ICSE Class 10 Sample Paper 2027 Chemistry

FOR ICSE CLASS 10 EXAM PREPARATION

ICSE Class 10 2027
Sample Paper ·
Chemistry
EXAM YEAR TYPE SUBJECT

ICSE Class 10 2027 Sample Paper Chemistry

Notes · Sample Papers · Previous Year Papers · Mock Tests

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g l a SPECIMEN QUESTION PAPER a
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CHEMISTRY
(SCIENCE PAPER – 2)

Maximum Marks: 80

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Time allowed: Two hours

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1. Answers to this Paper must be written on the paper provided separately.

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2. You will not be allowed to write during first 15 minutes.

3. This time is to be spent in reading the question paper.

4. The time given at the head of this Paper is the time allowed for writing the answers.

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5. Section A is compulsory. Attempt any four questions from Section B.
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Instruction for the Supervising Examiner

Kindly read aloud the Instructions given above to all the candidates present in the Examination
Hall.

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NOTE:

The Specimen Question Paper in the subject provides a realistic
format of the Board Examination Question Paper and should be used
as a practice tool. The questions for the Board Examination can be set
from any part of the syllabus. However, the format of the Board
Examination Question Paper will remain the same as that of the
Specimen Question Paper.

T27 522 – SPECIMEN 2 of 16

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SECTION A (40 Marks)a
(Attempt all questions from this Section.)

Question 1
Choose the correct answers to the questions from the given options. [15]
(Do not copy the question, write the correct answers only.)
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(i) X and Y are diatomic elements. X is less reactive than Y.

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What are elements X and Y?
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(a) X - chlorine, Y - iodine
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(b) a X - fluorine, Y - nitrogen

(c) X - iodine, Y - bromine

(d) X - oxygen, Y - nitrogen [Understanding]

(ii) The diagram given below represents the industrial process for the

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manufacture of concentrated sulphuric acid by the Contact process.

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What is used in step R to obtain sulphuric acid from sulphur trioxide?

(a) vanadium pentoxide

(b) water only

(c) water followed by concentrated sulphuric acid

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(d) concentrated sulphuric acid followed by water [Understanding]
o m
. c Which statement given below is correct with reference to the flow of em
e m electric current?
(iii)
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ag (a) In all aqueous solutions, current is carried by electrons.

(b) In all acidic solutions, current is carried by ions.

(c) In molten electrolytes, current is carried by electrons.

(d) In metal wires, current is carried by ions. [Understanding]

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(iv) The following statements are related to the properties of sulphuric acid:

1. Barium chloride reacts with sulphuric acid to give a white
precipitate.
2. Sulphur dioxide gas is evolved when sulphuric acid reacts with
carbon.
3. Sulphuric acid has a pH value of less than 7.0.
4. Copper (II) oxide reacts with sulphuric acid to form a blue
solution.

Which two statements confirm the acidic nature of sulphuric acid?

(a) 1 and 2

(b) 1 and 3

(c) 3 and 4

(d) 2 and 4 [Understanding]

(v) The diagram given below shows that P reacts with dilute hydrochloric
acid to produce a gas which when passed through substance Q, reduces
it.

What are substances P and Q?

(a) P - copper, Q - lead (II) oxide

(b) P - lead, Q - magnesium oxide

(c) P - magnesium, Q - calcium oxide

(d) P - zinc, Q - copper (II) oxide [Application]

T27 522 – SPECIMEN 4 of 16

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(vi) a give:
Non-metals like chlorine and iodine on reaction with hydrogen
(a) acid

(b) base

(c) salt

[Recall]
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(d) metal

(vii) Statement I:
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Halogens are very reactive.
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Statement II:m Halogens have high electron affinity. s e
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(a) Both a
a
(b) Both the statements are false.

(c) Statement I is true, and statement II is false.

(d) Statement I is false, and statement II is true. [Understanding]

(viii) Assertion (A): Ionic compounds have high melting points.

Reason (R):
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A strong electrostatic force of attraction exists between
the oppositely charged ions. .c
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(a) (A) is true but (R) is false.

(b) (A) is false but (R) is true. ag
(c) Both (A) and (R) are true, and (R) is the correct explanation of (A).

(d) Both (A) and (R) are true, but (R) is not the correct explanation of
(A). [Analysis]

(ix) A student tested the nature of four different solutions P, Q, R, and S using

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pH paper. He noted the following observations:
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P Q R S

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Colour of the pH paper after testing Blue Green Red Violet

las ag
ag Which of the above solutions is neutral in nature?
(a) P

(b) Q

(c) R
[Application]
(d) S

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(x) Identify the organic compound(s) with the molecular formula C3H8O.
1. propanol
2. propanal
3. propanoic acid
(a) Only 1

(b) Only 2

(c) Both 2 and 3

(d) Both 1 and 2 [Application]

(xi) An organic compound X containing carbon and hydrogen only has
Vapour Density (V.D.) 14. The molecular formula of X is
_____________. (At. wt. of C=12, H=1)

(a) CH

(b) C2H4

(c) C2H2
[Application]
(d) CH2
(xii) Identify the ion that contains one lone pair of electrons.

(a) OH-1

(b) H3O+

(c) NH4+

(d) H+ [Understanding]
(xiii) When compound X reacts with dilute hydrochloric acid, it releases a gas
that turns moist lead acetate paper black and decolourises acidified
potassium permanganate solution. Which of the following is compound
X?

(a) Sodium nitrate

(b) Sodium sulphide

(c) Sodium carbonate

(d) Sodium sulphite [Application]

T27 522 – SPECIMEN 6 of 16

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a in the diagram
(xiv) A teacher demonstrated four different reactions as shown
below:

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a

3.
4.
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Which reactions will produce water?
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(a) 1 and 2

(b) 1 and 3

(c) 3 and 4

(d) 2 and 3 [Analysis]

(xv) The volume occupied by 0.2 moles of a gas at S.T.P. is:
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(a) 22.4 litres
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a (d) 4.48 litres [Application]

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Question 2
(i) The diagram given below shows the electrolysis of acidulated water. With [5]
reference to the diagram, answer the following questions:

acidified
water
battery

(a) Write an equation for the reaction that takes place at A. [Application]
(b) Give a test to confirm the product formed at A. [Recall]
(c) Which gas is liberated at B? [Recall]
(d) Why is water acidified for electrolysis? [Understanding]

(e) What is the ratio by volume of the gases liberated at A and B? [Application]

(ii) Write balanced chemical equations for the following: [5]

(a) Chlorination of chloroform in the presence of diffused sunlight. [Application]

(b) Hydrated aluminium oxide is treated with caustic soda. [Application]

(c) Zinc oxide is treated with caustic alkali. [Application]

(d) Copper reacts with cold dilute nitric acid. [Application]

(e) Laboratory preparation of nitric acid using sodium nitrate. [Application]

T27 522 – SPECIMEN 8 of 16

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(iii) aoption from the
Complete the following sentences by choosing the correct [5]
brackets:

(a) The general formula of an alkyl group is __________ [Recall]
(CnH2n+1/CnH2n-1).

(b) The aqueous solution of ___________ (zinc chloride/ sodium [Application]
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sulphate) gives white precipitate with barium nitrate.

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The gas liberated when alkalis are heated with ammonium salts is
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[Recall]

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a
__________ (N2/NH3).

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(d) a The alloy that contains a non-metal as one of its constituents is
a
[Recall]
__________ (bronze/steel).

(e) A salt prepared by neutralization in which titration is involved is [Application]
__________ (CaCl2/ NH4Cl).

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(iv) Match Column A with Column B: [5]

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Column A
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(a) CuO + C
a
Cu + CO 1. Oxidation

(b) Al3+ + 3e– Al 2. Ionization

(c) PbBr2 Pb2+ + 2Br1– 3. Reduction

(d) 2O2– – 4e– O2 4. Redox

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(e) HCl H+ + Cl1– 5. Electrolytic dissociation om
c.[Understanding]
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a

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(v) (a) Give the IUPAC name of the following organic compounds: [5]

1.

2.

[Application]

(b) Draw the structural diagram for the following compounds:

1. diethyl ether

2. isopentane

3. propanone [Application]

SECTION B (40 Marks)
(Attempt any four questions.)

Question 3
(i) A compound commonly used in the laboratory has formula H2P. [2]
H represents hydrogen, P represents a non-metal.
Draw a dot and cross structure for the formation of the compound H2P. [Application]

(ii) Give one significant observation when: [2]

(a) Excess of chlorine gas reacts with ammonia. [Recall]

(b) Zinc nitrate is strongly heated in a test tube. [Recall]

T27 522 – SPECIMEN 10 of 16

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(iii) a was blue in
A student was given a crystalline salt ‘B’ for analysis which [3]
colour. He added a few drops of dense oily hygroscopic liquid to it and
observed a colourless neutral gas/vapour being released and the salt
turning white.

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Salt B

(a) Identify the blue crystalline salt B. [Analysis]
(b) Which property of the hygroscopic liquid is demonstrated in this
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reaction? [Understanding]

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(c)
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Write a balanced chemical equation for the above reaction. [Application]

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(iv) N is a metal which forms a basic oxide. [3]
N has atomic no. 11.

(a) What is the molecular formula of the oxide of N? [Application]
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(b) Write the balanced equation for the reaction that takes place when
c. o[Application]
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(c) State the formula of the product obtained other than water when
g
[Application]
a sulphuric acid is added to the product obtained in (b) above.

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Question 4

(i) Name the following: [3]

(a) The non-metallic element which is used as the anode during
electrolytic reduction of fused alumina in Hall Heroult’s process. [Recall]

(b) An alloy which is made up of aluminium and magnesium only. [Recall]

(c) The process of heating the concentrated ore in a limited supply of
air or in the absence of air. [Recall]

(ii) Rohit has three solutions X, Y and Z that have pH 2, 7 and 13 respectively. [3]
Which solution out of X, Y or Z will:

(a) liberate sulphur dioxide gas when heated with sodium sulphite? [Application]

(b) liberate ammonia gas when reacted with ammonium chloride? [Application]

(c) not have any effect on litmus paper? [Understanding]

(iii) A chloride of iron ‘R’, when treated with sodium hydroxide gives P and [4]
Q as a product. Q is a reddish-brown precipitate.

(a) Identify R. [Analysis]
(b) State the formula of the compounds P and Q formed after the
[Application]
reaction.

(c) What do you observe when excess NaOH is added to Q? [Recall]

Question 5

(i) 20 grams of a gas M2P has lesser number of moles than 20 grams of the [2]
gas MP.
Justify the above statement using mathematical calculations.
[At.wt. M=14, P=16] [Application]

T27 522 – SPECIMEN 12 of 16

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(ii) State giving reasons if: a [2]
(a) Zinc metal and aluminium metal can be distinguished by heating the
metal powders separately in two different test tubes with
concentrated sodium hydroxide solution. [Analysis]

(b) Zinc nitrate and lead nitrate can be distinguished by adding

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ammonium hydroxide solution to the salt solution. [Analysis]
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l [3]
(iii)
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Write balanced chemical equations for the following conversions
g a
a
(A to C):

[Application]
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(iv)
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An element ‘P' has 3 valence electrons in its L - shell and an element ‘Q’ [3]

g laUsing this information, answer the
has 7 valence electrons in its M - shell.
following questions: a
(a) Identify the exact position of element ‘Q’ in terms of group and
period in the Modern Periodic Table. [Application]

(b) The atomic radius of P is __________ (more/less) than that of Q. [Understanding]

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Question 6
c m.co
m . Identify the reactants P, Q and R in the following reactions: s e
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(i) [3]
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(a) Copper (II) oxide + P Copper + Water + Nitrogen [Analysis]

(b) Iron pyrite + Q Iron oxide + Sulphur dioxide [Understanding]

(c) Ammonia + R Nitrogen + Water [Analysis]

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(ii) Solid ammonium dichromate decomposes as under: [3]

(NH4)2Cr2O7 N2 + Cr2O3 + 4H2O

If 126 g of ammonium dichromate decomposes, calculate:

(a) the number of moles of ammonium dichromate that undergoes
decomposition.

(b) the mass of chromic oxide formed at the same time.

(c) the volume of nitrogen gas evolved at STP.

[ At wt: N = 14, Cr = 52, O = 16, H = 1] [Application]

(iii) Rohan has two test tubes, A containing sodium chloride and B containing [4]
ammonium chloride as shown in the diagram below. He adds sodium
hydroxide solution to both the test tubes and warms them gently.

Answer the following questions:

(a) In which test tube (A or B) will Rohan observe the evolution of a
gas? [Understanding]
(b) Name the gas that is evolved. [Recall]

(c) What will be the colour of the flame when this gas burns in oxygen? [Recall]

(d) Write an equation for the reaction that occurs in the test tube in
which the gas has evolved. [Application]

T27 522 – SPECIMEN 14 of 16

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Question 7 a
(i) What is the ratio of methane to the acidic gaseous product obtained when [2]
methane undergoes complete combustion? Give a balanced equation for
[Application]
the above reaction.

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(ii) The diagram below illustrates the structures of two atoms P and Q. [2]

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a
P Q

What is the formula and mass of one mole of the compound formed when
P and Q react together? [Application]

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[ At. wt of P is 23 and Q is 16]

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g lthea following:
(iii)
a
Give balanced equations for each of [3]

(a) Action of warm water on calcium carbide. [Recall]

(b) Oxidation of sulphur with conc. nitric acid. [Recall]

(c) Laboratory preparation of ethane by using sodium propionate and
[Application]
soda lime.

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c. o In a round bottom flask, a mixture of ethanol, acetic acid and concentratedm .co
(iv)
s e [3]

s em sulphuric acid was heated. g l a
la a
ag Answer the following questions:

(a) Name the type of reaction occurring in the above set up. [Understanding]

(b) What is the role of sulphuric acid in this reaction? [Understanding]

(c) State one observation that takes place during the reaction. [Recall]

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Question 8
(i) In the reactivity series of metals, Z is a metal above hydrogen and its [3]
oxide has the formula ZO. It was found that ZO reacted with water and
formed a hydroxide as the product. With reference to the above context,
answer the following questions:

(a) State the number of valence electrons present in element Z. [Recall]
(b) Name the group which Z belongs to. [Recall]
(c) What will be the formula of the hydroxide of Z? [Application]

(ii) Draw the electron dot structure of: [3]
(a) ammonium ion (also label the co-ordinate bond) [Application]
(b) nitrogen molecule [Application]
[Atomic No.: N = 7, H = 1]

(iii) The structures of five organic compounds, C, D, E, F and G are shown. [4]

Answer the following questions about these compounds.
(Each compound may be used once, more than once or not at all.)

State which compound, C, D, E, F or G:

(a) on halogenation will form F. [Analysis]

(b) is an alcohol. [Understanding]

(c) is an isomer of 2-methyl propane. [Analysis]

(d) is in the same homologous series as ethene. [Analysis]

T27 522 – SPECIMEN 16 of 16

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a
DRAFT MARKING SCHEME – CHEMISTRY (SCIENCE PAPER 2)

Question 1 [15x1]
(i) (c) X - iodine, Y - bromine

(ii) (d) concentrated sulphuric acid followed by water

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(iii) (b) In acidic solutions, current is carried by ions.
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(iv) (c) 3 and 4
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(v) (d) P - zinc, Q - copper (II) oxide

(vi)
l
(a)ag acid

(vii) (a) Both the statements are true.

(viii) (c) Both (A) and (R) are true and (R) is the correct explanation of (A).

(ix) (b) Q

(x) (a) Only 1
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(xi) (b) C2H4
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(xii) (b) H3O+

(xiii) (b) Sodium sulphide ag
(xiv) (c) 3 and 4

(xv) (d) 4.48 litres

Question 2
(i) (a) OH-1 - e → OH ; 4OH → 2H2O + O2
o m [5x1]
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The gas rekindles a glowing splinter / turns alkaline pyrogallol brown

s e
em a
(c) Hydrogen
s g lsulphuric acid is
la a
(d) Pure water does not conduct electricity, to produce ions,

ag added to water.
(e) The ratio of A : B is 1 : 2.

(ii) (a) CHCl3 + Cl2 → CCl4 + HCl [5x1]
(b) Al2O3.2H2O + 2NaOH → 2NaAlO2 + 3H2O
(c) ZnO + 2NaOH → Na2ZnO2 + H2O

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T27 522 - SPECIMEN

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(d) 3Cu + 8HNO3 → 3 Cu(NO3)2 + 4H2O + 2NO
(e) NaNO3 + H2SO4 NaHSO4 + HNO3
Below 200°C

(iii) (a) CnH2n+1 [5x1]
(b) Zinc chloride
(c) NH3
(d) Steel
(e) NH4Cl

(iv) [5x1]
A 4. Redox
B 3. Reduction
C 5. Electrolytic dissociation
D 1. Oxidation
E 2. Ionization

(v) (a) [5x1]
1) butan-1-oic acid / butanoic acid/ 1-butanoic acid
2) 2 - methyl pentane

(b)
1) diethyl ether

2) isopentane

3) propanone

T27 522 - SPECIMEN 2 of 5

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(i) a [2]

(ii) (a) Yellow oily liquid is formed which is explosive [2]
(b) Reddish-brown gas/ a gas which rekindles a glowing splinter/ a residue
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which is yellow when hot and white when cold is formed

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c
. O / copper sulphate pentahydrate s e
(iii) (a)
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CuSO .5H 4 2
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(b)
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Dehydrating property
ag
(c) g CuSO .5H O
a 4 2 CuSO + 5H O
Conc. H2SO4
4 2

(iv) (a) N2O [3]
(b) N2O + H2O → 2NOH
(c) N2SO4

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Question 4

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(i) (a) Carbon [3]
(b) Magnalium
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(c) Calcination
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(ii) (a) X [3]
(b) Z
(c) Y

(iii) (a) R=Ferric chloride [1]

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(b) P=NaCl Q= Fe(OH)3 [2]

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(c) The ppt. remains insoluble in excess of NaOH [1]
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m 5
eQuestion l as
s
la (i) ag
ag M2P MP [2]

44g of M2P = 1 Mole 30 g of MP = 1mole
20 g of M2P = 1×20/44=0.44moles 20g of MP= 1×20/30=0.66moles

Therefore, M2P has a lesser number of moles.

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T27 522 - SPECIMEN

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(ii) (a) No, both will liberate hydrogen gas which burns with a pop sound. [2]
(b) Yes, with zinc nitrate white ppt. will be formed which is soluble in excess of
ammonium hydroxide but with lead nitrate white ppt. is formed which
remains insoluble in excess.

(iii) A = Zn + H2SO4  ZnSO4 + H2 [3]
B = Zn + S ZnS
C = ZnSO4 + 2NaOH  Zn(OH)2 + Na2SO4 or with NH4OH

(iv) (a) Period 3, Group 17 [2]
(b) less [1]

Question 6
(i) (a) P- Ammonia [3]
(b) Q- Oxygen
(c) R- Oxygen

(ii) (a) 252 g of Ammonium dichromate = 1mole [3]
126 g of Ammonium dichromate = 0.5 moles

(b) 252 g of ammonium dichromate gives 152 g of chromic oxide
126 g of ammonium dichromate provides 152×126/ 252 = 76 g of
chromic oxide

(c) 252 g of ammonium dichromate produces 22.4 l of nitrogen
126 g of ammonium dichromate produces 22.4×126/ 252 = 11.2 l of
nitrogen

(iii) (a) Test tube B [4]
(b) Ammonia gas
(c) Green / Greenish yellow
(d) NH4Cl + NaOH → NaCl + NH3 + H2O

Question 7
(i) Ratio is 1:1 [2]
CH4 + 2O2 → CO2 + 2H2O

T27 522 - SPECIMEN 4 of 5

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se Formula - P2Q
g l a [2]
Molecular mass - 2x 23 + 16 a
= 46 +16
= 62
So, 1 mole of the compound = 62 g

(a) CaC2 + 2H2O → Ca(OH)2 + C2H2
m
(iii) [3]

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(b) S +conc. 6HNO3 → H2SO4 + 6NO2 + 2H2O
e m
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(c) C2H5COONa + NaOH → C2H6 + Na2CO3
l as
l as CaO
ag
(iv) g
(a)a Esterification [3]
(b) dehydrating agent
(c) Fruity smell is obtained

Question 8
(i) (a) 2 [3]
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(b) Group 2 / Alkaline earth metals
(c) Z(OH)2
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(ii) (a) ammonium ion ag [2]

(b) nitrogen molecule [1]
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m [Atomic No.: N = 7, H = 1]
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s em g l a
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a (iii) (a) G [4]
(b) D
(c) E
(d) C

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T27 522 - SPECIMEN

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