diff options
Diffstat (limited to 'Chemistry/Chapter_18.ipynb')
| -rwxr-xr-x | Chemistry/Chapter_18.ipynb | 284 |
1 files changed, 0 insertions, 284 deletions
diff --git a/Chemistry/Chapter_18.ipynb b/Chemistry/Chapter_18.ipynb deleted file mode 100755 index aabe2f15..00000000 --- a/Chemistry/Chapter_18.ipynb +++ /dev/null @@ -1,284 +0,0 @@ -{
- "metadata": {
- "name": ""
- },
- "nbformat": 3,
- "nbformat_minor": 0,
- "worksheets": [
- {
- "cells": [
- {
- "cell_type": "heading",
- "level": 1,
- "metadata": {},
- "source": [
- "Chapter 18:Entropy, Free Energy,and Equilibrium"
- ]
- },
- {
- "cell_type": "heading",
- "level": 2,
- "metadata": {},
- "source": [
- "Example no:18.2,Page no:809"
- ]
- },
- {
- "cell_type": "code",
- "collapsed": false,
- "input": [
- "#Variable declaration\n",
- "#(a)\n",
- "SCaO=39.8 #standard entropy of CaO, J/K mol\n",
- "SCO2=213.6 #standard entropy of CO2, J/K mol\n",
- "SCaCO3=92.9 #standard entropy of CaCO3, J/K mol\n",
- "#(b)\n",
- "SNH3=193 #standard entropy of NH3, J/K mol\n",
- "SN2=192 #standard entropy of N2, J/K mol\n",
- "SH2=131 #standard entropy of H2, J/K mol\n",
- "#(c)\n",
- "SHCl=187 #standard entropy of HCl, J/K mol\n",
- "SH2=131 #standard entropy of H2, J/K mol\n",
- "SCl2=223 #standard entropy of Cl2, J/K mol\n",
- "\n",
- "#Calculation\n",
- "#(a)\n",
- "deltaSrxn1=SCaO+SCO2-SCaCO3 #standard entropy change of the reaction, J/K mol\n",
- "#(b)\n",
- "deltaSrxn2=2*SNH3-(SN2+3*SH2) #standard entropy change of the reaction, J/K mol\n",
- "#(c)\n",
- "deltaSrxn3=2*SHCl-SH2-SCl2 #standard entropy change of the reaction, J/K mol\n",
- "\n",
- "#Result\n",
- "print\"(a) the standard entropy of reaction is :\",deltaSrxn1,\"J/K mol\"\n",
- "print\"(b) the standard entropy of reaction is :\",deltaSrxn2,\"J/K mol\"\n",
- "print\"(c) the standard entropy of reaction is :\",deltaSrxn3,\"J/K mol\""
- ],
- "language": "python",
- "metadata": {},
- "outputs": [
- {
- "output_type": "stream",
- "stream": "stdout",
- "text": [
- "(a) the standard entropy of reaction is : 160.5 J/K mol\n",
- "(b) the standard entropy of reaction is : -199 J/K mol\n",
- "(c) the standard entropy of reaction is : 20 J/K mol\n"
- ]
- }
- ],
- "prompt_number": 22
- },
- {
- "cell_type": "heading",
- "level": 2,
- "metadata": {},
- "source": [
- "Example no:18.4,Page no:817"
- ]
- },
- {
- "cell_type": "code",
- "collapsed": false,
- "input": [
- "#Variable declaration\n",
- "#(a)\n",
- "GCO2=-394.4 #free energy of formation of CO2, kJ/mol\n",
- "GH2O=-237.2 #free energy of formation of H2O, kJ/mol\n",
- "GCH4=-50.8 #free energy of formation of CH4, kJ/mol\n",
- "GO2=0 #free energy of formation of O2, kJ/mol\n",
- "#(b)\n",
- "GMg=0 #free energy of formation of Mg, kJ/mol\n",
- "GMgO=-569.6 #free energy of formation of MgO, kJ/mol\n",
- "GO2=0 #free energy of formation of O2, kJ/mol\n",
- "\n",
- "#Calculation\n",
- "deltaGrxn1=(GCO2+GH2O*2)-(GCH4+2*GO2) #standard free energy change of the reaction, kJ/mol\n",
- "deltaGrxn=(GO2+GMg*2)-(2*GMgO) #standard free energy change of the reaction, kJ/mol\n",
- "\n",
- "#Result\n",
- "print\"(a) The standard free energy change of reaction is :\",deltaGrxn1,\"kJ/mol\"\n",
- "print\"(b) The standard free energy change of reaction is :\",round(deltaGrxn),\"kJ/mol\""
- ],
- "language": "python",
- "metadata": {},
- "outputs": [
- {
- "output_type": "stream",
- "stream": "stdout",
- "text": [
- "(a) The standard free energy change of reaction is : -818.0 kJ/mol\n",
- "(b) The standard free energy change of reaction is : 1139.0 kJ/mol\n"
- ]
- }
- ],
- "prompt_number": 2
- },
- {
- "cell_type": "heading",
- "level": 2,
- "metadata": {},
- "source": [
- "Example no:18.5,Page no:820"
- ]
- },
- {
- "cell_type": "code",
- "collapsed": false,
- "input": [
- "#Variable declaration\n",
- "#for fusion\n",
- "T1=5.5+273 #temperature of fusion, K\n",
- "deltaH1=10.9*1000 #change in enthalpy, J/mol\n",
- "#for vaporisation\n",
- "T2=80.1+273 #temperature of vaporisation, K\n",
- "deltaH2=31*1000 #change in enthalpy, J/mol\n",
- "\n",
- "#Calculation\n",
- "deltaSf=deltaH1/T1 #since in fusion deltaG=0, J/ K mol\n",
- "deltaSv=deltaH2/T2 #since in vaporisation deltaG=0, J/ K mol\n",
- "\n",
- "#Result\n",
- "print\"The entropy change for fusion is\",round(deltaSf,1),\"J/K.mol\" \n",
- "print\"The entropy change for condensation is : \",round(deltaSv,1),\"J/K mol\"\n"
- ],
- "language": "python",
- "metadata": {},
- "outputs": [
- {
- "output_type": "stream",
- "stream": "stdout",
- "text": [
- "The entropy change for fusion is 39.1 J/K.mol\n",
- "The entropy change for condensation is : 87.8 J/K mol\n"
- ]
- }
- ],
- "prompt_number": 24
- },
- {
- "cell_type": "heading",
- "level": 2,
- "metadata": {},
- "source": [
- "Example no:18.6,Page no:823"
- ]
- },
- {
- "cell_type": "code",
- "collapsed": false,
- "input": [
- "T=298 #temperature, K\n",
- "R=8.314 #gas constant, J/K mol\n",
- "GH2=0 #free energy of formation of H2, kJ/mol\n",
- "GH2O=-237.2 #free energy of formation of H2O, kJ/mol\n",
- "GO2=0 #free energy of formation of O2, kJ/mol\n",
- "\n",
- "#Calculation\n",
- "import math\n",
- "deltaG=1000*(2*GH2+GO2-2*GH2O) #free energy of rxn, J/mol\n",
- "Kp=math.exp(-deltaG/(R*T)) #equilibrium constant for rxn\n",
- "\n",
- "#Result\n",
- "print\"deltaG_rxn=\",deltaG/1000,\"kJ/mol\"\n",
- "print\"The equilibrium constant for the given reaction is :%.e\"%Kp"
- ],
- "language": "python",
- "metadata": {},
- "outputs": [
- {
- "output_type": "stream",
- "stream": "stdout",
- "text": [
- "deltaG_rxn= 474.4 kJ/mol\n",
- "The equilibrium constant for the given reaction is :7e-84\n"
- ]
- }
- ],
- "prompt_number": 25
- },
- {
- "cell_type": "heading",
- "level": 2,
- "metadata": {},
- "source": [
- "Example no:18.7,Page no:824"
- ]
- },
- {
- "cell_type": "code",
- "collapsed": false,
- "input": [
- "#Variable declaration\n",
- "T=298 #temperature, K\n",
- "R=8.314 #gas constant, J/K mol\n",
- "Ksp=1.6*10**-10 #solubility constant\n",
- "\n",
- "#Calculation\n",
- "import math\n",
- "deltaG=-R*T*math.log(Ksp) #here solubility product is equal to equilibrium constant\n",
- "\n",
- "#Result\n",
- "print\"The free energy for the given reaction is :\",round(deltaG*10**-3),\"kJ/mol\""
- ],
- "language": "python",
- "metadata": {},
- "outputs": [
- {
- "output_type": "stream",
- "stream": "stdout",
- "text": [
- "The free energy for the given reaction is : 56.0 kJ/mol\n"
- ]
- }
- ],
- "prompt_number": 26
- },
- {
- "cell_type": "heading",
- "level": 2,
- "metadata": {},
- "source": [
- "Example no:18.8,Page no:825"
- ]
- },
- {
- "cell_type": "code",
- "collapsed": false,
- "input": [
- "#Variable declaration\n",
- "T=298 #temperature, K\n",
- "R=8.314 #gas constant, J/K mol\n",
- "deltaG0=5.4*10**3 #standard free energy, kJ/mol\n",
- "pNO2=0.122 #pressure of NO2, atm\n",
- "pN2O4=0.453 #pressure of N2O4, atm\n",
- "\n",
- "#Calculation\n",
- "import math\n",
- "deltaG=deltaG0+R*T*math.log(pNO2**2/pN2O4) #here solubility product is equal to equilibrium constant\n",
- "\n",
- "#Result\n",
- "if(deltaG<0):#equilibrium determination\n",
- " d=\"net reaction proceeds from left to right to reach equilibrium\" \n",
- "else:\n",
- " d=\"net reaction proceeds from right to left to reach equilibrium\" \n",
- "print\"The free energy for the given reaction is :\",round(deltaG*10**-3,2),\"kJ/mol and\",d\n"
- ],
- "language": "python",
- "metadata": {},
- "outputs": [
- {
- "output_type": "stream",
- "stream": "stdout",
- "text": [
- "The free energy for the given reaction is : -3.06 kJ/mol and net reaction proceeds from left to right to reach equilibrium\n"
- ]
- }
- ],
- "prompt_number": 27
- }
- ],
- "metadata": {}
- }
- ]
-}
\ No newline at end of file |