CO at 270C and 0.821 atm pressure is:
- 3.0 L
- 3 L
- 0.3 L
- 1.5 L
- The pressure of 2 moles of ideal gas at 546 K having volume 44.8 L is
- 2 atm. .
- 3 atm.
- 4 atm
- 1 atm.
- If the density of the Gas A is 1.5 times that of B, then the molecular mass of A is M the molecular mass of B will be
- 1.5 M
- M/1.5
- 3M
- M/3
- The molar mass of an ideal gas can be calculated from the expression
- M=ρRT/PV
- M=RT/Pρ
- M=Pρ/RT
- M=ρRT/P
- Vander waal’s real gas acts as ideal gas under which conditions?
- high temp. low pressure.
- low temp. ,high pressure
- high temp. high pressure
- low temp, low pressure
- A gas deviates from ideal gas behavior b’coz its molecules
- are colorless
- attract each other
- contain covalent bonds
- show Brownian movement
- The compressibility factor for an ideal gas is
- 1.5
- 1.0
- 2.0
- ∞
- The excluded volume per molecule of a gas is……….times the actual volume of the gas molecule
- 2
- 3
- 4
- 5
- The constant ‘a’ in a Vander waal’s eqn. is maximum in
- Helium
- hydrogen
- nitrogen
- ammonia
- Ideal gas eqn. was modified by
- Hunts
- Avogadro
- Vander waal
- Gram
- A real gas tends to behave more ideally at
- Low temp. Low pressure
- Low temp. High pressure
- high temp. & low pressure
- high temp. & high pressure
- If 2 moles of an ideal gas at 546 K occupy the volume of 44.8 L, the pressure must be :
- 3 atm
- 2 atm
- 1atm
- 4 atm
- The K.E. per moles of an ideal gas at 300 K in kj is
- 34.8
- 3.48
- 3.74
- 348.
- The gas i.e. heated up during Joule-Thompson effect at ordinary temp. is
- O2
- CO2
- H2
- SO2
- The temp. to which a gas must be cooled before it can be liquefied by Appling pressure is called:
- Boyle’s temp.
- Critical temp.
- Inversion temp.
- explosion temp.
- At what temp. is the K.E. of a gas molecule half that of its value at 270C
- 3.50C
- 1500C
- 150 K
- -123K
- The compressibility factor for H2 and He is usually
a. >1
b. <1
c. =1
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