For a monatomic ideal gas, γ = C_p/C_v = 5/3 = 1.67.

At constant volume, no work is done (W=0), and the heat added equals the change in internal energy (Q=ΔU).

In an isobaric process, the work done is calculated using the formula W = PΔV, where P is pressure and ΔV is the change in volume.

The Ideal Gas Law (PV = nRT) relates pressure (P), volume (V), and temperature (T) for an ideal gas.

The efficiency of a Carnot engine is given by η = 1 - T2/T1.

The efficiency of a Carnot engine is determined by the temperatures of the hot and cold reservoirs, given by the formula η = 1 - (T_c/T_h).

According to the First Law of Thermodynamics, ΔU = Q - W. Here, ΔU = 100 J - 40 J = 60 J.

In a cyclic process, the net work done is equal to the net heat added to the system, as the internal energy returns to its initial state.

Efficiency (η) = Work done / Input heat = 300 J / 500 J = 0.6 or 60%.

In an adiabatic process, the relationship is given by PV^n = constant, where n is the heat capacity ratio.

In an adiabatic process, there is no heat exchange with the surroundings, meaning no heat is absorbed or released.

In an adiabatic process, there is no heat exchange, so the internal energy remains constant for an ideal gas.

For an ideal gas, the internal energy depends only on temperature. Since the temperature remains constant in an isothermal process, the internal energy also remains constant.

In an isothermal process, the temperature of the system remains constant.

Enthalpy refers to the heat content of a system at constant pressure, defined as internal energy plus pressure times volume.

According to the second law of thermodynamics, the entropy of an isolated system always increases over time.

During an isothermal expansion, the temperature of the gas remains constant as the system absorbs heat to do work.

For an isothermal process, the change in internal energy ΔU = 0 for an ideal gas.

For an isothermal process, the change in internal energy (ΔU) for an ideal gas is zero, as ΔU depends only on temperature.

In an isothermal process for an ideal gas, the internal energy remains constant, hence the change in internal energy is zero.

At constant volume, the change in internal energy (ΔU) is equal to the heat added (Q). Therefore, ΔU = Q.

The efficiency (η) of a Carnot engine is given by η = 1 - (T2 / T1), where T1 is the higher temperature and T2 is the lower temperature.

For a monatomic ideal gas, the specific heat at constant volume (Cv) is 3R/2.

The specific heat capacity of water at constant pressure is approximately 4.18 J/g°C.

The specific heat capacity of water is approximately 4.18 J/g°C.

The work done during an isothermal expansion is given by W = nRT ln(V2/V1).

For an ideal gas undergoing isothermal expansion, the work done is given by W = nRT ln(Vf/Vi).

The First Law of Thermodynamics states that energy cannot be created or destroyed, only transformed.

Free expansion is an irreversible process as it occurs without any external pressure acting on the gas.

An isochoric process is one that occurs at constant volume.