Explanation: Density is mass per unit volume, so its unit is kilograms per cubic meter (kg/m³) in SI.

Explanation: Pressure (force/area) has dimensions of [M L T⁻²] ÷ [L²] = [M L⁻¹ T⁻²], as in Pascal.

Explanation: Work, like energy, is measured in Joules (J), equivalent to Newton-meter (N·m) in SI units.

Explanation: Volume is length cubed, so its dimension is [L³], measured in cubic meters (m³) in SI

Explanation: Entropy measures energy per temperature, so its unit is Joules per Kelvin (J/K) in SI.

Explanation: Power (energy/time) has dimensions of [M L² T⁻²] ÷ [T] = [M L² T⁻³], as in Watts (J/s).

Explanation: Specific heat capacity is energy per unit mass per unit temperature, so its unit is Joules per kilogram per Kelvin.

Explanation: Temperature is a fundamental dimension [θ], measured in Kelvin (K) in SI units, not derived from mass, length, or time.

Explanation: Pressure is force per unit area, measured in Pascal (Pa), equivalent to N/m² in SI units

Explanation: Energy (e.g., Joule) has dimensions of mass [M], length squared [L²], and time inverse squared [T⁻²], as in force × distance

Explanation: Quasi-static processes have well-defined properties, making them easier to analyze in thermodynamic calculations.

Explanation: Slow heating allows the system to adjust gradually, maintaining near-equilibrium, typical of quasi-static processes.

Explanation: Quasi-static processes are idealized as reversible since they occur slowly, minimizing energy losses.

Explanation: Quasi-static processes involve small, gradual changes, keeping the system near equilibrium at every step.

Explanation: An isothermal process keeps temperature constant, and in a quasi-static case, it occurs slowly to maintain equilibrium.

Explanation: Non-quasi-static processes, like rapid expansion, deviate from equilibrium and are often irreversible.

Explanation: In quasi-static processes, properties like pressure and temperature are uniform at each step, ideal for analysis.

Explanation: Slow compression allows the gas to adjust gradually, maintaining near-equilibrium conditions.

Explanation: The system remains infinitesimally close to equilibrium, allowing properties like temperature and pressure to be uniform.

Explanation: A quasi-static process happens slowly, keeping the system close to equilibrium, with well-defined properties at each step

Explanation: A sealed system with constant temperature, pressure, and no changes is in thermodynamic equilibrium.

Explanation: Thermal equilibrium requires uniform temperature throughout the system.

Explanation: Uniform temperature (thermal equilibrium) is a key condition for thermodynamic equilibrium, along with pressure and composition stability.

Explanation: Thermodynamic equilibrium requires no energy transfer (e.g., heat or work) as properties are stable

Explanation: If temperature, pressure, and composition are uniform and constant, the system is in thermodynamic equilibrium.

Explanation: Chemical equilibrium is achieved when no chemical reactions occur, and the composition remains stable.

Explanation: Mechanical equilibrium occurs when the system has uniform pressure, with no net forces causing motion

Explanation: Thermal equilibrium means the system has the same temperature throughout, with no heat flow.

Explanation: In thermodynamic equilibrium, properties like temperature and pressure stay constant with no tendency to change.

Explanation: A steam power plant uses a cycle (e.g., Rankine cycle) where the working fluid undergoes repeated processes to produce work.

Explanation: A process is a change from one state to another, e.g., expanding a gas from high to low pressure.

Explanation: The path describes the sequence of states during a process, like whether it’s isothermal or adiabatic.

Explanation: A cycle brings the system back to its starting state after a series of processes, e.g., in a heat engine.

Explanation: An isothermal process occurs at constant temperature, like compressing a gas while maintaining its temperature.

Explanation: State is defined by properties like temperature, pressure, and volume. Work is a path function, not a state property.

Explanation: A cycle involves processes that return the system to its initial state, like in a refrigeration system.

Explanation: A process is a transition from one state to another, e.g., heating a gas to increase its pressure

Explanation: The path is the series of states a system goes through during a change, like isothermal compression of a gas.

Explanation: A state is defined by properties like temperature, pressure, and volume at a specific point, e.g., water at 25°C and 1 atm.

Explanation: Internal energy is a point function, so its change depends only on initial and final states, not the path.

Explanation: Pressure and temperature are point functions, defined by the state. Heat and work are path functions

Explanation: Heat depends on the process (e.g., different heat in isothermal vs. isobaric processes), so it’s a path function.

Explanation: Entropy depends only on the system’s state, making it a point function, unlike work or heat.

Explanation: Heat transfer is a path function, varying with the process. Entropy, temperature, and specific volume are point functions.

Explanation: Pressure is a point function, with a definite value at any state, independent of the expansion process.

Explanation: Work is a path function, as its value depends on the process (e.g., isothermal vs. adiabatic compression).

Explanation: Point functions, like temperature or density, are defined by the system’s state and measurable at a single point.

Explanation: Heat is a path function because its value depends on the process (e.g., how energy is transferred), not just the state.

Explanation: Point functions, like temperature or pressure, have a fixed value at a specific state, regardless of the process taken

Explanation: Density and temperature are intensive, as they do not depend on the amount of matter. The other pairs include extensive properties like mass, volume, weight, energy, length, and surface area

Explanation: Density (mass/volume) is intensive. If both mass and volume double proportionally, density stays constant for the same substance.

Explanation: Melting point is intensive, so it remains the same for any sample of a substance (e.g., ice melts at 0°C), making it ideal for comparison.

Explanation: Volume is extensive because it increases with the amount of gas. More gas in the container means a larger volume.

Explanation: Pressure is an intensive property, as it does not depend on the amount of matter. Energy, weight, and surface area scale with the sample size.

Explanation: Specific heat is an intensive property, staying constant regardless of the sample size. Mass and volume halve when the sample is divided.

Explanation: Density is an intensive property, unique to a material (e.g., gold has a specific density), and does not vary with sample size.

Explanation: Temperature is intensive because it does not change with the amount of substance. A small or large sample of water at 25°C has the same temperature.

Explanation: Extensive properties, like mass or volume, depend on the amount of matter in the sample. More matter means a larger value.

Explanation: Intensive properties, like density or temperature, remain the same regardless of the sample size or amount of matter.

Explanation: In piston-cylinder systems, the piston moves — making it a movable boundary.

Explanation: Boundaries can be imagined based on how the system is defined in a given scenario.

 Explanation: Everything outside the system (e.g., steam engine), like the atmosphere, is considered surroundings.

Explanation: An isolated system has boundaries that prevent energy and matter exchange.

 Explanation: Diathermic boundaries allow heat exchange; adiabatic ones do not.

 Explanation: Closed systems allow energy (like heat/work) to pass but not matter.

 Explanation: System + surroundings = Universe, in thermodynamic terms.

Explanation: All energy or matter exchange between system and surroundings occurs across the boundary.

Explanation: A boundary can be fixed/movable and real or imaginary depending on the problem.

Explanation: Everything external to the system that can interact with it is called the surroundings.

Explanation: In a closed system, energy crosses the boundary but the matter remains fixed.

Explanation: A closed system does not allow mass to flow — only energy crosses.

 Explanation: No mass transfer but energy in the form of work/heat can move — closed system.

Explanation: A human body exchanges both energy and matter with the environment — an open system.

 Explanation: A perfectly insulated thermos prevents both heat and matter transfer — isolated in theory.

 Explanation: In a closed system, energy crosses the boundary but the matter remains fixed.

 Explanation: An isolated system does not interact with surroundings — no matter or energy crosses the boundary.

Explanation: A closed system doesn’t allow matter exchange, only energy like heat can pass.

Explanation: In open systems, both matter and energy can enter or leave the system.

Batteries involve chemical reactions with energy conversion — a thermodynamic process.

Heating, Ventilation, and Air Conditioning (HVAC) systems use heat transfer and energy balance concepts

Thermodynamics is used to improve fuel efficiency in jet engines and rockets.

The Rankine cycle is used in thermal power plants for steam turbine operation.

Refrigeration systems transfer heat from a cold space to a warmer one.

All convert natural energy to usable forms using thermodynamic concepts.

One major goal in engineering is to use thermodynamics to improve energy efficiency.

 Cooking involves heat transfer; cars run on engines based on thermodynamic cycles.

 Explanation: Power generation and engines rely on energy conversion principles of thermodynamics.

 Explanation: Mechanical engineering heavily uses thermodynamics for systems like engines, turbines, and HVAC.

 Explanation: Thermodynamics is fundamentally about energy, heat, and their relation with matter.

 Explanation: Power cycles are designed based on thermodynamic principles.

 Explanation: Thermodynamics is essential in designing engines and energy systems

 Explanation: Thermodynamics is a core part of mechanical, chemical, and physics-based engineering.

 Explanation: Power plants depend on thermodynamics to convert heat into electricity efficiently.

 Explanation: Rate of reaction is a kinetic concern, not a thermodynamic one.

 Explanation: Steam in a piston-cylinder is a good example of a defined thermodynamic system

 Explanation: Thermodynamic laws are derived from consistent experimental observations.

 Explanation: Thermodynamics focuses on how energy is converted from one form to another.

 Explanation: Thermodynamics deals with the transformation and transfer of heat and energy.