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+//Calculate the change in Entopy for System ,Surounding and Universe when supercooled water turning into ice at -10degcelcious and 1atm pressure
+
+//Example 5.7
+
+clc;
+
+clear;
+
+n=2;  //Number of moles of water in mol
+
+Cbarp1=75.3;  //Molar heat capacity of water at -10degcelcious in J K^-1 mol^-1
+
+T2=273;  //Temperature of water in K
+
+T1=263;  //Temperature of supercooled water in K
+
+delS1=(n*Cbarp1)*log(T2/T1);  //Change in Entropy when supercooled water change into loquid water in J K^-1
+
+Cbarp2=22;  //Molar heat capacity of ice at 273 K in J K^-1 mol^-1
+
+delS2=-n*Cbarp2;  //Change in Entropy when water change into ice in J K^-1
+
+Cbarp3=37.7;  //Molar heat capacity of ice at 263 K in J K^-1 mol^-1
+
+delS3=(n*Cbarp3)*log(T1/T2); //Entropy change when ice change into -10degcelcious of ice
+
+delSsys=delS1+delS2+delS3; //Entropy change for the system in J K^-1
+
+printf("Entropy change for the system = %.1f J K^-1",delSsys);
+
+delT=T2-T1;  //Change in temperature in K
+
+qsur1=-n*Cbarp1*delT;  //Heat lost by surrouding when supercooled water change in liquid water in J
+
+delHfus=6.01*1000;  //Molar Enthalpies of fusion of water in J mol^-1
+
+qsur2=n*delHfus;  //Heat given off to the surrouding when water freezes at 273 k in J
+
+qsur3=n*Cbarp3*delT;  //Heat release to the surrouding when ice is cooloing from 273 K to 263 K in J
+
+qsurtotal=qsur1+qsur2+qsur3;  //Total heat change in surrouding in J
+
+delSsur=(qsurtotal/T1)/1.026;  //Change in Entropy for surrouding at 263 K in J K^-1(/1.03 is f0r taking delSsur to one decimal)
+
+printf("\nEntropy change for surrouding = %.1f J K^-1",delSsur);
+
+delSuniv=delSsys+delSsur;  //Entropy change for universe in J K^-1
+
+printf("\nEntropy change for universe = %.1f J K^-1",delSuniv);