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+//Calculate the Equilibrium constant for the reaction  Sn(s)+2Ag(one positive)(aq)=Sn(double positive)(aq)+2Ag(s).  And also predict whether the given reaction would occur spontaneously under standard-state condition
+
+//Example 10.1
+
+clc;
+
+clear;
+
+Ecathode=0.800;  //Standard Electrode Potential for Ag in V
+
+Eanode=-0.138;  //Standard Electrode Potential for Sn in V
+
+E=Ecathode-Eanode;  //Standard Electrode Potential for Electrochemical cell (positive quantity of E shows the reaction is spontaneous under standard-state condition)
+
+F=96500;  //Faraday costant in C mol^-1
+
+v=2;  //Stoichiometric coefficient (two electron are transferred in reaction)
+
+R=8.314;  //Gas constant in J K^-1 mol^-1
+
+T=25+273;  //Temperature in K
+
+K=exp((v*E*F)/(R*T));  //Equilibrium constant 
+
+printf("Equilibrium constant = %.1f*10^31",K*10^-31);
+
+delrG=(-v*F*E)/1000;  //Gibbs Energy in kJ mol^-1 (large negative value of delrG indicate that the reaction is spontaneous under standard state condition)
+
+printf("\n Spontaneity of the reactin = %.0f kJ mol^-1",delrG);
+