For the reactions: ${\rm{C}} + {{\rm{O}}_2} \to {\rm{C}}{{\rm{O}}_2};\Delta H = - 393{\rm{kJ}}$ $2{\rm{Zn}} + {{\rm{O}}_2} \to 2{\rm{ZnO}};\Delta H = - 412{\rm{kJ}}$ which one is correct?

Oxidation of carbon is not feasible

Oxidation of Zn is not feasible

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JEE • CHEMISTRY • THERMODYNAMICS

Thermodynamics practice · Easy

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These sets use single-correct-answer MCQs. They do not cover every JEE Main or JEE Advanced question format and are not full-length mock papers.

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Showing 1-30 of 79 questions

1 Easy

1 of 79

Analyzing +4 | -1

For the reactions:

\mathrm{C} + {\mathrm{O}_2} \to \mathrm{C}{\mathrm{O}_2};\Delta H = - 393\mathrm{kJ}

2\mathrm{Zn} + {\mathrm{O}_2} \to 2\mathrm{ZnO};\Delta H = - 412\mathrm{kJ}

which one is correct?

View answer and explanation

Correct option: A

Carbon can reduce ZnO to Zn

Option D (Zn liberates more heat than carbon during oxidation) is correct because the absolute value of ∆H for the oxidation of Zn is greater than that of carbon.

2 Easy

2 of 79

Remembering +4 | -1

Which of the following is an example of extensive property?

View answer and explanation

Correct option: C

Mass

Option C (Mass) is correct because mass is an extensive property, meaning its value depends on the amount of substance.

3 Easy

3 of 79

Application +4 | -1

The melting point a solid is

27^{\circ} \mathrm{C}

and its latent heat of fusion is 600 calories/mole the entropy change for the fusion of one mole of the solid in

\mathrm{cal/K}

is ___.

View answer and explanation

Correct option: A

Option A (2) is correct because it is calculated using the formula

\Delta S = \Delta H / T

4 Easy

4 of 79

Understanding +4 | -1

Which equation is correct for adiabatic process

View answer and explanation

Correct option: B

Q = 0

Option B (Q = 0) is correct because an adiabatic process is defined as a process where no heat is exchanged with the surroundings.

5 Easy

5 of 79

Remembering +4 | -1

Which fuel provides the highest calorific value?

View answer and explanation

Correct option: B

Kerosene

Option B (Kerosene) is correct because Kerosene has a higher calorific value compared to Charcoal, Wood, and Dung.

6 Easy

6 of 79

Understanding +4 | -1

The entropy of the universe:

View answer and explanation

Correct option: A

Increasing and tending towards maximum value

Option A is correct because, according to the second law of thermodynamics, the entropy of the universe is always increasing and tending towards a maximum value.

7 Easy

7 of 79

Application +4 | -1

A gas is allowed to expand in an insulated container against a constant external pressure of

3.5 \, {~atm}

from an initial volume of

4.0 \, \mathrm{~L}

to a final volume of

10.0 \,\mathrm{~L}

. The change in internal energy of the gas will be

View answer and explanation

Correct option: C

-2.1 \,{~kJ}

Option C (-2.1 kJ) is correct because the change in internal energy equals the work done in an adiabatic process, which is calculated using the external pressure and volume change.

8 Easy

8 of 79

Analyzing +4 | -1

In a flask, colourless

{\mathrm{N}_2}{\mathrm{O}_4}

(g) is in equilibrium with brown coloured

\mathrm{N}{\mathrm{O}_2}

(g). At equilibrium when the flask is heated to 100℃, the brown colour deepens and on cooling it becomes coloured. Which statement is incorrect about this observation?

View answer and explanation

Correct option: C

The ∆H-∆U at 100℃ is equal to 200 cal

Option D (The ∆H-∆U at 100℃ is equal to 200 cal) is incorrect because the calculated value of ∆H-∆U is 746 cal, not 200 cal.

9 Easy

9 of 79

Application +4 | -1

Heat exchanged during the boiling of water is

0.900 \mathrm{~KJ} / \mathrm{mol}^{-1}

. What will be the increase in entropy.

View answer and explanation

Correct option: A

2.41 \mathrm{~JK}^{-1} \mathrm{~mol}^{-1}

Option A (

2.41 \mathrm{~JK}^{-1} \mathrm{~mol}^{-1}

) is correct because the entropy change is calculated by dividing the heat exchanged during a reversible process at constant temperature by the temperature.

10 Easy

10 of 79

Understanding +4 | -1

The Gibbs energy change and standard Gibbs energy change are equal if reaction quotient is equal to:

View answer and explanation

Correct option: B

Option B is correct. The Gibbs energy change (

\Delta G

) and standard Gibbs energy change (

\Delta G^\circ

) are equal when the reaction quotient (Q) is equal to 1, as

\Delta G = \Delta G^\circ + RT \ln Q

11 Easy

11 of 79

Remembering +4 | -1

The entropy of crystalline substances at
absolute zero going by the third law of
thermodynamics should be taken as

View answer and explanation

Correct option: C

zero

Option C (zero) is correct because the third law of thermodynamics states that the entropy of a perfectly crystalline substance at absolute zero is zero.

12 Easy

12 of 79

Remembering +4 | -1

Which among the following is not a state function?

View answer and explanation

Correct option: D

Work

Option D (Work) is correct because work is a path function, meaning its value depends on the path taken during a process, while Gibbs energy, pressure, and temperature are state functions.

13 Easy

13 of 79

Understanding +4 | -1

The change in the enthalpy during the reaction,

\;\mathrm{NaOH} + \mathrm{HCl} \to \;\mathrm{NaCl} + {\mathrm{H}_2}\mathrm{O},

is called :

View answer and explanation

Correct option: B

Heat of neutralization

Option B is correct because the reaction of a strong acid (HCl) with a strong base (NaOH) to form salt and water is specifically termed heat of neutralization.

14 Easy

14 of 79

Remembering +4 | -1

For a spontaneous chemical change the Gibbs energy change is:

View answer and explanation

Correct option: B

Negative

Option B (Negative) is correct because for a spontaneous chemical change, the Gibbs free energy change (∆G) must be negative.

15 Easy

15 of 79

Understanding +4 | -1

The Gibbs energy change and standard Gibbs energy change are equal if reaction quotient is equal to:

View answer and explanation

Correct option: B

Option B (1) is correct because when the reaction quotient Q is equal to 1, the Gibbs energy change equals the standard Gibbs energy change.

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16 Easy

16 of 79

Understanding +4 | -1

Statement I Entropy of a crystalline solid increases when
temperature is increased from 0 K to 115 K.
Statement II System becomes more disordered at its
higher temperature.

View answer and explanation

Correct option: B

Both Statement I and Statement II are correct and
Statement II is not the correct explanation of
Statement I

The correct answer is B (Both Statement I and Statement II are correct and Statement II is not the correct explanation of Statement I) because increasing temperature increases entropy, and higher temperature leads to more disorder, but the second statement isn't directly explaining the first.

17 Easy

17 of 79

Analyzing +4 | -1

A container has hydrogen and oxygen mixture in ratio of 1 : 1 by weight, then

View answer and explanation

Correct option: C

Entropy of the mixture increases

The correct answer is C (Entropy of the mixture increases) because mixing of different gases always leads to an increase in entropy due to increased disorder.

18 Easy

18 of 79

Remembering +4 | -1

Which is correct relation between

\mathrm{C}_{\mathrm{p}}

and

\mathrm{C}_{\mathrm{v}}

for one mole of ideal gas

View answer and explanation

Correct option: C

\mathrm{C}_{\mathrm{p}}-\mathrm{C}_{\mathrm{v}}=\mathrm{R}

Option C is correct because the relationship between

C_p

and

C_v

for one mole of an ideal gas is given by

C_p - C_v = R

19 Easy

19 of 79

Remembering +4 | -1

In the exothermic reaction, the enthalpy of reaction is always:

View answer and explanation

Correct option: C

Negative

Option C (Negative) is correct because in an exothermic reaction, heat is released, meaning the enthalpy change (

\Delta H

) is negative.

20 Easy

20 of 79

Remembering +4 | -1

For an adiabatic process:

View answer and explanation

Correct option: B

Q=0

Option B (Q=0) is correct because an adiabatic process is defined as a process in which there is no heat exchange between the system and the surroundings, therefore Q (heat) is equal to zero.

21 Easy

21 of 79

Understanding +4 | -1

Which of the following taking place in the blast furnace is endothermic?

View answer and explanation

Correct option: A

\mathrm{CaC}{\mathrm{O}_3} \to \mathrm{CaO} + \mathrm{C}{\mathrm{O}_2}

Option A (

\mathrm{CaC}{\mathrm{O}_3} \to \mathrm{CaO} + \mathrm{C}{\mathrm{O}_2}

) is correct because the decomposition of calcium carbonate requires energy input to break chemical bonds, making it an endothermic process.

22 Easy

22 of 79

Understanding +4 | -1

Thermochemistry is the study of relationship between heat energy and :

View answer and explanation

Correct option: A

Chemical energy

Option A (Chemical energy) is correct because thermochemistry specifically studies the relationship between heat energy and chemical energy changes during chemical reactions.

23 Easy

23 of 79

Understanding +4 | -1

The enthalpy of formation of

{HCl}(\mathrm{g})

from the following reaction

{H}_2(\mathrm{g})+{Cl}_2(\mathrm{g}) \rightarrow 2 {HCl}(\mathrm{g})+44 \mathrm{~kcal}

View answer and explanation

Correct option: B

-22 \mathrm{~kcal} \mathrm{~mol}^{-1}

Option B is correct. The enthalpy of formation is for 1 mole of HCl. Since the reaction produces 2 moles of HCl with -44 kcal, the enthalpy of formation for 1 mole is -22 kcal/mol.

24 Easy

24 of 79

Analyzing +4 | -1

Choose the reaction with negative

\Delta S

value.

View answer and explanation

Correct option: C

2 {SO}_{2({~g})}+{O}_{2({~g})} \rightarrow 2 {SO}_{3({~g})}

Option C (

2 {SO}_{2({~g})}+{O}_{2({~g})} \rightarrow 2 {SO}_{3({~g})}

) is correct because the number of gaseous moles decreases in this reaction, leading to a decrease in entropy (negative

\Delta S

25 Easy

25 of 79

Understanding +4 | -1

{HCl}

(in 20 moles

{H}_2 {O}

) +20 moles of

{H}_2 {O} \longrightarrow {HCl}

(in 40 moles of water).

\Delta {H}

for the above process is called.

View answer and explanation

Correct option: A

Enthalpy of dilution

Option A is correct because adding more water to a solution is a dilution process, and the enthalpy change is called the enthalpy of dilution.

26 Easy

26 of 79

Understanding +4 | -1

During an adiabatic process:

View answer and explanation

Correct option: C

There is perfect heat insulation

Option C (There is perfect heat insulation) is correct because an adiabatic process is defined as one with no heat exchange with the surroundings.

27 Easy

27 of 79

Analyzing +4 | -1

For which of the process, ∆S is negative?

View answer and explanation

Correct option: C

{\mathrm{N}_2}\left( {1\,\mathrm{g}\,\,\mathrm{atom}} \right) \to {\mathrm{N}_2}\left( {8\,\mathrm{g}\,\,\mathrm{atom}} \right)

The correct answer is C. When a gas is compressed, its entropy decreases, leading to a negative change in entropy (∆S).

28 Easy

28 of 79

Application +4 | -1

Equal volume of two monoatomic gases, A and B, at same temperature and pressure are mixed. The ratio of specific heats

(\;{C_P}/{C_V})

of the mixture will be:

View answer and explanation

Correct option: D

1.67

Option D (1.67) is correct because the ratio of specific heats for a monoatomic gas is always 5/3, which is approximately 1.67.

29 Easy

29 of 79

Understanding +4 | -1

∆H for transition of carbon in the diamond form to carbon in the graphite form, is – 453.5 cal. This suggests that :

View answer and explanation

Correct option: C

Graphite is more stable than diamond

The correct answer is that Graphite is more stable than diamond. A negative ∆H indicates that the conversion of diamond to graphite is exothermic, meaning graphite has lower energy and is therefore more stable.

30 Easy

30 of 79

Understanding +4 | -1

{q}=-{w}

is not true for :

View answer and explanation

Correct option: B

Adiabatic process

Option B (Adiabatic process) is correct because in an adiabatic process, q = 0, so -w must also be 0, meaning w=0, which is not always true.

Revision notes and key takeaways

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Key Takeaways

✓ This set contains 79 single-correct-answer MCQs on THERMODYNAMICS.
✓ Try each question before opening its answer. Read the explanation where one is available.
✓ Sign in to save submitted answers. Revisit incorrect answers alongside your textbook or class notes.

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