According to atomic hypothesis:
- AAtoms attract each other when they are little distance apart.
- BAtoms repel if they being squeezed into one another.
- ✓Both $(a)$ and $(b).$
- DNeither $(a)$ nor $(b).$
Answer: C.
View full solution →Question types
Kinetic Theory question types
507 questions across 7 question groups — pick any mix to generate a Physics paper with step-by-step answer keys.
507
Questions
7
Question groups
5
Question types
01
M.C.Q (1 Marks)
219 Q→02Fill In The Blanks[1 Marks ]
15 Q→031 Marks Question
55 Q→042 Marks Questions
58 Q→053 Marks Question
70 Q→065 Marks Questions
83 Q→07Case study (4 Marks)
7 Q→Sample Questions
Kinetic Theory questions
One sample from each question group in this chapter. Select any group above to see the full set with answer keys.
In a diatomic molecule, the rotational energy at a given temperature.
- AObeys Maxwell’s distribution.
- BHave the same value for all molecules.
- CIs $(2/3)^{rd}$ the translational kinetic energy for each molecule.
- ✓Both $A$ and $C$
Answer: D.
View full solution →The monoatomic molecules have only three degrees of freedom because they can possess:
- ✓Only translatory motion.
- BOnly rotatory motion.
- CBoth translatory and rotatory motion.
- DTranslatory, rotatory and vibratory motion.
Answer: A.
View full solution →The temperature of the mixture of one mole of helium and one mole of hydrogen is increased from $0^\circ C$ to $100^\circ C$ at constant pressure. The amount of heat delivered will be:
- A$600\ \text{cal}$
- ✓$1200\ \text{cal}$
- C$1800\ \text{cal}$
- D$3600\ \text{cal}$
Answer: B.
View full solution →The energy of a given sample of an ideal gas depends only on its:
- AVolume.
- BPressure.
- CDensity.
- ✓Temperature.
Answer: D.
View full solution →Relation between pressure P and average kinetic energy E per unit volume of gas is .
In ideal gas the size of a molecule is negligible compared with the between the molecules.
A rigid body has degree of freedom.
According to law of equipartition of energy average kinetic energy per molecule per degree of freedom is .
As per kinetic interpretation of temperature, the mean kinetic energy per molecule is proportional to the of the gas.
The pressure of a gas at -173°C is 1 atmosphere. Keeping the volume constant, to what temperature should the gas be heated so that its pressure becomes 2 atmosphere.
The specific heat of argon at constant volume is $0.075 ~kcal ~kg^{-1}K^{-1}$, then what will be its atomic weight?
$[Given, R = 2 ~cal ~mol^{-1}K^{-1}]$
View full solution →$[Given, R = 2 ~cal ~mol^{-1}K^{-1}]$
- On the basis of Charle's law, what is the minimum possible temperature?
- What is the volume of gas at absolute zero temperature?
What is the minimum possible temperature on the basis of Charles' law?
The ratio of vapour densities of two gases at the same temperature is 6 : 9. Compare the r.m.s. velocities of their molecules.
Shows plot of $\frac{\text{PV}}{\text{T}}$ versus P for $1.00 \times 10^{-3} \mathrm{~kg}$ of oxygen gas at two different temperatures. What does the dotted plot signify?
View full solution →Shows plot of $\frac{P V}{T}$ versus $P$ for $1.00 \times 10^{-3} \mathrm{~kg}$ of oxygen gas at two different temperatures: Which is true, $T_1>T_2$ or $T_1$ $<T_2$ ?
View full solution →Explain, why it is not possible to increase the temperature of a gas while keeping its volume and pressure constant?
Why gases at high pressure and low temperature show large deviation from ideal gas behavior?
Is a slow process always isothermal? ls a quick process always adiabatic?
Estimate the total number of air molecules (inclusive of oxygen, nitrogen, water vapour and other constituents) in a room of capacity $25.0m^3$ at a temperature of $27°C$ and $1$ atm pressure.
View full solution →Molar volume is the volume occupied by 1mol of any (ideal) gas at standard temperature and pressure: (STP: 1 atmospheric pressure, $0°C$). Show that it is $22.4$ litres.
View full solution →Calculate the temperature at which the root mean square velocity of nitrogen molecules will be equal to $8km-s^{-1}$.
View full solution →At what temperature would the root-mean square speed of a gas molecule have twice its value at 100°C?
On what parameter does the $\lambda ($mean free path$)$ depends?
View full solution →Estimate the fraction of molecular volume to the actual volume occupied by oxygen gas at STP. Take the diameter of an oxygen molecule to be $3\mathring{\text{A}}$
View full solution →Estimate the average thermal energy of a helium atom at:
View full solution →- Room temperature $(27°C)$
- The temperature on the surface of the Sun(6000K)
- The temperature of 10 million kelvin (the typical core temperature in the case of a star).
Given below are densities of some solids and liquids. Give rough estimates of the size of their atoms:
$\big[$Hint: Assume the atoms to be ‘tightly packed’ in a solid or liquid phase, and use the known value of Avogadro’s number. You should, however, not take the actual numbers you obtain for various atomic sizes too literally. Because of the crudeness of the tight packing approximation, the results only indicate that atomic sizes are in the range of a few $\mathring{\text{A}}\big].$
View full solution →|
Substance
|
Atomic Mass(u)
|
Density $(10^3kgm^{-3})$
|
|
Carbon (diamond)
Gold
Nitrogen (liquid)
Lithium
Fluorine (liquid)
|
12.01
197.00
14.01
6.94
19.00
|
2.22
19.32
1.00
0.53
1.14
|
From a certain apparatus, the diffusion rate of hydrogen has an average value of $28.7 \mathrm{~cm}^3 \mathrm{~s}^{-1}$. The diffusion of another gas under the same conditions is measured to have an average rate of $7.2 \mathrm{~cm}^3 \mathrm{~s}^{-1}$. Identify the gas. [Hint: Use Graham's law of diffusion $\frac{\mathrm{R}_1}{\mathrm{R}_2}=\left(\frac{\mathrm{M}_2}{\mathrm{M}_1}\right)^{\frac{1}{2}}$, where $\mathrm{R}_1, \mathrm{R}_2$ are diffusion rates of gases 1 and 2 , and $\mathrm{M}_1$ and $\mathrm{M}_2$ their respective molecular masses. The law is a simple consequence of kinetic theory]
View full solution →Shows plot of $\frac{\text{PV}}{\text{T}}$ versus P for $1.00 \times 10^{-3}kg$ of oxygen gas at two different temperatures: If we obtained similar plots for $1.00 \times 10^{-3}kg$ of hydrogen, would we get the same value of $\frac{\text{PV}}{\text{T}}$ at the point where the curves meet on the y-axis? If not, what mass of hydrogen yields the same value of $\frac{\text{PV}}{\text{T}}$ (for low pressure high temperature region of the plot)? (Molecular mass of $H_2 = 2.02u, of O_2 = 32.0u, R = 8.31J mo1^{-1}K^{-1}$).
View full solution →The human body has an average temperature of 98°F. Assume that the vapour pressure of the blood in the veins behaves like that of pure water. Find the minimum atmospheric pressure which is necessary to prevent the blood from boiling. Use figure. of the text for the vapour pressures. 
$50cc$ of oxygen is collected in an inverted gas jar over water. The atmospheric pressure is $99.4kPa$ and the room temperature is $27°C$. The water level in the jar is same as the level outside. The saturation vapour pressure at $27°C$ is $3.4kPa$. Calculate the number of moles of oxygen collected in the jar.
View full solution →On a winter day, the outside temperature is 0°C and relative humidity 40%. The air from outside comes into a room and is heated to 20°C. What is the relative humidity in the room? The saturation vapour pressure at 0°C is 4.6mm of mercury and at 20°C it is 18mm of mercury.
Read the passage given below and answer the following questions from (i) to (v). Monatomic Gases: The molecule of a monatomic gas has only three translational degrees of freedom. Thus, the average energy of a molecule at temperature T is $\frac{3}{2}\text{K}_\text{b}\text{T}$. The total internal energy of a mole of such a gas is $\text{U}=(\frac{3}{2})\text{RT}$. The molar specific heat at constant volume cv is given by$\text{C}_{\text{v}}=\frac{\text{Du}}{\text{Dt}}=(\frac{3}{2})\text{R}$
For an ideal gas, $C_p - C_v = R$ Where Cp is the molar specific heat at constant pressure. Thus, $\text{C}_\text{P} =(\frac{5}{2})\text{R}$ The ratio of specific heats IS $\gamma=\frac{\text{cp}}{\text{cv}}=\frac{5}{3}$ Diatomic Gases: a diatomic molecule treated as a rigid rotator, like a dumbbell, has 5 degrees of freedom: 3 translational and 2 rotational. Using the law of equipartition of energy, the total internal energy of a mole of such a gas is $\text{U}=\frac{5}{2}\text{RT}$ The molar specific heat at constant volume cv is given by$\text{Cv}=\frac{\text{DU}}{\text{DT}}=(\frac{5}{2})\text{R}$
For an ideal gas, $C_p – C_v= R$ Where Cp is the molar specific heat at constant pressure. Thus, $\text{C}_\text{P} =(\frac{7}{2})\text{R}$ The ratio of specific heats IS $γ( \text{for rigid diatomic)}=\frac{\text{C}_\text{P}}{\text{C}_\text{v}} =(\frac{7}{5})\text{R}$ For non rigid diatomic molecules they have additional mode of vibrations therefore$\gamma=\frac{\text{C}_\text{p}}{\text{C}_\text{v}}=\frac{9}{7}$
Polyatomic Gases: In general a polyatomic molecule has 3 translational, 3 rotational degrees of freedom and a certain number (f) of vibrational modes. According to the law of equipartition of energy, it is easily seen that one mole of such a gas has$ C_v= (3 + f)$ R and $C_p= (4 + f) R$ and $\gamma=\frac{(4 + \text{f})}{(3+\text{f})}$
View full solution →For an ideal gas, $C_p - C_v = R$ Where Cp is the molar specific heat at constant pressure. Thus, $\text{C}_\text{P} =(\frac{5}{2})\text{R}$ The ratio of specific heats IS $\gamma=\frac{\text{cp}}{\text{cv}}=\frac{5}{3}$ Diatomic Gases: a diatomic molecule treated as a rigid rotator, like a dumbbell, has 5 degrees of freedom: 3 translational and 2 rotational. Using the law of equipartition of energy, the total internal energy of a mole of such a gas is $\text{U}=\frac{5}{2}\text{RT}$ The molar specific heat at constant volume cv is given by$\text{Cv}=\frac{\text{DU}}{\text{DT}}=(\frac{5}{2})\text{R}$
For an ideal gas, $C_p – C_v= R$ Where Cp is the molar specific heat at constant pressure. Thus, $\text{C}_\text{P} =(\frac{7}{2})\text{R}$ The ratio of specific heats IS $γ( \text{for rigid diatomic)}=\frac{\text{C}_\text{P}}{\text{C}_\text{v}} =(\frac{7}{5})\text{R}$ For non rigid diatomic molecules they have additional mode of vibrations therefore$\gamma=\frac{\text{C}_\text{p}}{\text{C}_\text{v}}=\frac{9}{7}$
Polyatomic Gases: In general a polyatomic molecule has 3 translational, 3 rotational degrees of freedom and a certain number (f) of vibrational modes. According to the law of equipartition of energy, it is easily seen that one mole of such a gas has$ C_v= (3 + f)$ R and $C_p= (4 + f) R$ and $\gamma=\frac{(4 + \text{f})}{(3+\text{f})}$
- For monatomic molecules ratio of specific heats is $\gamma$
- $\frac{5}{3}$
- $\frac{7}{5}$
- $\frac{9}{5}$
- None of these
- For diatomic rigid molecules ratio of specific heats is γ
- $\frac{5}{3}$
- $\frac{7}{5}$
- $\frac{9}{7}$
- None of these
- For diatomic non rigid molecules ratio of specific heats is γ
- $\frac{5}{3}$
- $\frac{7}{5}$
- $\frac{9}{7}$
- None of these
- Give cp and cv values and ratio of specific heat for monatomic gas molecules.
- Give cp and cv values and ratio of specific heat for polyatomic gas molecules
Read the passage given below and answer the following questions from (i) to (v). Boyle’s law is a gas law which states that the pressure exerted by a gas (of a given mass, kept at a constant temperature) is inversely proportional to the volume occupied by it. In other words, the pressure and volume of a gas are inversely proportional to each other as long as the temperature and the quantity of gas are kept constant. For a gas, the relationship between volume and pressure (at constant mass and temperature) can be expressed mathematically as follows.$\text{P}\infty(\frac{1}{\text{V}})$ Where P is the pressure exerted by the gas and V is the volume occupied by it. This proportionality can be converted into an equation by adding a constant, k.
Charles law states that the volume of an ideal gas is directly proportional to the absolute temperature at constant pressure. The law also states that the Kelvin temperature and the volume will be in direct proportion when the pressure exerted on a sample of a dry gas is held constant. Charles law and Boyle’s law applied to low density gas only. The total pressure of a mixture of ideal gases is the sum of partial pressures. This is Dalton’s law of partial pressures.
View full solution →Charles law states that the volume of an ideal gas is directly proportional to the absolute temperature at constant pressure. The law also states that the Kelvin temperature and the volume will be in direct proportion when the pressure exerted on a sample of a dry gas is held constant. Charles law and Boyle’s law applied to low density gas only. The total pressure of a mixture of ideal gases is the sum of partial pressures. This is Dalton’s law of partial pressures.
- Boyle’s law is obeyed by high as well as low density gases. True or False?
- True
- False
- Charles law is states that volume of an ideal gas is directly proportional to temperature at constant
- Temperature
- Pressure
- Volume
- None of these
- State Daltons law of partial pressures
- State Boyle’s law
- State Charles law
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