Gas laws from KTG
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- At a given temperature, pressure of a given mass of gas is inversely proportional to its volume.
- At a given temperature, pressure of a given mass of gas is directly proportional to its volume.
- At a given volume, pressure of a given mass of gas is inversely proportional to its temperature.
- At a given volume, pressure of a given mass of gas is directly proportional to its temperature.
A vessel has of oxygen at pressure P and temperature of . A small hole is made in it so that oxygen leaks out. How much oxygen leaks out if the final pressure is at and the temperature is ?
- At a given temperature, pressure of a given mass of gas is inversely proportional to its volume.
- At a given temperature, pressure of a given mass of gas is directly proportional to its volume.
- At a given pressure, volume of a given mass of gas is inversely proportional to its absolute temperature.
- At a given pressure, volume of a given mass of gas is directly proportional to its absolute temperature.
Two gases of equal mass are in thermal equilibrium. If Pa, Pb and Va and Vb are their respective pressures and volumes, then which relation is true
Pa≠Pb;Va=Vb
Pa=Pb;Va≠Vb
PaVa=PbVb
PaVa=PbVb
- False
- True
- Charles's Law
- Boyle's Law
- Avogadro's Law
- Gay-Lussac's Law
- 2 g
- 1 g
- 16 g
- 8 g
- 1500 cc
- 2000 cc
- 1000 cc
- 750 cc
- 2
- 10
- 4
- 5
- Diffusion is the intermixing of the gas molecules at any direction and effusion is the reverse of diffusion.
- Diffusion is the property of the gas molecules and effusion is the property of the gas container only.
- Diffusion occurs at any direction, whereas effusion occurs under the potential difference.
- Diffusion is the intermixing of the gas molecules due to concentration gradient, whereas effusion is the escaping of gas molecules through the pores without collision.
The molecular weight of gas A is 10 times greater than the molecular weight of gas B . These two gases are taken in cylinders of 5L volume at 1 atm pressure and . Comment on the number of molecules in the two gases. Justify with respect of kinetic molecular theory of gases.
Boyle's law holds for an ideal gas during
Isobaric changes
Isothermal changes
Isochoric changes
Isotonic changes
- 50∘C
- 80∘C
- 91∘C
- 130∘C
[Take R=8.3 J/mol K]
- Mass of Nitrogen in the mixture is 5.6 g.
- Mass of Nitrogen in the mixture is 1.28 g.
- Mass of Oxygen in the mixture is 1.28 g.
- Mass of oxygen in the mixture is 5.6 g.
- 8.1 %
- 9.1 %
- 10.1 %
- 11.1 %
- 104 cc
- 2.5 cc
- 400 cc
- 10 cc
- 50∘C
- 80∘C
- 91∘C
- 130∘C
400 cm3 of hydrogen is at normal temperature. Find the temperature of gas for the following volume when pressure remains constant.
Volume increases by 800 %
The volume of a gas at 200∘C is 200 ml. If the temperature is reduced to −20∘C at constant pressure, its volume will be
172.6 ml
17.26 ml
192.7 ml
19.27 ml
- + 20 %
- - 20 %
- + 25 %
- - 25 %
(Assume that the radius of bubble is neglegible)
- V0
- V0(ρghP)
- V0(1+ρghP)
- V0(1+ρghP)
- H2
- O2
- Cl2
- All have same value
- 104 cc
- 2.5 cc
- 400 cc
- 10 cc
(Assume that the radius of bubble is neglegible)
- V0
- V0(ρghP)
- V0(1+ρghP)
- V0(1+ρghP)
- 1:12
- 12
- 1:16
- 16
- 2
- 1
- 4
- 8
- Pressure
- Volume
- Temperature
- None of the above.