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100+ Free Kerala Plus Two Chemistry Practice Questions

Kerala DHSE Higher Secondary Plus Two Chemistry (Class 12) practice questions are available now; exam metadata is being verified.

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Key Facts: Kerala Plus Two Chemistry Exam

~2 h + cool-off

Typical duration of the Plus Two Chemistry theory paper under DHSE Kerala, plus cool-off as notified

Kerala DHSE Higher Secondary examination timetable practice

TE + CE + Practical

Official subject total is 100 marks combining theory, continuous evaluation, and practical; this bank is an English MCQ study adaptation only

Kerala DHSE Higher Secondary Chemistry assessment pattern

D+ / ~30%

Typical minimum grade band ~30% aggregate with about ~30% TE as notified for promotion — confirm the year's grading circular

DHSE Higher Secondary grading notifications

Fee via school

Examination fees are typically paid through the school under DHSE notifications (not a fixed chemistry-only marketplace price)

DHSE fee notification practice

DHSE Kerala

Administrator is the Directorate of Higher Secondary Education (DHSE), Kerala, with SCERT syllabus support

dhsekerala.gov.in / SCERT Kerala

100 FREE MCQs

Local practice bank size for concept and calculation drill (not the official item count)

OpenExamPrep practice bank

Free 100-question English MCQ study bank for Kerala DHSE Plus Two Chemistry (Class 12). Official exams use TE + CE + Practical (100 marks total), ~2 h theory + cool-off; pass typically D+/~30% aggregate with ~30% TE as notified; fee via schools as notified by DHSE. Not an official full-format simulation. Sources: dhsekerala.gov.in, beta.hseportal.kerala.gov.in, SCERT Kerala, and NCERT Class 12 Chemistry.

Sample Kerala Plus Two Chemistry Practice Questions

Try these sample questions to test your Kerala Plus Two Chemistry exam readiness. Each question includes a detailed explanation. Start the interactive quiz above for the full 100+ question experience with AI tutoring.

1Molality of a solution is defined as the number of moles of solute per:
A.Kilogram of solution
B.Litre of solution
C.Litre of solvent
D.Kilogram of solvent
Explanation: Molality (m) = moles of solute / mass of solvent in kg. Molarity uses litres of solution.
2Which concentration unit is independent of temperature?
A.Volume percent
B.Normality
C.Molality
D.Molarity
Explanation: Molality is based on mass of solvent, which does not change with temperature. Volume-based units vary as density changes with T.
3For an ideal binary solution of A and B, Raoult's law for the partial vapour pressure of A is:
A.p_A = x_B p_A°
B.p_A = (1 − x_A) p_A°
C.p_A = x_A p_B°
D.p_A = x_A p_A°
Explanation: Raoult's law: partial pressure of a component equals its mole fraction times its pure-component vapour pressure.
4A non-volatile solute is dissolved in a solvent. The vapour pressure of the solution compared with pure solvent is:
A.Higher
B.Unchanged
C.Lower
D.Zero always
Explanation: Non-volatile solute lowers the mole fraction of solvent at the surface, so solvent vapour pressure decreases (Raoult's law).
5Relative lowering of vapour pressure for a dilute solution of a non-volatile non-electrolyte equals:
A.Mole fraction of solvent
B.Molality of solute
C.Molarity of solute
D.Mole fraction of solute
Explanation: For non-volatile non-electrolyte: (p° − p)/p° = x_solute.
6Elevation of boiling point of a solvent by a non-volatile solute is proportional to:
A.Molarity of the solution only
B.Atmospheric pressure only
C.Density of pure solvent only
D.Molality of the solution
Explanation: ΔT_b = K_b m, where m is molality of solute particles (van't Hoff factor included for electrolytes).
7A solution contains 0.2 mol of a non-volatile non-electrolyte in 0.8 mol of solvent. The relative lowering of vapour pressure is:
A.0.25
B.0.80
C.0.20
D.1.0
Explanation: x_solute = 0.2/(0.2+0.8) = 0.2; relative lowering = x_solute = 0.20.
8Osmotic pressure of a dilute solution of a non-electrolyte is given by π =:
A.nRT only
B.RT/C
C.CRT
D.MRT/2
Explanation: van't Hoff equation: π = CRT, where C is molar concentration of solute.
9Which solution shows positive deviation from Raoult's law?
A.Acetone + carbon disulphide
B.Benzene + toluene (nearly ideal)
C.Chloroform + acetone (strong association)
D.n-Hexane + n-heptane (nearly ideal)
Explanation: Acetone–CS2 interactions are weaker than pure-component interactions, giving higher total vapour pressure (positive deviation).
10For a dilute aqueous solution of a strong electrolyte that fully dissociates into two ions (e.g., NaCl), the van't Hoff factor i approaches:
A.0
B.3
C.2
D.1
Explanation: NaCl → Na+ + Cl− gives two particles per formula unit, so i ≈ 2 (ignoring ion pairing).

About the Kerala Plus Two Chemistry Practice Questions

Verified exam format metadata for Kerala DHSE Higher Secondary Plus Two Chemistry (Class 12) is pending. The practice questions above remain available while official exam length, timing, passing score, fee, and administrator details are reviewed.