If a gas follows Boyle's law then what will be the form of the graph between PV and V?
- A
- B
- C
- ✓
Answer: D.
View full solution →Question types
PART - 2 CH - 12 Kinetic Theory question types
140 questions across 9 question groups — pick any mix to generate a Physics paper with step-by-step answer keys.
140
Questions
9
Question groups
5
Question types
01
M.C.Q (1 Marks)
23 Q→02Fill In The Blanks[1 Marks ]
9 Q→03True False[1 Marks ]
10 Q→041 Marks Question
44 Q→052 Marks Questions
29 Q→063 Marks Question
4 Q→074 Marks Question
2 Q→08Match the following.
2 Q→095 Marks Questions
17 Q→Sample Questions
PART - 2 CH - 12 Kinetic Theory questions
One sample from each question group in this chapter. Select any group above to see the full set with answer keys.
Which of the following statements is true regarding the molecular kinetic theory of gases?
- Apressure of gas is directly proportional to the mean speed of the molecule.
- BThe root mean square speed of molecules is directly proportional to pressure.
- ✓The average energy per molecule is directly proportional to the absolute temperature
- DNone of the above
Answer: C.
View full solution →The reason for the force exerted by a gas on the wall of the vessel is that the molecules of the gas:
- ALosing its kinetic energy
- BClinging to the walls
- ✓Their momentum is changing due to collision
- Dare accelerating towards the walls.
Answer: C.
View full solution →Oxygen and hydrogen are at the same tempeature T. The kinetic energy of the oxygen molecule is equal to the kinetic energy of the hydrogen molecule.
- Awill be 16 times
- Bwill be 4 times
- ✓will be equal
- Dwill be one-fourth
Answer: C.
View full solution →The value of root mean square velocity at normal temperature and pressure will be maximum for which of following gases?
- AOxygen
- BAir
- ✓Hydrogen
- DHelium
Answer: C.
View full solution →If the number of gas molecules is doubled then the values of pressure and kinetic energy_________will change.
For a triatomic gas with linear molecules f =_________.
The highest capacity for_________ found in diffusion.
The volume of 1 mole of any gas at normal temperature and_________pressure is liter.
Diffusion speeds of two gases at constant temperature and pressure (root mean square velocity) are_________of inversely proportional to their density.
If the number of molecules in a container is doubled, the rms speed of the molecules is affected.
According to the law of energy equilization, the average energy of a molecule of a diatomic gas is 5/2 KT.
It is the ratio of molar specific heats for oxygen.
K is a Boltzmann constant whose value is 1.38 $\times 10^{-23}$ joule/per mole Kelvin.
View full solution →Number of heavy molecules in a mixture of gases at a constant temperature the average speed is relatively high.
Two gases A and B have been mixed. Each has volume V, pressure P and temperature is T, then what will be the value of pressure of their mixture?
If the density of a gas is kept constant but the root mean square velocity of the gas molecules is doubled, then how much will the pressure of the gas increase?
Two gases are at the same temperature, can we conclude that the r.m.s. of gas molecules? Will the velocities be the same? Why?
For an ideal gas, what is the volume and mass of the container? Write the equation of pressure in terms of velocity.
What is R in the gas equation PV = nRT? Value of R write in liter atmosphere per Kelvin per mole.
At what temperature will the root mean square velocity of helium molecules be half the root mean square velocity of hydrogen molecules at normal temperature and pressure?
8 gm of oxygen, 14 gm of nitrogen and 22 gm of carbon dioxide are mixed in a vessel of 10 liters volume and $27^{\circ} C$. Find the pressure exerted by the mixture.
View full solution →Explain temperature on the basis of molecular kinetic theory.
The diameter of an oxygen molecule is approximately $3 \text Å $. Calculate the mean free path of oxygen molecules and the mean time taken between collisions at normal temperature and pressure. At normal temperature and pressure the number of molecules per cubic is $3 \times 10^{19}$.
View full solution →The free path of molecules of a gas at $27^{\circ} C$ temperature is $2.76 \times 10^{-5}$ meter. If the diameter of the molcule is $3.0 \text Å $, then find the pressure of the gas.
View full solution →Molar volume is the volume occupied by 1 mole of gas (ideal) at STP. (STP : 1 atm pressure, $0^{\circ} C$ show that it is 22.4 litres.
View full solution →According to the molecular kinetic theory of gases, what is the mean free path?
Prove that the average kientic energy of molecule is equal to $\frac{3}{2} kT$
View full solution →What is Graham's law of gas diffusion ? Propound this law on the basis of molecular motion theory.
An air bubble, whose volume is $1.0 cm^3$ rises from the bottom of a 40 m deep lake where the temperature is $12^{\circ} C$ and comes to the surface where the temperature is $35^{\circ} C$. Now what will be its volume?
View full solution →Find the ratio of the volume of oxygen molecules and the total volume occupied by them at STP. Take the diameter of an oxygen molecule as 3Å.
| A | B |
| 1. Any gas behave at high temperature and low pressure | (A) $\frac{89}{27 b^2}$ |
| 2. The value of $N_A$ will be | (B) $6.023 \times 10^{26}$ per kg mol. |
| 3. $P _{ C }=$ | (C) Like ideal gas |
| 4. $T _{ C }=$ | (D)$\frac{a}{27 b^2}$ |
| 5. In a container the mean free path of molecule is inversely proportional to | (E) Density |
| A | B |
| 1. Dalton's Partial Pressure law | (A) $\frac{2}{3}$ |
| 2. PV = | (B) Excessive |
| 3. The part of mean K.E of unit volume gas isequal to | (C) $\begin{array}{l} P = P _1+ P _2+ P _3+\ldots\end{array}$ |
| 4. The value of KE. due to r.m.s. velocity is zero | (D) $\frac{1}{3} MC _{r m s}^2$ |
| 5. The gas that's density ( $\rho$ ) become less than value of $C _{ rms }$ | (E) zero |
In an oxygen cylinder whose volume is 30 litres the initial pressure of oxygen is 15 atm and temperature is $27^{\circ} C$. After taking out some gas from it, the gauge pressure falls to 11 atm and the temperature fall to $17^{\circ} C$. Find out how much oxygen has been removed from the cylinder ( $R=8.31 J$ $mol ^{-1} K^{-1}$, molecular mass of oxygen $O _2=32 u$ )
View full solution →In the figure, graphs of PV/T and P for $1.00 \times 10^{-3} kg$ mass of oxygen at two different temperature are shown.
(a) What does the dotted line show?
(b) What is true : $T _1> T _2$ or $T _1< T _2$ ?
(c) What is the value of PV/T where the curves meet on the $y$-axis?
(d) If we make a similar graph for $1.00 \times 10^{-3} kg$ hydrogen, will the value of PV/T be same at the point where the curves meet the $y$-axis?
If not, for what mass of hydrogen will the value of PV/T be the same as for the region of low pressure and high temperature? (Molecular mass of $H _2=2.02$ $u$, Mass of $O_2=32.04 u, R=8.31 J mol ^{-1} K^{-1}$ )
View full solution →(a) What does the dotted line show?
(b) What is true : $T _1> T _2$ or $T _1< T _2$ ?
(c) What is the value of PV/T where the curves meet on the $y$-axis?
(d) If we make a similar graph for $1.00 \times 10^{-3} kg$ hydrogen, will the value of PV/T be same at the point where the curves meet the $y$-axis?
If not, for what mass of hydrogen will the value of PV/T be the same as for the region of low pressure and high temperature? (Molecular mass of $H _2=2.02$ $u$, Mass of $O_2=32.04 u, R=8.31 J mol ^{-1} K^{-1}$ )
Estimate the mean free path and collision frequency of nitrogen molecules in a cylinder of nitrogen gas at 2.0 atm pressure and $17^{\circ} C$ temperature take the radius of nitrogen molecule to be approximately 1.0. Compare the collision time with the time taken by the molecules to move freely between two collisions (Molecular mass of nitrogen $=28.0 u$ ).
View full solution →What is mean free path? Explain and obtain its expression and prove that $\lambda \propto T$ and $\lambda \propto \lambda_{ P }.$
View full solution →What is the law of equal division of energy, prove it the tatal energy of $\text n$ moles of gas molecules is $\text E =\frac{ 1 }{ 2 } \text {fnRT}$ energy. Explain the specific heats of monatomic, diatomic and triatomic gases from uniform distribution.
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