{
"cells": [
 {
		   "cell_type": "markdown",
	   "metadata": {},
	   "source": [
       "# Chapter 3: Reactive Systems"
	   ]
	},
{
		   "cell_type": "markdown",
		   "metadata": {},
		   "source": [
			"## Example 3.10: The_enthalpy_of_reaction.sce"
		   ]
		  },
  {
"cell_type": "code",
	   "execution_count": null,
	   "metadata": {
	    "collapsed": true
	   },
	   "outputs": [],
"source": [
"clc\n",
"clear\n",
"//Input data\n",
"T=1500;//The given temperature in K\n",
"\n",
"//Calculations\n",
"hfco=-393.52;//The enthalpy of formation for carbondioxide in MJ/kmol\n",
"hf1=61.714;//The change in enthalpy for actual state and reference state in MJ/kmol\n",
"HP=hfco+hf1;//The total enthalpy in the products side in MJ/kmol\n",
"hfc=-110.52;//The enthalpy of formation for carbonmonoxide in MJ/kmol\n",
"hf2=38.848;//The change in enthalpy of CO for actual and reference state in MJ/kmol\n",
"hfo=0;//The enthalpy of formation for oxygen gas\n",
"hf3=40.61;//The change in enthalpy of oxygen for different states in MJ/kmol\n",
"HR=[hfc+hf2]+[0.5*(hfo+hf3)];//The total enthalpy in the reactants side in MJ/kmol\n",
"H=HP-HR;//The enthalpy of combustion in MJ/kmol \n",
"\n",
"//Output\n",
"printf(' The enthalpy of combustion is  %3.3f MJ/kmol CO ',H)"
   ]
   }
,
{
		   "cell_type": "markdown",
		   "metadata": {},
		   "source": [
			"## Example 3.11: The_heat_transfer.sce"
		   ]
		  },
  {
"cell_type": "code",
	   "execution_count": null,
	   "metadata": {
	    "collapsed": true
	   },
	   "outputs": [],
"source": [
"clc\n",
"clear\n",
"//Input data\n",
"E=30;//The amount of excess air in percentage\n",
"tp=400;//The temperature at which propane enters in K\n",
"ta=300;//The temperature at which air enters in K\n",
"T=900;//The temperature at which products leave in K\n",
"m=83.7;//The average molar specific heat of propane at constant pressure in kJ/kmolK\n",
"Mp=44;//The molecular weight of propane\n",
"\n",
"//Calculations\n",
"hfc=-393.52;//The enthalpy of formation for carbondioxide in MJ/kmol\n",
"hf1=28.041;//The change in enthalpy of CO2 for actual and reference state in MJ/kmol\n",
"hfh=-241.82;//The enthalpy of formation for water in MJ/kmol\n",
"hf2=21.924;//The change in enthalpy of water for actual and reference state in MJ/kmol\n",
"hfn=0;//The enthalpy of nitrogen gas \n",
"hf3=18.221;//The change in enthalpy of nitrgen for actual and reference state in MJ/kmol\n",
"hfo=0;//The enthalpy of oxygen gas \n",
"hf4=19.246;//The change in enthalpy of oxygen for actual and reference state in MJ/kmol\n",
"HP=[3*(hfc+hf1)]+[4*(hfh+hf2)]+[24.44*(hfn+hf3)]+[1.5*(hfo+hf4)];//The total enthalpy in the products side in MJ/kmol\n",
"hfp=-103.85;//The enthalpy of formation for propane in MJ/kmol\n",
"R=0.0837;//Universal gas constant \n",
"hfo1=0;//The enthalpy of oxygen gas \n",
"hf11=0.054;//The change in enthalpy of oxygen gas for actual and reference state in MJ/kmol\n",
"hfn1=0;//The enthalpy of nitrogen gas\n",
"hfn22=0.054;//The change in enthalpy of nitrogen for actual and reference state in MJ/kmol\n",
"HR=[1*(hfp+(R*(tp-ta)))]+[6.5*(hfo1+hf11)]+[24.44*(hfn1+hfn22)];//The total enthalpy on the reactants side in MJ/kmol\n",
"Q=HP-HR;//The amount of heat liberated in MJ/kmol\n",
"Q1=[-Q/Mp];//The amount of heat liberated in MJ/kg\n",
"\n",
"//Output\n",
"printf(' The amount of heat transfer per kg of fuel is  %3.0f MJ/kg',Q1)"
   ]
   }
,
{
		   "cell_type": "markdown",
		   "metadata": {},
		   "source": [
			"## Example 3.12: The_standard_enthalpy.sce"
		   ]
		  },
  {
"cell_type": "code",
	   "execution_count": null,
	   "metadata": {
	    "collapsed": true
	   },
	   "outputs": [],
"source": [
"clc\n",
"clear\n",
"//Input data\n",
"Ta=150;//The presence of Theoretical air\n",
"\n",
"//Calculations\n",
"hfc=-393.52;//The enthalpy of formation for carbondioxide in MJ/kmol\n",
"hfh=-285.8;//The enthalpy of formation for water in MJ/kmol\n",
"hfon=0;//The enthalpy of formation for oxygen and nitrogen gas \n",
"hfch=-74.87;//The enthalpy of formation for methane in MJ/kmol\n",
"HP=[hfc]+[2*hfh];//The total enthalpy on the products side in MJ/kmol\n",
"HR=1*hfch;//The total enthalpy on the reactants side in MJ/kmol\n",
"H=HP-HR;//The total change in enthalpy of reactants and products in MJ/kmol\n",
"np=2;//Number of moles of product\n",
"nr=4;//Number of moles of reactant\n",
"n=np-nr;//The difference in moles\n",
"R=8.314*10^-3;//Universal gas constant \n",
"t=298;//The temperature in K\n",
"U1=H-[n*R*t];//The standard internal energy in MJ/kmol\n",
"hfh1=-241.82;//The enthalpy of formation for water in MJ/kmol\n",
"HP1=[1*hfc]+[2*hfh1];//The total enthalpy on the products side in MJ/kmol\n",
"H1=HP1-HR;//The change in enthalpy for reactants and products in MJ/kmol\n",
"np1=4;//Number of moles of product\n",
"nr1=4;//Number of moles of reactant\n",
"n1=np1-nr1;//The difference in moles\n",
"U2=H1-[n1*R*t];//The standard internal energy in MJ/kmol\n",
"\n",
"//Output\n",
"printf(' (a)The water as liquid , \n    The standard enthalpy of combustion is  %3.2f MJ/kmol \n    The standard internal energy of combustion is  %3.2f MJ/kmol \n (b)The water as a gas , \n    The standard enthalpy of combustion is  %3.2f MJ/kmol \n    The standard internal energy of combustion is  %3.2f MJ/kmol ',H,U1,H1,U2)"
   ]
   }
,
{
		   "cell_type": "markdown",
		   "metadata": {},
		   "source": [
			"## Example 3.13: The_calorific_value.sce"
		   ]
		  },
  {
"cell_type": "code",
	   "execution_count": null,
	   "metadata": {
	    "collapsed": true
	   },
	   "outputs": [],
"source": [
"clc\n",
"clear\n",
"//Input data\n",
"cv=44000;//The lower calorific value of liquid fuel in kJ/kg\n",
"C=84;//The carbon content present in the fuel in percentage\n",
"H=16;//The hydrogen content present in the fuel in percentage\n",
"t=25;//The temperature in degree centigrade\n",
"hfg=2442;//The enthalpy of vaporization for water in kJ/kg\n",
"c=12;//Molecular weight of carbon \n",
"h=2;//Molecular weight of hydrogen\n",
"co2=44;//Molecular weight of carbondioxide\n",
"h2o=18;//Molecular weight of water \n",
"o2=32;//Molecular weight of oxygen\n",
"R=8.314;//Universal gas constant in J/molK\n",
"\n",
"//Calculations\n",
"CO2=[0.84*(co2/c)];//The amount of carbondioxide present per kg of fuel in kg\n",
"H2O=[0.16*(h2o/h)];//The amount of water present per kg of fuel in kg\n",
"cvd=H2O*hfg;//The difference in the higher and lower calorific value in kJ/kg fuel \n",
"HHV=cv+cvd;//The higher calorific value of the liquid fuel in kJ/kg fuel\n",
"np=3.08/co2;//number of moles of product in kmol/kg fuel\n",
"nr=3.52/o2;//The number of moles of reactant in kmol/kg fuel\n",
"n=np-nr;//The difference in the moles\n",
"HHVv=HHV+[n*R*(t+273)];//The higher calorific value at constant volume in kJ/kg fuel\n",
"LHVv=cv+[n*R*(t+273)];//The lower calorific value at constant volume in kJ/kg fuel\n",
"\n",
"//Output\n",
"printf(' The higher calorific value at constant pressure = %3.0f kJ/kg fuel \n The higher calorific value at constant volume = %3.0f kJ/kg fuel \n The lower calorific value at constant volume = %3.0f kJ/kg fuel',HHV,HHVv,LHVv)"
   ]
   }
,
{
		   "cell_type": "markdown",
		   "metadata": {},
		   "source": [
			"## Example 3.14: The_adiabatic_flame_temperature.sce"
		   ]
		  },
  {
"cell_type": "code",
	   "execution_count": null,
	   "metadata": {
	    "collapsed": true
	   },
	   "outputs": [],
"source": [
"clc\n",
"clear\n",
"//Input data\n",
"E=100;//The amount of excess air in percent\n",
"T=298;//The temperature of reactants in K\n",
"nc=1;//Number of moles of propane\n",
"\n",
"//Calculations\n",
"hfch=-103.85;//Enthalpy of formation for propane in MJ/kmol fuel\n",
"HR=nc*hfch;//Total enthalpy on the reactants side in MJ/kmol fuel\n",
"hfc=-393.52;//Enthalpy of formation for carbondioxide in MJ/kmol fuel\n",
"hfh=-241.82;//Enthalpy of formation for water in MJ/kmol fuel\n",
"hfon=0;//Enthalpy of formation for both oxygen and nitrogen gas\n",
"x=HR-[(3*hfc)+(4*hfh)+(5*hfon)+(37.6*hfon)];//For adiabatic combustion enthalpy obtained for equating reactants and products in MJ/kmol fuel\n",
"hfn=x/37.6;//trail to get the change in enthalpy of nitrogen in MJ/kmol\n",
"T1=1500;//Assuming the products temperature for fist trail in K\n",
"hfc1=61.714;//The change in enthalpy for corbondioxide for trail temp in MJ/kmol fuel\n",
"hfh1=48.095;//The change in enthalpy for water for trail temp in MJ/kmol fuel\n",
"hfo1=40.61;//The change in enthalpy for oxygen for trail temp in MJ/kmol fuel\n",
"hfn1=38.405;//The change in enthalpy for nitrogen for trail temp in MJ/kmol fuel\n",
"HP1=(HR-x)+(3*hfc1)+(4*hfh1)+(5*hfo1)+(37.6*hfn1);//Total enthalpy of products for first trail in MJ/kmol fuel\n",
"T2=1600;//Assuming the products temperature for second trail in K\n",
"hfc2=67.58;//The change in enthalpy for corbondioxide for trail temp in MJ/kmol fuel\n",
"hfh2=52.844;//The change in enthalpy for water for trail temp in MJ/kmol fuel\n",
"hfo2=44.279;//The change in enthalpy for oxygen for trail temp in MJ/kmol fuel\n",
"hfn2=41.903;//The change in enthalpy for nitrogen for trail temp in MJ/kmol fuel\n",
"HP2=(HR-x)+(3*hfc2)+(4*hfh2)+(5*hfo2)+(37.6*hfn2);//Total enthalpy of products for second trail in MJ/kmol fuel\n",
"Te=[[(HR-HP1)/(HP2-HP1)]*(T2-T1)]+T1;//The eatimated adiabatic flame temperature in K\n",
"\n",
"//Output\n",
"printf(' The adiabatic flame temperature for steady-flow process is  %3.1f K',Te)"
   ]
   }
,
{
		   "cell_type": "markdown",
		   "metadata": {},
		   "source": [
			"## Example 3.15: The_adiabatic_flame_temperature.sce"
		   ]
		  },
  {
"cell_type": "code",
	   "execution_count": null,
	   "metadata": {
	    "collapsed": true
	   },
	   "outputs": [],
"source": [
"clc\n",
"clear\n",
"//Input data\n",
"T=600;//The initial temperature of air in K\n",
"p=1;//The initial pressure of air in atm\n",
"R=8.314;//Universal gas constant in J/molK\n",
"Tr=298;//The temperature of reactants in K\n",
"a=4.503;//Given Constant \n",
"b=-8.965*10^-3;//Given Constant\n",
"c=37.38*10^-6;//Given Constant\n",
"d=-36.49*10^-9;//Given Constant\n",
"e=12.22*10^-12;//Given Constant\n",
"\n",
"//Calculations\n",
"hfc=-393.52;//Enthalpy of formation for carbondioxide in MJ/kmol fuel\n",
"hfh=-241.82;//Enthalpy of formation for water in MJ/kmol fuel\n",
"hfn=0;//Enthalpy of formation for nitrogen gas\n",
"HP=[1*hfc]+[2*hfh]+[7.52*hfn];//The enthalpy on the products side in MJ/kmol fuel\n",
"hch=[R*[(a*(T-Tr))+((b/2)*(T^2-Tr^2))+((c/3)*(T^3-Tr^3))+((d/4)*(T^4-Tr^4))+((e/5)*(T^5-Tr^5))]]/1000;//The change in enthalpy of the methane in MJ/kmol\n",
"hfc1=-74.87;//The enthalpy of formation for methane in MJ/kmol fuel \n",
"hfh1=9.247;//The change in enthalpy of the water in MJ/kmol\n",
"hfn1=8.891;//The change in enthalpy of nitrogen in MJ/kmol\n",
"HR=[(hfc1+hch)+(2*hfh1)+(7.52*hfn1)];//The enthalpy on the reactants side in MJ/kmol\n",
"x=HR-HP;//The enthalpy for the remaining gases in the product side in MJ/kmol\n",
"hfn2=x/7.52;//The guess enthalpy for the nitrogen gas in MJ/kmol\n",
"Tc=3700;//The corresponding temperature for the enthalpy of guess nitrogen in K\n",
"T1=2800;//The temperature assumed for the first trail in K\n",
"hco1=140.444;//The change in enthalpy for the assume temp for carbondioxide in MJ/kmol\n",
"hh1=115.294;//The change in enthalpy for the assume temp for water in MJ/kmol\n",
"hn1=85.345;//The change in enthalpy for the assume temp for nitrogen in MJ/kmol\n",
"HP1=hco1+(2*hh1)+(7.52*hn1)+(HR-x);//The total enthalpy on the products side for first trail in MJ/kmol fuel\n",
"T2=2500;//The temperature assumed for the second trail in K\n",
"hco2=121.926;//The change in enthalpy for the assume temp for carbondioxide in MJ/kmol\n",
"hh2=98.964;//The change in enthalpy for the assume temp for water in MJ/kmol\n",
"hn2=74.312;//;//The change in enthalpy for the assume temp for nitrogen in MJ/kmol\n",
"HP2=hco2+(2*hh2)+(7.52*hn2)+(HR-x);//The total enthalpy on the products side for the second trail in MJ/kmol\n",
"T3=2600;//The temperature fo the third trail in K\n",
"hco3=128.085;//The change in enthalpy for the assume temp for carbondioxide in MJ/kmol\n",
"hh3=104.37;//The change in enthalpy for the assume temp for water in MJ/kmol\n",
"hn3=77.973;//The change in enthalpy for the assume temp for nitrogen in MJ/kmol\n",
"HP3=hco3+(2*hh3)+(7.52*hn3)+(HR-x);//The total enthalpy on the products side for the third trail in MJ/kmol\n",
"Ta1=[[(HR-HP2)/(HP3-HP2)]*(T3-T2)]+T2;//The adiabatic temperature for constant pressure process in K\n",
"UR1=HR-(10.52*R*10^-3*T);//The internal energy of reactant in MJ/kmol fuel\n",
"Tc1=3000;//Assume temperature for first trail in K\n",
"hcoa1=146.645;//The change in enthalpy for the assume temp for carbondioxide in MJ/kmol\n",
"hha1=120.813;//The change in enthalpy for the assume temp for carbondioxide in MJ/kmol\n",
"hna1=89.036;//The change in enthalpy for the assume temp for nitrogen in MJ/kmol\n",
"UP1=hcoa1+(2*hha1)+(7.52*hna1)+(HR-x)-(0.08746*Tc1);//The internal energy of products in MJ/kmol fuel\n",
"Tc2=3200;//Assume temperature for the second trail in K\n",
"hcoa2=165.331;//;//The change in enthalpy for the assume temp for carbondioxide in MJ/kmol\n",
"hha2=137.553;//The change in enthalpy for the assume temp for water in MJ/kmol\n",
"hna2=100.161;//The change in enthalpy for the assume temp for nitrogen in MJ/kmol\n",
"UP2=hcoa2+(2*hha2)+(7.52*hna2)+(HR-x)-(0.08746*Tc2);//The internal energy of products in MJ/kmol fuel\n",
"Tu=[[(UR1-UP1)/(UP2-UP1)]*(Tc2-Tc1)]+Tc1;//The adiabatic flame temperature at constant pressure process in K\n",
"\n",
"//Output\n",
"printf('The adiabatic flame temperature at  \n    (a)Constant pressure process is %3.0f K \n    (b)Constant volume process is %3.1f K',Ta1,Tu)\n",
"\n",
"\n",
""
   ]
   }
,
{
		   "cell_type": "markdown",
		   "metadata": {},
		   "source": [
			"## Example 3.16: The_adiabatic_flame_temperature.sce"
		   ]
		  },
  {
"cell_type": "code",
	   "execution_count": null,
	   "metadata": {
	    "collapsed": true
	   },
	   "outputs": [],
"source": [
"clc\n",
"clear\n",
"//Input data\n",
"T=600;//Temperature at constant pressure process in K\n",
"p=1;//The pressure in atm\n",
"E=50;//The amount of excess air in percent\n",
"L=20;//The amount of less air in percent\n",
"cp=52.234;//Specific constant for methane in kJ/kmolK\n",
"T1=298;//Assume the normal temperature in K\n",
"\n",
"//Calculations\n",
"hfch=-74.87;//The enthalpy of formation for carbondioxide in MJ\n",
"hch=cp*(T-T1)*10^-3;//The change in enthalpy of carbondioxide in MJ\n",
"ho=9.247;//The change in enthalpy of oxygen in MJ\n",
"hn=8.891;//The change in enthalpy of nitrogen in MJ\n",
"HR=hfch+hch+(3*ho)+(11.28*hn);//The total enthalpy on the reactants side in MJ\n",
"hfc1=-393.52;//The enthalpy of formation of carbondioxide in MJ\n",
"hfh1=-241.82;//The enthalpy of formation of water in MJ\n",
"HP=hfc1+(2*hfh1);//The enthalpy of products side in MJ\n",
"x=HR-HP;//The change in enthalpy for the remaining in MJ\n",
"hn2=x/11.28;//The enthalpy of nitrogen assumed to be in MJ/kmol\n",
"Tc=2800;//The corresponding temperature in K\n",
"T1=2000;//The temperature for first trail in K\n",
"hfc11=91.45;//The enthalpy for the assume temp for carbondioxide in MJ\n",
"hfh11=72.689;//The change in enthalpy for the assume temp for water in MJ\n",
"hfn11=56.141;//The change in enthalpy for the assume temp for nitrogen in MJ\n",
"hfo11=59.199;//;//The change in enthalpy for the assume temp for oxygen in MJ\n",
"HP1=hfc11+(2*hfh11)+(11.28*hfn11)+(hfo11)+(HR-x);//The total enthalpy on the products side for first trail in MJ\n",
"T2=2100;//The temperature for second trail in K\n",
"hfc22=97.5;//The enthalpy for the assume temp for carbondioxide in MJ\n",
"hfh22=77.831;//The change in enthalpy for the assume temp for water in MJ\n",
"hfn22=59.748;//The change in enthalpy for the assume temp for nitrogen in MJ\n",
"hfo22=62.986;//;//The change in enthalpy for the assume temp for oxygen in MJ\n",
"HP2=hfc22+(2*hfh22)+(11.28*hfn22)+(hfo22)+(HR-x);//The total enthalpy on the products side for second trail in MJ\n",
"Ta1=[[(HR-HP1)/(HP2-HP1)]*(T2-T1)]+T1;//The adiabatic temperature for constant pressure process in K\n",
"X=2*[2-1.6];//By balance oxygen\n",
"hfchr=-74.87;//The enthalpy of formation for methane in MJ\n",
"hor=9.247;//The change in enthalpy for oxygen in MJ\n",
"hnr=8.891;//The change in enthalpy for nitrogen in MJ\n",
"HRr=hfchr+hch+(1.6*hor)+(6.01*hnr);//The total enthalpy on reactants side in MJ\n",
"hfcop=-110.52;//The formation of enthalpy for carbonmoxide in MJ\n",
"hfcp=-393.52;//The formation of enthalpy for carbondioxide in MJ\n",
"hfhp=-241.82;//The formation of enthalpy for water in MJ\n",
"HPp=(0.8*hfcop)+(0.2*hfcp)+(2*hfhp);//The enthalpy on product side in MJ\n",
"Tp1=2000;//The temperature for first trail in K\n",
"hco11=56.739;//The change in enthalpy for CO in MJ\n",
"hco211=91.45;//The change in enthalpy for CO2 in MJ\n",
"hh11=72.689;//The change in enthalpy for water in MJ\n",
"hn11=56.141;//The change in enthalpy for nitrogen in MJ\n",
"HPp1=(0.8*hco11)+(0.2*hco211)+(2*hh11)+(6.016*hn11)-HPp;///The enthalpy on the products side for trail temp in MJ\n",
"Tp2=2400;//The temperature for second trail in K\n",
"hco22=71.34;//The change in enthalpy for CO in MJ\n",
"hco222=115.788;//The change in enthalpy for CO2 in MJ\n",
"hh22=93.604;//The change in enthalpy for water in MJ\n",
"hn22=70.651;//The change in enthalpy for nitrogen in MJ\n",
"HPp2=(0.8*hco22)+(0.2*hco222)+(2*hh22)+(6.016*hn22)+HPp;///The enthalpy on the products side for trail temp in MJ\n",
"Tp3=2300;//The temperature for first trail in K\n",
"hco33=67.676;//The change in enthalpy for CO in MJ\n",
"hco233=109.671;//The change in enthalpy for CO2 in MJ\n",
"hh33=88.295;//The change in enthalpy for water in MJ\n",
"hn33=67.007;//The change in enthalpy for nitrogen in MJ\n",
"HPp3=(0.8*hco33)+(0.2*hco233)+(2*hh33)+(6.016*hn33)+HPp;///The enthalpy on the products side for trail temp in MJ\n",
"Ta2=[[(HRr-HPp3)/(HPp2-HPp3)]*(Tp2-Tp3)]+Tp3;//The adiabatic temperature for constant pressure process in K\n",
"hccc=-283.022;//The only combustible substance is CO in MJ/kmol\n",
"Q=-0.8*hccc;//The thermal energy loss in MJ/kmol fuel\n",
"\n",
"//Output\n",
"printf(' The adiabatic flame temperature having \n    (a)50 percent excess air is %3.1f K \n    (b)20 percent less air is %3.1f K \n The loss of thermal energy due to incomplete combustion is %3.1f MJ/kmol fuel',Ta1,Ta2,Q)"
   ]
   }
,
{
		   "cell_type": "markdown",
		   "metadata": {},
		   "source": [
			"## Example 3.18: Dissociation_of_carbondioxide.sce"
		   ]
		  },
  {
"cell_type": "code",
	   "execution_count": null,
	   "metadata": {
	    "collapsed": true
	   },
	   "outputs": [],
"source": [
"clc\n",
"clear\n",
"//Input data\n",
"T1=3000;//Given temperature in K\n",
"T2=4000;//Given temperature in K\n",
"p=1;//The pressure in atm\n",
"KP1=1.117;//Natural logarithm of equilibrium constant at 3000 K \n",
"KP2=-1.593;//Natural logarithm of equilibrium constant at 4000 K\n",
"\n",
"//Calculations\n",
"Kp1=exp(KP1);//The value of equilibrium constant at 3000 K\n",
"Kp2=exp(KP2);//The value of equilibrium constant at 4000 K\n",
"a1=0.4;//The dissociation of 1 mole of CO2 for the first trail\n",
"a2=0.5;//The dissociation of 1 mole of CO2 for the second trail \n",
"K1=3.674;//The value of equilibrium constant for the first trail \n",
"K2=2.236;//The value of equilibrium constant for the second trail\n",
"a12=[[(K1-Kp1)/(K1-K2)]*(a2-a1)]+a1;//The approximate dissociation of 1 mole of CO2\n",
"A12=a12*100;//The amount of CO2 will dissociate in percent\n",
"a3=0.9;//The dissociation of 1 mole of CO2 for the first trail\n",
"a4=0.89;//The dissociation of 1 mole of CO2 for the second trail\n",
"K3=0.1995;//The value of equilibrium constant for the first trail \n",
"K4=0.2227;//The value of equilibrium constant for the second trail \n",
"a23=[[(Kp2-K4)/(K3-K4)]*(a3-a4)]+a4;//The approximate dissociation of 1 mole of CO2\n",
"A23=a23*100;//The amount of CO2 will dissociate in percent\n",
"\n",
"//output\n",
"printf('The percent dissociation of carbondioxide into carbonmonoxide and oxygen at \n    (a) at 3000 K and 1 atm pressure = %3.1f percent \n    (b) at 4000 K and 1 atm pressure = %3.2f percent ',A12,A23)"
   ]
   }
,
{
		   "cell_type": "markdown",
		   "metadata": {},
		   "source": [
			"## Example 3.19: The_mole_fractio.sce"
		   ]
		  },
  {
"cell_type": "code",
	   "execution_count": null,
	   "metadata": {
	    "collapsed": true
	   },
	   "outputs": [],
"source": [
"clc\n",
"clear\n",
"//Input data\n",
"p=1;//Initial pressure in atm\n",
"T=300;//Initial temperature in K\n",
"Tc=2400;//To calculate the molefraction of the products at this temperature in K\n",
"KP1=3.866;//Natural logarithm of equilibrium constant at 2400 K for the equation \n",
"\n",
"//Calculations\n",
"K1=exp(KP1);//The value of equilibrium constant at 2400 K\n",
"nr=1+0.5;//The number of moles of reactants\n",
"Pp=(p*Tc)/(nr*T);//Pressure exercted on the products side per mole in atm/mole\n",
"a=0.098;//The dissociation of 1 mole of CO2\n",
"np=(a+2)/2;//The number of moles of products\n",
"xco=[2*(1-a)]/(2+a);//Mole fraction of CO2\n",
"xc=[2*a]/(2+a);//Mole fraction of CO\n",
"xo=a/(2+a);//Mole fraction of O2\n",
"PP=5.333*np;//Pressure of the product in bar\n",
"\n",
"//output\n",
"printf('Mole fraction of the carbondioxide is %3.4f \n Mole fraction of the carbonmonoxide is %3.4f \n Mole fraction of oxygen is %3.4f \n Pressure of the product is %3.3f bar',xco,xc,xo,PP)"
   ]
   }
,
{
		   "cell_type": "markdown",
		   "metadata": {},
		   "source": [
			"## Example 3.1: Volume_of_air.sce"
		   ]
		  },
  {
"cell_type": "code",
	   "execution_count": null,
	   "metadata": {
	    "collapsed": true
	   },
	   "outputs": [],
"source": [
"clc\n",
"clear\n",
"//Input data\n",
"E=20;//Methanol burned with excess air in percentage \n",
"p=1;//Pressure of air in bar\n",
"t=27;//Temperature of air in degree centigrade\n",
"O=32;//The molecular weight of oxygen\n",
"N=28;//The molecular weight of nitrogen\n",
"R=8314;//Universal gas constant in Nm/kmolK\n",
"C=32;//Molecular weight of methanol\n",
"CO=44;//Molecular weight of the carbondioxide \n",
"H=18;//Molecular weight of the water\n",
"\n",
"//Calculations\n",
"S=[(1.8*O)+(6.768*N)]/C;//Stoichiometric air/fuel ratio\n",
"A=[(1.8*O)+(6.768*N)]/C;//Actual air/fuel ratio\n",
"M=1.8+6.768;//1 kmole of fuel reacts with air in kmole\n",
"V=(M*R*(t+273))/(p*10^5);//Volume of air in m^3/kmole fuel\n",
"T=(1+1.8+6.768);//The total number of moles in the reactants when excess air is supplied in moles\n",
"Cm=(1/T);//Mole fraction of the methanol\n",
"Om=(1.8/T);//Mole fraction of the oxygen\n",
"Nm=(6.768/T);//Mole fraction of the nitrogen\n",
"Mr=(Cm*C)+(Om*O)+(Nm*N);//Molecular weight of reactants \n",
"Tp=(1+2+6.768+0.3);//Total number of moles in the products in moles\n",
"COm=(1/Tp);//Mole fraction of the carbondioxide\n",
"Hp=(2/Tp);//Mole fraction of the water \n",
"Np=(6.768/Tp);//Mole fraction of the nitrogen\n",
"Op=(0.3/Tp);//Mole fraction of the oxygen\n",
"Mp=(COm*CO)+(Hp*H)+(Np*N)+(Op*O);//Molecular weight of products\n",
"Pp=(Hp*p);//Partial pressure of water vapour in bar\n",
"D=60;//The dew point is the saturation temp corresponding to partial pressure in degree centigrade\n",
"\n",
"//Output\n",
"printf(' (a) The volume of air supplied per kmole of fuel = %3.1f m^3/kmole fuel \n (b) The molecular weight of the reactants = %3.2f \n The molecular weight of the products = %3.2f \n (c) The dew point of the products = %3.0f degree centigrade ',V,Mr,Mp,D)"
   ]
   }
,
{
		   "cell_type": "markdown",
		   "metadata": {},
		   "source": [
			"## Example 3.20: The_adiabatic_flame_temperature.sce"
		   ]
		  },
  {
"cell_type": "code",
	   "execution_count": null,
	   "metadata": {
	    "collapsed": true
	   },
	   "outputs": [],
"source": [
"clc\n",
"clear\n",
"//Input data\n",
"t=25;//The temperature of air in degree centigrade\n",
"p=1;//The pressure of air in atm\n",
"T1=2200;//Given first temperature in K\n",
"T2=2400;//Given second temperature in K\n",
"h1=59.86;//The change in enthalpy of hydrogen at 2200 K in MJ/kmol\n",
"h2=66.915;//The change in enthalpy of hydrogen at 2400 K in MJ/kmol\n",
"T=298;//The temperature of air in K\n",
"\n",
"//Calculations\n",
"HR=0;//The total enthalpy on the reactants side since all the reactants are elements\n",
"Kp1=-6.774;//Natural logarithm of equilibrium constant at 2200 K for the equation \n",
"K1=exp(Kp1);//The value of equilibrium constant at 2200 K\n",
"a1=0.02;//By trail and error method the degree of dissociation of H2O\n",
"hfh=-241.82;//The enthalpy of formation of water at both 2200 and 2400 K in MJ/kmol\n",
"hfh1=83.036;//The change in enthalpy of water at 2200 K in MJ/kmol\n",
"hfd1=59.86;//The change in enthalpy of hydrogen at 2200 K in MJ/kmol\n",
"hfo1=66.802;//The change in enthalpy of oxygen at 2200 K in MJ/kmol\n",
"hfn1=63.371;//The change in enthalpy of nitrogen at 2200 K in MJ/kmol\n",
"HP1=(0.98*(hfh+hfh1))+(0.02*hfd1)+(0.01*hfo1)+(1.88*hfn1);//The enthalpy on the products side in MJ/kmol \n",
"a2=0.04;//By trail and error method the degree of dissociation of H2O at 2400 K\n",
"hfh2=93.604;//The change in enthalpy of water at 2400 K in MJ/kmol\n",
"hfd2=66.915;//The change in enthalpy of hydrogen at 2400 K in MJ/kmol\n",
"hfo2=74.492;//The change in enthalpy of oxygen at 2400 K in MJ/kmol\n",
"hfn2=70.651;//The change in enthalpy of nitrogen at 2400 K in MJ/kmol\n",
"HP2=(0.96*(hfh+hfh2))+(0.04*hfd2)+(0.02*hfo2)+(1.88*hfn2);//The enthalpy on the products side in MJ/kmol \n",
"H1=HP1-HR;//The total change in enthalpy at 2200 K in MJ/kmol\n",
"H2=HP2-HR;//The total change in enthalpy at 2400 K in MJ/kmol\n",
"Tl=[[[T2-T1]/[HP2-HP1]]*[HR-HP1]]+T1;//The required temperature in K\n",
"\n",
"//Output\n",
"printf('The adiabatic flame temperature taking dissociation into account is %3.0f K',Tl)"
   ]
   }
,
{
		   "cell_type": "markdown",
		   "metadata": {},
		   "source": [
			"## Example 3.2: Mass_of_exhaust_gases.sce"
		   ]
		  },
  {
"cell_type": "code",
	   "execution_count": null,
	   "metadata": {
	    "collapsed": true
	   },
	   "outputs": [],
"source": [
"clc\n",
"clear\n",
"//Input data\n",
"C1=40;//The content of C7H16 in the fuel in percentage\n",
"C2=60;//The content of C8H18 in the fuel in percentage\n",
"d=0.12;//The diameter of the bore in m\n",
"l=0.145;//The length of the bore in m\n",
"r=8.5;//Compression ratio \n",
"p=1.1;//Pressure at exhaust stroke in bar\n",
"T=720;//The temperature at the exhaust stroke in K\n",
"pi=3.141;//Mathematical constant pi\n",
"O=32;//The molecular weight of oxygen\n",
"N=28;//The molecular weight of nitrogen\n",
"C3=100;//Molecular weight of C7H16\n",
"C4=114;//The molecular weight of C8H18\n",
"R=8314;//Universal gas constant in Nm/kmolK\n",
"CO2=44;//Molecular weight of the carbondioxide \n",
"C5=28;//Molecular weight of the carbonmonoxide\n",
"H=18;//Molecular weight of the water\n",
"\n",
"//Calculations\n",
"N2=100-(12+1.5+2.5);//Percentage of nitrogen in the dry products of combustion\n",
"Y=84/3.76;//The number of moles oxygen is supplied\n",
"X=13.5/7.6;//Moles of carbon\n",
"Z=(22.34-15.25)*2;//The number of moles of hydrogen\n",
"Hl=(6.4+10.8)/2;//Number of moles of hydrogen on L.H.S\n",
"Hr=7.98;//Number of moles of hydrogen on R.H.S\n",
"Hd=Hl-Hr;//Difference of hydrogen moles\n",
"A=[[12.58*(O+(3.76*N))]/[((C1/100)*C3)+((C2/100)*C4)]];//The Air/fuel ratio\n",
"Vs=(pi/4)*d^2*l;//Swept volume of the cylinder in m^3\n",
"Vc=Vs/(r-1);//Clearance volume in m^3\n",
"M=[(6.757*CO2)+(0.8446*C5)+(1.408*O)+(47.3*N)+(8.6*H)]/[6.757+0.8446+1.408+47.3+8.6];//Molecular weight of the product\n",
"R1=R/M;//Gas constant in J/kgK\n",
"m=[(p*10^5)*Vc]/[R1*T];//Mass of the exhaust gases in the clearance space in kg\n",
"\n",
"//Output \n",
"printf('(a)The air/fuel ratio =%3.2f \n (b)The mass of the exhaust gases in the clearance space =%3.7f kg ',A,m)"
   ]
   }
,
{
		   "cell_type": "markdown",
		   "metadata": {},
		   "source": [
			"## Example 3.3: Volumetric_analysis.sce"
		   ]
		  },
  {
"cell_type": "code",
	   "execution_count": null,
	   "metadata": {
	    "collapsed": true
	   },
	   "outputs": [],
"source": [
"clc\n",
"clear\n",
"//Input data\n",
"C=0.86;//The amount of carbon content in the 1kg of fuel by weight in kg\n",
"H=0.05;//The amount of hydrogen content in the 1kg of fuel by weight in kg\n",
"O=0.02;//The amount of oxygen content in the 1kg of fuel by weight in kg\n",
"S=0.005;//The amount of sulphur content in the 1kg of fuel by weight in kg\n",
"N=0.065;//The amount of nitrogen content in the 1kg of fuel by weight in kg\n",
"E=25;//The amount of excess air supplied in percentage\n",
"o=32;//Molecular weight of the oxygen\n",
"co=44;//Molecular weight of the carbondioxide \n",
"c=12;//Molecular weight of the carbon\n",
"s=32;//Molecular weight of the sulphur\n",
"so=64;//Molecular weight of sulphur dioxide\n",
"n=28;//Molecular weight of the nitrogen\n",
"\n",
"//Calculations\n",
"o1=(o/c)*C;//The amount of oxygen required for 0.86 kg of carbon in kg\n",
"coa=(co/c)*C;//The amount of carbondioxide produced for 0.86 kg of carbon in kg\n",
"o2=(o/4)*H;//The amount of oxygen required for 0.05 kg of hydrogen in kg\n",
"h2=(36/4)*H;//The amount of water produced for 0.05 kg of hydrogen in kg\n",
"o3=(o/s)*S;//The amount of oxygen required for 0.005 kg of sulphur in kg\n",
"s1=(so/s)*S;//The amount of sulphur dioxide produced for 0.005 kg of sulphur in kg\n",
"To=o1+o2+o3;//Total oxygen required for the complete combustion of fuel in kg\n",
"Tt=To-O;//The amount of oxygen required per kg of fuel for complete combustion theoretically in kg\n",
"As=(Tt*100)/23;//Stoichiometric air/fuel ratio\n",
"as=As*(1+(E/100));//The actual quantity of air supplied per kg of fuel in kg\n",
"o2a=0.23*(E/100)*As;//The oxygen in the excess air in kg\n",
"n2a=0.77*(1+(E/100))*As;//The nitrogen in the air in kg\n",
"n2e=n2a+N;//Total nitrogen in the exhaust in kg\n",
"Tw=coa+n2e+o2a;//Total weight in kg\n",
"pco=(coa/Tw)*100;//Percentage composition of carbondioxide\n",
"pn=(n2e/Tw)*100;//Percentage composition of nitrogen\n",
"po=(o2a/Tw)*100;//Percentage composition of oxygen\n",
"mco=(coa/co);//Moles of carbondioxide\n",
"mn=(n2e/n);//Moles of nitrogen\n",
"mo=(o2a/o);//Moles of oxygen\n",
"Tm=mco+mn+mo;//Total moles\n",
"vco=(mco/Tm)*100;//Volumetric analysis of carbondioxide in percentage\n",
"vn=(mn/Tm)*100;//Volumetric analysis of nitrogen in percentage\n",
"vo=(mo/Tm)*100;//Volumetric analysis of oxygen in percentage\n",
"\n",
"//Output\n",
"printf(' (a)Stoichiometric air/fuel ratio = %3.2f \n (b)The percentage of dry products of combustion by weight : \n   CO2 = %3.2f percent \n   N2 = %3.2f percent \n   O2 = %3.2f percent \n (c)The percentage of dry products of combustion by volume : \n   CO2 = %3.2f percent \n   N2 = %3.2f percent \n   O2= %3.2f percent ',As,pco,pn,po,vco,vn,vo)"
   ]
   }
,
{
		   "cell_type": "markdown",
		   "metadata": {},
		   "source": [
			"## Example 3.4: Fuel_consumption.sce"
		   ]
		  },
  {
"cell_type": "code",
	   "execution_count": null,
	   "metadata": {
	    "collapsed": true
	   },
	   "outputs": [],
"source": [
"clc\n",
"clear\n",
"//Input data\n",
"CO=12;//The composition of carbondioxide of combustion by volume in percentage \n",
"C=0.5;//The composition of carbonmoxide of combustion by volume in percentage \n",
"O=4;//The composition of oxygen of combustion by volume in percentage \n",
"N=83.5;//The composition of nitrogen of combustion by volume in percentage \n",
"o=32;//Molecular weight of the oxygen\n",
"co=44;//Molecular weight of the carbondioxide \n",
"c=12;//Molecular weight of the carbon\n",
"s=32;//Molecular weight of the sulphur\n",
"so=64;//Molecular weight of sulphur dioxide\n",
"n1=28;//Molecular weight of the nitrogen\n",
"h=2;//Molecular weight of the hydrogen\n",
"\n",
"//Calculations\n",
"m=12+0.5;//Balancing carbon\n",
"x=N/3.76;//Balancing nitrogen\n",
"z=[x-(CO+(C/2)+O)]*2;//Balancing oxygen\n",
"n=z*h;//Balancing hydrogen\n",
"Af=[(x*o)+(N*n1)]/[(m*c)+(n)];//Air/fuel ratio\n",
"As=[(18.46*o)+(69.41*n1)]/173.84;//Stoichiometric air/fuel ratio\n",
"Ta=(Af/As)*100;//Percent theoretical air\n",
"mc=[(m*c)/173.84]*100;//Composition of carbon on mass basis in percent\n",
"mh=(n/173.84)*100;//Composition of hydrogen on mass basis in percent\n",
"\n",
"//Output\n",
"printf(' (a)The air/fuel ratio = %3.2f \n (b)The percent theoretical air = %3.1f percent \n (c)The percentage composition of fuel on a mass basis : \n   C = %3.1f percent \n   H = %3.1f percent ',Af,Ta,mc,mh)"
   ]
   }
,
{
		   "cell_type": "markdown",
		   "metadata": {},
		   "source": [
			"## Example 3.5: Percentage_analysis.sce"
		   ]
		  },
  {
"cell_type": "code",
	   "execution_count": null,
	   "metadata": {
	    "collapsed": true
	   },
	   "outputs": [],
"source": [
"clc\n",
"clear\n",
"//Input data\n",
"C=86;//The composition of carbon in the fuel by weight in percentage\n",
"H=14;//The composition of hydrogen in the fuel by weight in percentage\n",
"e=1.25;//Equivalent ratio\n",
"o=32;//Molecular weight of the oxygen\n",
"co=44;//Molecular weight of the carbondioxide \n",
"c=12;//Molecular weight of the carbon\n",
"s=32;//Molecular weight of the sulphur\n",
"so=64;//Molecular weight of sulphur dioxide\n",
"n=28;//Molecular weight of the nitrogen\n",
"h2=2;//Molecular weight of the hydrogen\n",
"Fc=0.86;//Fraction of C\n",
"\n",
"//Calculations\n",
"Ra=1/Fc;//Relative air/fuel ratio\n",
"x=2*[1+(0.9765/2)-(1.488*0.8)];//By oxygen balance\n",
"Tm=0.5957+0.4043+4.476;//Total number of moles of dry exhaust gas\n",
"vc=(0.5957/Tm)*100;//Volumetric analysis of carbonmonoxide of combustion in percentage\n",
"vco=(0.4043/Tm)*100;//Volumetric analysis of carbondioxide of combustion in percentage\n",
"vn=(4.476/Tm)*100;//Volumetric analysis of nitrogen of combustion in percentage\n",
"\n",
"//Calculations\n",
"printf(' The percentage analysis of dry exhaust gas by volume : \n    CO = %3.2f percent \n    CO2 = %3.2f percent \n    N2 = %3.2f percent ',vc,vco,vn)"
   ]
   }
,
{
		   "cell_type": "markdown",
		   "metadata": {},
		   "source": [
			"## Example 3.6: Heat_transfer.sce"
		   ]
		  },
  {
"cell_type": "code",
	   "execution_count": null,
	   "metadata": {
	    "collapsed": true
	   },
	   "outputs": [],
"source": [
"clc\n",
"clear\n",
"//Input data\n",
"t=25;//The temperature of both reactants and products in degree centigrade\n",
"p=1;//The pressure of both reactants and products in bar\n",
"\n",
"//Calculations \n",
"h=0;//Enthalpy of all elements at given temp and pressure \n",
"hf1=-103.85;//The enthalpy of the compound C3H8 in the reactants side at given temp and pressure in MJ/kmol\n",
"hf2=-393.52;//The enthalpy of carbondioxide for the given temp and pressure in MJ/kmol\n",
"hf3=-285.8;//The enthalpy of the water for the given temp and pressure in MJ/kmol\n",
"hf4=[3*hf2]+[4*hf3];//Total enthalpy in the products side in MJ/kmol\n",
"Q=hf4-hf1;//The heat transfer per mole of fuel in MJ/kmol fuel\n",
"\n",
"//Output\n",
"printf(' The heat transfer per mole of fuel = %3.2f kJ/mol fuel',Q)"
   ]
   }
,
{
		   "cell_type": "markdown",
		   "metadata": {},
		   "source": [
			"## Example 3.7: The_work_for_a_fuel_rate.sce"
		   ]
		  },
  {
"cell_type": "code",
	   "execution_count": null,
	   "metadata": {
	    "collapsed": true
	   },
	   "outputs": [],
"source": [
"clc\n",
"clear\n",
"//Input data\n",
"t=25;//The temperature of the air entering the diesel engine in degree centigrade \n",
"T=600;//The temperature at which the products are released in K\n",
"Ta=200;//Theoretical air used in percentage \n",
"Q=-93;//Heat loss from the engine in MJ/kmol fuel\n",
"f=1;//The fuel rate in kmol/h\n",
"\n",
"//Calculations \n",
"hfr=-290.97;//The enthalpy of C12H26 for the given conditions in the reactants side in MJ/kmol\n",
"h1=-393.52;//Enthalpy of carbondioxide at formation state in MJ/kmol\n",
"h11=12.916;//The change in enthalpy for the given temp of CO2 in MJ/kmol\n",
"hfc=h1+h11;//The enthalpy of the carbondioxide in MJ/kmol\n",
"h2=-241.82;//The enthalpy of water at formation state in MJ/kmol\n",
"h22=10.498;//The change in enthalpy for the given temp of water in MJ/kmol\n",
"hfh=h2+h22;//The enthalpy of the water in MJ/kmol\n",
"h3=0;//Enthalpy of the oxygen gas \n",
"h33=9.247;//The change in enthalpy for the given temp of oxygen in MJ/kmol\n",
"hfo=h3+h33;//The enthalpy of oxygen in MJ/kmol\n",
"h4=0;//The enthalpy of the nitrogen gas\n",
"h44=8.891;//The change in enthalpy of the nitrogen for the given temp in MJ/kmol\n",
"hfn=h4+h44;//The enthalpy of nitrogen in MJ/kmol\n",
"hfp=(12*hfc)+(13*hfh)+(18.5*hfo)+(139.12*hfn);//The total enthalpy on the products side in MJ/kmol\n",
"W=Q+hfr-hfp;//The work in MJ/kmol fuel\n",
"W1=(f*W*10^3)/3600;//The work in kW\n",
"\n",
"//Output\n",
"printf('The work for a fuel rate of 1 kmol/h is %3.1f kW',W1)"
   ]
   }
,
{
		   "cell_type": "markdown",
		   "metadata": {},
		   "source": [
			"## Example 3.8: The_fuel_consumption.sce"
		   ]
		  },
  {
"cell_type": "code",
	   "execution_count": null,
	   "metadata": {
	    "collapsed": true
	   },
	   "outputs": [],
"source": [
"clc\n",
"clear\n",
"//Input data\n",
"P=600;//Power of an engine in kW\n",
"t=25;//Temperature at which fuel is used in degree centigrade\n",
"Ta=150;//Theoretical air used in percentage\n",
"T1=400;//The temperature at which air enters in K\n",
"T2=700;//The temperature at which the products of combustion leave in K\n",
"Q=-150;//The heat loss from the engine in kW\n",
"C=12;//Molecular weight of carbon\n",
"h=1;//Molecular weight of hydrogen\n",
"\n",
"//Calculations\n",
"hfc=-259.28;//The enthalpy of the compound C8H18 for the given conditions in MJ/kmol fuel\n",
"hfo1=3.029;//The enthalpy of the oxygen gas in MJ/kmol fuel\n",
"hfn1=2.971;//The enthalpy of the nitrogen gas in MJ/kmol fuel\n",
"HR=(hfc)+(1.5*12.5*hfo1)+(1.5*12.5*3.76*hfn1);//The total enthalpy on the reactants side in MJ/kmol fuel\n",
"hfco=-393.52;//The enthalpy of carbondioxide for formation state in MJ/kmol fuel\n",
"hfco1=17.761;//The change in enthalpy of the carbondioxide for temp difference in MJ/kmol fuel\n",
"hfh=-241.82;//The enthalpy of water for formation state in MJ/kmol fuel\n",
"hfh1=14.184;//The change in the enthalpy of the water for temp difference in MJ/kmol fuel\n",
"hfo2=12.502;//The enthalpy of the oxygen gas in MJ/kmol fuel\n",
"hfn2=11.937;//The enthalpy of the nitrogen gas in MJ/kmol fuel\n",
"HP=(8*(hfco+hfco1))+(9*(hfh+hfh1))+(6.25*hfo2)+(70.5*hfn2);//The total enthalpy on the products side in MJ/kmol fuel\n",
"H=HP-HR;//The total change in enthalpy of reactants and products in MJ/kmol fuel\n",
"nf=([Q-P]*3600)/[H*10^3];//The fuel rate in kmol/s\n",
"M=(8*C)+(18*h);//Molecular weight of fuel \n",
"mf=nf*M;//The fuel consumption in kg/h\n",
"\n",
"//Output\n",
"printf(' The fuel consumption for complete combustion is %3.2f kg/h',mf)"
   ]
   }
,
{
		   "cell_type": "markdown",
		   "metadata": {},
		   "source": [
			"## Example 3.9: The_heat_transfer.sce"
		   ]
		  },
  {
"cell_type": "code",
	   "execution_count": null,
	   "metadata": {
	    "collapsed": true
	   },
	   "outputs": [],
"source": [
"clc\n",
"clear\n",
"//Input data\n",
"t=25;//Temperature at which fuel is used for combustion in degree centigrade \n",
"p=1;//The pressure at which fuel is used in bar\n",
"T=400;//The temperature of the products of combustion in K\n",
"R=8.314*10^-3;//Universal gas constant\n",
"\n",
"//Calculations\n",
"hfc=-103.85;//Enthalpy of the compound C3H8 in MJ/kmol fuel \n",
"HR=[1*(hfc-(R*(t+273)))]+[5*(-R*(t+273))];//The total enthalpy of the reactants in MJ/kmol fuel\n",
"hfco=-393.52;//The enthalpy of the carbondioxide in MJ/kmol fuel\n",
"hfco1=4.008;//The change in enthalpy of the carbondioxide for the given conditions in MJ/kmol fuel\n",
"hfh=-241.82;//The enthalpy of the water in MJ/kmol fuel\n",
"hfh1=3.452;//The change in enthalpy of the water for the given conditions in MJ/kmol fuel\n",
"HP=[3*(hfco+hfco1-(R*T))]+[4*(hfh+hfh1-(R*T))];//The total enthalpy of the products in MJ/kmol fuel\n",
"Q=HP-HR;//The total change in the enthalpy of reactans and products in MJ/kmol fuel\n",
"Q1=-Q;//Heat liberated in kJ/mol propane\n",
"\n",
"//Output\n",
"printf('The heat transfer per mole of propane = %3.1f kJ/mol propane',Q1)"
   ]
   }
],
"metadata": {
		  "kernelspec": {
		   "display_name": "Scilab",
		   "language": "scilab",
		   "name": "scilab"
		  },
		  "language_info": {
		   "file_extension": ".sce",
		   "help_links": [
			{
			 "text": "MetaKernel Magics",
			 "url": "https://github.com/calysto/metakernel/blob/master/metakernel/magics/README.md"
			}
		   ],
		   "mimetype": "text/x-octave",
		   "name": "scilab",
		   "version": "0.7.1"
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		 },
		 "nbformat": 4,
		 "nbformat_minor": 0
}