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+{
+ "cells": [
+  {
+   "cell_type": "markdown",
+   "metadata": {},
+   "source": [
+    "# Appendix D"
+   ]
+  },
+  {
+   "cell_type": "markdown",
+   "metadata": {},
+   "source": [
+    "## Example 2"
+   ]
+  },
+  {
+   "cell_type": "code",
+   "execution_count": 1,
+   "metadata": {
+    "collapsed": false
+   },
+   "outputs": [
+    {
+     "name": "stdout",
+     "output_type": "stream",
+     "text": [
+      "Change in gibbs free energy at 298K : 457.179 KJ\n",
+      "Change in gibbs free energy at 298K : 271.04 KJ\n"
+     ]
+    }
+   ],
+   "source": [
+    "# -*- coding: utf8 -*-\n",
+    "from __future__ import division\n",
+    "#Example: 16.2\n",
+    "'''Determine the value of \u0002G0 for the reaction 2H2O \u0003\u0004 2H2 + O2 at 25◦C and at 2000 K,\n",
+    "with the water in the gaseous phase.'''\n",
+    "\n",
+    "#Keys:\n",
+    "#1-H2\n",
+    "#2-O2\n",
+    "#3-H2O\n",
+    "\n",
+    "#Variable Declaration: \n",
+    "def dG(T1,Hf1,Hf2,Hf3,Sf1,Sf2,sf3):\n",
+    "\tdH = 2*Hf1+Hf2-2*Hf3\t#Change in enthalpy in kJ\n",
+    "\tdS = 2*Sf1+Sf2-2*sf3 \t#Change in entropy in J/K\n",
+    "\tdG = dH-T1*dS/1000\t#change n gibbs free energy in kJ\n",
+    "\treturn dG\n",
+    "\n",
+    "#Results:\n",
+    "print 'Change in gibbs free energy at 298K :',round(dG(298,0, 0, -241.826, 130.678,205.148,188.834),3),\"KJ\"\n",
+    "print 'Change in gibbs free energy at 298K :',round(dG(2000,52.942, 59.176, -241.826+72.788,188.419,268.748,264.769),3),\"KJ\"\n"
+   ]
+  },
+  {
+   "cell_type": "markdown",
+   "metadata": {},
+   "source": [
+    "## Example 3"
+   ]
+  },
+  {
+   "cell_type": "code",
+   "execution_count": 2,
+   "metadata": {
+    "collapsed": false
+   },
+   "outputs": [
+    {
+     "name": "stdout",
+     "output_type": "stream",
+     "text": [
+      "Equilibrium constant at 298K:  -184.51\n",
+      "Equilibrium constant at 2000K:  -16.299\n"
+     ]
+    }
+   ],
+   "source": [
+    "# -*- coding: utf8 -*-\n",
+    "from __future__ import division\n",
+    "#Example: 16.3\n",
+    "'''Determine the equilibrium constant K, expressed as ln K, for the reaction 2H2O <--->\n",
+    "2H2 + O2 at 25◦C and at 2000 K.'''\n",
+    "\n",
+    "#Variable Declaration: \n",
+    "dG1 = -457.166\t\t\t#change in gibbs free energy at temp 298 K from example2 in kJ\n",
+    "dG2 = -271.040\t\t\t#change in gibbs free energy at temp 2000 K from example2 n kJ\n",
+    "T1 = 298\t\t\t\t#K\n",
+    "T2 = 2000\t\t\t\t#K\n",
+    "R = 8.3145\t\t\t\t#gas constant\n",
+    "\n",
+    "#Calculations:\n",
+    "K1 = dG1*1000/(R*T1)\n",
+    "K2 = dG2*1000/(R*T2)\n",
+    "\n",
+    "#Results:\n",
+    "print 'Equilibrium constant at 298K: ',round(K1,2)\n",
+    "print 'Equilibrium constant at 2000K: ',round(K2,3)"
+   ]
+  }
+ ],
+ "metadata": {
+  "kernelspec": {
+   "display_name": "Python 2",
+   "language": "python",
+   "name": "python2"
+  },
+  "language_info": {
+   "codemirror_mode": {
+    "name": "ipython",
+    "version": 2
+   },
+   "file_extension": ".py",
+   "mimetype": "text/x-python",
+   "name": "python",
+   "nbconvert_exporter": "python",
+   "pygments_lexer": "ipython2",
+   "version": "2.7.6"
+  }
+ },
+ "nbformat": 4,
+ "nbformat_minor": 0
+}