Sulphuric Acid Class-10 Goyal Brothers ICSE Solutions Ch-10

Sulphuric Acid Class-10 Goyal Brothers Prakashan ICSE Chemistry Solutions Ch-10. Step by Step Solutions of Exercise and Objective Type Questions of Goyal Brothers Prakashan Chapter-10 Sulphuric Acid for ICSE Class 10 .

Sulphuric Acid –  Test , use, observation seen , preparation , properties (physical and chemical) of Sulphuric Acid explain with suitable chemical reaction. Visit official Website CISCE  for detail information about ICSE Board Class-10 Chemistry .

Sulphuric Acid Class-10 Goyal Brothers Prakashan ICSE Chemistry Solutions Ch-10


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Exercise

Objective Type Questions


Exercise Page – 183

Class-10 Sulphuric Acid Goyal Brothers ICSE Solutions Ch-10

Question 1.

(a)How is sulphuric acid prepared industrially by contact process? Support your answer by writing fully balanced Chemical equations.
(b) Why is sulphur trioxide formed in this process not absorbed directly in water?
(c) Why is vanadium pentoxide considered a better catalyst than platinised asbestos?

(d) Why is heating of the catalyst discontinued the moment the oxidation of sulphur dioxide takes place.

Answer :

(a) Contact process for manufacturing of sulphuric acid:

Steps involved in the manufacturing of sulphuric acid are as stated below:

Preparation of sulphur dioxide.

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S(s) + O2 (g) → SO2(g)

Conversion of sulphur dioxide into sulphur trioxide.

2SO2(g) + O2(g) ⇌ 2SO3(g)

Conversion of sulphur trioxide formed into concentrated H2SO4

H2SO4 + SO3(g) → H2S2O7(l)

H2S2O7(l) + H2O(l) → 2H2SO4

(b) Directly dissolving sulphur trioxide in water is not possible due to highly exothermic nature of the reaction. Acidic vapors are formed. Oleum is reacted with water to form conc. sulphuric acid
(c)  Platinum used to be the catalyst for this reaction; however, as it is susceptible to reacting with arsenic impurities in the sulfur feedstock, Vanadium Oxide (V2O5) is now preferred. 

(d)  heating of the catalyst discontinued the moment oxidation of sulphur dioxide takes place because of exothermic nature of reaction

Question 2. Explain the following

(1) Why are the wooden shelves on which concentrated sulphuric acid bottles are kept stained black
(2) Why is concentrated sulphuric acid always added to water and not water to concentrated sulphuric acid? Why does the mixture get hot?

Answer :

(1) Concentrated sulphuric acid is a very powerful dehydrating agent. It removes atoms of hydrogen and oxygen in the form of water from the cellulose [(C6H12O5)n], leaving behind carbon. It is black carbon which appears in the form of black stains
(2) Because dilution of concentrated sulphuric acid with water is an exothermic reaction. If you add water to concentrated sulphuric acid, it can boil and spit and you may get splashed by boiling acidWater has a higher heat capacity than the acid, and so a vessel of cold water will absorb heat as acid is added

Question 3. How does sulphuric acid react with the following? State experimental conditions and write fully balanced chemical equations.

(i) Copper oxide (ii) Iron (iii) An insoluble metal hydroxide (iv) Sodium bicarbonate (v) Lead acetate solution (vi) Copper (vii) Sugar crystals (viii) Zinc nitrate (ix) Iron (II) sulphide (x) Alcohol.

Answer :

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Sulphuric Acid react with the following conditions with  fully balanced chemical equations.

(i) Copper oxide

CuO +H2SO4 -> CuSO4 + H2O

Copper oxide(solid) + Sulphuric Acid (aqueous)-> Copper Sulphate (aqueous)+ Water(liquid

(ii) Iron

2Fe (s) + 6H2SO4 (l) → Fe2(SO4)3 (aq) + 3SO2 (g) + 6H2O (l)

(iii) An insoluble metal hydroxide

(iv) Sodium bicarbonate

2NaHCO3(aq)+H2SO4(aq)Na2SO4(aq)+2CO2(g)+2H2O(l)

(v) Lead acetate solution

H2SO4(aq) + Pb(C2H3O2)2(aq) → PbSO4(s) + 2 HC2H3O2(aq)

(vi) Copper

only copper no reaction take place

CuO +H2SO4 -> CuSO4 + H2O

Copper oxide(solid) + Sulphuric Acid (aqueous)-> Copper Sulphate (aqueous)+ Water(liquid)

(vii) Sugar crystals

The sulfuric acid removes water from the sugar in a highly exothermic reaction, releasing heat, steam, and sulfur oxide fumes. Aside from the sulfurous odor, the reaction smells a lot like caramel. The white sugar turns into a black carbonized tube that pushes itself out of the beaker

C12H22O11 (sugar) + H2SO4 (sulfuric acid) → 12 C (carbon) + 11 H2O (water) + mixture water and acid

(viii) Zinc nitrate

zinc nitrate reacts with concentrated sulphuric acid to produced zinc sulphate solution , nitrous oxide gas and water. .

Zn(NO3)2+H2SO4=ZnSO4+2HNO3

(ix) Iron (II) sulphide

iron II sulphide reacts with dilute sulphuric acid to give solutions of iron II sulphate on crystallization, the solutions yields crystal of FeSo4. 7H2O

FeS + H2SO4 = FeSO4 + 7H20
FeSO4 + 7H2O= FeSO4.7H2O

(x) Alcohol.

Concentrated sulphuric acid produces messy results. Not only is it an acid, but it is also a strong oxidising agent. It oxidises some of the alcohol to carbon dioxide and at the same time is reduced itself to sulphur dioxide. . It also reacts with the alcohol to produce a mass of carbon

Question 4. What will you observe when concentrated sulphuric acid is poured on (i) sugar crystals (ii) copper sulphate crystals?

Answer :

observe when concentrated sulphuric acid is poured on

(i) sugar crystals —

The sulfuric acid removes water from the sugar in a highly exothermic reaction, releasing heat, steam, and sulfur oxide fumes. Aside from the sulfurous odor, the reaction smells a lot like caramel. The white sugar turns into a black carbonized tube that pushes itself out of the beaker

C12H22O11 (sugar) + H2SO4 (sulfuric acid) → 12 C (carbon) + 11 H2O (water) + mixture water and acid

(ii) copper sulphate crystals–

Concentrated Sulphuric acid acts as dehydrating agent and removes the water of crystallisation from hydrated copper sulphate to produce  anhydrous copper(II) sulfate. The reaction is reversible. Hydrated copper sulphate is blue in colour. Anhydrous copper sulphate is colourless/white

Question 5. State six industrial uses of sulphuric acid.

Answer :

Sulfuric acid is one of the most important industrial chemicals.

It is widely used in the manufacture of chemicals, e.g., in making hydrochloric acid, nitric acid, sulfate salts,

synthetic detergents, dyes and pigments, explosives, and drugs

Question 6. Give one test for dilute sulphuric acid and one test for concentrated sulphuric acid.

Answer :

Chemical test to distinguish between : dilute sulphuric acid and conc. Sulphuric acid.

1 Dilute sulphuric acid treated with zinc gives Hydrogen gas which bums with pop sound.
Concentrated H2SO4 gives SO2 gas with zinc and the gas turns Acidified potassium dichromate paper green.
2. Barium chloride solution gives white ppt. with dilute H2SO4, This white ppt. is insoluble in all acids.
Concentrated H2SO4 and NaCl mixture when heated gives dense white fumes if glass rod dipped in Ammonia solution is brought near it.

Question 7. Distinguish between the following pairs of compounds:
(i) Dil. and conc. sulphuric acid. (ii) HCl and H2SO4 (iii) HNO3 and H2SO4

(i) Distinguish between Dil. and conc. sulphuric acid

With dil. gives no ppt with Con.  gives a white insoluble ppt of .

 (ii) Distinguish between HCl and H2SO4 

Sulphuric acid precipitates the insoluble sulphate of barium from the solution of barium chloride.
BaCl2 + H2SO4→ BaSO4 + 2HCl
Dilute HCl does not react with barium chloride solution, and thus, no precipitate is produced in the reaction.

(iii) Distinguish between HNO3 and H2SO4

add a few drops of barium chloride (BaCl22) to both of them. Barium will react with the sulfuric acid to make the solid precipitate, BaSO4. while There will be no reaction with the nitric acid

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