Thermodynamics

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CBSE Learning Objectives – Key Concepts & Skills You Must Know

Learning Objectives

Explain the terms: system and surroundings.
Discriminate between closed, open, and isolated systems.
Explain internal energy, work, and heat.
State the first law of thermodynamics and express it mathematically.
Calculate energy changes as work and heat contributions in chemical systems.
Explain state functions: U, H.
Correlate ΔU and H.
Measure experimentally ΔU and H.
Define standard states for H.
Calculate enthalpy changes for various types of reactions.
State and apply Hess's law of constant heat summation.
Differentiate between extensive and intensive properties.
Define spontaneous and non-spontaneous processes.
Explain entropy as a thermodynamic state function and apply it for spontaneity.
Explain Gibbs energy change (G).
Establish the relationship between G and spontaneity, G and equilibrium constant.

CBSE Revision Notes & Quick Summary for Last-Minute Study

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CBSE Exam Tips, Important Questions & Common Mistakes to Avoid

Common Mistakes and Exam Tips in Thermodynamics

Common Pitfalls

Misunderstanding System Types: Students often confuse open, closed, and isolated systems. Remember:
- Open System: Exchanges both matter and energy with surroundings.
- Closed System: Exchanges energy but not matter.
- Isolated System: No exchange of matter or energy.
Confusing State Functions: State functions like internal energy (U), enthalpy (H), and entropy (S) depend only on the state of the system, not the path taken. Ensure you understand their definitions and applications.
Incorrect Application of Hess's Law: When using Hess's law, ensure that you account for the correct signs of enthalpy changes and that you sum them correctly around the cycle.
Neglecting Temperature Effects on Spontaneity: Remember that spontaneity can depend on temperature. For example, a reaction may be spontaneous at high temperatures but not at low ones.

Exam Tips

Review Definitions: Make sure you can define and differentiate between key terms such as system, surroundings, and types of thermodynamic processes.
Practice Calculations: Work through problems involving energy changes, enthalpy, and Gibbs free energy to solidify your understanding.
Understand Diagrams: Familiarize yourself with reaction coordinate diagrams and enthalpy diagrams, as they can help visualize energy changes in reactions.
Memorize Key Formulas: Ensure you know the first law of thermodynamics and how to apply it in various scenarios.
Use Practice Questions: Engage with multiple-choice questions to test your understanding of concepts like state functions and enthalpy changes.

CBSE Quiz & Practice Test – MCQs, True/False Questions with Solutions

Multiple Choice Questions

The internal energy change is zero because there is no heat exchange.

The internal energy change is equal to the work done on the system.

The internal energy change is equal to the heat absorbed by the system.

The internal energy change depends on the path taken by the reaction.

Correct Answer: B

Solution:

In a closed, insulated container (adiabatic system), there is no heat exchange with the surroundings (

q = 0

). Therefore, the change in internal energy (

\Delta U

) is equal to the work done on the system, as per the first law of thermodynamics:

\Delta U = q + W

. Since

q = 0

\Delta U = W

Surroundings

Boundary

System

Universe

Correct Answer: C

Solution:

In thermodynamics, the 'system' is the part of the universe being studied.

It can exchange both matter and energy with its surroundings.

It can exchange energy but not matter with its surroundings.

It cannot exchange either matter or energy with its surroundings.

It can exchange matter but not energy with its surroundings.

Correct Answer: C

Solution:

An isolated system is defined as one that does not exchange either matter or energy with its surroundings. This is in contrast to open systems, which can exchange both, and closed systems, which can exchange energy but not matter.

W = -P_{\text{ext}}(V_f - V_i)

W = P_{\text{ext}}(V_f - V_i)

W = -p(V_f - V_i)

W = p(V_f - V_i)

Correct Answer: A

Solution:

The work done on the gas during compression is given by the formula

W = -P_{\text{ext}}(V_f - V_i)

. The negative sign indicates that work is done on the system.

2000 K

1000 K

500 K

1500 K

Correct Answer: A

Solution:

For a reaction to be spontaneous, the Gibbs free energy change (

\Delta G

) must be negative.

\Delta G

is given by

\Delta G = \Delta H - T\Delta S

. Setting

\Delta G < 0

gives

T > \frac{\Delta H}{\Delta S}

. Here,

\Delta H = -200

kJ/mol = -200,000 J/mol and

\Delta S = 100

J/mol·K. Thus,

T > \frac{-200,000}{100} = 2000

K > 1

K < 1

K = 1

K = 0

Correct Answer: A

Solution:

The standard Gibbs energy change is related to the equilibrium constant by the equation

\Delta G^\circ = -RT \ln K

. A negative

\Delta G^\circ

indicates that

K > 1

, meaning the reaction favors the formation of products at equilibrium.

250 J released

250 J absorbed

550 J released

550 J absorbed

Correct Answer: A

Solution:

Using the first law of thermodynamics,

\Delta U = q - w

. Here,

\Delta U = -400 \text{ J}

and

w = -150 \text{ J}

(since work is done on the system, it is negative). Solving for

q

, we get

q = \Delta U + w = -400 \text{ J} + 150 \text{ J} = -250 \text{ J}

. Thus, 250 J of heat is released.

Entropy is a measure of energy conservation in a system.

Entropy is a measure of disorder or randomness in a system.

Entropy is a measure of the heat capacity of a system.

Entropy is a measure of the work done by a system.

Correct Answer: B

Solution:

Entropy is a thermodynamic state function that measures the disorder or randomness of a system.

Internal energy (

U

)

Enthalpy (

H

)

Work (

W

)

Entropy (

S

)

Correct Answer: C

Solution:

Work (

W

) is not a state function because it depends on the path taken during the process, unlike internal energy, enthalpy, and entropy, which depend only on the initial and final states.

300 J

700 J

500 J

200 J

Correct Answer: A

Solution:

According to the first law of thermodynamics,

\Delta U = q - W

. Here,

q = 500

J and

W = 200

J, so

\Delta U = 500 - 200 = 300

The compound is more stable than its elements.

The compound is less stable than its elements.

The compound has the same stability as its elements.

Stability cannot be inferred from enthalpy of formation.

Correct Answer: A

Solution:

A negative enthalpy of formation indicates that the formation of the compound from its elements releases energy, suggesting that the compound is more stable than its constituent elements.

\Delta U > 0

\Delta S > 0

\Delta G < 0

\Delta H < 0

Correct Answer: B

Solution:

For a spontaneous process in an isolated system, the total entropy change (

\Delta S

) must be greater than zero. This is because spontaneous processes increase the disorder or randomness of the system.

200 J

800 J

500 J

300 J

Correct Answer: A

Solution:

According to the first law of thermodynamics,

\Delta U = q + W

. Here,

q = 500

J and

W = -300

J (since work is done by the system). Therefore,

\Delta U = 500 - 300 = 200

Heat (q)

Work (W)

Internal Energy (U)

Path length

Correct Answer: C

Solution:

Internal energy (U) is a state function because it depends only on the initial and final states of a system, not on the path taken. In contrast, heat (q) and work (W) are path functions and depend on the specific process.

Work done is zero.

Work done is positive.

Work done is negative.

Work done depends on the path taken.

Correct Answer: B

Solution:

In an isothermal compression, work is done on the system, which means the system gains energy. Therefore, the work done is positive.

There is no exchange of energy or matter with the surroundings.

There is exchange of energy but not matter with the surroundings.

There is exchange of matter but not energy with the surroundings.

There is exchange of both energy and matter with the surroundings.

Correct Answer: A

Solution:

In an isolated system, there is no exchange of energy or matter with the surroundings.

\Delta U = 0

and

\Delta S > 0

\Delta U > 0

and

\Delta S = 0

\Delta U = 0

and

\Delta S < 0

\Delta U < 0

and

\Delta S = 0

Correct Answer: A

Solution:

In an isolated system, the change in internal energy

\Delta U = 0

, and for a spontaneous process, the change in entropy

\Delta S > 0

Heat (q)

Work (w)

Internal energy (U)

Path length

Correct Answer: C

Solution:

State functions are properties that depend only on the state of the system, not on how it got there. Internal energy (

U

) is a state function, while heat (

q

) and work (

w

) are path-dependent and not state functions.

-912.7 J

912.7 J

-303.9 J

303.9 J

Correct Answer: B

Solution:

The work done on the system is given by the equation:

W = -P_{ext} \Delta V

. Here,

P_{ext} = 3 \text{ atm}

and

\Delta V = (2 - 5) \text{ L} = -3 \text{ L}

. Thus,

W = -3 \times (-3) \times 101.3 = 912.7 \text{ J}

There is no exchange of heat with the surroundings.

The pressure remains constant.

The volume remains constant.

The temperature remains constant.

Correct Answer: A

Solution:

In an adiabatic process, the system is insulated from its surroundings, hence no heat exchange occurs. This is characterized by the condition

q = 0

Energy can be created or destroyed.

Energy can neither be created nor destroyed, only transformed.

The entropy of a system always decreases.

The universe is an open system.

Correct Answer: B

Solution:

The first law of thermodynamics states that energy can neither be created nor destroyed, only transformed.

-700 J

-300 J

300 J

700 J

Correct Answer: B

Solution:

According to the first law of thermodynamics,

\Delta U = q + w

. Here,

q = -500 \text{ J}

(heat released) and

w = -200 \text{ J}

(work done on surroundings). Thus,

\Delta U = -500 \text{ J} + (-200 \text{ J}) = -700 \text{ J}

-74.8 kJ/mol

-52.27 kJ/mol

+74.8 kJ/mol

+52.26 kJ/mol

Correct Answer: A

Solution:

The enthalpy of formation of CH₄ can be calculated using Hess's law:

\Delta H_{formation} = \Delta H_{combustion}^{CH_4} - (\Delta H_{combustion}^{C} + 2 \Delta H_{combustion}^{H_2})

. Substituting the given values:

\Delta H_{formation} = -890.3 - (-393.5 + 2 \times -285.8) = -74.8

kJ/mol.

It depends on the path taken to reach a particular state.

It is used to determine the amount of work done by the system.

It is independent of the path and depends only on the initial and final states.

It depends solely on the temperature of the system.

Correct Answer: C

Solution:

A state function is a property whose value is determined only by the state of the system, not by the path taken to reach that state. Examples include internal energy, enthalpy, and entropy.

A beaker open to the air.

A sealed container where energy can be exchanged but not matter.

A thermos flask with a lid.

A room with an open window.

Correct Answer: B

Solution:

A closed system allows the exchange of energy but not matter with its surroundings. A sealed container fits this description.

\Delta G > 0

\Delta G < 0

\Delta G = 0

\Delta G

is independent of spontaneity.

Correct Answer: B

Solution:

For a process to be spontaneous at constant temperature and pressure, the change in Gibbs free energy (

\Delta G

) must be negative, i.e.,

\Delta G < 0

. This indicates that the process can occur without external input.

Internal energy (

U

)

Heat (

q

)

Work (

W

)

Path length

Correct Answer: A

Solution:

Internal energy (

U

) is a state function because its value depends only on the initial and final states of the system, not on the path taken.

The reaction is non-spontaneous at all temperatures.

The reaction is spontaneous at all temperatures.

The reaction is spontaneous only at high temperatures.

The reaction is spontaneous only at low temperatures.

Correct Answer: B

Solution:

For a reaction where

\Delta H < 0

and

\Delta S > 0

, the Gibbs free energy change

\Delta G = \Delta H - T\Delta S

will always be negative, indicating that the reaction is spontaneous at all temperatures.

The reaction is possible at any temperature.

The reaction is possible only at low temperatures.

The reaction is possible only at high temperatures.

The reaction is not possible at any temperature.

Correct Answer: A

Solution:

A positive entropy change (

\Delta S > 0

) indicates increased disorder, which favors spontaneity. Thus, the reaction is possible at any temperature.

A property that depends on the path taken to reach a specific state.

A property that depends only on the initial and final states of the system.

A property that changes with time.

A property that is always constant.

Correct Answer: B

Solution:

State functions depend only on the initial and final states of the system, not on the path taken.

\Delta S > 0

\Delta U = 0

\Delta S < 0

\Delta U = 0

\Delta S = 0

\Delta U > 0

\Delta S > 0

\Delta U > 0

Correct Answer: A

Solution:

In an isolated system, the internal energy change

\Delta U = 0

because no energy is exchanged with the surroundings. For a spontaneous process, the total entropy change

\Delta S > 0

. Thus, option a is correct.

U = q + W

q = mC\Delta T

PV = nRT

F = ma

Correct Answer: A

Solution:

The first law of thermodynamics is represented by

U = q + W

, where

U

is the change in internal energy,

q

is the heat added to the system, and

W

is the work done on the system.

\Delta U = q + W

\Delta U = 0

\Delta U = q - W

\Delta U = W

Correct Answer: B

Solution:

For an isolated system, there is no exchange of heat or work with the surroundings, hence

\Delta U = 0

Open system

Closed system

Isolated system

Adiabatic system

Correct Answer: B

Solution:

A closed system allows the exchange of energy but not matter with its surroundings.

303.9 J

405.2 J

506.5 J

607.8 J

Correct Answer: A

Solution:

The work done by the gas during isothermal expansion can be calculated using

W = -P_{\text{ex}}(V_f - V_i)

. Substituting the given values,

W = -1.0 \, \text{atm} \times (5.0 \, \text{L} - 2.0 \, \text{L}) \times 101.3 \, \text{J/L} = -303.9 \, \text{J}

. The negative sign indicates work done by the system.

Unity

Zero

Less than zero

Different for each element

Correct Answer: B

Solution:

The enthalpy of all elements in their standard states is defined as zero.

The reaction is non-spontaneous.

The reaction is spontaneous.

The reaction is at equilibrium.

The reaction will become spontaneous at higher temperatures.

Correct Answer: B

Solution:

Using the Gibbs free energy equation,

\Delta G = \Delta H - T\Delta S

, we calculate

\Delta G = -500,000 J/mol - 298 K \times (-100 J/mol\cdot K) = -470,200 J/mol

. Since

\Delta G < 0

, the reaction is spontaneous.

The process is spontaneous.

The process is non-spontaneous.

The process is at equilibrium.

The process is reversible.

Correct Answer: A

Solution:

For an isolated system, a positive entropy change (

\Delta S > 0

) indicates that the process is spontaneous. This is because entropy is a measure of disorder, and an increase in entropy suggests a natural progression towards greater disorder.

The internal energy decreases.

The entropy increases.

The enthalpy remains constant.

The Gibbs free energy decreases.

Correct Answer: B

Solution:

For an isolated system, the internal energy remains constant (

\Delta U = 0

), but the entropy increases (

\Delta S > 0

) for a spontaneous process.

They depend on the path taken to reach a state.

They depend only on the initial and final states of a system.

They are always zero for any cyclic process.

They are the same for all substances at the same temperature.

Correct Answer: B

Solution:

State functions depend only on the initial and final states of a system, not on the path taken.

Heat

Work

Internal energy

Path taken

Correct Answer: C

Solution:

Internal energy is a state function because it depends only on the initial and final states of the system, not on the path taken.

q = 0

w = 0

T = 0

p = 0

Correct Answer: A

Solution:

In an adiabatic process, there is no heat exchange between the system and its surroundings. Therefore, the condition for adiabatic process is

q = 0

An open system exchanges both energy and matter with its surroundings, while a closed system exchanges only energy.

A closed system exchanges both energy and matter with its surroundings, while an open system exchanges only energy.

An open system exchanges neither energy nor matter with its surroundings, while a closed system exchanges both.

A closed system exchanges neither energy nor matter with its surroundings, while an open system exchanges both.

Correct Answer: A

Solution:

An open system allows for the exchange of both energy and matter, whereas a closed system allows only for the exchange of energy.

A system with no exchange of energy or matter with the surroundings.

A system that allows exchange of energy but not matter with the surroundings.

A system that allows exchange of both energy and matter with the surroundings.

A system that allows exchange of matter but not energy with the surroundings.

Correct Answer: A

Solution:

An isolated system does not exchange energy or matter with its surroundings.

250 J

550 J

-250 J

-550 J

Correct Answer: D

Solution:

The change in enthalpy at constant pressure is given by

\Delta H = q_p

. Since the system releases 400 J of heat,

q_p = -400 \, \text{J}

. The work done on the surroundings is 150 J, which does not affect

\Delta H

directly. Therefore,

\Delta H = -400 \, \text{J}

Open system

Closed system

Isolated system

Adiabatic system

Correct Answer: B

Solution:

A closed system allows for the exchange of energy (heat and work) with its surroundings but does not allow the exchange of matter. This is in contrast to an open system, which allows both energy and matter exchange, and an isolated system, which allows neither.

T = 0

p = 0

q = 0

w = 0

Correct Answer: C

Solution:

For a process to occur under adiabatic conditions, there must be no heat exchange, hence

q = 0

A system where energy and matter can be exchanged with the surroundings.

A system where only energy can be exchanged with the surroundings.

A system where neither energy nor matter can be exchanged with the surroundings.

A system where only matter can be exchanged with the surroundings.

Correct Answer: C

Solution:

An isolated system does not allow the exchange of energy or matter with its surroundings.

There is exchange of both matter and energy.

There is no exchange of matter, but energy can be exchanged.

There is no exchange of energy, but matter can be exchanged.

Neither matter nor energy can be exchanged.

Correct Answer: B

Solution:

In a closed system, energy can be exchanged with the surroundings, but matter cannot.

0.001

0.01

Correct Answer: A

Solution:

The relationship between Gibbs energy and the equilibrium constant is given by

\Delta G^\circ = -RT \ln K

. Rearranging gives

K = e^{-\Delta G^\circ / RT}

. Substituting the values,

K = e^{-40000 J/mol / (8.314 J/K·mol \times 298 K)} = 0.001

Heat

Work

Internal energy

All of the above

Correct Answer: C

Solution:

Internal energy is a state function because it depends only on the initial and final states of the system, not on the path taken.

T = 0

p = 0

q = 0

w = 0

Correct Answer: C

Solution:

In an adiabatic process, there is no heat exchange with the surroundings, hence

q = 0

250 J

550 J

150 J

400 J

Correct Answer: A

Solution:

According to the first law of thermodynamics, the change in internal energy (

\Delta U

) is given by

\Delta U = q - W

, where

q

is the heat absorbed by the system and

W

is the work done by the system. Here,

q = 400

J and

W = 150

J. Therefore,

\Delta U = 400 - 150 = 250

307 J

1095 J

701 J

394 J

Correct Answer: A

Solution:

The change in internal energy is given by the first law of thermodynamics:

\Delta U = q - w = 701 \text{ J} - 394 \text{ J} = 307 \text{ J}

A process where no heat is exchanged with the surroundings.

A process where no work is done by the system.

A process where the temperature remains constant.

A process where the pressure remains constant.

Correct Answer: A

Solution:

An adiabatic process is characterized by no heat exchange with the surroundings, meaning the system is perfectly insulated.

The internal energy increases by 307 J.

The internal energy decreases by 307 J.

The internal energy remains unchanged.

The internal energy decreases by 1095 J.

Correct Answer: A

Solution:

According to the first law of thermodynamics,

U = q + W

. Here,

q = 701

J and

W = -394

J (since work is done by the system), so

U = 701 - 394 = 307

\Delta H = q

\Delta H = U + pV

\Delta H = q - W

\Delta H = 0

Correct Answer: A

Solution:

At constant pressure, the enthalpy change is equal to the heat exchanged,

\Delta H = q_p

Greater than zero

Less than zero

Equal to zero

Cannot be determined

Correct Answer: C

Solution:

At equilibrium, the Gibbs energy change (

\Delta G

) is equal to zero.

T = 0

p = 0

q = 0

w = 0

Correct Answer: C

Solution:

In an adiabatic process, there is no transfer of heat between the system and its surroundings, so q = 0.

At low temperatures

At high temperatures

At any temperature

The reaction will never be spontaneous

Correct Answer: B

Solution:

For a reaction with

\Delta H > 0

and

\Delta S > 0

, the reaction will be spontaneous at high temperatures because the

T\Delta S

term will dominate and make

\Delta G < 0

-74.8 kJ/mol

-52.27 kJ/mol

+74.8 kJ/mol

+52.26 kJ/mol

Correct Answer: A

Solution:

The enthalpy of formation of CH₄(g) is calculated using the given enthalpy values and Hess's law.

700 J

300 J

500 J

200 J

Correct Answer: B

Solution:

According to the first law of thermodynamics,

\Delta U = q - w

, where

q

is the heat absorbed and

w

is the work done by the system. Substituting the given values,

\Delta U = 500 J - 200 J = 300 J

-25.5 kJ

-175 kJ

-25.5 J

-175 J

Correct Answer: A

Solution:

The Gibbs free energy change is given by

\Delta G = \Delta H - T \Delta S

. Substituting the values,

\Delta G = -100,000 - 298 \times 250 = -25,500 \text{ J} = -25.5 \text{ kJ}

The change in internal energy.

The heat absorbed or released by the system.

The work done by the system.

The change in temperature.

Correct Answer: B

Solution:

At constant pressure, the enthalpy change is equal to the heat absorbed or released by the system.

The rate at which energy transformations occur.

The initial and final states of a system undergoing change.

The microscopic details of molecular interactions.

The specific path taken by the system during transformation.

Correct Answer: B

Solution:

Thermodynamics focuses on the initial and final states of a system undergoing change, not the path or rate of transformation.

It is used to determine heat changes.

Its value is independent of path.

It is used to determine pressure volume work.

Its value depends on temperature only.

Correct Answer: B

Solution:

A thermodynamic state function is a property whose value is determined by the state of the system and is independent of the path taken to reach that state.

It states that energy can be created or destroyed.

It states that energy can neither be created nor destroyed.

It only applies to closed systems.

It is concerned with the rate of energy transformations.

Correct Answer: B

Solution:

The first law of thermodynamics, also known as the law of conservation of energy, states that energy can neither be created nor destroyed.

750 K

500 K

300 K

450 K

Correct Answer: A

Solution:

The reaction becomes non-spontaneous when

\Delta G > 0

. Using

\Delta G = \Delta H - T \Delta S

, set

\Delta G = 0

to find the threshold temperature:

0 = -150,000 + T(-200)

. Solving for

T

gives

T = 750 \text{ K}

It states that energy can be created and destroyed.

It states that the total energy of an isolated system is constant.

It states that entropy always decreases in a closed system.

It states that work done on a system is always zero.

Correct Answer: B

Solution:

The first law of thermodynamics, also known as the law of conservation of energy, states that the total energy of an isolated system is constant.

U = q + W

U = q - W

U = W - q

U = q

Correct Answer: A

Solution:

The first law of thermodynamics is expressed as

U = q + W

, where

U

is the change in internal energy,

q

is the heat added to the system, and

W

is the work done on the system.

Freezing of water

Condensation of steam

Dissolution of salt in water

Formation of ice from liquid water

Correct Answer: C

Solution:

The dissolution of salt in water increases the disorder of the system, leading to a positive change in entropy (

\Delta S > 0

). Processes like freezing and condensation decrease entropy as they lead to more ordered states.

300 J

700 J

500 J

200 J

Correct Answer: A

Solution:

For a closed system at constant pressure, the change in enthalpy (

\Delta H

) is given by

\Delta H = q_p

, where

q_p

is the heat absorbed at constant pressure. Here,

\Delta H = 500 \text{ J} - 200 \text{ J} = 300 \text{ J}

The rate of chemical reactions.

The energy changes in macroscopic systems.

The microscopic interactions of molecules.

The color changes in chemical reactions.

Correct Answer: B

Solution:

Thermodynamics deals with energy changes in macroscopic systems involving a large number of molecules.

True or False

Correct Answer: False

Solution:

The internal energy change

\Delta U

Correct Answer: True

Solution:

Gibbs energy change,

\Delta G

, helps determine spontaneity. A negative

\Delta G

indicates that the process is spontaneous.

Correct Answer: True

Solution:

Enthalpy change, denoted as

\Delta H

, is a state function that can be directly measured as the heat change at constant pressure, represented by

Solution:

Entropy, denoted as

S

, is actually a measure of disorder or randomness in a system. For a spontaneous change, the total entropy change is positive.

Correct Answer: True

Solution:

In an isolated system, a spontaneous process is characterized by no change in internal energy (

\Delta U = 0

) and a positive change in entropy (

\Delta S > 0

Correct Answer: False

Solution:

The laws of thermodynamics deal with energy changes between initial and final states and are not concerned with the rate of energy transformations.

Correct Answer: True

Solution:

The internal energy change

\Delta U

is a state function, meaning it depends only on the initial and final states of the system, not on the path taken.

Correct Answer: True

Solution:

The internal energy change, denoted as

\Delta U

, is a state function and depends only on the initial and final states, not on the path taken.

Correct Answer: False

Solution:

An isolated system does not allow the exchange of either energy or matter with its surroundings. This is the defining characteristic of an isolated system.

Correct Answer: True

Solution:

The internal energy

\Delta U

U

, is a state function in thermodynamics. This means it depends only on the initial and final states of the system, not on the path taken to reach these states.

Correct Answer: True

Solution:

In an open system, there is an exchange of energy and matter between the system and its surroundings.

Correct Answer: True

Solution:

The internal energy change

\Delta U

depends only on the initial and final states of the system, making it a state function, and is independent of the path taken.

Correct Answer: False

Solution:

For an isolated system, the change in internal energy is zero (

\Delta U = 0

), but the change in entropy is positive for spontaneous processes (

\Delta S > 0

Correct Answer: False

Solution:

Entropy

S

is indeed a measure of disorder, but for a spontaneous process, the total entropy change is positive, not negative.

Correct Answer: True

Solution:

An adiabatic process is defined by the absence of heat transfer between the system and its surroundings.

Correct Answer: True

Solution:

Entropy,

S

, measures the disorder of a system. For a spontaneous process, the change in total entropy is positive.

Correct Answer: True

Solution:

Entropy, denoted as

S

, is a measure of disorder or randomness, and for a spontaneous change, the total entropy change is positive.

Correct Answer: True

Solution:

In thermodynamics, the universe is considered to be the sum of the system and its surroundings. This definition helps in analyzing energy changes within the system while considering its interaction with the surroundings.

Correct Answer: True

Solution:

By definition, the enthalpy of formation of any element in its standard state is zero.

Correct Answer: False

Solution:

The first law of thermodynamics states that the energy of an isolated system is constant, meaning it cannot increase or decrease over time.

Thermodynamics

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Multiple Choice Questions

Q1.Consider a chemical reaction occurring in a closed, insulated container. Which of the following statements is true about the internal energy change (ΔU\Delta UΔU) of the system?

Correct Answer: B

Q2.In thermodynamics, what is the term used to describe the part of the universe being studied?

Correct Answer: C

Q3.Which of the following statements is true about an isolated system?

Correct Answer: C

Q4.Consider a closed system where a gas is compressed by an external pressure PextP_{\text{ext}}Pext​ which is greater than the internal pressure ppp of the gas. If the initial volume of the gas is ViV_iVi​ and it is compressed to a final volume VfV_fVf​, what is the work done on the gas?

Correct Answer: A

Q5.A reaction has an enthalpy change (ΔH\Delta HΔH) of -200 kJ/mol and an entropy change (ΔS\Delta SΔS) of 100 J/mol·K. At what minimum temperature will the reaction become spontaneous?

Correct Answer: A

Q6.A chemical reaction has a standard Gibbs energy change (ΔG∘\Delta G^\circΔG∘) of -50 kJ/mol at 298 K. What can be inferred about the equilibrium constant KKK for this reaction?

Correct Answer: A

Q7.A system undergoes a process where the internal energy decreases by 400 J and 150 J of work is done on the system. How much heat is exchanged with the surroundings?

Correct Answer: A

Q8.Which statement about entropy is correct in the context of thermodynamics?

Correct Answer: B

Q9.Which of the following is NOT a state function?

Correct Answer: C

Q10.Consider a system where 500 J of heat is absorbed and 200 J of work is done by the system. What is the change in internal energy?

Correct Answer: A

Q11.If the enthalpy of formation of a compound is given as -100 kJ/mol, what can be inferred about the stability of the compound relative to its elements?

Correct Answer: A

Q12.For a spontaneous process in an isolated system, which of the following conditions must be true?

Correct Answer: B

Q13.In a thermodynamic process, 500 J of heat is added to a system and 300 J of work is done by the system. What is the change in internal energy of the system?

Correct Answer: A

Q14.Which of the following is a thermodynamic state function?

Correct Answer: C

Q15.Consider a closed system where a gas is compressed isothermally. Which statement is true about the work done on the system?

Correct Answer: B

Q16.Which of the following is true for an isolated system?

Correct Answer: A

Q17.For a spontaneous process in an isolated system, which of the following is true?

Correct Answer: A

Q18.Which of the following is a state function?

Correct Answer: C

Q19.Consider a closed system where a gas is compressed isothermally. If the initial volume of the gas is 5 L and it is compressed to 2 L under a constant external pressure of 3 atm, what is the work done on the system? (1 atm = 101.3 J/L)

Correct Answer: B

Q20.In an adiabatic process, which of the following is true about the system?

Correct Answer: A

Q21.What is the first law of thermodynamics?

Correct Answer: B

Q22.Consider a closed system where a chemical reaction occurs, releasing 500 J of heat while doing 200 J of work on the surroundings. What is the change in internal energy (ΔU\Delta UΔU) of the system?

Correct Answer: B

Q23.The enthalpy of formation of methane (CH₄) is calculated using the enthalpies of combustion of methane, graphite, and dihydrogen as -890.3 kJ/mol, -393.5 kJ/mol, and -285.8 kJ/mol respectively. What is the enthalpy of formation of CH₄?

Correct Answer: A

Q24.Which of the following statements correctly describes a state function in thermodynamics?

Correct Answer: C

Q25.Which of the following is an example of a closed system?

Correct Answer: B

Q26.Which of the following statements about Gibbs free energy (GGG) is correct for a spontaneous process at constant temperature and pressure?

Correct Answer: B

Q27.Which of the following is a state function in thermodynamics?

Correct Answer: A

Q28.If the enthalpy change (ΔH\Delta HΔH) for a reaction is negative and the entropy change (ΔS\Delta SΔS) is positive, what can be inferred about the spontaneity of the reaction?

Correct Answer: B

Q29.For a reaction A+B→C+DA + B \rightarrow C + DA+B→C+D with a positive entropy change, which of the following statements is true?

Correct Answer: A

Q30.In thermodynamics, what does the term 'state function' refer to?

Correct Answer: B

Q31.In an isolated system, a spontaneous process occurs. Which of the following statements correctly describes the change in entropy (ΔS\Delta SΔS) and internal energy (ΔU\Delta UΔU) of the system?

Correct Answer: A

Q32.Which of the following equations represents the first law of thermodynamics?

Correct Answer: A

Q33.In thermodynamics, what is the internal energy change (ΔU\Delta UΔU) for an isolated system?

Correct Answer: B

Q34.Which of the following systems allows the exchange of energy but not matter with its surroundings?

Correct Answer: B

Correct Answer: A

Q36.What is the enthalpy of all elements in their standard states?