CBSE Class 10 Science Chemistry Different Types of Chemical Reactions Assignment

Combination reaction

Objectives: To study the Combination reaction of Quick lime (CaO) in water

Requirements: CaO, water, beaker, thermometer, stirrer, etc.

Points to remember:

1. CaO is a white powder

2. It reacts with water to form slaked lime [Ca(OH)₂]

3. This process is called slaking of lime

4. Slaked lime is a suspension of Ca(OH)₂ in water.

5. Clear solution of Ca(OH)₂ in water is known as lime water

6. Slaking of lime is an exothermic reaction releasing a lot of heat energy.

7. CaO_(s) + H₂O_(l) →Ca(OH)_2(s/aq)

Procedure:

1. Take about 50 ml of water is a beaker and note its temperature and record as T₁⁰C

2. Add 2 spatula of CaO to it.

3. Stir well

4. Note the temperature again and record the same as T₂⁰C

5. Compare the temperature. (Which is greater? T₁ or T₂?)

Observations:

1. Initial temperature: T₁⁰C = ………….⁰C

2. Final Temperature: T₂⁰C = ………… ⁰C

Result: Reaction between CaO and water is an example of combination reaction and it is an exothermic combination reaction.

Preacautions:

1. Water used may boil due to chemical reaction and hence touching the hot beaker with bare hand should be avoided.

2. Use goggles and lab coat

3. Hg thermometer should be handled with care.

Answer the following questions:

1. What is meant by combination reaction?

2. What is the colour of CaO or quick lime?

3. How do you know that dissolution of CaO in water is exothermic?

4. What are exothermic reactions?

5. Does this reaction belong to REDOX type? (Ans: No. No electron exchange takes place)

Objectives: To study the decomposition reaction of FeSO₄ Requirements: Iron sulphate hepta hydrate (FeSO₄.7H₂O), test tube, spatula, Bunsen burner, etc.

Points to remember:
1. Ferrous sulphate hepta hydrate crystals are light green (pale green) in colour.
2. On heating iron sulphate undergoes decomposition to form solid iron oxide and sulphur dioxide and sulphur trioxide gases. (2FeSO₄.7H₂O A_→ Fe₂O₃ + SO₂ + SO₃ + 14H₂O)
3. The gases formed has smell of burning sulphur
4. Iron sulphide is brown in colour.
5. The sulphur oxide gases produced are acidic and can be tested using moist blue litmus paper.
6. Both SO₂ and SO₃ are soluble in water
7. SO₂ + H₂O → H₂SO₃ (Sulphurous acid)
8. SO₃ + H₂O → H₂SO₄ (Sulphuric acid)
9. SO₂ will dissolve in water and can be tested using acidified potassium dichromate solution (Yellow solution turns green)
10. The seven water molecules present in the crystal are known as water of crystallisation.

Procedure:
1. Take a few crystals of iron sulphate hepta hydrate in a clean dry test tube.
2. Heat the test tube strongly on a Bunsen burner.
3. Introduce a moist blue litmus paper near the mouth of the test tube

Observations:
1. Green colour of the substance gradually changes to brown
2. The white fuming kind of gas released has smell of burning sulphur
3. Blue litmus paper turns to red.
Result: Light green iron sulphate undergoes decomposition to form brown iron oxide and acidic SO₂ and SO₃
gases. It also loses its water of crystallisation.

Precautions:
1. Do not inhale the gases that are released.
2. Avoid your eyes getting exposed to the gases.
3. Wear goggle and lab coat.

Answer the following questions:
1. What are decomposition reactions?
2. What is the colour of hydrated FeSO4?
3. What is the colour of the residue formed after the experiment? What is it chemically?
4. The gases emitted are ……….. oxides.

Experiment No: …1 (c) Displacement reaction Date: ………..

Objectives: To study the Displacement reaction of iron in copper sulphate

Requirements: Iron nails, thread, test tubes, copper sulphate, distilled water, spatula, TT stand, sand paper, etc.

Points to remember:
1. Colour of pure iron is greyish
2. Colour of pure copper is brownish.
3. Aqueous solution of copper sulphate is blue due to the presence of Cu2+ ions and ferrous sulphate is light green due to the presence of Fe²⁺ ions.
4. Fe is more reactive than Cu. Due to their difference in reactivity, copper gets deposited on iron when iron is kept in a solution of copper sulphate and metallic iron dissolves in water to form iron sulphate.
5. Due to the above mentioned reactions, the colour of the solution gradually changes from blue to light green.
6. Fe(s) + Cu²⁺_(aq) → Fe²⁺_(aq) + Cu(s).
7. This is an example of a single displacement reaction. (Fe2+ ions displace Cu2+ ions)

Procedure:
1. Take 10 ml each of copper sulphate solution in two test tubes and keep on a TT stand.
2. Take two iron nails and clean them using a sand paper to remove any rust.
3. Put one iron nail in one of the test tubes.
4. After 15 minutes, take out the iron nail keep it on a filter paper next to the clean iron nail and compare them. Compare also the solutions in both the test tubes.
5. Record your observation in the following table.

Nature of the:	Observation	Inference
Iron nail before the experiment	Silvery grey in colour and lustrous	Metals are lustrous.
Iron nail after the experiment	Brown deposit on the nai	Copper is deposited on the nail due the displacement reaction that takes place between Fe & Cu.
Solution before the experiment	Light blue and transparent	Copper sulphate solution is peacock blue in colour
Solution after the experiment	Light green and dirty	Due to the chemical reaction, Fe displaces Cu fromCuSO4 and FeSO4 is formed in the solution. Dirtiness is due to the rusting of iron.

Conclusions:
Fe displaces Cu from CuSO₄ and forms FeSO₄ in the solution hence the colour of the solution changes from light blue to pale green. The displaced copper gets deposited on iron nail. It appears as brown coating on iron nail.
1. Iron nail should be clean; otherwise impurity such as rust will cause interference to the expected reaction.
2. During the experiment the test tube should not be disturbed. (The deposit of copper might fall off)
3. More the time taken better will be the result.

Questions:
1. What is meant by displacement reaction? (Ans: A stronger element displaces a weaker element from its compound)
2. Which is more reactive? Copper or iron and why? (Ans: Fe is more reactive as it displaces Cu from its compounds)
3. Name the reaction that takes place, when an iron nail is kept in copper sulphate solution. (Single displacement or REDOX)
4. What happens when (write also the chemical equations involved):
a. Zn strip is kept in copper sulphate solution? (Blue solution becomes colourless and brown deposit of Cu)
b. Copper wire is kept in ferrous sulphate solution? (No visible change as Cu cannot displace Fe)
c. Copper wire is kept in silver nitrate solution? (Black deposit of Ag and colourless solution becomes blue)
d. Copper sulphate solution is stored in iron vessel? (Hole will be formed on Fe vessel as Fe displaces Cu from Copper sulphate. Precious copper sulphate solution will be lost)
5. What is the colour of copper sulphate solution before the experiment? (Blue/Peacock blue)
6. Which out of the following get coated on iron nail? What is its colour?
(Copper oxide, copper sulphate, copper sulphide, copper metal) [Reddish brown copper metal)
7. What is the type of reaction that takes place in this experiment? (Chemical displacement)

Double displacement reaction

Experiment No: …1 (d)                                    Date......

Objectives: To study the chemical reaction between Sodium sulphate and Barium Chloride.

Requirements: Solutions of Na₂SO₄ & BaCl₂, test tubes etc.

Points to remember:
1. Sodium sulphate contains 2 sodium ions and one sulphate ion.
2. On mixing the solutions a double displacement reactions takes place.
3. Na₂SO_4(aq) + BaCl_2(aq) → 2NaCl_(aq) + BaSO_4(aq).

EXPERIMENT	OBSERVATION	INFERENCE
Take 1 ml of Sodium sulphate solution in a test tube and add 1ml of BaCl2 solution to it. Record the change observed.	A white precipitate is formed	The white precipitate formed is BaSO4  Na2SO4+BaCl2 → BaSO4+2NaCl
Add 1 ml of con. HCl acid to one portion of the precipitate taken in another test tube.	The precipitate remains insoluble.	Confirms the presence of BaSO4. Questions:

Questions:
1. What is meant by displacement reaction?
2. What is meant by double displacement reaction?
3. Write the formulae of sodium sulphate, barium chloride and barium sulphate.

4. What is the valency of:
a. Sodium in sodium sulphate
b. Barium ion in barium sulphate and barium chloride
c. Chloride ion in barium chloride and sodium chloride.
Ans: (a) +1, (b) +2+ and (c) -1

5. What is the colour of barium chloride solution? What is the colour of barium sulphate recipitate?

Multiple choice type questions
1. A student took solid quick lime in a china dish and added a small amount of water. He heard
a) A popping sound
b) A crackling sound
c) A hissing sound
d) No sound at all

2. On heating ferrous sulphate crystals one would get
a) Sweet smell
b) Rotten egg smell
c) Irritating choking smell
d) None of the above

3. Iron nails were dipped in a solution kept in a test tube. After half an hour, it was observed that
the colour of the solution had changed. The solution in the test tube was that of
a) Zinc sulphate
b) Copper sulphate
c) Iron sulphate
d) Aluminium sulphate

4. Which of the following will give a white precipitate with sodium sulphate solution?
a) Barium sulphate
b) Barium carbonate
c) Barium chloride
d) Sodium chloride

5. Iron nails were dipped in a solution of copper sulphate. After 10 minutes, it was observed that
the blue colour of the solution changes and a layer gets deposited on iron nails. The colour of the
solution and that of the coating would respectively be
a) Yellow and green
b) Brown and blue
c) Red and greenish blue
d) Green and reddish brown

6. The solution obtained after the reaction of water on calcium oxide is
a) Neutral
b) Acidic
c) Amphoteric
d) Basic

7. Although a group of the students dipped the iron nails for 10 minutes in the copper sulphate
solution they could not get the result. The possible reason could be
a) Copper sulphate was freshly prepared
b) The iron nail did not provide enough area for reacting
c) The iron nails have to be kept in solution atleast for 24 hr
d) Iron nails were not rubbed clean with sand paper.

8. The first change observed when crystals of ferrous sulphate are heated is
a) Evolution of brown fumes
b) Pale green colour fades
c) Crystals turn green
d) Yellow fumes evolve.

9. The colour of fumes observed on heating ferrous sulphate in a test tube is
a) White
b) Reddish brown
c) Dark brown
d) Black.

10. When you place an iron nail in copper sulphate, the reddish brown coating formed is
a) Soft and dull
b) Hard and flaky
c) Smooth and shiny
d) Rough and granular

Objectives: To study the decomposition reaction of FeSO₄

Requirements: Iron sulphate hepta hydrate (FeSO₄.7H₂O), test tube, spatula, Bunsen burner, etc.

Points to remember:

11. Ferrous sulphate hepta hydrate crystals are light green (pale green) in colour.
12. On heating iron sulphate undergoes decomposition to form solid iron oxide and sulphur dioxide and sulphur trioxide gases. (2FeSO₄.7H₂O A_→ Fe₂O₃ + SO₂ + SO₃ + 14H₂O)
13. The gases formed has smell of burning sulphur
14. Iron sulphide is brown in colour.
15. The sulphur oxide gases produced are acidic and can be tested using moist blue litmus paper.
16. Both SO₂ and SO₃ are soluble in water
17. SO₂ + H₂O → H₂SO₃ (Sulphurous acid)
18. SO₃ + H₂O → H₂SO₄ (Sulphuric acid)
19. SO₂ will dissolve in water and can be tested using acidified potassium dichromate solution (Yellow solution turns green)
20. The seven water molecules present in the crystal are known as water of crystallisation.'

Procedure:
4. Take a few crystals of iron sulphate hepta hydrate in a clean dry test tube.
5. Heat the test tube strongly on a Bunsen burner.
6. Introduce a moist blue litmus paper near the mouth of the test tube

Observations:
4. Green colour of the substance gradually changes to brown
5. The white fuming kind of gas released has smell of burning sulphur
6. Blue litmus paper turns to red.

Result: Light green iron sulphate undergoes decomposition to form brown iron oxide and acidic SO₂ and SO₃ gases. It also loses its water of crystallisation.

Precautions:
4. Do not inhale the gases that are released.
5. Avoid your eyes getting exposed to the gases.
6. Wear goggle and lab coat.

Answer the following questions:
5. What are decomposition reactions?
6. What is the colour of hydrated FeSO4?
7. What is the colour of the residue formed after the experiment? What is it chemically?
8. The gases e􀅵itted are ……….. oxides.

Experiment No: …1 (e) Displacement reaction Date: ………..

Objectives: To study the Displacement reaction of iron in copper sulphate

Requirements: Iron nails, thread, test tubes, copper sulphate, distilled water, spatula, TT stand, sand paper, etc.

Points to remember:
8. Colour of pure iron is greyish
9. Colour of pure copper is brownish.
10. Aqueous solution of copper sulphate is blue due to the presence of Cu2+ ions and ferrous sulphate is
light green due to the presence of Fe2+ ions.
11. Fe is more reactive than Cu. Due to their difference in reactivity, copper gets deposited on iron when
iron is kept in a solution of copper sulphate and metallic iron dissolves in water to form iron sulphate.
12. Due to the above mentioned reactions, the colour of the solution gradually changes from blue to light
green. 
13. Fe_(s) + Cu²⁺_(aq) → Fe²⁺_(aq) + Cu_(s).
14. This is an example of a single displacement reaction. (Fe2+ ions displace Cu2+ ions)

Procedure:
6. Take 10 ml each of copper sulphate solution in two test tubes and keep on a TT stand.
7. Take two iron nails and clean them using a sand paper to remove any rust.
8. Put one iron nail in one of the test tubes.
9. After 15 minutes, take out the iron nail keep it on a filter paper next to the clean iron nail and compare them. Compare also the solutions in both the test tubes.
10. Record your observation in the following table.

Nature of the:	Observation	Inference
Iron nail before the experiment	Silvery grey in colour and lustrous	Metals are lustrous.
Iron nail after the experiment	Brown deposit on the nai	Copper is deposited on the nail due the displacement reaction hat takes place between Fe & Cu.
Solution before the experiment	Light blue and transparent	Copper sulphate solution is peacock blue in colour
Solution after the experiment	Light green and dirty	Due to the chemical reaction, Fe displaces Cu fromCuSO4 and FeSO4 is formed in the solution.Dirtiness is due to the rusting of iron.

Conclusions:
Fe displaces Cu from CuSO₄ and forms FeSO₄ in the solution hence the colour of the solution changes from light blue to pale green. The displaced copper gets deposited on iron nail. It appears as brown coating on iron nail.

4. Iron nail should be clean; otherwise impurity such as rust will cause interference to the expected reaction.
5. During the experiment the test tube should not be disturbed. (The deposit of copper might fall off)6. More the time taken better will be the result.

Questions:

8. What is meant by displacement reaction? (Ans: A stronger element displaces a weaker element from its
compound)
9. Which is more reactive? Copper or iron and why? (Ans: Fe is more reactive as it displaces Cu from its compounds)
10. Name the reaction that takes place, when an iron nail is kept in copper sulphate solution. (Single displacement or REDOX)
11. What happens when (write also the chemical equations involved):
a. Zn strip is kept in copper sulphate solution? (Blue solution becomes colourless and brown deposit of Cu)
b. Copper wire is kept in ferrous sulphate solution? (No visible change as Cu cannot displace Fe)
c. Copper wire is kept in silver nitrate solution? (Black deposit of Ag and colourless solution becomes blue)
d. Copper sulphate solution is stored in iron vessel? (Hole will be formed on Fe vessel as Fe displaces Cu
from Copper sulphate. Precious copper sulphate solution will be lost)
12. What is the colour of copper sulphate solution before the experiment? (Blue/Peacock blue)
13. Which out of the following get coated on iron nail? What is its colour?
(Copper oxide, copper sulphate, copper sulphide, copper metal) [Reddish brown copper metal)
14. What is the type of reaction that takes place in this experiment? (Chemical displacement)

Double displacement reaction

Experiment No: …1 (d)                                        Date......

Objectives: To study the chemical reaction between Sodium sulphate and Barium Chloride.

Requirements: Solutions of Na₂SO₄ & BaCl₂, test tubes etc.

Points to remember:

4. Sodium sulphate contains 2 sodium ions and one sulphate ion.

5. On mixing the solutions a double displacement reactions takes place.

6. Na₂SO_4(aq) + BaCl_2(aq) → 2NaCl_(aq) + BaSO_4(aq).

EXPERIMENT	OBSERVATION	INFERENCE
Take 1 ml of Sodium sulphate solution in a test tube and add 1 ml of BaCl2 solution to it. Recordthe change observed	A white precipitate is formed	The white precipitate formed is BaSO4 Na2SO4+BaCl2 →BaSO4+2NaCl
Take 1 ml of Sodium sulphate solution in a test tube and add 1 ml of BaCl2 solution to it. Record the change observed	The precipitate remains insoluble	Confirms the presence of BaSO4.

Questions:
6. What is meant by displacement reaction?
7. What is meant by double displacement reaction?
8. Write the formulae of sodium sulphate, barium chloride and barium sulphate.
9. What is the valency of:
a. Sodium in sodium sulphate
b. Barium ion in barium sulphate and barium chloride
c. Chloride ion in barium chloride and sodium chloride.
Ans: (a) +1, (b) +2+ and (c) -1
10. What is the colour of barium chloride solution? What is the colour of barium sulphate recipitate?

Multiple choice type questions

1. A student took solid quick lime in a china dish and added a small amount of water. He heard
e) A popping sound
f) A crackling sound
g) A hissing sound
h) No sound at all

2. On heating ferrous sulphate crystals one would get
e) Sweet smell
f) Rotten egg smell
g) Irritating choking smell
h) None of the above

3. Iron nails were dipped in a solution kept in a test tube. After half an hour, it was observed that
the colour of the solution had changed. The solution in the test tube was that of
e) Zinc sulphate
f) Copper sulphate
g) Iron sulphate
h) Aluminium sulphate

4. Which of the following will give a white precipitate with sodium sulphate solution?
e) Barium sulphate
f) Barium carbonate
g) Barium chloride
h) Sodium chloride

5. Iron nails were dipped in a solution of copper sulphate. After 10 minutes, it was observed that
the blue colour of the solution changes and a layer gets deposited on iron nails. The colour of the
solution and that of the coating would respectively be
e) Yellow and green
f) Brown and blue
g) Red and greenish blue
h) Green and reddish brown

6. The solution obtained after the reaction of water on calcium oxide is
e) Neutral
f) Acidic
g) Amphoteric
h) Basic

7. Although a group of the students dipped the iron nails for 10 minutes in the copper sulphate
solution they could not get the result. The possible reason could be
e) Copper sulphate was freshly prepared
f) The iron nail did not provide enough area for reacting
g) The iron nails have to be kept in solution atleast for 24 hr
h) Iron nails were not rubbed clean with sand paper.

8. The first change observed when crystals of ferrous sulphate are heated is
e) Evolution of brown fumes
f) Pale green colour fades
g) Crystals turn green
h) Yellow fumes evolve.

9. The colour of fumes observed on heating ferrous sulphate in a test tube is
e) White
f) Reddish brown
g) Dark brown
h) Black.

10. When you place an iron nail in copper sulphate, the reddish brown coating formed is
e) Soft and dull
f) Hard and flaky
g) Smooth and shiny
h) Rough and granular

Experiment No: …1 (c)                       Displacement reaction Date: ………..

Objectives: To study the Displacement reaction of iron in copper sulphate

Requirements: Iron nails, thread, test tubes, copper sulphate, distilled water, spatula, TT stand, sand paper, etc.

Points to remember:
15. Colour of pure iron is greyish
16. Colour of pure copper is brownish.
17. Aqueous solution of copper sulphate is blue due to the presence of Cu²⁺ ions and ferrous sulphate is light green due to the presence of Fe²⁺ ions.
18. Fe is more reactive than Cu. Due to their difference in reactivity, copper gets deposited on iron when iron is kept in a solution of copper sulphate and metallic iron dissolves in water to form iron sulphate.
19. Due to the above mentioned reactions, the colour of the solution gradually changes from blue to light green.
20. Fe(s) + Cu²⁺_(aq) → Fe²⁺_(aq) + Cu_(s).
21. This is an example of a single displacement reaction. (Fe²⁺ ions displace Cu²⁺ ions)

Procedure:
11. Take 10 ml each of copper sulphate solution in two test tubes and keep on a TT stand.
12. Take two iron nails and clean them using a sand paper to remove any rust.
13. Put one iron nail in one of the test tubes.
14. After 15 minutes, take out the iron nail keep it on a filter paper next to the clean iron nail and compare them. Compare also the solutions in both the test tubes

Nature of the	Observation	Inference
Iron nail before the experiment	Silvery grey in colour and lustrous	Metals are lustrous.
Iron nail after the experiment	Brown deposit on the nai	Copper is deposited on the nail due the displacement reaction that takes place between Fe & Cu.
Solution before the experiment	Light blue and transparent	Light blue andtransparent
Solution after the experiment	Light green and dirty	Due to the chemical reaction, Fe displaces Cu from CuSO4 and FeSO4 is formed in the solution. Dirtiness is due to the rusting of iron.

Conclusions:

Fe displaces Cu from CuSO4 and forms FeSO4 in the solution hence the colour of the solution changes from light blue to pale green. The displaced copper gets deposited on iron nail. It appears as brown coating on iron nail.