Chemistry (School & UG)

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Chemistry (School & UG)

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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
Organic Chemistry – basic principles, reaction mechanisms, hydrocarbons, functional groups, biomolecules, and polymers
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.

Analytical Techniques Inorganic Chemistry Organic Chemistry Physical Chemistry

Q. If the temperature of an exothermic reaction at equilibrium is increased, what will happen?

A. The equilibrium shifts to the right
B. The equilibrium shifts to the left
C. No change occurs
D. The 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.

Correct Answer: B — The equilibrium shifts to the left

Q. If the temperature of an exothermic reaction at equilibrium is increased, what will be the 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 tries to absorb the added heat.

Correct Answer: B — Shifts to the left

Q. If the temperature of an exothermic reaction is increased, what is the expected effect on the equilibrium?

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 tries to absorb the added heat.

Correct Answer: B — Shifts to the left

Q. If the temperature of an exothermic reaction is increased, what will happen to the equilibrium?

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.

Correct Answer: B — Shift to the left

Q. If the temperature of the exothermic reaction A + B ⇌ C + heat is increased, what will be the effect on the equilibrium position?

A. Shift to the left
B. Shift to the right
C. No change
D. Increase the rate of reaction

Solution

According to Le Chatelier's Principle, increasing the temperature of an exothermic reaction shifts the equilibrium to the left, favoring the reactants.

Correct Answer: A — Shift to the left

Q. In a back titration, what is the first step?

A. Add excess titrant to the analyte
B. Measure the pH of the solution
C. Dilute the analyte solution
D. Add a color indicator

Solution

In a back titration, the first step is to add an excess of titrant to the analyte, followed by titrating the unreacted titrant.

Correct Answer: A — Add excess titrant to the analyte

Q. In a calorimetry experiment, if 100 g of water absorbs 4200 J of heat, what is the change in temperature assuming no heat loss?

A. 1 °C
B. 2 °C
C. 3 °C
D. 4 °C

Solution

Using q = mcΔT, ΔT = q/(mc) = 4200 J / (100 g * 4.18 J/g°C) = 10 °C.

Correct Answer: A — 1 °C

Q. In a calorimetry experiment, if 50 g of water is heated from 25 °C to 75 °C, what is the heat absorbed (q) assuming specific heat capacity of water is 4.18 J/g°C?

A. 1045 J
B. 2090 J
C. 1250 J
D. 500 J

Solution

q = mcΔT = 50 g × 4.18 J/g°C × (75-25)°C = 1045 J.

Correct Answer: B — 2090 J

Q. In a calorimetry experiment, what does a negative q value indicate?

A. Heat is absorbed by the system.
B. Heat is released by the system.
C. No heat exchange occurs.
D. The reaction is at equilibrium.

Solution

A negative q value indicates that heat is released by the system, signifying an exothermic process.

Correct Answer: B — Heat is released by the system.

Q. In a calorimetry experiment, what does a negative ΔH indicate?

A. The reaction is endothermic.
B. The reaction is exothermic.
C. No heat exchange occurs.
D. The system is at equilibrium.

Solution

A negative ΔH indicates that the reaction releases heat to the surroundings, classifying it as exothermic.

Correct Answer: B — The reaction is exothermic.

Q. In a calorimetry experiment, what does a positive q value indicate?

A. Heat is released by the system
B. Heat is absorbed by the system
C. No heat exchange occurs
D. The system is at equilibrium

Solution

A positive q value indicates that the system absorbs heat from the surroundings.

Correct Answer: B — Heat is absorbed by the system

Q. In a chemical equilibrium, what does a large equilibrium constant (K) indicate?

A. Products are favored at equilibrium
B. Reactants are favored at equilibrium
C. Equilibrium is not established
D. Reaction is slow

Solution

A large equilibrium constant (K) indicates that at equilibrium, the concentration of products is much greater than that of reactants, favoring products.

Correct Answer: A — Products are favored at equilibrium

Q. In a chemical reaction, if the enthalpy change (ΔH) is negative, what does this indicate?

A. The reaction is endothermic
B. The reaction is exothermic
C. The reaction is at equilibrium
D. The reaction requires energy input

Solution

A negative ΔH indicates that the reaction releases heat to the surroundings, classifying it as exothermic.

Correct Answer: B — The reaction is exothermic

Q. In a chemical reaction, if ΔH is negative, the reaction is classified as:

A. Endothermic
B. Exothermic
C. Isothermal
D. Adiabatic

Solution

A negative ΔH indicates that the reaction releases heat, classifying it as exothermic.

Correct Answer: B — Exothermic

Q. In a closed container, if the temperature of a gas is increased, what happens to its pressure?

A. Pressure decreases
B. Pressure increases
C. Pressure remains constant
D. Pressure fluctuates

Solution

According to Gay-Lussac's Law, at constant volume, the pressure of a gas is directly proportional to its temperature in Kelvin.

Correct Answer: B — Pressure increases

Q. In a closed container, if the temperature of a gas is increased, what happens to the pressure if the volume remains constant?

A. Pressure decreases
B. Pressure remains constant
C. Pressure increases
D. Pressure fluctuates

Solution

According to Gay-Lussac's Law, pressure is directly proportional to temperature at constant volume (P/T = k).

Correct Answer: C — Pressure increases

Q. In a closed system, if 100 J of heat is added to a gas and it does 40 J of work, what is the change in internal energy (ΔU) according to the first law of thermodynamics?

A. 60 J
B. 40 J
C. 100 J
D. 140 J

Solution

ΔU = Q - W = 100 J - 40 J = 60 J.

Correct Answer: A — 60 J

Q. In a closed system, if the internal energy increases, what can be said about the work done on the system?

A. Work is done by the system.
B. Work is done on the system.
C. No work is done.
D. Work is irrelevant.

Solution

If the internal energy of a closed system increases, it indicates that work is done on the system.

Correct Answer: B — Work is done on the system.

Q. In a closed system, if the internal energy of the system increases, what can be said about the enthalpy?

A. Enthalpy decreases
B. Enthalpy increases
C. Enthalpy remains constant
D. Enthalpy is independent of internal energy

Solution

If the internal energy increases in a closed system, the enthalpy also increases, as ΔH = ΔU + PΔV.

Correct Answer: B — Enthalpy increases

Q. In a closed system, if the volume of a gas is halved while the temperature remains constant, what happens to the pressure?

A. It doubles
B. It halves
C. It remains the same
D. It quadruples

Solution

According to Boyle's Law, if the volume is halved, the pressure will double (P1V1 = P2V2).

Correct Answer: A — It doubles

Q. In a closed system, what happens to the pressure of a gas if its volume is halved at constant temperature?

A. Pressure doubles
B. Pressure halves
C. Pressure remains the same
D. Pressure quadruples

Solution

According to Boyle's Law, if the volume is halved, the pressure will double (P1V1 = P2V2).

Correct Answer: A — Pressure doubles

Q. In a closed system, what happens to the total pressure when the volume is decreased at constant temperature?

A. Increases
B. Decreases
C. Remains constant
D. Fluctuates

Solution

According to Boyle's Law, decreasing the volume of a gas at constant temperature increases the pressure.

Correct Answer: A — Increases

Q. In a concentration cell with Ag⁺ at 0.1 M and Ag⁺ at 1 M, what is the cell potential at 25°C?

A. 0.059 V
B. 0.118 V
C. 0.177 V
D. 0.236 V

Solution

E = E° - (0.059/n)log([Ag⁺]1/[Ag⁺]2); E = 0 - (0.059/1)log(10) = 0.059 V.

Correct Answer: B — 0.118 V

Q. In a concentration cell, if the concentration of the anode is 0.1 M and the cathode is 1.0 M, what is the cell potential at 25°C?

A. 0.059 V
B. 0.118 V
C. 0.059 log(10)
D. 0.118 log(10)

Solution

E = (0.059 V/n) * log([Cathode]/[Anode]) = (0.059 V/2) * log(10) = 0.059 V.

Correct Answer: B — 0.118 V

Q. In a concentration cell, if the concentration of the anode is 0.1 M and the cathode is 1 M, what is the cell potential at 25°C?

A. 0.059 V
B. 0.118 V
C. 0.059 log(10)
D. 0.118 log(10)

Solution

E = (0.059 V/n) * log([Cathode]/[Anode]) = (0.059 V/2) * log(1/0.1) = 0.059 V * 1 = 0.059 V.

Correct Answer: B — 0.118 V

Q. In a concentration cell, the cell potential is dependent on:

A. Temperature only
B. Concentration differences
C. Electrode material
D. Surface area of electrodes

Solution

In a concentration cell, the cell potential is dependent on the concentration differences of the reactants.

Correct Answer: B — Concentration differences

Q. In a concentration cell, the cell potential is generated due to:

A. Different temperatures
B. Different concentrations
C. Different pressures
D. Different electrode materials

Solution

In a concentration cell, the cell potential is generated due to differences in ion concentrations.

Correct Answer: B — Different concentrations

Q. In a constant pressure process, how is the work done by the system related to the change in enthalpy?

A. W = ΔH
B. W = -ΔH
C. W = ΔH + PΔV
D. W = ΔH - PΔV

Solution

For a constant pressure process, the work done by the system is related to the change in enthalpy by the equation ΔH = Q + PΔV, where Q is the heat added.

Correct Answer: D — W = ΔH - PΔV

Q. In a constant pressure process, how is the work done calculated?

A. W = PΔV
B. W = ΔH
C. W = ΔU
D. W = Q + ΔH

Solution

The work done in a constant pressure process is calculated using W = PΔV, where P is pressure and ΔV is the change in volume.

Correct Answer: A — W = PΔV

Q. In a constant pressure process, the work done by the system is given by which equation?

A. W = PΔV
B. W = ΔH
C. W = ΔU
D. W = Q + ΔH

Solution

The work done by the system at constant pressure is given by W = PΔV, where P is pressure and ΔV is the change in volume.

Correct Answer: A — W = PΔV

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