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| author | prashantsinalkar | 2017-10-10 12:27:19 +0530 |
|---|---|---|
| committer | prashantsinalkar | 2017-10-10 12:27:19 +0530 |
| commit | 7f60ea012dd2524dae921a2a35adbf7ef21f2bb6 (patch) | |
| tree | dbb9e3ddb5fc829e7c5c7e6be99b2c4ba356132c /3856/CH9/EX9.3/Ex9_3.sce | |
| parent | b1f5c3f8d6671b4331cef1dcebdf63b7a43a3a2b (diff) | |
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initial commit / add all books
Diffstat (limited to '3856/CH9/EX9.3/Ex9_3.sce')
| -rw-r--r-- | 3856/CH9/EX9.3/Ex9_3.sce | 24 |
1 files changed, 24 insertions, 0 deletions
diff --git a/3856/CH9/EX9.3/Ex9_3.sce b/3856/CH9/EX9.3/Ex9_3.sce new file mode 100644 index 000000000..b95eb85a2 --- /dev/null +++ b/3856/CH9/EX9.3/Ex9_3.sce @@ -0,0 +1,24 @@ +//Calculate the Equilibrium constant for the reaction 2H2(g)+O2(g)=2H2O(l)
+
+//Example 9.3
+
+clc;
+
+clear;
+
+delG1=-237.2; //Standard Gibbs enaergy for H2O in kJ mol^-1
+
+delG2=0; //Standard Gibbs enaergy for H2 in kJ mol^-1
+
+delG3=0; //Standard Gibbs enaergy for O2 in kJ mol^-1
+
+delG=2*delG1-2*delG2-delG3; //Standard Gibbs enaergy change for the reaction in kJ mol^-1
+
+R=8.314; //Gas constant in J K^-1 mol^-1
+
+T=298; //Temperature in K
+
+Kp=exp(-(delG*1000)/(R*T)); //Equilibrium constant
+
+printf("Equilibrium constant = %.1f*10^83",Kp*10^-83);
+
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