Class 12 PT I Question Paper 2025-26 Chemistry

PERIODIC TEST
QUESTION
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PT1 - PT2

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PT-1 SESSION 2025-26
TIME-90 MIN​ SUBJECT- CHEMISTRY
M.M.-40
1.Which of the following is a colligative propert
a)Ph b)Boiling point elevation c)Refractive index
d)Surface tension
2.The van’t Hoff factor for K₂SO₄ in aqueous solution is:
a)1 b)2 c)3
d)4
3.Which law relates molar conductivity to concentration?
a)Raoult’s law b) Faraday’s law c)Kohlrausch’s law
d)Henry’s law
4..Which of the following metals shows the maximum number of
oxidation states?
a)Fe b)Mn c)Cu
d)Zn
5.The colour of transition metal compounds is mainly due to:
a)d–d transitions b)s–s transitions c)p–p
transitions d)f–f transitions
6.Which of the following is used to make a salt bridge in
electrochemical cells?
a)NaCl b)KNO₃ c)CuSO₄
d)HCl
7.Which of the following is an ideal solution?
a)Benzene + Toluene b)Acetone + Water c)Ethanol +
Water d)HCl + Water
8. Faraday’s first law of electrolysis states that:
a)Mass deposited ∝ current b)Mass deposited ∝
time
c)Mass deposited ∝ charge d)Mass deposited ∝
voltage
These questions consist of two statements, each printed as

Assertion and Reason. While answering these questions, you are
required to choose any one of the following four responses.​
(a) If both Assertion and Reason are correct and the Reason is a
correct explanation of the Assertion.​

(b) If both Assertion and Reason are correct but Reason is not a
correct explanation of the Assertion.​
(c) If the Assertion is correct but Reason is incorrect.​
(d) If both the Assertion and Reason are incorrect.
9.Assertion : Cuprous ion (Cu+) has unpaired electrons while cupric
ion (Cu++) does not.​
Reason : Cuprous ion (Cu+) is colourless whereas cupric ion (Cu++)
is blue in the aqueous solution 10.Assertion: On increasing dilution,
the specific conductance keeps on increasing.​
Reason: On increasing dilution, the degree of ionisation of weak
electrolyte increases, and molality of ions also increases
Section A – Very Short Answer (1 mark each)
11.Define osmotic pressure.
12.State Henry’s law?
13.Write the cell reaction and cell notation for the Daniell cell.
14.Why is Mn²⁺ more stable than Fe²⁺ towards oxidation to +3
state?
15.what is semi permeable membrane ? give one example.
Section B – Short Answer I (2 marks each)
16.Calculate the boiling point elevation when 0.2 mol of NaCl is
dissolved in 1 kg of water. (Kb = 0.52 K kg/mol)
17.State Kohlrausch’s law and give one application.
18.Write the electronic configuration of Cu⁺ and explain why it is
not stable in aqueous solution.
19.What is lanthanoid contraction? Mention two consequence.
20.Differentiate positive and negative deviation from ideal
solution with suitable example.
Section C – Short Answer II (3 marks each)
21.X and Y are two electrolytes, on dilution, molar conductivityof X
increases 2.5 times while that of Y increases 25 times . Which of the
two is a weak electrolyte and why?
22.Calculate the EMF of the cell:​
Zn | Zn²⁺ (0.1 M) || Cu²⁺ (0.01 M) | Cu​

Given: E°(Zn²⁺/Zn) = –0.76 V, E°(Cu²⁺/Cu) = +0.34
​ Or
Define a)Cellconstant b)Conductivityc)Standard hydrogen electrode
23.Account for the following

a)Zn,Cd and Hg are volatile metals.
b)Cr has highest melting point.
c)Sc salts are colourless.
24.a)100 grams of ethylene glycol is added to 500 grams of water.
Find the depression in freezing point , given that the cryoscopic
constant (Kf) of water is 1.86°C/m.
b)Why do azeotropes form? Give on example of maximum boiling
azeotrope.
25.a)State Faraday’s first law of electrolysis.
b)Calculate the mass of copper deposited when a current of 2 A is
passed through CuSO₄ solution for 30 minutes. (M = 63.5 g/mol, n =
2, F = 96500 C/mol)

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