Real Gases
Trending Questions
- PV=RT+Pb
- PV=RT
- PV=RT+aV
- PV=RT−aV
- 1.335×10−10 cm
- 1.335×10−8 cm
- 2.670×10−8 cm
- 4.340×10−8 cm
Write short notes on the behavior of real gases.
Calculate the pressure exerted by 5 mol of CO2 in 1 L vessel at 47∘C using van der Waals equation. Also, calculate the pressure for an ideal gas. Given a=3.592 atm L2mol−2, b = 0.0427 L mol−1 .
131.2 , 77.01
69.83, 126.22
77.01, 131.2
114 , 122
- O2
- CO2
- NH3
- SO2
- a is large and b is small
- constants a and b are large
- a is small and b is large
- constants a and b are negligibly small
- 5 mol
- 2 mol
- 8 mol
- 3 mol
When is deviation more in the behaviour of a gas from the ideal gas equation PV=nRT
At high temperature and low pressure
At low temperature and high pressure
At high temperature and high pressure
At low temperature and low high pressure
Van der waals constant "b" of helium is 24 mL mol−1. Find molecular diameter of helium.
1.335×10−10 cm
1.35×10−8 cm
2.67×10−8 cm
4.34×10−8 cm
XYZPQa66200.0530b0.0250.150.10.020.2
The gas with the highest critical temperature is:
- P
- Q
- Y
- Z
- X
If v is the volume of one molecule of a gas under given conditions then va der Waals' constant b is
4v
152
N04v
4v N0
Which of the following graphs correctly represents the variation of β = - (dVdPV)γ with P for an ideal gas at constant temperature.
- P1<P2<P3
- P2<P1<P3
- P2<P3<P1
- P1=P2=P3
- 5 mol
- 7 mol
- 3 mol
- 2 mol
Give any two examples of gases.
Gas deviates from ideal gas nature because molecules
Are colourless
Attract each other
Contain covalent bond
Show Brownian movement
Calculate the pressure exerted by 5 mol of CO2 in 1 L vessel at 47∘C using van der Waals equation. Also, calculate the pressure for an ideal gas. Given a=3.592 atm L2mol−2, b = 0.0427 L mol−1 .
131.2 , 77.01
69.83, 126.22
77.01, 131.2
114 , 122
Which of the given sets of temperature and pressure will cause a gas to exhibit the greatest deviation from ideal gas behavior
100∘ C and 4 atm
100∘ C and 2 atm
-100∘ C and 4 atm
0∘ C and 2 atm
A real gas most closely approaches the behaviour of an ideal gas at
15 atm and 200 K
1 atm and 273 K
0.5 atm and 500 K
15 atm and 500 K
- A→R, B→P, C→S, D→Q
- A→Q, B→R, C→S, D→P
- A→P, B→R, C→S, D→Q
- A→Q, B→P, C→S, D→R
- Molecular interaction and PVnRT>1
- Molecular interaction and PVnRT<1
- Finite atomic size and PVnRT>1
- Finite atomic size and PVnRT<1
- P1<P2<P3
- P2<P1<P3
- P2<P3<P1
- P1=P2=P3
- 36%
- 54%
- 27%
- 72%
- 0∘ C and 1.0 atm
- 100∘ C and 2.0 atm
- −13∘ C and 1.0 atm
- −13∘ C and 2.0 atm
- 125R
- 3R
- 12−5R4R
- 15−4R5R
At high temperature, van der Waal’s equation can be expressed as
PV=RT
PV=nRT
Both a and b
(P+an2v2)(V−nb)=nRT