Kerala SSLC Chemistry Model Question Paper 2 English Medium

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Kerala SSLC Chemistry Model Question Paper 2 English Medium

General Instructions:

1. The first 15 minutes is the cool off time. You may use the time to read and plan your answers.
2. Answer the questions only after reading the instructions and questions thoroughly.
3. Questions with marks series 1, 2, 3 and 4 are categorized as sections A, B, C and D respectively.
4. Five questions are given in each section. Answer any four from each section.
5. Answer each question by keeping the time.

Time: 1½ Hours
Total Score: 40 Marks

Section  – A

(Answer any 4 questions from 1 to 5. Each question carries 1 score) (4 × 1 = 4)

Question 1.
Which one of the following is not possible?
a) 2s ²
b) 3p³
c) 2d⁵
d) 4F²
Answer:
NH₄OH

Question 2.
Which metal cannot displace copper from CuSO₄. solution.
a) Magnessium
b) Silver
c) Zinc
d) Iron
Answer:
Silver

Question 3.
The substance obtained at the cathode when NaCl solution is electrolysed is …………..
a) Sodium
b) Chlorine
c) Hydrogen
d) Sodium hydroxide
Answer:
Hydrogen

Question 4.
The chemical formula of liquor ammonia is ………..
a) NH₄OH
b) NH₄Cl
c) (NH₂)SO₄
d) NH₃
Answer:
NH₄OH

Question 5.
The symbol of carboxylase functional group is ……………
a) -OH
b) – COOH
c) -CH₃
d) – O –
Answer:
-COOH

Section – B

(Answer any 4 questions from 6 to 10. Each question carries 2 scores)(4 × 2 = 8)

Question 6.
The subshell electron Configuration of certain elements are given below.
Find out the wrong ones and correct them (symbols are not real)
a) ₁₂P = 1s²2s²2p⁶3s²
b) ₆Q = 1s²2s²3s²
c) ₁₇₈R = 1s²2s²2p⁶3s²3p⁶
d) ₂₀S = 1s²2s²2p⁶3s²3p⁶3d²
Answer:
Q – 1s²2s²2p²
S – 1s²2s²2p⁶3s²3p⁶3d⁶4s²

Question 7.
Calculate the number of molecules in 90g of water.
(Hint -Atomic mass H = 1 O = 16)
Answer:
1 GMM of water = 18 g.
90 g water = \(\frac{90}{18}\) = 5 mol
No. of molecules in 5 mol = 5 x 6.022 x 10²³

Question 8.
Observe the solutions and the metals placed in three test tubes.

a) In which test tube a chemical reaction is likely to take place? Why. (1)
b) Write the name of the reaction. (1)
c) Write the equation of the redox reaction taking place here. (1)
Answer:
a) In test tube 2. More reactive iron displaces copper from CuSO₄ solution.
b) Displacement reactions
c) Fe + Cu²⁺ → Fe²⁺ + Cu

Question 9.
Metallurgy involves all the process leading to the separation of a pure metal from its ore.
a) Distinguish a mineral from an ore. (1)
b) What type of ores are usually concentrated by froth floatation process. Given an example. (2)
Answer:
a) Elements or their compounds, occurring naturally and obtained by mining are called minerals, Ore is the mineral from which a metal is extracted economically, easily and quickly.
b) Sulphide ores eg. Copper pyrites.

Question 10.
Analyse the chemical equations given below and answer the questions that follow.

a) Identify A, B and C. (2)
b) Write what type of chemical reactions (i) and (ii) are (1)
Answer:
a) A = CH₃-CH = CH₂ or C₃H₆
B = CH₃ – CH₂ – CH₃ or C₃H₈
C = CH₃ – CH₂ – CH₂ – Cl

b) i) Addition reaction
ii) Substitution reaction

Section – C

(Answer any 4 questions from 11 to 15. Each question carries 3 scores) (4 × 3 = 12)

Question 11.
The outermost electronic configuration of an element , X is 3s² 3p¹. Answer the questions given below related
to this element. (Symbol of the element is not actual).
a) What is the atomic number of this element? (1)
b) Write the group number and period number of X? (1)
c) Write the formula of the oxide of this element?(1)
Answer:
a) 13
b) Group-13, Period-3
c) X₂O₃

Question 12.
The atomic masses of certain elements are S = 32, O = 16, H = 1,C = 12
a) Find out 1 GMM of H₂SO₄ (1)
b) Find out the number of molecules in 220 gCO₂(2)
c) What will be the volume of 1 mole SO₂ at STP?(1)
Answer:
a) 98g
b) 220g CO₂ = \(\frac{220}{44}\) = 5 mol
No. of molecules in 5 mol = 5 x 6.022 x 10²³
c) 22.4 L

Question 13.
Analyse the picture of an electro chemical cell given below, and answer the questions that follow.

a) Which are the anode and cathode in this cell?(1)
b) Write the equation of chemical reaction taking
place at both of the electrodes. (2)
c) Write the equation of the redox reaction.
Answer:
a) Anode – Mg
Cathode – Cu
b) At anode Mg →Mg²⁺ + 2e^–
At cathode Ca²⁺ + 2e^– → Cu
c) Mg + Cu²⁺ → Mg²⁺ + Cu

Question 14.
Certain metals their characteristics and the method of refining are tabled below. Match them suitably.(3)

Answer:
Tin-Low melting point – Liquation
Mercury – Low boiling point – Distillation
Copper – Low electropositivity – Electrolysis

Question 15.
The structural formula of an organic compound is given below.
CH₃-CH₂-CH₂-CH₂-OH
a) Write the IUPAC name of the compound. (1)
b) Write the structure of a position isomer of this compound. (1)
c) Write the structure of a functional group isomer of this compound. (1)
Answer:
a) Butan -1 – ol

(c) CH₃ – CH₂ – O – CH₂ – CH₃ (OR)
CH₃ – O – CH₂ – CH₂ – CH₃

Section – D

(Answer any 4 questions from 16 to 20. Each question carries 4 scores)(4 × 4 = 16)

Question 16.
The chemical equation showing the preparation of 8 -10% of ethnol is given below

a) Write the products A and B. (1)
b) How the product obtained is converted in to rectified spirit? (1)
c) What is denatured spirit? (1)
Answer:
a) A = C₆H₁₂O₆
A = CO₂
b) By fractional distillation
c) Ethanol added with poisonous substances to avoid its misuse as a beverage.

Question 17.
Analyse the compounds given below

a) Which among these compounds is an ester?(1)
b) Choose the compounds required to form this ester and write the chemical equation. (1)
c) Write any two uses of esters. (1)
Answer:
a) CH₃-COO-CH₃
b) CH₃-COOH-CH₃-OH →CH₃-COO-CH₃
c) Used as a flavouring agent for food. Used for making perfumes.

Question 18.
Two reversible reactions are given below:
i) H₂(g) + l₂(g)⇌ 2Hl(g)
ii) N₂(g) + 3H₂(g) ⇌ 2NH₃(g) + Heat
a) In which reaction change of pressure has no effect.
b) Suggest two methods to increase the amount of product in the second reaction.
c) Even though the forward reaction is exothermic the temperature is maintained at 450°C. Why?
Answer:
a) Pressure has no effect in reaction -1. Because there is no change in number of molecules due to forward and backward reactions.
b) Increase pressure Increase the concentration of the reactants Remove the products continuously from the system.
c) 450°C is the optimum temperature of this reaction. At this temperature maximum product is obtained. At low temperature NH₃ decomposes back in the reactants.

Question 19.
At one end of a glass tube cotton soaked in cone.
HCl and at the other end of it cotton soaked in cone.
NH₄OH solution is inserted.

a) What will be the observation after sometime?
b) What will happen if the glass tube is heated?
c) Write equations of the chemical reactions in a and b
Answer:
a) A white precipitate is formed inside the glass tube. NH₃ gas and HCI gas combines to form NH₄Cl.
b) The precipitate disappears on heating. On heating NH₄Cl decomposes into NH₃ and HCl

c) NH₃ + HCI → NH₄Cl
NH₄Cl → NH₃ + HCl

Question 20.
Match those given in columns A, B and C suitably.

A	B	C
Bayles Law	Reversible Reaction	V&T
Charles Law	Volume & number of molecules	V ∝ 1/p
Avagadros Law	Volume & pressure	V ∝ η
Le-Chatelers principle	Volume and temperature	Equillibrium state

Answer:

A	B	C
Bayles Law	Volume & pressure	V&T
Charles Law	Volume and temperature	V ∝ 1/p
Avagadros Law	Volume & number of molecules	V ∝ η
Le-Chatelers principle	Reversible Reaction	Equillibrium state