The Chemistry (School & UG) category covers the fundamental to advanced concepts of Chemistry, structured to support Class 11–12 students, competitive exam aspirants, and undergraduate learners. The content emphasizes conceptual clarity, problem-solving skills, and strong alignment with NCERT and university syllabi.
In this category, you will study:
Physical Chemistry – atomic structure, thermodynamics, chemical kinetics, equilibrium, electrochemistry, and solutions
Inorganic Chemistry – periodic trends, chemical bonding, coordination compounds, metallurgy, and s-, p-, d-, and f-block elements
Numerical problem-solving – formula-based calculations, mole concept, and graph-based questions
Reaction mechanisms and derivations with step-by-step explanations
Comparisons, trends, and exceptions important for exams
NCERT-based theory, supported by diagrams, tables, MCQs, assertion–reason questions, numericals, and PYQs
The content is designed to build strong foundations, improve analytical and quantitative skills, and prepare students for school examinations, competitive exams, and undergraduate assessments.
Develop a clear, logical, and application-oriented understanding of Chemistry to excel academically and confidently tackle problem-based and conceptual questions at both school and UG levels.
Q. If the activation energy of a reaction is 50 kJ/mol, what is the effect of increasing the temperature from 300 K to 350 K on the rate constant?
A.
Rate constant decreases
B.
Rate constant remains the same
C.
Rate constant increases
D.
Rate constant doubles
Solution
According to the Arrhenius equation, an increase in temperature generally increases the rate constant, as it provides more energy to overcome the activation energy barrier.
Q. If the concentration of Cu²⁺ in a cell is 0.01 M and the standard reduction potential is +0.34 V, what is the cell potential at 25°C using the Nernst equation?
A.
0.34 V
B.
0.30 V
C.
0.28 V
D.
0.25 V
Solution
E = E° - (RT/nF)ln(Q); E = 0.34 - (0.0257/2)ln(100) = 0.30 V.
Q. If the enthalpy change (ΔH) for a reaction is -150 kJ and the reaction occurs at constant pressure, how much heat is released when 3 moles of reactants are consumed?
A.
50 kJ
B.
150 kJ
C.
450 kJ
D.
300 kJ
Solution
Heat released = ΔH * n = -150 kJ * 3 mol = -450 kJ.
Q. If the equilibrium constant Kp for the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) is 25 at a certain temperature, what is Kp if the volume of the system is halved?
A.
12.5
B.
25
C.
50
D.
100
Solution
Kp is independent of volume changes; it remains 25.
Q. If the rate constant of a reaction doubles when the temperature increases by 10°C, what is the approximate activation energy?
A.
20 kJ/mol
B.
40 kJ/mol
C.
60 kJ/mol
D.
80 kJ/mol
Solution
Using the Arrhenius equation and the rule of thumb that a 10°C increase roughly doubles the rate constant, we can estimate the activation energy to be around 40 kJ/mol.
Q. If the rate of a reaction is tripled when the concentration of reactant A is doubled, what is the order of the reaction with respect to A?
A.
0
B.
1
C.
2
D.
3
Solution
If tripling the rate occurs when doubling the concentration, the reaction is first order with respect to A, as rate ∝ [A]^n implies 3 = 2^n, leading to n = 1.
Q. If the temperature of an exothermic reaction at equilibrium is increased, what is the expected effect on the equilibrium position?
A.
Shifts to the right
B.
Shifts to the left
C.
No effect
D.
Reaction rate increases
Solution
For an exothermic reaction, increasing the temperature shifts the equilibrium to the left, favoring the reactants, as the system attempts to absorb the added heat.
Q. If the temperature of an exothermic reaction at equilibrium is increased, what will happen to the equilibrium position?
A.
Shift to the right
B.
Shift to the left
C.
No change
D.
Reaction rate increases
Solution
For an exothermic reaction, increasing the temperature shifts the equilibrium to the left, favoring the reactants, as the system tries to absorb the added heat.
