blob: 02d659e310847bf91b17b037d8063aaeba71545e (
plain)
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
19
20
21
22
23
24
25
26
27
28
29
30
|
//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);
|
