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| author | priyanka | 2015-06-24 15:03:17 +0530 |
|---|---|---|
| committer | priyanka | 2015-06-24 15:03:17 +0530 |
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| tree | ab291cffc65280e58ac82470ba63fbcca7805165 /479/CH14/EX14.5/Example_14_5.sce | |
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diff --git a/479/CH14/EX14.5/Example_14_5.sce b/479/CH14/EX14.5/Example_14_5.sce new file mode 100755 index 000000000..3a2d45ea5 --- /dev/null +++ b/479/CH14/EX14.5/Example_14_5.sce @@ -0,0 +1,29 @@ +//Chemical Engineering Thermodynamics
+//Chapter 14
+//Thermodynamics of Chemical Reactions
+
+//Example 14.5
+clear;
+clc;
+
+//Given
+T = 298;//Temperature in Kelvin
+//Standard enthalpy in Kcal/Kgmole of the following components at 298 K are given as
+H_SO2 = -70960;
+H_SO3 = -94450;
+H_O2 = 0;
+//Standard entropy in Kcal/Kgmole K of the following components at 298 K are given as
+S_SO2 = 2.48;
+S_SO3 = -19.7
+S_O2 = 0;
+//Basis: 1 Kgmole of SO2
+//SO2 +(1/2)O2 - SO3
+
+//To Calculate the standard free energy for the reaction
+n_SO2 = 1;//Kgmole of SO2 fed
+n_O2 = (1/2)*2;//Kgmole of O2 fed as 100% excess O2 is given
+n_SO3 = n_SO2;//Kgmole of SO3 formed
+//From equation 14.38 (page no 312)
+del_F = (H_SO3-(T*S_SO3))-(H_SO2-(T*S_SO2))-(H_O2-(T*S_O2));
+mprintf('The standard free energy for the reaction at 25 degree celsius is %f Kcal/Kgmole',del_F);
+//end
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