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  • General

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  • Entropy increase calculated from thermodynamic function

    • Introduction of thermodynamic functions

      Here, the thermodynamic equation finally comes into play in order to better understand entropy.

       

      【First law of thermodynamics】

      　When heat (⊿Q) is added to an object, it is used to increase the internal energy of the object (⊿U) and change the volume of the object (work = P⊿V).

      　P is pressure and ⊿V is volume change. 

                                  ⊿Q ＝ ⊿U ＋ P⊿V

       

      【Ideal gas law】

      　Volume (V) is inversely proportional to pressure (P) and proportional to temperature (T)

       

                                  PV = nRT　　→　PV = RT, per mol.

       

      　　　　　　　　R：gas constant、T：absolute temperature(K)

       

      【Internal energy (U) is proportional to temperature】（For now, I hope you believe that. I'll add more later.）

       

      U = n3/2・RT　→　U = 3/2・RT, per mol.

       

      Internal energy change is, ⊿U = 3/2・R⊿T.


                                                                                                                                   

       

      Based on these, we calculate the entropy change when changing from state 0 (T0, V0) to state 1 (T1, V1).

       

      Definition of entropy change：　⊿S ＝ ⊿Q／T

       

      ⊿S = ⊿Q／T = ( ⊿U + P⊿V)／T

          = (3/2・R⊿T ＋ P⊿V)／T

          =3/2・R⊿T／T ＋ R⊿V／V                         （Transformation of the ideal gas law：1／T = R／PV）

          =3/2・R （∫1/T dT） ＋ R（∫1/V dV）　　　←At the integral, T0→T1 and V0→V1.

          =3/2・R・Ln(T1／T0) ＋ R・Ln(V1／V0)

    • Here we have the important equation to calculate the entropy change from state 0 (T0, V0) to state 1 (T1, V1).

       

      ⊿S = ⊿Q／T

          =3/2・R・Ln(T1／T0) ＋ R・Ln(V1／V0)

       

      (The above equation is the entropy change per mole. n should be multiplied by n when dealing with n moles of material.)


  • Calculate the amount of entropy change

    • 　Using the entropy change equation above, let's actually calculate the amount of entropy change.

      　First, for one mole of ideal gas, the entropy change when the temperature is kept constant (Ln(T1/T0) = 0) and the volume is increased tenfold is ⊿S = R・Ln(10) = 19.3 (J/K). When the volume is restored, ⊿S = -19.3 (J/K) as well.

      Fig. 1

      　Earlier, I mentioned that entropy always increases, and this is only true for adiabatic systems. It is possible to decrease the entropy of a substance, and in doing so, heat must be transferred to the outside world.

      　Examples of calculations of entropy change are still to come.

    • Example of calculation of entropy change

      　

      　Gas A (1 mol) is in a 1 m3 container. Adjacent to it, gas B (1 mol) is in a 1 m3 container (see picture below). Calculate the entropy change when the partition between containers AB is removed and gases A and B are mixed.


      　For gas A, the volume in existence has increased from 1 to 2 m3, and for gas B, the volume has increased from 1 to 2 m3. The entropy changes (SA, SB) for gas A and gas B, respectively, are then, 

      SA = 1・8.31・Ln(2/1) = 5.76

      SB = 1・8.31・Ln(2/1) = 5.76.

      The entropy change of the entire system is,

      SA + SB ＝ 11.52 (J/K).


      Fig. 2

      We simply removed the partitions between the spaces in contact and mixed the respective gases.
      No work was done on the outside world, no chemical changes occurred, but entropy increased.