Question

NCERT Solutions Class 12 Chemistry Chapter 5 Surface Chemistry has discussed all the topics thoroughly to make it easy for students to learn and revise difficult concepts. In this particular NCERT Solutions has covered all the topics in-depth. NCERT Solutions Class 12 solutions of all kinds of difficult concepts and intext questions as well.

• Surface Chemistry – surface chemistry deals with the science which studies the phenomenon which occurs on the surface of the substances. It usually occurs at the interface of two mediums. These two mediums can be done on the surface of solid gas, solid-vacuum, liquid gas, etc. the study of chemistry is known as surface engineering. Some processes are occurring on the surface that is
  • Adsorption
  • Heterogeneous catalysis
  • Corrosion
  • crystallization
• Adsorption – adsorption is the process which helps the solid material to hold the gas, liquid, or solute as a thin sheath around the solid material is called the process of adsorption. Adsorption is a surface-related phenomenon while absorption involves the complete volume at the play.  
• Catalysis – catalysis is the process in which the outcome of the reaction is influenced by some outside factor under the influence of some outside material which is known as the catalyst. In the process of catalysis, the rate of a chemical reaction is increased when some new substance is added during the process of a chemical reaction.
• Colloids – such substances which remain suspended in the solution of two mixtures. These suspended substances are microscopically small and are dispersed throughout the solution.
• Classification of Colloids – there are many ways the colloidal solution is classified such as
  • Solid solution
  • Aerosol
  • Gels
  • Emulsion
  • Hydrosol
  • Alcohol
  • Aerosol
  • Multi molecular colloids
  • Macromolecular colloids
• Colloids Around Us – many colloidal solutions are useful for us and some example of colloidal solutions is blood, milk, fog, mist, and many more.

Our NCERT Solutions Class 12 Chemistry has discussed all the concepts and it is designed in the pointwise method for giving clarity to all students.

Answer 1

NCERT Solutions Class 12 Chemistry Chapter 5 Surface Chemistry

1. Distinguish between the meaning of the terms adsorption and absorption. Give one example of each.

Answer:

Adsorption is a surface phenomenon of accumulation of molecules of a substance at the surface rather than in the bulk of a solid or liquid. The substance that gets adsorbed is called the ‘adsorbate’ and the substance on whose surface the adsorption takes place is called the ‘adsorbent’. Here, the concentration of the adsorbate on the surface of the adsorbent increases. In adsorption, the substance gets concentrated at the surface only. It does not penetrate through the surface to the bulk of the solid or liquid. For example, when we dip a chalk stick into an ink solution, only its surface becomes coloured. If we break the chalk stick, it will be found to be white from inside. 

On the other hand, the process of absorption is a bulk phenomenon. In absorption, the substance gets uniformly distributed throughout the bulk of the solid or liquid.

2. What is the difference between physisorption and chemisorption?

Answer:

Physisorption		Chemisorption
1.	In this type of adsorption, the adsorbate is attached to the surface of the adsorbent with weak van der Waal’s forces of attraction.	In this type of adsorption, strong chemical bonds are formed between the adsorbate and the surface of the adsorbent.
2.	No new compound is formed in the process.	New compounds are formed at the surface of the adsorbent.
3.	It is generally found to be reversible in nature.	It is usually irreversible in nature.
4.	Enthalpy of adsorption is low as weak van der Waal’s forces of attraction are involved. The values lie in the range of 20- 40 kJ mol−1.	Enthalpy of adsorption is high as chemical bonds are formed. The values lie in the range of 40-400 kJ mol−1.
5.	It is favoured by low temperature conditions.	It is favoured by high temperature conditions.
6.	It is an example of multi-layer adsorption.	It is an example of mono-layer adsorption.

3. Give reason why a finely divided substance is more effective as an adsorbent.

Answer:

Adsorption is a surface phenomenon. Therefore, adsorption is directly proportional to the surface area. A finely divided substance has a large surface area. Both physisorption and chemisorption increase with an increase in the surface area. Hence, a finely divided substance behaves as a good adsorbent.

4. What are the factors which influence the adsorption of a gas on a solid?

Answer:

There are various factors that affect the rate of adsorption of a gas on a solid surface. 

(1) Nature of the gas: 

Easily liquefiable gases such as NH₃, HCl etc. are adsorbed to a great extent in comparison to gases such as H₂, O₂ etc. This is because Van der Waal’s forces are stronger in easily liquefiable gases. 

(2) Surface area of the solid:

The greater the surface area of the adsorbent, the greater is the adsorption of a gas on the solid surface. 

(3) Effect of pressure:

Adsorption is a reversible process and is accompanied by a decrease in pressure. Therefore, adsorption increases with an increase in pressure. 

(4) Effect of temperature:

Adsorption is an exothermic process. Thus, in accordance with Le-Chatelier’s principle, the magnitude of adsorption decreases with an increase in temperature.

5. What is an adsorption isotherm? Describe Freundlich adsorption isotherm.

Answer:

The plot between the extent of adsorption (\(\frac xm\)) against the pressure of gas (P) at constant temperature (T) is called the adsorption isotherm. 

Freundlich adsorption isotherm:

Freundlich adsorption isotherm gives an empirical relationship between the quantity of gas adsorbed by the unit mass of solid adsorbent and pressure at a specific temperature.

From the given plot it is clear that at pressure PS, \(\frac xm\) reaches the maximum valve. Ps is called the saturation pressure. Three cases arise from the graph now. 

Case I- At low pressure:

The plot is straight and sloping, indicating that the pressure in directly proportional to

\(\frac xm\) i.e. \(\frac xm aP\) 

\(\frac xm = kP\)      (k is a constant)

Case II- At high pressure: 

When pressure exceeds the saturated pressure,\(\frac xm\) becomes independent of P values.

\(\frac xm aP^o\)

\(\frac xm = kP^o\)

Case III- At intermediate pressure: 

At intermediate pressure, \(\frac xm\) depends on P raised to the powers between 0 and 1. This relationship is known as the Freundlich adsorption isotherm.

\(\frac xm aP^{\frac1n}\)

\(\frac xm = kP^{\frac1n}\)      n > 1

Now, taking log:

\(log\frac xm=log\,k+ \frac1nlog\,P\)

On plotting the graph between log (\(\frac xm\)) and log P, a straight line is obtained with the slope equal to \(\frac1n\)

6. What do you understand by activation of adsorbent? How is it achieved?

Answer:

By activating an adsorbent, we tend to increase the adsorbing power of the adsorbent. Some ways to activate an adsorbent are: 

(i) By increasing the surface area of the adsorbent. This can be done by breaking it into smaller pieces or powdering it. 

(ii) Some specific treatments can also lead to the activation of the adsorbent. For example, wood charcoal is activated by heating it between 650 K and 1330 K in vacuum or air. It expels all the gases absorbed or adsorbed and thus, creates a space for adsorption of gases.

7. What role does adsorption play in heterogeneous catalysis?

Answer:

A catalytic process in which the catalyst and the reactants are present in different phases is known as a heterogeneous catalysis. This heterogeneous catalytic action can be explained in terms of the adsorption theory. The mechanism of catalysis involves the following steps: 

(i) Adsorption of reactant molecules on the catalyst surface. 

(ii) Occurrence of a chemical reaction through the formation of an intermediate.

(iii) De-sorption of products from the catalyst surface 

(iv) Diffusion of products away from the catalyst surface. 

In this process, the reactants are usually present in the gaseous state and the catalyst is present in the solid state. Gaseous molecules are then adsorbed on the surface of the catalyst. As the concentration of reactants on the surface of the catalyst increases, the rate of reaction also increases. In such reactions, the products have very less affinity for the catalyst and are quickly desorbed, thereby making the surface free for other reactants.

Answer 2

8. Why is adsorption always exothermic?

Answer:

Adsorption is always exothermic. This statement can be explained in two ways. 

(i) Adsorption leads to a decrease in the residual forces on the surface of the adsorbent. This causes a decrease in the surface energy of the adsorbent. Therefore, adsorption is always exothermic. 

(ii) ∆H of adsorption is always negative. When a gas is adsorbed on a solid surface, its movement is restricted leading to a decrease in the entropy of the gas i.e., ∆S is negative. 

Now for a process to be spontaneous, ∆G should be negative. 

\(\therefore\) ∆G = ∆H − T∆S 

Since ∆S is negative, ∆H has to be negative to make ∆G negative. Hence, adsorption is always exothermic.

9. How are the colloidal solutions classified on the basis of physical states of the dispersed phase and dispersion medium?

Answer:

One criterion for classifying colloids is the physical state of the dispersed phase and dispersion medium. Depending upon the type of the dispersed phase and dispersion medium (solid, liquid, or gas), there can be eight types of colloidal systems.

Dispersed phase		Dispersion medium	Type of colloid	Example
1.	Solid	Solid	Solid Sol	Gemstone
2.	Solid	Liquid	Sol	Paint
3.	Solid	Gas	Aerosol	Smoke
4.	Liquid	Solid	Gel	Cheese
5.	Liquid	Liquid	Emulsion	Milk
6.	Liquid	Gas	Aerosol	Fog
7.	Gas	Solid	Solid foam	Pumice stone
8.	Gas	Liquid	Foam	Froth

10. Discuss the effect of pressure and temperature on the adsorption of gases on solids.

Answer:

Effect of pressure 

Adsorption is a reversible process and is accompanied by a decrease in pressure. Therefore, adsorption increases with an increase in pressure. 

Effect of temperature

 Adsorption is an exothermic process. Thus, in accordance with Le-Chatelier’s principle, the magnitude of adsorption decreases with an increase in temperature.

11. What are lyophilic and lyophobic sols? Give one example of each type. Why are hydrophobic sols easily coagulated?

Answer:

(i) Lyophilic sols:

Colloidal sols that are formed by mixing substances such as gum, gelatin, starch, etc. with a suitable liquid (dispersion medium) are called lyophilic sols. These sols are reversible in nature i.e., if two constituents of the sol are separated by any means (such as evaporation), then the sol can be prepared again by simply mixing the dispersion medium with the dispersion phase and shaking the mixture. 

(ii) Lyophobic sols: 

When substances such as metals and their sulphides etc. are mixed with the dispersion medium, they do not form colloidal sols. Their colloidal sols can be prepared only by special methods. Such sols are called lyophobic sols. These sols are irreversible in nature. For example: sols of metals. 

Now, the stability of hydrophilic sols depends on two things- the presence of a charge and the salvation of colloidal particles. On the other hand, the stability of hydrophobic sols is only because of the presence of a charge. Therefore, the latter are much less stable than the former. If the charge of hydrophobic sols is removed (by addition of electrolytes), then the particles present in them come closer and form aggregates, leading to precipitation.

12. What is the difference between multimolecular and macromolecular colloids? Give one example of each. How are associated colloids different from these two types of colloids?

Answer:

(i) In multi-molecular colloids, the colloidal particles are an aggregate of atoms or small molecules with a diameter of less than 1 nm. The molecules in the aggregate are held together by van der Waal’s forces of attraction. Examples of such colloids include gold sol and sulphur sol. 

(ii) In macro-molecular colloids, the colloidal particles are large molecules having colloidal dimensions. These particles have a high molecular mass. When these particles are dissolved in a liquid, sol is obtained. For example: starch, nylon, cellulose, etc. 

(iii) Certain substances tend to behave like normal electrolytes at lower concentrations. However, at higher concentrations, these substances behave as colloidal solutions due to the formation of aggregated particles. Such colloids are called aggregated colloids.

13. What are enzymes? Write in brief the mechanism of enzyme catalysis.

Answer:

Enzymes are basically protein molecules of high molecular masses. These form colloidal solutions when dissolved in water. These are complex, nitrogenous organic compounds produced by living plants and animals. Enzymes are also called ‘biochemical catalysts’.

Mechanism of enzyme catalysis:

On the surface of the enzymes, various cavities are present with characteristic shapes. These cavities possess active groups such as −NH₂, −COOH, etc. The reactant molecules having a complementary shape fit into the cavities just like a key fits into a lock. This leads to the formation of an activated complex. This complex then decomposes to give the product. 

Hence, 

Step 1: E + S → ES⁺  

(Activated complex)

Step 2: ES⁺ → E + P

14. How are colloids classified on the basis of 

(i) Physical states of components 

(ii) Nature of dispersion medium and 

(iii) Interaction between dispersed phase and dispersion medium? 

Answer: 

Colloids can be classified on various bases:

(i) On the basis of the physical state of the components (by components we mean the dispersed phase and dispersion medium). Depending on whether the components are solids, liquids, or gases, we can have eight types of colloids. 

(ii) On the basis of the dispersion medium, sols can be divided as:

(iii) On the basis of the nature of the interaction between the dispersed phase and dispersion medium, the colloids can be classified as lyophilic (solvent attracting) and lyophobic (solvent repelling).

Answer 3

15. Explain what is observed 

(i) When a beam of light is passed through a colloidal sol. 

(ii) An electrolyte, NaCl is added to hydrated ferric oxide sol. 

(iii) Electric current is passed through a colloidal sol?

Answer:

(i) When a beam of light is passed through a colloidal solution, then scattering of light is observed. This is known as the Tyndall effect. This scattering of light illuminates the path of the beam in the colloidal solution. 

(ii) When NaCl is added to ferric oxide sol, it dissociates to give Na⁺ and Cl^- ions. Particles of ferric oxide sol are positively charged. Thus, they get coagulated in the presence of negatively charged Cl^- ions. 

(iii) The colloidal particles are charged and carry either a positive or negative charge. The dispersion medium carries an equal and opposite charge. This makes the whole system neutral. Under the influence of an electric current, the colloidal particles move towards the oppositely charged electrode. When they come in contact with the electrode, they lose their charge and coagulate.

16. What are emulsions? What are their different types? Give example of each type.

Answer:

The colloidal solution in which both the dispersed phase and dispersion medium are liquids is called an emulsion. 

There are two types of emulsions: 

(a) Oil in water type: 

Here, oil is the dispersed phase while water is the dispersion medium. 

For example: milk, vanishing cream, etc.

(b) Water in oil type: 

Here, water is the dispersed phase while oil is the dispersion medium. 

For example: cold cream, butter, etc.

17. What is demulsification? Name two demulsifiers.

Answer:

The process of decomposition of an emulsion into its constituent liquids is called demulsification. 

Examples of demulsifiers are surfactants, ethylene oxide, etc.

18. Action of soap is due to emulsification and micelle formation. Comment.

Answer:

The cleansing action of soap is due to emulsification and micelle formation. Soaps are basically sodium and potassium salts of long chain fatty acids, R-COO-Na⁺. The end of the molecule to which the sodium is attached is polar in nature, while the alkyl-end is non-polar. Thus, a soap molecule contains a hydrophilic (polar) and a hydrophobic (nonpolar) part. 

When soap is added to water containing dirt, the soap molecules surround the dirt particles in such a manner that their hydrophobic parts get attached to the dirt molecule and the hydrophilic parts point away from the dirt molecule. This is known as micelle formation. Thus, we can say that the polar group dissolves in water while the non-polar group dissolves in the dirt particle. Now, as these micelles are negatively charged, they do not coalesce and a stable emulsion is formed.

19. Give four examples of heterogeneous catalysis.

Answer:

(i) Oxidation of sulphur dioxide to form sulphur trioxide. In this reaction, Pt acts as a catalyst.

(ii) Formation of ammonia by the combination of dinitrogen and dihydrogen in the presence of finely divided iron.

This process is called the Haber’s process. 

(iii) Oswald’s process: Oxidation of ammonia to nitric oxide in the presence of platinum.

(iv) Hydrogenation of vegetable oils in the presence of Ni.

20. What do you mean by activity and selectivity of catalysts?

Answer: 

(a) Activity of a catalyst:

The activity of a catalyst is its ability to increase the rate of a particular reaction. Chemisorption is the main factor in deciding the activity of a catalyst. The adsorption of reactants on the catalyst surface should be neither too strong nor too weak. It should just be strong enough to make the catalyst active.

(b) Selectivity of the catalyst:

The ability of the catalyst to direct a reaction to yield a particular product is referred to as the selectivity of the catalyst. For example, by using different catalysts, we can get different products for the reaction between H₂ and CO.

21. Describe some features of catalysis by zeolites.

Answer:

Zeolites are alumino-silicates that are micro-porous in nature. Zeolites have a honeycomblike structure, which makes them shape-selective catalysts. They have an extended 3Dnetwork of silicates in which some silicon atoms are replaced by aluminium atoms, giving them an Al−O−Si framework. The reactions taking place in zeolites are very sensitive to the pores and cavity size of the zeolites. Zeolites are commonly used in the petrochemical industry.

22. What is shape selective catalysis?

Answer:

A catalytic reaction which depends upon the pore structure of the catalyst and on the size of the reactant and the product molecules is called shape-selective catalysis. 

For example, catalysis by zeolites is a shape-selective catalysis. The pore size present in the zeolites ranges from 260-740 pm. Thus, molecules having a pore size more than this cannot enter the zeolite and undergo the reaction.

23. Explain the following terms: 

(i) Electrophoresis 

(ii) Coagulation 

(iii) Dialysis

(iv) Tyndall effect.

Answer:

(i) Electrophoresis:

The movement of colloidal particles under the influence of an applied electric field is known as electrophoresis. Positively charged particles move to the cathode, while negatively charged particles move towards the anode. As the particles reach oppositely charged electrodes, they become neutral and get coagulated. 

(ii) Coagulation:

The process of settling down of colloidal particles i.e., conversion of a colloid into a precipitate is called coagulation. 

(iii) Dialysis:

The process of removing a dissolved substance from a colloidal solution by the means of diffusion through a membrane is known as dialysis. This process is based on the principle that ions and small molecules can pass through animal membranes unlike colloidal particles. 

(iv) Tyndall effect:

When a beam of light is allowed to pass through a colloidal solution, it becomes visible like a column of light. This is known as the Tyndall effect. This phenomenon takes place as particles of colloidal dimensions scatter light in all directions.

24. Give four uses of emulsions.

Answer:

Four uses of emulsions:

(i) Cleansing action of soaps is based on the formation of emulsions. 

(ii) Digestion of fats in intestines takes place by the process of emulsification. 

(iii) Antiseptics and disinfectants when added to water form emulsions. 

(iv) The process of emulsification is used to make medicines.

Answer 4

25. What are micelles? Give an example of a micellers system.

Answer:

Micelle formation is done by substances such as soaps and detergents when dissolved in water. The molecules of such substances contain a hydrophobic and a hydrophilic part. When present in water, these substances arrange themselves in spherical structures in such a manner that their hydrophobic parts are present towards the centre, while the hydrophilic parts are pointing towards the outside (as shown in the given figure). This is known as micelle formation.

26. Explain the terms with suitable examples: 

(i) Alcosol 

(ii) Aerosol 

(iii) Hydrosol

Answer:

(i) Alcosol:

A colloidal solution having alcohol as the dispersion medium and a solid substance as the dispersed phase is called an alcosol. 

For example: colloidal sol of cellulose nitrate in ethyl alcohol is an alcosol. 

(ii) Aerosol:

A colloidal solution having a gas as the dispersion medium and a solid as the dispersed phase is called an aerosol. 

For example: fog 

(iii) Hydrosol:

A colloidal solution having water as the dispersion medium and a solid as the dispersed phase is called a hydrosol. 

For example: starch sol or gold sol

27. Comment on the statement that “colloid is not a substance but a state of substance”.

Answer:

Common salt (a typical crystalloid in an aqueous medium) behaves as a colloid in a benzene medium. Hence, we can say that a colloidal substance does not represent a separate class of substances. When the size of the solute particle lies between 1 nm and 1000 nm, it behaves as a colloid. 

Hence, we can say that colloid is not a substance but a state of the substance which is dependent on the size of the particle. A colloidal state is intermediate between a true solution and a suspension.