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NEET • CHEMISTRY • STATES OF MATTER

States of matter practice · Mixed difficulty

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Showing 1-30 of 394 questions

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1 Easy

1 of 394

Analyzing +4 | -1

If for the gases, the critical temperatures are mentioned below i.e.

\begin{array}{cccccccccccccccccccc} {\underline {{\text{Gas}}} }&{\underline {\,{\text{Critical}}\,\,{\text{temperature}}} } \\ {\text{A}}&{{T_{{C_1}}}} \\ {\text{B}}&{{T_{{C_2}}}} \\ {\text{C}}&{{T_{{C_3}}}} \\ {\text{D}}&{{T_{{C_4}}}} \end{array}

{T_{{C_1}}} > {T_{{C_2}}} > {T_{{C_3}}} > {T_{{C_4}}}

Which of the following can be predicted

View answer and explanation

Correct option: D

All of these

Option D (All of these) is correct because ease of liquefaction is directly related to the critical temperature and van der Waals constant 'a'.

2 Medium

2 of 394

Analyzing +4 | -1

Which of the following statements is incorrect?

View answer and explanation

Correct option: C

Average translational kinetic energy of a molecule in a gas at a given temperature is doubled when its molar mass is increased twice

Option C is correct because the average translational kinetic energy depends only on temperature and not on the molar mass, so doubling the molar mass will not double the kinetic energy.

3 Easy

3 of 394

Understanding +4 | -1

Among the following metals interatomic forces are probably weakest in:

View answer and explanation

Correct option: D

\mathrm{Hg}

Option D (

\mathrm{Hg}

) is correct because mercury (Hg) is a liquid at room temperature, indicating weaker interatomic forces compared to the other solid metals.

4 Medium

4 of 394

Remembering +4 | -1

The interaction energy of London forces between two particles is proportional to

{r^x}

, where

r

is the distance between the particles. The value of

x

View answer and explanation

Correct option: C

-6

Option C (-6) is correct because the interaction energy of London forces is inversely proportional to the sixth power of the distance between the particles.

5 Easy

5 of 394

Understanding +4 | -1

In deriving the kinetic equation we make use of the root mean square speed of the molecules which is:

View answer and explanation

Correct option: C

The square root of the average of the square of the speed of the molecules

Option C is correct because root mean square speed is defined as the square root of the average of the squares of the speeds of the molecules.

6 Easy

6 of 394

Remembering +4 | -1

Which force is strongest?

View answer and explanation

Correct option: B

Ion-ion forces

Option B (Ion-ion forces) is correct because ion-ion forces are the strongest intermolecular forces due to the strong electrostatic attraction between oppositely charged ions.

7 Medium

7 of 394

Analyzing +4 | -1

Which of the following is incorrect for pressure units?

View answer and explanation

Correct option: B

1.01325 bar is equal to 0.875 atmosphere

Option B (1.01325 bar is equal to 0.875 atmosphere) is incorrect because 1.01325 bar is approximately equal to 1 atmosphere, not 0.875 atmosphere.

8 Easy

8 of 394

Understanding +4 | -1

As the temperature increases, average kinetic energy of molecules increases. What would be the effect of increase of temperature on pressure provided the volume is constant

View answer and explanation

Correct option: A

Increases

Option A (Increases) is correct because, according to the ideal gas law, pressure is directly proportional to temperature when volume is constant.

9 Hard

9 of 394

Understanding +4 | -1

The product of pressure and volume

\left( {PV} \right)

has a unit of:

View answer and explanation

Correct option: B

Energy or work

Option B (Energy or work) is correct because pressure times volume has the same units as energy or work, as seen in the formula for work done by a gas:

W = P\Delta V

10 Medium

10 of 394

Analyzing +4 | -1

S-I: Helium shows only positive deviation from ideal behavior at room temperature.

S-II: Helium is an inert gas.

View answer and explanation

Correct option: B

Both statements are correct and statement-II is not correct explanation of statement-I

Option B (Both statements are correct and statement-II is not correct explanation of statement-I) is correct because Helium's positive deviation is due to its small size and weak intermolecular forces, not simply because it's an inert gas.

11 Easy

11 of 394

Remembering +4 | -1

Unit of surface tension is

View answer and explanation

Correct option: C

\mathrm{N}{\mathrm{m}^{ - \mathrm{1}}}

Option C is correct because surface tension is defined as force per unit length, hence the unit is Newton per meter (

\mathrm{N}{\mathrm{m}^{ - \mathrm{1}}}

12 Hard

12 of 394

Application +4 | -1

A given mass of helium at STP is allowed to expand to 1.4 times its initial volume by changing the temperature and pressure, then its resultant density would be

View answer and explanation

Correct option: C

0.13 \mathrm{~kg} \mathrm{~m}^{-3}

The correct answer is

0.13 \mathrm{~kg} \mathrm{~m}^{-3}

. The density is inversely proportional to the volume when the mass is constant. Since the volume increases by a factor of 1.4, the density decreases by a factor of 1.4.

13 Easy

13 of 394

Understanding +4 | -1

Statement I: A lighter gas diffuses more rapidly than a heavier gas.

Statement II: At a given temperature, rate of diffusion of a gas is inversely proportional to square root of its density.

View answer and explanation

Correct option: A

Both Statement I and Statement II are correct and Statement II is the correct explanation of Statement I

Option A (Both statements are correct and Statement II is the correct explanation of Statement I) is correct because Graham's law of diffusion states that the rate of diffusion is inversely proportional to the square root of the density, which explains why lighter gases diffuse more rapidly.

14 Easy

14 of 394

Application +4 | -1

500 ml of

{N_2}

{27^ \circ }C

is cooled to

- {5^ \circ }C

at the same pressure. The new volume becomes

View answer and explanation

Correct option: B

446.66 ml

Option B (446.66 ml) is correct because it is calculated using Charles's Law, which relates volume and temperature at constant pressure.

15 Easy

15 of 394

Remembering +4 | -1

In an ideal gas equation which is constant?

View answer and explanation

Correct option: D

Universal gas constant

Option D (Universal gas constant) is correct because the universal gas constant (R) remains constant in the ideal gas equation.

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16 Easy

16 of 394

Remembering +4 | -1

For a given gas at a particular temperature the relationship between root mean square speed

\left(U_{\text {rms}}\right)

, average speed

\left(U_{\mathrm{av}}\right)

, and most probable speed

\left(U_{\mathrm{mp}}\right)

View answer and explanation

Correct option: B

U_{\text {rms }} > U_{\text{av}} > U_{\text{mp}}

Option B (

U_{\text {rms }} > U_{\text{av}} > U_{\text{mp}}

) is correct because the root mean square speed is always greater than the average speed, which is greater than the most probable speed for a given gas at a particular temperature.

17 Medium

17 of 394

Understanding +4 | -1

For a given mass of gas isobar is the graph drawn between

View answer and explanation

Correct option: C

T and V at constant P

Option C (T and V at constant P) is correct because an isobaric process occurs at constant pressure, so the graph represents the relationship between temperature and volume while keeping the pressure constant.

18 Easy

18 of 394

Understanding +4 | -1

Consider an ideal gas contained in a vessel. If the intermolecular interactions suddenly begins to act, which of the following will happen?

View answer and explanation

Correct option: B

The pressure decreases

Option B (The pressure decreases) is correct because intermolecular attractions would reduce the force with which the gas molecules hit the walls of the container, thus decreasing pressure.

19 Easy

19 of 394

Remembering +4 | -1

The compressibility factor for an ideal gas is

View answer and explanation

Correct option: B

Option B is correct. The compressibility factor for an ideal gas is always 1 because it perfectly obeys the ideal gas law.

20 Medium

20 of 394

Remembering +4 | -1

Which gas cannot be kept in a glass bottle because it chemically reacts with glass?

View answer and explanation

Correct option: A

{\mathrm{F}_2}

Option A (

{\mathrm{F}_2}

) is correct because fluorine is highly reactive and can react with the silica in glass.

21 Medium

21 of 394

Remembering +4 | -1

Adiabatic demagnetisation is a technique used for:

View answer and explanation

Correct option: B

Production of low temperature

Option B (Production of low temperature) is correct because adiabatic demagnetization is a technique used to achieve very low temperatures by removing heat from a paramagnetic salt.

22 Medium

22 of 394

Application +4 | -1

Which of the following gases would have the highest rms speed at 

0\,^\circ C

View answer and explanation

Correct option: D

\mathrm{CO}

Option D (

\mathrm{CO}

) is correct because the RMS speed is inversely proportional to the square root of the molar mass. CO has the lowest molar mass among the given options.

23 Hard

23 of 394

Understanding +4 | -1

The number of collisions depends on

View answer and explanation

Correct option: D

All of these

Option D is correct because the number of collisions in a gas depends on the mean free path, pressure, and temperature.

24 Easy

24 of 394

Remembering +4 | -1

The value of gas constant

R

in SI unit is

View answer and explanation

Correct option: C

8.3\,\,\mathrm{J}\,\,\mathrm{mo}{\mathrm{l}^{ - 1}}{\mathrm{K}^{ - 1}}

Option C (8.3 J mol⁻¹K⁻¹) is correct because the value of the gas constant R in SI units is approximately 8.314 J mol⁻¹K⁻¹.

25 Easy

25 of 394

Application +4 | -1

If two moles of a ideal gas at 546 K occupy volume 44.8 L, then pressure must be

View answer and explanation

Correct option: A

2\mathrm{ }\,atm

Option A (

2\mathrm{ }\,atm

) is correct because using the ideal gas law, PV=nRT, and substituting the given values, the pressure is calculated to be approximately 2 atm.

26 Easy

26 of 394

Understanding +4 | -1

Vapour pressure increases with increase in

View answer and explanation

Correct option: B

Temperature up to boiling point

Option B (Temperature up to boiling point) is correct because as temperature increases, the kinetic energy of the molecules increases, leading to higher vapor pressure until the boiling point is reached.

27 Easy

27 of 394

Understanding +4 | -1

Which statement violates the assumptions of the kinetic theory of gases?

View answer and explanation

Correct option: B

The molecules are at rest

Option B (The molecules are at rest) is correct because the kinetic theory of gases states that gas molecules are in constant, random motion, not at rest.

28 Easy

28 of 394

Understanding +4 | -1

At constant volume, the pressure of a monoatomic gas depends upon:

View answer and explanation

Correct option: B

The absolute temperature

Option B (The absolute temperature) is correct because, according to the ideal gas law at constant volume, pressure is directly proportional to absolute temperature.

29 Hard

29 of 394

Application +4 | -1

The rate of diffusion of methane at a given temperature is twice that of a gas

X

. If the molecular weight of

X

8 y

then what will be the value of

y

View answer and explanation

Correct option: A

Option A (8) is correct because it applies Graham's Law of Diffusion to relate the rates of diffusion to the molecular weights of the gases.

30 Easy

30 of 394

Understanding +4 | -1

For the diffusion of a gas at pressure

P

, therate of diffusion is expressed by :

View answer and explanation

Correct option: A

r \propto \frac{1}{\sqrt{M}}

Option A (

r \propto \frac{1}{\sqrt{M}}

) is correct because, according to Graham's law, the rate of diffusion is inversely proportional to the square root of the molar mass at a given temperature.

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Key Takeaways

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