States of Matter Questions in English

(N/A) The characteristics of the three states of matter are as follows:
$1.$ $\text{Solid}:$
- Solids have a definite volume.
- Solids do not flow.
- Solids are rigid.
- Solids have a definite shape (with few exceptions like sponge or rubber band).
- Solids are generally incompressible.
$2.$ $\text{Liquid}:$
- Liquids have a definite volume.
- Liquids tend to flow (fluids).
- Liquids are not rigid.
- Liquids do not have a definite shape; they take the shape of the container.
- Liquids are almost incompressible.
$3.$ $\text{Gas}:$
- Gases do not have a definite volume; they occupy the entire space of the container.
- Gases flow easily.
- Gases are not rigid.
- Gases do not have a definite shape.
- Gases are highly compressible.

(N/A) The force of attraction between the molecules of gases is negligible.
As a result,gas molecules are free to move in all directions and occupy the maximum space available to them.
Additionally,the high kinetic energy possessed by gas molecules allows them to move rapidly and fill the entire volume of the container.

(N/A) wooden table is classified as a solid because it possesses a fixed shape and a definite volume. In solids,the constituent particles are held together by strong intermolecular forces of attraction,which keeps them in fixed positions. Additionally,the intermolecular space between these particles is negligible. Due to these properties,a wooden table maintains its structure and does not flow,which are the defining characteristics of a solid state.

(B) Generally,solids have a higher density than liquids. However,water is an exception.
When water freezes to form ice,the molecules arrange themselves in a specific cage-like structure due to hydrogen bonding.
This structure creates vacant spaces between the water $(H_2O)$ molecules.
Because of these vacant spaces,the volume of ice increases for the same mass,which decreases its density compared to liquid water.
Since ice is less dense than liquid water,it floats on the surface.

(C) Fluids are substances that have the ability to flow and take the shape of the container they are placed in. Both liquids and gases possess this property because the intermolecular space between their molecules is sufficient to allow them to move past one another,facilitating flow.

(B) To convert temperature from Celsius $(^{\circ}C)$ to Kelvin $(K)$,we use the formula: $K = ^{\circ}C + 273$.
$1$. For $25\,^{\circ}C$: $25 + 273 = 298\,K$.
$2$. For $38\,^{\circ}C$: $38 + 273 = 311\,K$.
$3$. For $66\,^{\circ}C$: $66 + 273 = 339\,K$.
Therefore,the correct sequence is $298\,K$,$311\,K$,and $339\,K$.

(N/A) Yes,this statement is correct.
In both diffusion and osmosis,particles move from a region of higher concentration to a region of lower concentration.
However,osmosis is considered a special kind of diffusion because it specifically involves the movement of solvent molecules (usually water) across a semi-permeable membrane.
Diffusion can occur in any medium (solid,liquid,or gas) and does not require a membrane,whereas osmosis is restricted to liquid media and requires a semi-permeable membrane to allow only specific molecules to pass through.

(B) In the gaseous state, particles possess significantly higher kinetic energy compared to solids and liquids.
Due to this high kinetic energy, the particles move randomly at very high speeds.
Additionally, the intermolecular space between gas particles is much larger, allowing them to move freely and mix with other gases rapidly.
Therefore, the rate of diffusion is much faster in gases.

(B) Gases exhibit high compressibility because the intermolecular forces of attraction between their particles are extremely weak.
Additionally,there is a large amount of empty space between the gas particles.
When pressure is applied,these particles can be easily pushed closer together,significantly reducing the volume of the gas.

(N/A) The three states of matter exist due to differences in the following characteristics:
$(i)$ Interparticle space: The distance between particles varies,being minimum in solids and maximum in gases.
$(ii)$ Interparticle force: The force of attraction between particles is strongest in solids and weakest in gases.
$(iii)$ Kinetic energy: The movement of particles depends on their kinetic energy,which is lowest in solids and highest in gases.

(D) substance is called a vapour if it exists as a liquid or solid at room temperature $(25^{\circ}C)$ and standard atmospheric pressure,but is present in the gaseous state.
Helium,nitrogen,and carbon dioxide are gases at room temperature.
Sulphur is a solid at room temperature,but it can exist in a gaseous state (vapour) upon heating. Therefore,sulphur in the gaseous state is called a vapour.

(N/A) At $0\,^oC$,water exists in a state of equilibrium between solid (ice) and liquid phases. At $100\,^oC$,water exists in a state of equilibrium between liquid and gaseous (steam) phases. Between $0\,^oC$ and $100\,^oC$,water remains in the liquid state.
$(a)$ At $25\,^oC$: Liquid state.
$(b)$ At $0\,^oC$: Solid and liquid state (melting point).
$(c)$ At $100\,^oC$: Liquid and gaseous state (boiling point).

(N/A) Water is a liquid at room temperature because:
$1$. It has a tendency to flow (fluidity).
$2$. It takes the shape of the container in which it is kept,but its volume remains fixed.
$(b)$ An iron almirah is a solid at room temperature because:
$1$. It has a definite shape and a fixed volume.
$2$. It is hard and rigid,meaning it resists change in shape when subjected to external force.

(N/A) In the gaseous state,the particles move randomly at high speeds. Due to this random movement,the particles collide with each other and also strike the walls of the container. This continuous bombardment of gas particles against the walls of the container exerts force per unit area,which is known as gas pressure.

(N/A) $(i)$ Liquid: In the liquid state,the intermolecular forces are weaker than in solids,allowing the layers of particles to slip and slide over one another,which gives liquids their property of fluidity.
$(ii)$ Gaseous: In the gaseous state,the intermolecular forces of attraction are negligible,allowing particles to move randomly and freely in all directions at high speeds.

(N/A) wooden chair is classified as a solid at room temperature due to the following reasons:
$(i)$ It possesses a definite shape and a fixed volume,as the constituent particles are held together by strong intermolecular forces.
$(ii)$ It is rigid and cannot be compressed,as there is negligible space between its particles.

(N/A) sponge has minute holes,in which air is trapped.
When we press the sponge,the air is expelled out from these holes,which allows us to compress it.

(A) rubber band is classified as a solid. Although it changes its shape when stretched,it regains its original shape when the external force is removed. This behavior is characteristic of solids,which maintain their structure under normal conditions and return to their original state after the removal of deforming forces.

(N/A)

Gas	Vapour
It is a stable state at room temperature. $e.g., O_2, H_2$.	It is an unstable state at room temperature; it changes into a liquid state upon normal cooling. $e.g., \text{Water vapour}$.

(N/A) When pressure is applied to a gas,the particles are forced closer together. As the distance between the particles decreases,the intermolecular forces of attraction become strong enough to hold the particles together. During this process,the particles lose kinetic energy in the form of heat,leading to a change in state from gaseous to liquid. This process is known as the liquefaction of gases. By using this method,a large volume of gas can be compressed into a small cylinder for storage and transport.

(N/A) $(i)$ Solids possess the property of Rigidity,which liquids do not possess.
$(ii)$ Liquids possess the property of Fluidity,which solids do not possess.

(N/A) rubber band is classified as a solid because it maintains a definite shape and volume.
It changes its shape under the application of an external force and regains its original shape when the force is removed.
It does not change its shape on its own,which is a characteristic property of solids.

(N/A) In solids,the constituent particles are very closely packed with negligible intermolecular space. Due to this high density and lack of space between particles,they cannot be compressed further,making them incompressible.
$(b)$ In solids,the intermolecular forces of attraction are very strong,which holds the particles in fixed positions. Since the particles can only vibrate about their mean positions and cannot move freely,their kinetic energy is negligible at room temperature.

(N/A) $(i)$ Gases are highly compressible because the intermolecular forces of attraction between gas molecules are very weak,and they have large intermolecular spaces.
$(ii)$ In liquids,the intermolecular forces of attraction are stronger than in gases,and the molecules are packed more closely together,which makes them incompressible under normal conditions.

(A) The intermolecular space is the distance between particles. In solids,particles are tightly packed; in liquids,they are slightly apart; and in gases,they are far apart. Therefore,the order of increasing intermolecular space is: $Solids < Liquids < Gases$.
$(b)$ The intermolecular force is the attraction between particles. Solids have the strongest forces holding particles together,while gases have the weakest. Therefore,the order of increasing intermolecular force is: $Gases < Liquids < Solids$.

(N/A) $(i)$ The $SI$ unit of temperature is Kelvin $(K)$.
$(ii)$ The relationship between Celsius and Kelvin scales is given by $T(K) = T(^{\circ}C) + 273.15$. For general calculations,we use $T(K) = T(^{\circ}C) + 273$.
Given,the boiling point of water is $100^{\circ} C$.
Therefore,in $SI$ units: $100 + 273 = 373 \ K$.

(A) $(i)$ Rate of diffusion: The rate of diffusion is lowest in solids, higher in liquids, and highest in gases because particles in gases have the most kinetic energy and freedom of movement.
Order: $\text{Solid} < \text{Liquid} < \text{Gas}$.
$(ii)$ Particle motion: The motion of particles is restricted in solids due to strong intermolecular forces, whereas particles in gases move randomly and rapidly.
Order: $\text{Solid} < \text{Liquid} < \text{Gas}$.

(N/A) $(i)$ Both liquids and gases do not have a fixed shape and take the shape of the container in which they are kept.
$(ii)$ Both liquids and gases have the property of fluidity,meaning they can flow easily.

(N/A) The differences between the three states of matter based on the given properties are summarized in the table below:

Property	Solid State	Liquid State	Gaseous State
$(a)$ Density	High	Lower than solids	Very low
$(b)$ Diffusion	Negligible	Slow	Very fast
$(c)$ Particle motion	Vibratory motion only	Random motion within the bulk	Rapid,random motion in all directions

(N/A)

Characteristics	Solid	Liquid	Gas
$(a)$ Interparticle force of attraction	Maximum	Moderate	Least
$(b)$ Diffusion	Cannot diffuse	Can diffuse to some extent	Can easily diffuse
$(c)$ Fluidity	Rigid (no fluidity)	Can flow (less than gases)	Can easily flow (maximum)

$(A-D)$ $(i)$ Rigidity: $Gas < Liquid < Solid$
$(ii)$ Diffusion: $Solid < Liquid < Gas$
$(iii)$ Compressibility: $Solid < Liquid < Gas$
$(b)$ $(i)$ Expansion of gas: Gases expand upon heating because the kinetic energy of the particles increases, which overcomes the interparticle forces of attraction. This allows gas molecules to move randomly in all directions and exert pressure on the walls of the container.
$(ii)$ Compressibility of gas: Gases have very weak interparticle forces of attraction and large intermolecular spaces. Therefore, when external pressure is applied, the gas particles are forced closer together, significantly reducing the volume and potentially leading to liquefaction.

(N/A) Water is found in all three states during the water cycle:
$(i)$ Gaseous state: Water exists as water vapour in the atmosphere.
$(ii)$ Liquid state: Water exists as liquid water in oceans,rivers,lakes,and as rain.
$(iii)$ Solid state: Water exists as ice and snow in polar regions and high altitudes.

(N/A) Solid $CO_2$ is known as dry ice. It is called dry ice because,at a constant pressure of $1 \text{ atmosphere}$,solid $CO_2$ undergoes sublimation,meaning it converts directly from a solid state to a gaseous state without passing through the liquid phase.

(N/A) $(i)$ The molecules of a gas are in constant,random motion in all directions. As they move,they collide with each other and strike the walls of the container,exerting a force per unit area,which is perceived as pressure.
$(ii)$ The force of attraction between the particles of a gas is negligible,and the particles possess high kinetic energy. This allows them to move freely and occupy all the available space in the vessel in which they are kept.

(N/A)

Variation in Characteristic	Effect on State of Matter
$(i)$ Temperature	With an increase in temperature,the solid state melts to form a liquid,and a liquid boils to form a gaseous state.
$(ii)$ Pressure	With an increase in pressure,the gaseous state liquefies,and liquids can be compressed further.
$(iii)$ Interparticle space	The space between particles is minimal in solids,moderate in liquids,and maximum in gases,determined by temperature and pressure.
$(iv)$ Interparticle forces	Strongest in solids,weaker in liquids,and negligible in gases,which dictates the physical state.
$(v)$ Kinetic energy	Higher kinetic energy at higher temperatures leads to the transition from solid to liquid to gas.

(N/A) $(i)$ Oxygen has neither a fixed shape nor a fixed volume,which is a characteristic property of gases.
$(ii)$ Oxygen particles have high kinetic energy and large intermolecular spaces,allowing it to diffuse easily into the air.
$(iii)$ Oxygen exerts pressure on the walls of its container and can be compressed or liquefied under high pressure and low temperature.

(N/A) The state of matter in which layers of particles can slip and slide over one another easily is the liquid state. In liquids,the intermolecular forces are weaker than in solids,allowing particles to flow.
$(b)$ The state of matter in which particles move around randomly due to very weak forces of attraction is the gaseous state. In gases,the intermolecular forces are negligible,allowing particles to move freely and randomly in all directions.

(N/A) Solid state: Solids have a rigid structure,resulting in a definite shape,volume,and mass.
$(b)$ Gaseous state: In gases,particles are far apart with negligible intermolecular forces,leading to the minimum force of attraction.
$(c)$ Solid state: In solids,particles are closely packed with strong intermolecular forces,resulting in the maximum force of attraction.

(D) $(i)$ Carbon dioxide is classified as a gas due to the following reasons:
$(a)$ It lacks both a fixed volume and a fixed shape,as it completely fills the container in which it is stored.
$(b)$ It exerts pressure on the walls of the container due to the high kinetic energy and collisions of its particles.
$(ii)$ In gases,the intermolecular distances are very large,and the intermolecular forces of attraction are extremely weak. Because of this,gas particles are free to move randomly in the entire space available to them. Consequently,a gas fills the vessel completely.
$(iii)$ The intermolecular space is maximum in gases,intermediate in liquids,and minimum in solids. When pressure is applied to a gas,the particles move closer together,significantly reducing the volume,which makes gases highly compressible. In contrast,the particles in solids and liquids are already closely packed,leaving very little space for further compression,making them almost incompressible.

(A) Diffusion is the movement of particles from a region of higher concentration to a region of lower concentration.
In $Gases$,the particles are far apart and have high kinetic energy,allowing them to move freely and rapidly in all directions.
In $Liquids$,particles are closer together than in gases,and in $Solids$,they are tightly packed with very little movement.
Therefore,due to high kinetic energy and large intermolecular spaces,the rate of diffusion is highest in $Gases$.

(D) The stability of a state of matter depends on the kinetic energy of its particles.
At higher temperatures,particles have high kinetic energy,leading to a gaseous state.
As the temperature decreases,the kinetic energy of the particles decreases,causing them to come closer together and form a liquid,and eventually a solid.
However,at extremely low temperatures (near absolute zero),the Bose-Einstein Condensate $(BEC)$ state is formed,which is a state of matter characterized by extremely low energy and high stability in quantum terms.
Among the standard states,solid is the most stable at low temperatures,but $BEC$ is specifically defined by its existence and stability at temperatures near absolute zero.

(C) Intermolecular forces of attraction are the forces that hold particles (atoms, molecules, or ions) together in a substance.
In $Solids$, these forces are very strong, keeping particles in a fixed position.
In $Liquids$, these forces are weaker than in solids, allowing particles to move past each other.
In $Gases$, the particles are far apart and move randomly at high speeds, meaning the intermolecular forces of attraction are negligible or least effective.
$Plasma$ consists of ionized gas particles, where the high kinetic energy further overcomes attractive forces.
Therefore, the correct answer is $Gases$.

(A) In physics and chemistry,a fluid is defined as a substance that has the ability to flow and does not resist a permanent deformation when subjected to a shear stress.
Both liquids and gases possess the ability to flow,which is why they are collectively referred to as fluids.
Solids,on the other hand,maintain a fixed shape and do not flow under normal conditions.
Therefore,the statement that gases and liquids behave like fluids is correct.

(B) To convert temperature from Celsius $(^{\circ} C)$ to Kelvin $(K)$,we use the formula: $K = ^{\circ} C + 273.15$ (or approximately $273$).
For $25^{\circ} C$: $25 + 273 = 298 \, K$.
For $46^{\circ} C$: $46 + 273 = 319 \, K$.
For $109^{\circ} C$: $109 + 273 = 382 \, K$.
Thus,the correct sequence is $298 \, K, 319 \, K, 382 \, K$.

(TRUE) The statement is $True$.
Solids possess a definite shape and a fixed volume due to strong intermolecular forces of attraction between their constituent particles.
Because of these strong forces,the particles are held in fixed positions and can only vibrate about their mean positions,which prevents them from flowing like liquids or gases.

(FALSE) The statement is False.
An absolute temperature scale is one that starts at absolute zero $(0 \ K)$,which is the lowest possible temperature where all molecular motion ceases.
The Celsius scale is a relative scale based on the freezing point $(0 \ ^\circ C)$ and boiling point $(100 \ ^\circ C)$ of water at standard atmospheric pressure.
The Kelvin scale is the absolute temperature scale used in science.

(FALSE) The statement is False.
The relationship between the Celsius scale and the Kelvin scale is given by the formula: $T(K) = T(^{\circ}C) + 273.15$.
For $0^{\circ} C$,the temperature in Kelvin is $0 + 273.15 = 273.15 \ K$ (often approximated as $273 \ K$).
Therefore,$0^{\circ} C = 273 \ K$,not $-273 \ K$.

(N/A) Water exists in three physical states during the water cycle:
$(a)$ Gas: Water vapour in the atmosphere and clouds.
$(b)$ Liquid: Water found in ponds,rivers,lakes,oceans,seas,and springs.
$(c)$ Solid: Water found as snow,hail,ice,or sleet.