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. What is the rate law for a reaction that is first order with respect to A and second order with respect to B?
A.
Rate = k[A][B]
B.
Rate = k[A]^1[B]^2
C.
Rate = k[A]^2[B]^1
D.
Rate = k[A]^2[B]^2
Solution
The rate law is determined by the order of the reaction with respect to each reactant. For first order in A and second order in B, the rate law is Rate = k[A]^1[B]^2.
Q. What is the rate law for a reaction that is second order in A and first order in B?
A.
Rate = k[A]^2[B]
B.
Rate = k[A][B]^2
C.
Rate = k[A][B]
D.
Rate = k[A]^2 + k[B]
Solution
The rate law is determined by the stoichiometry of the rate-determining step. For second order in A and first order in B, the rate law is Rate = k[A]^2[B].
Q. What is the rate law for the reaction A + B → C if the rate is found to be first order in A and second order in B?
A.
Rate = k[A][B]
B.
Rate = k[A]^2[B]
C.
Rate = k[A][B]^2
D.
Rate = k[A]^2[B]^2
Solution
The rate law is determined by the orders of the reactants. Since the reaction is first order in A and second order in B, the rate law is Rate = k[A][B]^2.
Q. What is the relationship between enthalpy and internal energy at constant pressure?
A.
ΔH = ΔU + PΔV.
B.
ΔH = ΔU - PΔV.
C.
ΔH = ΔU.
D.
ΔH = PΔV.
Solution
At constant pressure, the change in enthalpy (ΔH) is related to the change in internal energy (ΔU) and the pressure-volume work done (PΔV) by the equation ΔH = ΔU + PΔV.
Q. What is the relationship between Gibbs free energy and cell potential?
A.
G = -nFE
B.
G = nFE
C.
G = 0
D.
G = nF/E
Solution
The relationship is given by the equation G = -nFE, where G is Gibbs free energy, n is moles of electrons, F is Faraday's constant, and E is cell potential.
Q. What is the relationship between pressure and volume for an ideal gas at constant temperature?
A.
Boyle's Law
B.
Charles's Law
C.
Avogadro's Law
D.
Graham's Law
Solution
Boyle's Law states that for a given mass of gas at constant temperature, the pressure of the gas is inversely proportional to its volume (P1V1 = P2V2).
Q. What is the relationship between the rate constant and temperature according to the Arrhenius equation?
A.
Rate constant is independent of temperature
B.
Rate constant increases with temperature
C.
Rate constant decreases with temperature
D.
Rate constant is constant at all temperatures
Solution
According to the Arrhenius equation, the rate constant increases with temperature due to the exponential dependence on the negative activation energy divided by temperature.
Correct Answer:
B
— Rate constant increases with temperature
