Given: temperature of the iron cube = 400o C = 400 + 273 = 673 K Temperature of water = 10 kg Temperature of water and cube after equilibrium = 50o C = 50 +273 = 323 K Specific heat of water, cpw = 4186 J/kg K Entropy changes ...

For one mole of an ideal gas: dS = Cv dT / T + R dV / V Integrating the above equation, assuming that Cv remains constant for an ideal gas, we have: S = Cv ln T + R ln V + So Where So represents the ...

There are three types of processes in which entropy changes of an ideal gas. These three processes are: 1. Isothermal process 2. Isobaric process 3. Isochoric process 1. Isothermal process: The process in which there is no change in temperature is known as Isothermal process. Entropy changes from S1 to ...

Let us consider entropy at the initial state 1 is S1 and entropy at the final state 2 is S2. Hence, the change in entropy of a system, as it undergoes a change from state 1 to 2, becomes S2 - S1 = 2∫1 (δQ / T) ...

In order to prove that entropy is a property, we will suppose two cycles i.e. 1-A-2-B-1 and 1-A-2-C-1 as shown in For a reversible cycle 1-A-2-B-1: ∫1-A-2 δQ / T + ∫2-B-1 δQ / T = 0 For a reversible cycle 1-A-2-C-1: ∫1-A-2 δQ / T + ∫2-C-1 ...

The various relationships between internal energy (U), enthalpy (H), Helmholtz free energy (a) and Gibbs free energy (g), with relevant parameters such as entropy, pressure, temperature and volume are given by the following equations: 1. dU = TdS – PdV 2. dH = TdS + VdP 3. dA = - SdT ...

Entropy Principle: Form the Clausius inequality, ∫ δQ / T ≤ 0 As the entropy is a property of the system, therefore the cyclic integral of a property is zero and the above equation can also be written as: ∫ δQ / T ≤ ∫ dS SQ / T ...

Entropy is a measure of the degree of randomness of the molecules comprising the system. Higher the disorder, greater is the increase in entropy. Entropy is the function of a quantity of heat which shows the possibility of conversion of that heat into work. The ...