summaryrefslogtreecommitdiff
path: root/Basic_And_Applied_Thermodynamics_by_P._K._Nag/Chapter16.ipynb
diff options
context:
space:
mode:
Diffstat (limited to 'Basic_And_Applied_Thermodynamics_by_P._K._Nag/Chapter16.ipynb')
-rw-r--r--Basic_And_Applied_Thermodynamics_by_P._K._Nag/Chapter16.ipynb548
1 files changed, 548 insertions, 0 deletions
diff --git a/Basic_And_Applied_Thermodynamics_by_P._K._Nag/Chapter16.ipynb b/Basic_And_Applied_Thermodynamics_by_P._K._Nag/Chapter16.ipynb
new file mode 100644
index 00000000..bd0ffde7
--- /dev/null
+++ b/Basic_And_Applied_Thermodynamics_by_P._K._Nag/Chapter16.ipynb
@@ -0,0 +1,548 @@
+{
+ "cells": [
+ {
+ "cell_type": "markdown",
+ "metadata": {},
+ "source": [
+ "# Chapter 16:Reactive Systems"
+ ]
+ },
+ {
+ "cell_type": "markdown",
+ "metadata": {},
+ "source": [
+ "## Ex16.2:pg-675"
+ ]
+ },
+ {
+ "cell_type": "code",
+ "execution_count": 2,
+ "metadata": {
+ "collapsed": false
+ },
+ "outputs": [
+ {
+ "name": "stdout",
+ "output_type": "stream",
+ "text": [
+ "\n",
+ " Example 16.2\n",
+ "\n",
+ "\n",
+ " K is 0.314529177004 atm\n",
+ "\n",
+ " Epsilon is 0.611607081035\n",
+ "\n",
+ " The heat of reaction is 60974.6120608 kJ/kg mol\n"
+ ]
+ }
+ ],
+ "source": [
+ "import math\n",
+ "eps_e = 0.27 # Constant\n",
+ "P = 1.0 # Atmospheric pressure in bar\n",
+ "K = (4*eps_e**2*P)/(1-eps_e**2) \n",
+ "P1 = 100.0/760.0 # Pressure in Pa\n",
+ "eps_e_1 = math.sqrt((K/P1)/(4.0+(K/P1)))\n",
+ "T1 = 318.0 # Temperature in K\n",
+ "T2 = 298.0# Temperature in K\n",
+ "R = 8.3143 # Gas constant\n",
+ "K1 = 0.664 # dissociation constant at 318K\n",
+ "K2 = 0.141# dissociation constant at 298K\n",
+ "dH = 2.30*R*((T1*T2)/(T1-T2))*(math.log10(K1/K2))\n",
+ "print \"\\n Example 16.2\\n\"\n",
+ "print \"\\n K is \",K ,\" atm\"\n",
+ "print \"\\n Epsilon is \",eps_e_1\n",
+ "print \"\\n The heat of reaction is \",dH ,\" kJ/kg mol\"\n",
+ "#The answers vary due to round off error\n",
+ "\n"
+ ]
+ },
+ {
+ "cell_type": "markdown",
+ "metadata": {},
+ "source": [
+ "## Ex16.3:pg-675"
+ ]
+ },
+ {
+ "cell_type": "code",
+ "execution_count": 4,
+ "metadata": {
+ "collapsed": false
+ },
+ "outputs": [
+ {
+ "name": "stdout",
+ "output_type": "stream",
+ "text": [
+ "\n",
+ " Example 16.3\n",
+ "\n",
+ "\n",
+ " Equilibrium constant is 1.61983471074\n",
+ "\n",
+ " Gibbs function change is -4812.22485358 J/gmol\n"
+ ]
+ }
+ ],
+ "source": [
+ "v1 = 1.0 # Assumed\n",
+ "v2 = v1# Assumed \n",
+ "v3 = v2 # Assumed\n",
+ "v4 = v2# Assumed\n",
+ "e = 0.56 # Degree of reaction\n",
+ "P = 1.0 # Dummy\n",
+ "T = 1200.0 # Reaction temperature in K\n",
+ "R = 8.3143 # Gas constant\n",
+ "x1 = (1-e)/2.0 # \n",
+ "x2 = (1-e)/2.0\n",
+ "x3 = e/2.0 \n",
+ "x4 = e/2.0\n",
+ "K = (((x3**v3)*(x4**v4))/((x1**v1)*(x2**v2)))*P**(v3+v4-v1-v2) # Equilibrium constant\n",
+ "dG = -R*T*math.log(K) #Gibbs function change\n",
+ "\n",
+ "print \"\\n Example 16.3\\n\"\n",
+ "print \"\\n Equilibrium constant is \",K\n",
+ "print \"\\n Gibbs function change is \",dG ,\"J/gmol\"\n",
+ "#The answers vary due to round off error"
+ ]
+ },
+ {
+ "cell_type": "markdown",
+ "metadata": {},
+ "source": [
+ "## Ex16.5:pg-678"
+ ]
+ },
+ {
+ "cell_type": "code",
+ "execution_count": 6,
+ "metadata": {
+ "collapsed": false
+ },
+ "outputs": [
+ {
+ "name": "stdout",
+ "output_type": "stream",
+ "text": [
+ "\n",
+ " Example 16.5\n",
+ "\n",
+ "\n",
+ " The value of equillibrium constant is 0.755668681281 atm\n"
+ ]
+ }
+ ],
+ "source": [
+ "Veo = 1.777 # Ve/Vo\n",
+ "e = 1.0-Veo # Degree of dissociation\n",
+ "P = 0.124 # in atm\n",
+ "K = (4*e**2*P)/(1.0-e**2)\n",
+ "\n",
+ "print \"\\n Example 16.5\\n\"\n",
+ "print \"\\n The value of equillibrium constant is \",K ,\" atm\""
+ ]
+ },
+ {
+ "cell_type": "markdown",
+ "metadata": {},
+ "source": [
+ "## Ex16.6:pg-680"
+ ]
+ },
+ {
+ "cell_type": "code",
+ "execution_count": 7,
+ "metadata": {
+ "collapsed": false
+ },
+ "outputs": [
+ {
+ "name": "stdout",
+ "output_type": "stream",
+ "text": [
+ "\n",
+ " Example 16.6\n",
+ "\n",
+ "\n",
+ " Cp is 4.48364424966 J/g mol K\n"
+ ]
+ }
+ ],
+ "source": [
+ "v1 = 1.0 # Assumed\n",
+ "v2 = 0 # Assumed\n",
+ "v3 = 1.0 # Assumed\n",
+ "v4 = 1.0/2.0# Assumed\n",
+ "dH = 250560.0 # Enthalpy change in j/gmol\n",
+ "e = 3.2e-03 # Constant\n",
+ "R = 8.3143 # Gas constant\n",
+ "T = 1900.0 # Reaction temperature\n",
+ "Cp = ((dH**2)*(1+e/2)*e*(1+e))/(R*T**2*(v1+v2)*(v3+v4))\n",
+ "print \"\\n Example 16.6\\n\"\n",
+ "print \"\\n Cp is \",Cp ,\" J/g mol K\"\n",
+ "#The answers vary due to round off error"
+ ]
+ },
+ {
+ "cell_type": "markdown",
+ "metadata": {},
+ "source": [
+ "## Ex16.7:pg-681"
+ ]
+ },
+ {
+ "cell_type": "code",
+ "execution_count": 8,
+ "metadata": {
+ "collapsed": false
+ },
+ "outputs": [
+ {
+ "name": "stdout",
+ "output_type": "stream",
+ "text": [
+ "\n",
+ " Example 16.7\n",
+ "\n",
+ "\n",
+ " The composition of fuel is 14.7645650439 percent Hydrogen and 85.2354349561 percent Carbon\n",
+ "\n",
+ " Air fuel ratio is 23.9829146049\n",
+ "\n",
+ " Percentage of excess air used is 67.2268907563 percent\n"
+ ]
+ }
+ ],
+ "source": [
+ "\n",
+ "a = 21.89 # stochiometric coefficient\n",
+ "y = 18.5 # stochiometric coefficient\n",
+ "x = 8.9 # stochiometric coefficient\n",
+ "PC = 100*(x*12)/((x*12)+(y)) # Carbon percentage\n",
+ "PH = 100-PC # Hydrogen percentage\n",
+ "AFR = ((32*a)+(3.76*a*28))/((12*x)+y) #Air fuel ratio\n",
+ "EAU = (8.8*32)/((21.89*32)-(8.8*32)) # Excess air used\n",
+ "\n",
+ "print \"\\n Example 16.7\\n\"\n",
+ "print \"\\n The composition of fuel is \",PH ,\" percent Hydrogen and \",PC ,\" percent Carbon\"#The answer provided in the textbook is wrong\n",
+ "print \"\\n Air fuel ratio is \",AFR\n",
+ "print \"\\n Percentage of excess air used is \",EAU*100 ,\" percent\"\n",
+ "#The answers vary due to round off error\n"
+ ]
+ },
+ {
+ "cell_type": "markdown",
+ "metadata": {},
+ "source": [
+ "## Ex16.8:pg-682"
+ ]
+ },
+ {
+ "cell_type": "code",
+ "execution_count": 9,
+ "metadata": {
+ "collapsed": false
+ },
+ "outputs": [
+ {
+ "name": "stdout",
+ "output_type": "stream",
+ "text": [
+ "\n",
+ " Example 16.8\n",
+ "\n",
+ "\n",
+ " Heat transfer per kg mol of fuel is -965198.0 kJ\n",
+ "\n",
+ " Q_cv is -890324.0 kJ\n"
+ ]
+ }
+ ],
+ "source": [
+ "hf_co2 = -393522.0 # Enthalpy of reaction in kJ/kg mol\n",
+ "hf_h20 = -285838.0# Enthalpy of reaction in kJ/kg mol\n",
+ "hf_ch4 = -74874.0# Enthalpy of reaction in kJ/kg mol\n",
+ "D = hf_co2 + (2*hf_h20) #Heat transfer \n",
+ "QCV = D-hf_ch4 # Q_cv\n",
+ "\n",
+ "print \"\\n Example 16.8\\n\"\n",
+ "print \"\\n Heat transfer per kg mol of fuel is \",D ,\" kJ\"\n",
+ "print \"\\n Q_cv is \",QCV ,\" kJ\"\n",
+ "#The answers vary due to round off error"
+ ]
+ },
+ {
+ "cell_type": "markdown",
+ "metadata": {},
+ "source": [
+ "## Ex16.9:pg-683"
+ ]
+ },
+ {
+ "cell_type": "code",
+ "execution_count": 10,
+ "metadata": {
+ "collapsed": false
+ },
+ "outputs": [
+ {
+ "name": "stdout",
+ "output_type": "stream",
+ "text": [
+ "\n",
+ " Example 16.9 \n",
+ "\n",
+ "\n",
+ " Fuel consumption rate is 38.5131749981 kg/h\n"
+ ]
+ }
+ ],
+ "source": [
+ "# Below values are taken from table\n",
+ "Hr = -249952+(18.7*560)+(70*540)\n",
+ "Hp = 8*(-393522+20288)+9*(-241827+16087)+6.25*14171+70*13491\n",
+ "Wcv = 150.0 # Energy out put from engine in kW\n",
+ "Qcv = -205.0 # Heat transfer from engine in kW\n",
+ "n = (Wcv-Qcv)*3600/(Hr-Hp)\n",
+ "print \"\\n Example 16.9 \\n\"\n",
+ "print \"\\n Fuel consumption rate is \",n*114 ,\" kg/h\"\n",
+ "#The answers vary due to round off error"
+ ]
+ },
+ {
+ "cell_type": "markdown",
+ "metadata": {},
+ "source": [
+ "## Ex16.11:pg-684"
+ ]
+ },
+ {
+ "cell_type": "code",
+ "execution_count": 13,
+ "metadata": {
+ "collapsed": false
+ },
+ "outputs": [
+ {
+ "name": "stdout",
+ "output_type": "stream",
+ "text": [
+ "\n",
+ " Example 16.11 \n",
+ "\n",
+ "\n",
+ " Reversible work is 47139 kJ/kg\n",
+ "\n",
+ " Increase in entropy during combustion is 3699.6688 kJ/kg mol K\n",
+ "\n",
+ " Irreversibility of the process 25056.8559091 kJ/kg\n",
+ "\n",
+ " Availability of products of combustion is 22082.1440909 kJ/kg\n"
+ ]
+ }
+ ],
+ "source": [
+ "# Refer table 16.4 for values\n",
+ "T0 = 298.0 # Atmospheric temperature in K\n",
+ "Wrev = -23316-3*(-394374)-4*(-228583) # Reversible work in kJ/kg mol\n",
+ "Wrev_ = Wrev/44 # Reversible work in kJ/kg\n",
+ "Hr = -103847 # Enthalpy of reactants in kJ/kg\n",
+ "T = 980.0 # Through trial and error\n",
+ "Sr = 270.019+20*205.142+75.2*191.611 # Entropy of reactants\n",
+ "Sp = 3*268.194 + 4*231.849 + 15*242.855 + 75.2*227.485 # Entropy of products\n",
+ "IE = Sp-Sr # Increase in entropy\n",
+ "I = T0*3699.67/44 # Irreversibility\n",
+ "Si = Wrev_ - I# Availability of products of combustion \n",
+ "\n",
+ "print \"\\n Example 16.11 \\n\"\n",
+ "print \"\\n Reversible work is \",Wrev_ ,\" kJ/kg\"\n",
+ "print \"\\n Increase in entropy during combustion is \",Sp-Sr ,\" kJ/kg mol K\"\n",
+ "print \"\\n Irreversibility of the process \",I ,\" kJ/kg\"\n",
+ "print \"\\n Availability of products of combustion is \",Si ,\" kJ/kg\"\n",
+ "#The answers vary due to round off error\n"
+ ]
+ },
+ {
+ "cell_type": "markdown",
+ "metadata": {},
+ "source": [
+ "## Ex16.12:pg-685"
+ ]
+ },
+ {
+ "cell_type": "code",
+ "execution_count": 14,
+ "metadata": {
+ "collapsed": false
+ },
+ "outputs": [
+ {
+ "name": "stdout",
+ "output_type": "stream",
+ "text": [
+ "\n",
+ " Example 6.12\n",
+ "\n",
+ "\n",
+ " The chemical energy of carbon is 410541.588354 kJ/k mol\n",
+ "\n",
+ " The chemical energy of hydrogen is 235211.889921 kJ/k mol\n",
+ "\n",
+ " The chemical energy of methane is 821580.156423 kJ/k mol\n",
+ "\n",
+ " The chemical energy of Carbon monoxide is 275364.910207 kJ/k mol\n",
+ "\n",
+ " The chemical energy of liquid methanol is 716698.69005 kJ/k mol\n",
+ "\n",
+ " The chemical energy of nitrogen is 691.0909601 kJ/k mol\n",
+ "\n",
+ " The chemical energy of Oxygen is 3946.64370597 kJ/k mol\n",
+ "\n",
+ " The chemical energy of Carbon dioxide is 20108.2320604 kJ/k mol\n",
+ "\n",
+ " The chemical energy of Water is 5.21177422707 kJ/k mol\n"
+ ]
+ }
+ ],
+ "source": [
+ "\n",
+ "T0 = 298.15 # Environment temperature in K\n",
+ "P0 = 1 # Atmospheric pressure in bar\n",
+ "R = 8.3143# Gas constant\n",
+ "xn2 = 0.7567 # mole fraction of nitrogen\n",
+ "xo2 = 0.2035 # mole fraction of oxygen\n",
+ "xh2o = 0.0312 # mole fraction of water\n",
+ "xco2 = 0.0003# mole fraction of carbon dioxide\n",
+ "# Part (a)\n",
+ "g_o2 = 0 # Gibbs energy of oxygen\n",
+ "g_c = 0 # Gibbs energy of carbon\n",
+ "g_co2 = -394380 # Gibbs energy of carbon dioxide\n",
+ "A = -g_co2 + R*T0*math.log(xo2/xco2) # Chemical energy\n",
+ "\n",
+ "# Part (b)\n",
+ "g_h2 = 0 # Gibbs energy of hydrogen\n",
+ "g_h2o_g = -228590# # Gibbs energy of water\n",
+ "B = g_h2 + g_o2/2 - g_h2o_g + R*T0*math.log(xo2**0.5/xh2o)\n",
+ "# Chemical energy\n",
+ "# Part (c)\n",
+ "g_ch4 = -50790 # Gibbs energy of methane\n",
+ "C = g_ch4 + 2*g_o2 - g_co2 - 2*g_h2o_g + R*T0*math.log((xo2**2)/(xco2*xh2o))\n",
+ "# Chemical energy\n",
+ "# Part (d)\n",
+ "g_co = -137150# # Gibbs energy of carbon mono oxide\n",
+ "D = g_co + g_o2/2 - g_co2 + R*T0*math.log((xo2**0.5)/xco2)\n",
+ "# Chemcal energy\n",
+ "# Part (e)\n",
+ "g_ch3oh = -166240 # Gibbs energy of methanol\n",
+ "E = g_ch3oh + 1.5*g_o2 - g_co2 - 2*g_h2o_g + R*T0*math.log((xo2**1.5)/(xco2*(xh2o**2)))\n",
+ "# Chemical energy\n",
+ "# Part (f)\n",
+ "F = R*T0*math.log(1/xn2)\n",
+ "# Chemical energy\n",
+ "# Part (g)\n",
+ "G = R*T0*math.log(1/xo2)\n",
+ "# Chemical energy\n",
+ "# Part (h)\n",
+ "H = R*T0*math.log(1/xco2)\n",
+ "# Chemical energy\n",
+ "# Part (i)\n",
+ "g_h2o_l = -237180 # Gibbs energy of liquid water\n",
+ "I = g_h2o_l - g_h2o_g + R*T0*math.log(1/xh2o)\n",
+ "# Chemical energy\n",
+ "print \"\\n Example 6.12\\n\"\n",
+ "print \"\\n The chemical energy of carbon is \",A ,\" kJ/k mol\"\n",
+ "print \"\\n The chemical energy of hydrogen is \",B ,\" kJ/k mol\"\n",
+ "print \"\\n The chemical energy of methane is \",C ,\" kJ/k mol\"\n",
+ "print \"\\n The chemical energy of Carbon monoxide is \",D ,\" kJ/k mol\"\n",
+ "print \"\\n The chemical energy of liquid methanol is \",E ,\" kJ/k mol\"\n",
+ "print \"\\n The chemical energy of nitrogen is \",F ,\" kJ/k mol\"\n",
+ "print \"\\n The chemical energy of Oxygen is \",G ,\" kJ/k mol\"\n",
+ "print \"\\n The chemical energy of Carbon dioxide is \",H ,\" kJ/k mol\"\n",
+ "print \"\\n The chemical energy of Water is \",I ,\" kJ/k mol\"\n",
+ "#The answers vary due to round off error"
+ ]
+ },
+ {
+ "cell_type": "markdown",
+ "metadata": {},
+ "source": [
+ "## Ex16.13:pg-686"
+ ]
+ },
+ {
+ "cell_type": "code",
+ "execution_count": 15,
+ "metadata": {
+ "collapsed": false
+ },
+ "outputs": [
+ {
+ "name": "stdout",
+ "output_type": "stream",
+ "text": [
+ "\n",
+ " Example 6.13\n",
+ "\n",
+ "\n",
+ " The rate of heat transfer from the engine = -4.33120060702 kW,\n",
+ " The second law of efficiency of the engine = 13.3396896634 percent\n"
+ ]
+ }
+ ],
+ "source": [
+ "# Environmet\n",
+ "T0 = 298.15 # Environment temperature in K\n",
+ "P0 = 1.0 # Atmospheric pressure in atm\n",
+ "R = 8.3143# Gas constant\n",
+ "xn2 = 0.7567 # mole fraction of nitrogen\n",
+ "xo2 = 0.2035 # mole fraction of oxygen\n",
+ "xh2o = 0.0312 # mole fraction of water\n",
+ "xco2 = 0.0003# mole fraction of carbon dioxide\n",
+ "xother = 0.0083 # Mole fraction of other gases\n",
+ "# Liquid octane\n",
+ "t1 = 25.0 # Temperature of liquid octane in degree centigrade\n",
+ "m = 0.57 # Mass flow rate in kg/h\n",
+ "T2 = 670 # Temperature of combustion product at exit in K\n",
+ "x1 = 0.114 # Mole fraction of CO2\n",
+ "x2 = .029 # Mole fraction of CO\n",
+ "x3 = .016 # Mole fraction of O2\n",
+ "x4 = .841 # Mole fraction of N2\n",
+ "Wcv = 1 # Power developed by the engine in kW\n",
+ "print \"\\n Example 6.13\\n\"\n",
+ "# By carbon balance \n",
+ "b = 55.9 \n",
+ "# By hydrogen balace\n",
+ "c=9\n",
+ "# By oxygen balance\n",
+ "a = 12.58\n",
+ "Qcv = Wcv- 3845872*(.57/(3600*114.22))\n",
+ "E = 5407843.0 # Chemical exergy of C8H18\n",
+ "nII = Wcv/(E*.57/(3600*114.22))\n",
+ "print \"\\n The rate of heat transfer from the engine = \",Qcv ,\" kW,\\n The second law of efficiency of the engine = \",nII*100 ,\" percent\""
+ ]
+ }
+ ],
+ "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": "2.7.11"
+ }
+ },
+ "nbformat": 4,
+ "nbformat_minor": 0
+}
generated by cgit (git 2.34.1) at 2025-04-01 03:52:26 +0000