Your Progress 0 / 25 attempted
Q 01 / 25
Thermodynamics mainly deals with macroscopic quantities like pressure, volume, and temperature of a system.
Q 02 / 25
A thermodynamic system is always the entire universe including surroundings.
Q 03 / 25
In thermodynamic equilibrium, the system must be in thermal, mechanical, and chemical equilibrium simultaneously.
Q 04 / 25
Temperature is the property that decides the direction of spontaneous heat flow between two bodies in contact.
Q 05 / 25
A quasi-static process is one that proceeds infinitely slowly so that the system passes through a continuous sequence of equilibrium states.
Q 06 / 25
The work done by a gas in a quasi-static pressure–volume process is equal to the area under the P–T curve.
Q 07 / 25
Heat and work are state functions because their values depend only on the initial and final states of the system.
Q 08 / 25
Internal energy of an ideal gas depends only on its temperature and not on its volume or pressure.
Q 09 / 25
For a cyclic process, the change in internal energy of the system over one complete cycle is zero.
Q 10 / 25
In an isothermal expansion of an ideal gas, the internal energy increases because the gas does work on the surroundings.
Q 11 / 25
In an adiabatic process, the system does not exchange heat with its surroundings, but it can still do work.
Q 12 / 25
A free expansion of an ideal gas into vacuum is an isothermal process in which the gas does maximum work.
Q 13 / 25
The first law of thermodynamics can be written for a closed system as \(\Delta U = Q - W\), where \(W\) is the work done by the system.
Q 14 / 25
If a system undergoes a process for which \(Q = 0\;W = 0\), then its internal energy must remain constant.
Q 15 / 25
\(\text{Enthalpy }H\) of a system is defined as \(H = U - PV\).
Q 16 / 25
At constant pressure, the heat supplied to a system equals the change in its enthalpy for a process in which only \(PV\text{ work is involved.}\)
Q 17 / 25
For one mole of an ideal gas, the difference between molar heat capacities at constant pressure and constant volume is equal to the universal gas constant \(R\).
Q 18 / 25
In all reversible cycles, the net entropy change of the system over one full cycle is positive.
Q 19 / 25
If two systems are each in thermal equilibrium with a third system, then they are in thermal equilibrium with each other.
Q 20 / 25
The efficiency of any heat engine operating between two given thermal reservoirs can never exceed that of a reversible engine operating between the same reservoirs.
Q 21 / 25
For a Carnot engine operating between temperatures \(T_1\) and \(T_2\ (T_1 > T_2)\), the efficiency decreases if both \(T_1\) and \(T_2\) are multiplied by the same factor.
Q 22 / 25
In any reversible adiabatic expansion of an ideal gas, both entropy and temperature of the gas decrease.
Q 23 / 25
The entropy change of the universe for any real (irreversible) process is always greater than zero.
Q 24 / 25
During the free expansion of an ideal gas into a vacuum, the entropy of the gas remains constant because its internal energy does not change.
Q 25 / 25
A process in which the entropy of an isolated system decreases can occur if the internal energy of the system decreases sufficiently.

Frequently Asked Questions

Thermodynamics is the branch of physics that deals with heat, work, energy, and the laws governing their interconversion in macroscopic systems.

A thermodynamic system is a specified quantity of matter or a region of space chosen for study, separated from its surroundings by a real or imaginary boundary.

The surroundings include everything outside the thermodynamic system that can interact with it by exchanging heat or work.

The thermodynamic state of a system is its condition described completely by state variables such as pressure, volume, and temperature.

State variables are physical quantities whose values depend only on the current state of the system and not on the path followed.

Pressure, volume, temperature, internal energy, entropy, and enthalpy are state variables.

Path variables are quantities whose values depend on the path taken during a process, such as heat and work.

A system is in thermodynamic equilibrium when it is simultaneously in thermal, mechanical, and chemical equilibrium.

An equation of state is a mathematical relation connecting state variables of a system in equilibrium, such as \(PV = nRT\).

An ideal gas is a hypothetical gas whose molecules do not interact except during elastic collisions and obey the ideal gas equation exactly.

The ideal gas equation is \(PV = nRT\), where symbols have their usual meanings.

Internal energy is the total microscopic energy of a system arising from molecular motion and interactions.

The internal energy of an ideal gas depends only on temperature.

The first law states that heat supplied to a system equals the increase in internal energy plus work done by the system.

\(\Delta Q = \Delta U + W\).
📰 Recent Posts

    THERMODYNAMICS – Learning Resources

    Detailed Notes
    Practice MCQs
    NCERT Solutions
    Q&A Discussion
    Practice Advance MCQs

    Warning: Undefined variable $subject in /home/u159659565/domains/academia-aeternum.com/public_html/includes/footer.php on line 110

    Get in Touch

    Let's Connect

    Questions, feedback, or suggestions?
    We'd love to hear from you.