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+//Chemical Engineering Thermodynamics

+//Chapter 14

+//Thermodynamics of Chemical Reactions

+

+//Example 14.13

+clear;

+clc;

+

+//Given

+T1 = 273+110;//Temperature in K

+T = 298;//Room temperature in K

+P = 1;//Pressure in atm

+R = 1.98;//gas constant in Kcal/Kgmole

+//Ag2CO3(s) (A) = Ag2O(s) (B) + CO2(g) (C)

+a = 1;//Stoichiometry coefficient of A

+b = 1;//Stoichiometry coefficient of B

+c = 1;//Stoichiometry coefficient of C

+//Standard entropy of the above components in Kcal/Kgmole K at 25 deg cel are given as

+S_A = 40.17;

+S_B = 29.09;

+S_C = 51.08;

+//Standard enthalpy of the above components in Kcal/Kgmole at 25 deg cel are given as

+H_A = -119900;

+H_B = -6950;

+H_C = -94036;

+//Specific heat (assumed constant) of the above components in Kcal/Kgmole K are given as

+C_A = 26.1;

+C_B = 16.5;

+C_C = 9.6;

+

+//To Calculate the partial pressure of CO2 required for decomposition and thus determine whether Ag2CO3 will decomposes or not at the given pressure and temperature

+del_H = H_C+H_B-H_A;//Standard heat of reaction  at 25 deg cel in Kcal/Kgmole

+del_C = b*C_B+c*C_C-a*C_A;

+//From equation 14.15 (page no 340)

+del_Ht = del_H +del_C*(T1-T);

+del_F = del_H-(T*(S_B+S_C-S_A));//Standard free energy in Kcal/Kgmole

+Ka1 = %e^(-del_F/(R*T));//Equilibrium constant at temperature T

+//Since del_Ht is constant(as del_C = 0),Ka2 can be calculated by equation 14.43 (page no 316)

+Ka2 = Ka1* %e^((del_Ht/R)*(1/T1-1/T));

+p_CO2 = Ka2;

+mprintf('The partial pressure of CO2 required for decomposition is %4.3e atm',p_CO2);

+if p_CO2 < P 

+    mprintf('\n Silver carbonate will not decompose at 110 deg celsius as the pressure given is 1 atm');

+else

+    mprintf('\n Silver carbonate will decompose at 110 deg celsius');

+end

+//end
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