ICSE 2018 Chemistry Question Paper Solved for Class 10

Solving ICSE Class 10 Chemistry Previous Year Question Papers ICSE Class 10 Chemistry Question Paper 2018 is the best way to boost your preparation for the board exams.

ICSE Class 10 Chemistry Question Paper 2018 Solved

Time: 2 hours
Maximum Marks: 80

General Instructions:

Answers to this Paper must be written on the paper provided separately.
You will not be allowed to write during the first 15 minutes.
This time is to be spent in reading the Question Paper.
The time given at the head of this paper is the time allowed for writing the answers.
Section I is compulsory. Attempt any four questions from Section II.
The intended marks for questions or parts of questions are given in brackets [ ].

Section – I (40 MARKS)
(Attempt all questions from this Section)

Question 1.
(a) Choose the correct answer from the options given below: [5]
(i) The salt solution which does not react with ammonium hydroxide is :
(A) Calcium Nitrate
(B) Zinc Nitrate
(C) Lead Nitrate
(D) Copper Nitrate
Answer:
(A) Calcium Nitrate

(ii) The organic compound which undergoes substitution reaction is :
(A) C₂H₂
(B) C₂H₄
(C) C₁₀H₁₈
(D) C₂H₆
Answer:
(D) C₂H₆

(iii) The electrolysis of acidified water is an example of:
(A) Reduction
(B) Oxidation
(C) Redox reaction
(D) Synthesis
Answer:
(C) Redox reaction

(iv) The TUPAC name of dimethyl ether is :
(A) Ethoxy methane
(B) Methoxy methane
(C) Methoxy ethane
(D) Ethoxy ethane
Answer:
(B) Methoxy methane

(v) The catalyst used in the Contact Process is :
(A) Copper
(B) Iron
(C) Vanadium pentoxide
(D) Manganese dioxide
Answer:
(C) Vanadium pentoxide

(b) Give one word or a phrase for the following statements: [5]
(i) The energy released when an electron is added to a neutral gaseous isolated atom to form a negatively charged ion.
(ii) Process of formation of ions from molecules which are not in ionic state.
(iii) The tendency ofan element to form chains of identical atoms.
(iv) The property by which certain hydrated salts, when left exposed to atmosphere, lose their water of crystallization and crumble into powder.
(v) The process by which sulphide ore is concentrated.
Answer:
(i) Electron affinity
(ii) Ionisation
(iii) Catenation
(iv) Efflorescence
(v) Froth floatation process.

(c) Write, a balanced chemical equation for each of the following: [5]
(i) Action of concentrated sulphuric acid on carbon.
Answer:
C + 2H₂SO₄ → 2H₂O + 2SO₂↑ + CO₂ ↑

(ii) Reaction of sodium hydroxide solution with iron (III) chloride solution.
Answer:
FeCl₃ + 3NaOH → Fe(OH)₃ + 3 NaCl

(iii) Action of heat on aluminium hydroxide.
Answer:

(iv) Reaction of zinc with potassium hydroxide solution.
Answer:
Zn + 2KOH → K₂ZnO₂ + H₂O

(v) Action of dilute hydrochloric acid on magnesium sulphite.
Answer:
MgSO₃ +2HCl → MgCl₂ + H₂O + SO₂↑

(d) (i) Give the IUPAC name for each of the following: [5]

Answer:
(1) Methanal
(2) Propanol
(3) But-2-ene

(ii) Write the structural formula of the two isomers of butane.
Answer:

(e) State one relevant observation for each of the following: [5]
(i) Lead nitrate solution is treated with sodium hydroxide solution drop wise till it is in excess.
Answer:
Pb(NO₃)₂ + 2 NaOH → Pb(OH)₂ ↓ (white precipitate) + 2NaNO₃
Pb(OH)₂ + 2NaOH → Na₂PbO₂ (soluble) + 2H₂O
when drop by drop of sodium hydroxide is added, chalky white precipitates appear. These precipitates dissolve in excess of sodium hydroxide forming sodium plumbite.

(ii) At the anode, when molten lead bromide is electrolyzed using graphite electrodes.
Answer:

At Anode
2Br^– – 2e → 2Br
Br + Br → Br₂ ↑
At anode reddish vapours of bromine escape in air from lead bromide.

(iii) Lead nitrate solution is mixed with dilute hydrochloric acid and heated.
Answer:

White precipitates of lead chloride are formed which are soluble in hot water and insoluble in cold water.

(iv) Anhydrous calcium chloride is exposed to air for sometime.
Answer:
Anhydrous calcium chloride absorbs moisture becomes moist and loose its crystalline form showing its deliquescent nature.

(v) Barium chloride solution is slowly added to sodium sulphate solution.
Answer:
BaCl₂ + Na₂SO₄ → BaSO₄ + 2NaCl

(f) Give a reason for each of the following: [5]
(i) Ionic compounds have a high melting point.
Answer:
Ionic compounds have ions held strongly by electrostatic forces of attraction. These strong forces need more energy to be broken apart.Hence, they have high melting point.

(ii) Inert gases do not form ions.
Answer:
Inert gases do not form ions because they have completely filled octet. They are extremely stable. Hence, they neither loose, nor gain electrons.

(iii) Ionisation potential increases across a period, from left to right.
Answer:
As we move from left to right along a period, the atomic size decreases due to the increase in nuclear charge thus more energy is required to remove the electron, hence ionisation potential increase.

(iv) Alkali metals are good reducing agents.
Answer:
Alkali metals have free electrons. They can easily loose electrons to form positive ions. The loss of electron is known as oxidation and the substance/element that lose electrons is said to be reducing agent.

Example:

(v) Conductivity of dilute hydrochloric acid is greater than that of acetic acid.
Answer:
Hydrochloric acid is a strong acid. It splits to give more hydrogen ions as compared to acetic acid. Hence conductivity of dilute hydrochloric acid is more than that of acetic acid.

(g) Name the gas that is produced in each of the following cases : [5]
(i) Sulphur is oxidized by concentrated nitric acid.
(ii) Action of dilute hydrochloric acid on sodium sulphide.
(iii) Action of cold and dilute nitric acid on copper.
(iv) At the anode during the electrolysis of acidified water.
(v) Reaction of ethanol and sodium.
Answer:
(i) Nitrogen dioxide
(ii) hydrogen sulphide
(iii) nitrogen monoxide
(iv) oxygen
(v) hydrogen

(h) Fill up the blanks with the correct choice given in brackets. [5]
(i) Ionic or electrovalent compounds do not conduct electricity in their ______________ state, (fused/solid)
(ii) Electrolysis of aqueous sodium chloride solution will form ______________ at the cathode. (hydrogen gas/sodium metal)
(iii) Dry hydrogen chloride gas can be collected by displacement of air.
(downward/upward)
(iv) The most common ore of iron is .
(calamine / haematite) (v) The salt prepared by the method ofdirect combination is .
(iron (II) chloride / iron (III) chloride)
Answer.
(i) fused
(ii) hydrogen gas
(iii) upward
(iv) haematite
(v) Iron (III) chloride

Section – II (40 Marks)
(Attempt any four questions from this Section)

Question 2.
(a) (i) What do you understand by a lone pair of electrons? [3]
(ii) Draw the electron dot diagram of Hydronium ion. (H = 1, O = 8)
Answer:
(i) The unshared pair of electron that does not normally take part in a chemical reaction is known as lone pair.

(ii) Hydronium ion Formation of proton :

(b) In Period 3 of the Periodic Table, element B is placed to the left of element A. [3]
On the basis of this information, choose the correct word from the brackets to complete the following statements :
(i) The element B would have (lower/higher) metallic character than A.
(ii) The element A would probably have (lesser/higher) electron affinity than B.
(iii) The element A would have (greater/smaller) atomic size than B.
Answer:
(i) Higher
(ii) higher
(iii) smaller

Conversion	Ionic equation	Oxidation/Reduction
Chloride ion to chlorine molecule	(i) Cl^– – 1 e^– → Cl Cl + Cl → Cl₂	(ii) Oxidation
Lead (ii) ion to lead	(ii) pb²⁺ + 2e^– → Pb	(iv) Reduction

Question 3.
(a) (i) Write the balanced chemical equation to prepare ammonia gas in the laboratory by using an alkali. [3]
(ii) State why concentrated sulphuric acid is not used for drying ammonia gas.
(iii) Why is ammonia gas not collected over water ?
Answer:
(i)

(ii) Concentrated sulphuric acid is not used for drying ammonia gas because it reacts with ammonia.
2NH₃ + H₂SO₄ → (NH₄)₂SO₄

(iii) Ammonia is highly soluble gas one volume of water can dissolve 702 volumes of ammonia at 20°C and at 1 atmospheric pressure. Hence it is not collected over water.

(b) (i) Name the acid used for the preparation of hydrogen chloride gas in the laboratory. Why is this particular acid preferred to other acids ? [3]
(ii) Write the balanced chemical equation for the laboratory preparation of hydrogen chloride gas.
Answer:
(i) Sulphuric acid
[It is preferred to other acids because it is non-volatile acid]

(ii)

(c) For the preparation of hydrochloric acid in the laboratory: [2]
(i) Why is direct absorption of hydrogen chloride gas in water not feasible?
(ii) What arrangement is done to dissolve hydrogen chloride gas in water?
Answer:
(i) Direct absorption of hydrogen chloride gas in water is not feasible as it leads to back suction.
(ii) “Inverted funnel arrangement” is done to dissolve hydrogen chloride gas in water.

(d) For the electrorefining of copper [2]
(i) What is the cathode made up of ?
(ii) Write the reaction that takes place at the anode.
Answer:
(i) Cathode is made-up of thin sheets of pure copper connected in parallel.
(ii) Cu – 2e^– → Cu²⁺
Copper anode undergoes oxidation forming Cu²⁺ ions which pass into the solution.

Question 4.
(a) The percentage composition of a gas is: [2]
Nitrogen 82.35%, Hydrogen 17.64%
Find the empirical formula of the gas. [N = 14, H = 1]
Answer:

(b) Aluminium carbide reacts with water according to the following equation: [4]
Al₄C₃ + 12H₂O → 4Al(OH)₃ + 3CH₄
(i) What mass of aluminum hydroxide is formed from 12 g of aluminum carbide ?
(ii) What volume of methane at s.t.p. is obtained from 12 g of aluminum carbide ?
[Relative molecular weight of Al₄Cl₃ = 144; Al(OH)₃ = 78]
Answer:

144 g of Al₄Cl₃ produce 312 g of Al(OH)₃
1 g of Al₄C₃ produce \(\frac{312}{144}\)g of Al(OH)₃
12 g of Al₄C₃ produce \(\frac{312}{144}\) × 12 = 26 g of Al(OH)₃

(ii)

144 g of Al₄C₃ will produce 67.2 l of methane
1 g of Al₄C₃ will produce \(\frac{67.2}{144}\)l of methane
12g of Al₄C₃ will produce \(\frac{67.2}{144}\) × 12 = 5.6 g

(c) (i) If 150 cc of gas A contains X molecules, how many molecules of gas B will be present in 75 cc ofB ? [2]
The gases A and B all under the same conditions of temperature and pressure.
(ii) Name the law on which the above problem is based.
Answer:
(i) 150 ccofgas A contain X molecules
150 cc of gas B will also contain X molecules
75 cc of gas B will contain \(\frac{X}{2}\) molecules under the same conditions of temperature and pressure.

(ii) Avogadro’s law

(d) Name the main component of the following alloys : [2]
(i) Brass
(ii) Duralumin
Answer:
(i) Brass → Copper, zinc and tin
(ii) Duralumin → Aluminium, copper, magnesium and manganese

Question 5.
(a) Complete the following table which relates to the homologous series of hydrocarbons. [6]

Answer:
(A) Alkynes
(B) triple bond
(C) ethyne
(D) Alkane
(E) Single bond
(F) Methane

(b) (i) Name the most common ore of the metal aluminum from which the metal is extracted. Write the chemical formula of the ore. [4]
(ii) Name the process by which impure ore of aluminum gets purified by using concentrated solution of an alkali.
(iii) Write the equation for the formation of aluminum at the cathode during the electrolysis of alumina.
Answer:
(i) Bauxite (Al₂O₃.2H₂O)
(ii) Bayer’s process
(iii)

Cathode
Al³⁺ + 3e^– → Al

Question 6.
(a) A compound X (having vinegar like smell) when treated with ethanol in the presence of the acid Z, gives a compound Y which has a fruity smell. [4]
The reaction is:

(i) Identify Y and Z.
(ii) Write the structural formula of X.
(iii) Name the above reaction.
Answer:

(i) Y is ethyl ethanoate and Z is concentrated sulphuric acid.

(ii)

(iii) Esterification reaction

(b) Ethane burns in oxygen to form CO₂ and H₂O according to the equation: [4]
2C₂H₆ + 7O₂ → 4CO₂ + 6H₂O
If 1250 cc of oxygen is burnt with 300 cc of ethane. Calculate:
(i) the volume of CO₂ formed.
(ii) the volume of unused O₂.
Answer:

(i)

2 vol. of ethane forms 4 volumes of carbon dioxide
1 vol. of ethane forms \(\frac{4}{2}\) volumes of carbon dioxide.
300cc will form \(\frac{4}{2}\) × 300 = 600 cc of CO₂.

(ii) 2 vol. of ethane requires 7 volumes of oxygen
2 vol. of ethane requires \(\frac{7}{2}\) volumes of oxygen
300 cc of ethane requires \(\frac{7}{2}\) × 300 = 1050 cc
Total volume of Oxygen= 1250 cc
Volume of oxygen used= 1050 cc
Unused oxygen= (1250 – 1050) cc = 200 cc

(c) Three solutions P, Q and R have pH value of 3.5, 5.2 and 12.2 respectively. [2]
Which one of these is a :
(i) Weak acid ?
(ii) Strong alkali ?
Answer:
P = 3.5
Q = 5.2
R = 12.2

(i) Weak acid = Q
(ii) Strong alkali = R

Question 7.
(a) Give a chemical test to distinguish between the following pairs of chemicals : [4]
(i) Lead nitrate solution and Zinc nitrate solution.
(ii) Sodium chloride solution and Sodium nitrate solution.
Answer:
(i) Add ammonium hydroxide to the solutions of lead nitrate and zinc nitrate dropwise and then in excess.

Lead Nitrate	Zinc Nitrate
(i) On adding ammonium hydroxide chalky white precipitates of lead hydroxide are formed. Pb(NO₃)₂ + 2NH₄OH → Pb(OH)₂ + 2NH₄NO₃	(i) On adding ammonium hydroxide gelatinous white precipitates of zinc hydroxide are formed. Zn(NO₃)₂ + 2NH₄OH → Zn(OH)₂ + 2NH₄NO₃
(ii)On adding excess of ammonium hydroxide, the precipitates do not dissolve.	(ii) On adding excess of ammonium hydroxide, the precipitates dissolve forming a soluble complex. Zn(OH)₂ + 2NH₄NO₂₃ + 2NH₄OH → [Zn(NH₃)₄] (NO₃)₂ + 4H₂O

(ii) Add silver nitrate solution to both sodium chloride and sodium nitrate solution and observe.

Sodium

Chloride

(i) Add silver nitrate solution to sodium chloride

NaCl + AgNO₃ → AgCl ↓ + NaNO₃
You will observe curdy white precipitates of silver chloride.

(i) Add silver nitrate solution to sodium nitrate. No reaction will take place.

NaNO₃+ AgNO₃→ No reaction

(b) Write a balanced equation for the preparation of each of the following salts : [2]
(i) Copper sulphate from Copper carbonate
(ii) Zinc carbonate from Zinc sulphate.
Answer:
(i) CuCO₃ + H₂SO₄ → CuSO₄ + H₂O + CO₂↑
(ii) ZnSO₄ + Na₂CO₃ → ZnCO₃ + Na₂SO₄

(c) (i) What is the type of salt formed when the reactants are heated at a suitable temperature for the preparation of Nitric acid ? [2]
(ii) State why for the preparation of Nitric acid, the complete apparatus is made up of glass.
(d) Which property of sulphuric acid is shown by the reaction of concentrated sulphuric acid with: [2]
(i) Ethanol ?
(ii) Carbon ?
Answer:
(i) Dehydrating agent

(ii) Oxidising agent
C + 2H₂SO₄ → CO₂ + 2H₂O + 2SO₂