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 effect of a higher concentration of reactants on the rate of a reaction?
A.
Rate decreases
B.
Rate increases
C.
Rate remains constant
D.
Rate becomes zero
Solution
According to the rate laws, increasing the concentration of reactants generally increases the rate of reaction, as it leads to more frequent collisions.
Q. What is the effect of adding a strong acid to a reaction at equilibrium involving a weak base?
A.
Shifts equilibrium to the right
B.
Shifts equilibrium to the left
C.
No effect on equilibrium
D.
Increases reaction rate
Solution
Adding a strong acid increases the concentration of H+ ions, which can react with the weak base, shifting the equilibrium to the left to favor the formation of reactants.
Correct Answer:
B
— Shifts equilibrium to the left
Q. What is the effect of adding an inert gas at constant volume to a reaction at equilibrium?
A.
Shifts equilibrium to the right
B.
Shifts equilibrium to the left
C.
No effect on equilibrium
D.
Increases the reaction rate
Solution
Adding an inert gas at constant volume does not change the partial pressures of the reactants or products, thus it has no effect on the position of the equilibrium.
Q. What is the effect of adding an inert gas at constant volume to a system at equilibrium?
A.
Shifts the equilibrium to the right
B.
Shifts the equilibrium to the left
C.
No effect
D.
Increases the reaction rate
Solution
Adding an inert gas at constant volume does not change the partial pressures of the reactants or products, thus it has no effect on the equilibrium position.
Q. What is the effect of adding an inert gas to a reaction at equilibrium at constant volume?
A.
Shifts the equilibrium to the right
B.
Shifts the equilibrium to the left
C.
No effect
D.
Increases the reaction rate
Solution
Adding an inert gas at constant volume does not change the partial pressures of the reactants or products, thus having no effect on the equilibrium position.
Q. What is the effect of decreasing the volume of a gaseous reaction mixture at equilibrium?
A.
Shifts to the side with more moles of gas
B.
Shifts to the side with fewer moles of gas
C.
No effect
D.
Increases the temperature
Solution
Decreasing the volume increases the pressure, and according to Le Chatelier's Principle, the equilibrium will shift to the side with fewer moles of gas to counteract the change.
Correct Answer:
B
— Shifts to the side with fewer moles of gas
Q. What is the effect of decreasing the volume of the container on the equilibrium of the reaction 2N2O(g) ⇌ 2N2(g) + O2(g)?
A.
Shift to the left
B.
Shift to the right
C.
No change
D.
Increase the rate of reaction
Solution
Decreasing the volume increases the pressure, shifting the equilibrium towards the side with fewer moles of gas. The left side has 2 moles (N2O) compared to 3 moles (N2 + O2), so it shifts to the left.
Q. What is the effect of increasing temperature on the rate of a chemical reaction according to the Arrhenius equation?
A.
Rate decreases
B.
Rate remains constant
C.
Rate increases exponentially
D.
Rate increases linearly
Solution
According to the Arrhenius equation, an increase in temperature results in an exponential increase in the rate constant, thus increasing the reaction rate.
Q. What is the effect of increasing temperature on the rate of a chemical reaction according to collision theory?
A.
Decreases the rate
B.
Increases the rate
C.
No effect
D.
Depends on the reaction
Solution
Increasing temperature increases the kinetic energy of molecules, leading to more frequent and effective collisions, thus increasing the reaction rate.
Q. What is the effect of increasing the concentration of a product in a reaction at equilibrium?
A.
Shifts equilibrium to the right
B.
Shifts equilibrium to the left
C.
No change occurs
D.
Increases reaction rate
Solution
Increasing the concentration of a product will shift the equilibrium to the left, favoring the formation of reactants, according to Le Chatelier's Principle.
Correct Answer:
B
— Shifts equilibrium to the left
