initial commit / add all books

18 files changed, 352 insertions, 0 deletions

diff --git a/884/CH5/EX5.1/Example5_1.sce b/884/CH5/EX5.1/Example5_1.sce
new file mode 100755
index 000000000..2a36315b8
--- /dev/null
+++ b/884/CH5/EX5.1/Example5_1.sce
@@ -0,0 +1,13 @@
+//Pressure Units

+

+clear;

+clc;

+

+printf("\t Example 5.1\n");

+

+Pbaro=688;//pressure in mm Hg

+Patm=Pbaro/760;//pressure in atm

+

+printf("\t the presuure in atmospheres is : %4.3f atm\n",Patm);

+

+//End

diff --git a/884/CH5/EX5.10/Example5_10.sce b/884/CH5/EX5.10/Example5_10.sce
new file mode 100755
index 000000000..8257d1255
--- /dev/null
+++ b/884/CH5/EX5.10/Example5_10.sce
@@ -0,0 +1,24 @@
+//Computation of Molar Mass

+

+clear;

+clc;

+

+printf("\t Example 5.10\n");

+

+percentSi=33;//percent of Si in compound

+percentF=67;//percent of F in compound

+nSi=percentSi/28.01;//moles of Si in 100g compound

+nF=percentF/19;//moles of F in 100g compound

+

+P=1.7;//pressure, atm

+T=35+273;//temp. in K

+m=2.38;//mass, g

+V=0.21;//volume, L

+R=0.0821;//universal Gas constant, L.atm/K.mol

+n=P*V/(R*T);//moles

+M=m/n;//mol. mass=mass/moles, g/mol

+

+printf("\t the molecular mass of given compound is : %4.0f g/mol\n",M);

+

+

+//End

diff --git a/884/CH5/EX5.11/Example5_11.sce b/884/CH5/EX5.11/Example5_11.sce
new file mode 100755
index 000000000..b31cc320a
--- /dev/null
+++ b/884/CH5/EX5.11/Example5_11.sce
@@ -0,0 +1,14 @@
+//Gas Stoichiometry

+

+clear;

+clc;

+

+printf("\t Example 5.11\n");

+

+VC2H2=7.64;//volume of acetylene, L

+VO2=VC2H2*5/2;//volume of O2 required for complete combustion as 5mol O2 react with 2mol acetylene for complete combustion

+

+printf("\t the volume of O2 required for complete combustion of acetylene is : %4.1f L\n",VO2);

+

+

+//End

diff --git a/884/CH5/EX5.12/Example5_12.sce b/884/CH5/EX5.12/Example5_12.sce
new file mode 100755
index 000000000..ef1796009
--- /dev/null
+++ b/884/CH5/EX5.12/Example5_12.sce
@@ -0,0 +1,19 @@
+//Gas Stoichiometry

+

+clear;

+clc;

+

+printf("\t Example 5.12\n");

+

+R=0.0821;//universal Gas constant, L.atm/K.mol

+T=80+273;//temp in K

+P=823/760;//pressure in atm

+m=60;//mass of NaN3, g

+NaN3=65.02;//mol. mass of NaN3, g

+nN2=m*3/(2*NaN3);//moles of N2

+VN2=nN2*R*T/P;//from ideal gas law

+

+printf("\t the volume of N2 generated is : %4.1f L\n",VN2);

+

+

+//End

diff --git a/884/CH5/EX5.13/Example5_13.sce b/884/CH5/EX5.13/Example5_13.sce
new file mode 100755
index 000000000..98b559600
--- /dev/null
+++ b/884/CH5/EX5.13/Example5_13.sce
@@ -0,0 +1,21 @@
+//Gas Stoichiometry

+

+clear;

+clc;

+

+printf("\t Example 5.13\n");

+

+R=0.0821;//universal Gas constant, L.atm/K.mol

+T=312;//temp in K

+V=2.4*10^5;//volume, L

+P1=7.9*10^-3;//pressure initial in atm

+P2=1.2*10^-4;//pressure final in atm

+Pdrop=P1-P2;//pressure drop, atm

+n=Pdrop*V/(R*T);//moles of Co2 reacted

+Li2CO3=73.89;//mol. mass of Li2CO3, g

+mLi2CO3=n*Li2CO3;//mass of Li2CO3, g

+

+printf("\t the mass of Li2CO3 formed is : %4.1f *10^3 g\n",mLi2CO3*10^-3);

+

+

+//End

diff --git a/884/CH5/EX5.14/Example5_14.sce b/884/CH5/EX5.14/Example5_14.sce
new file mode 100755
index 000000000..417670b75
--- /dev/null
+++ b/884/CH5/EX5.14/Example5_14.sce
@@ -0,0 +1,22 @@
+//Dalton's Law of Partial Pressures

+

+clear;

+clc;

+

+printf("\t Example 5.14\n");

+

+nNe=4.46;//moles of Ne

+nXe=2.15;//moles of Xe

+nAr=0.74;//moles of Ar

+PT=2;//total pressure in atm

+XNe=nNe/(nNe+nAr+nXe);//mole fraction of Ne

+XAr=nAr/(nNe+nAr+nXe);//mole fraction of Ar

+XXe=nXe/(nNe+nAr+nXe);//mole fraction of Xe

+PNe=XNe*PT;//partial pressure of Ne

+PAr=XAr*PT;//partial pressure of Ar

+PXe=XXe*PT;//partial pressure of Xe

+

+printf("\t the partial pressures of Ne, Ar and Xe are : %4.2f atm, %4.2f atm and %4.3f atm respectively\n",PNe,PAr,PXe);

+

+

+//End

diff --git a/884/CH5/EX5.15/Example5_15.sce b/884/CH5/EX5.15/Example5_15.sce
new file mode 100755
index 000000000..69e72ae59
--- /dev/null
+++ b/884/CH5/EX5.15/Example5_15.sce
@@ -0,0 +1,20 @@
+//Dalton's Law of Partial Pressures

+

+clear;

+clc;

+

+printf("\t Example 5.15\n");

+

+PT=762;//pressure total, mmHg

+PH2O=22.4;//pressure of water vapor, mmHg

+PO2=PT-PH2O;//pressure of O2, frm Dalton's law, mmHg

+M=32;//mol mass of O2, g

+R=0.0821;//universal Gas constant, L.atm/K.mol

+T=24+273;//temp in K

+V=0.128;//volume in L

+m=(PO2/760)*V*M/(R*T);//mass of mass of O2 collected, g

+

+printf("\t the mass of O2 collected is : %4.3f g\n",m);

+

+

+//End

diff --git a/884/CH5/EX5.16/Example5_16.sce b/884/CH5/EX5.16/Example5_16.sce
new file mode 100755
index 000000000..c7e363ca8
--- /dev/null
+++ b/884/CH5/EX5.16/Example5_16.sce
@@ -0,0 +1,23 @@
+//Root Mean Square velocity

+

+clear;

+clc;

+

+printf("\t Example 5.16\n");

+

+R=8.314;//universal Gas constant, J/K mol

+T=25+273;//temp in K

+

+//for O2

+M=4.003*10^-3;//mol mass in kg

+Urms=sqrt(3*R*T/M);//rms velocity, m/s

+

+printf("\t the rms velocity of O2 collected is : %4.2f *10^3 m/s\n",Urms*10^-3);

+

+//for N2

+M=28.02*10^-3;//mol mass in kg

+Urms=sqrt(3*R*T/M);//rms velocity, m/s

+

+printf("\t the rms velocity of N2 collected is : %4.0f m/s\n",Urms);

+

+//End

diff --git a/884/CH5/EX5.17/Example5_17.sce b/884/CH5/EX5.17/Example5_17.sce
new file mode 100755
index 000000000..4136eaeda
--- /dev/null
+++ b/884/CH5/EX5.17/Example5_17.sce
@@ -0,0 +1,15 @@
+//Gas Effusion

+

+clear;

+clc;

+

+printf("\t Example 5.17\n");

+

+t2=1.5;//diffusion time of compound, min

+t1=4.73;//diffusion time of Br, min

+M2=159.8;//mol mass of Br gas, g

+M=(t2/t1)^2*M2;//molar gas of unknown gas, g(from Graham's Law of Diffusion)

+

+printf("\t the molar mass of unknown gas is : %4.1f g/mol\n",M);

+

+//End

diff --git a/884/CH5/EX5.18/Example5_18.sce b/884/CH5/EX5.18/Example5_18.sce
new file mode 100755
index 000000000..af28765a3
--- /dev/null
+++ b/884/CH5/EX5.18/Example5_18.sce
@@ -0,0 +1,26 @@
+//deviation from ideal behaviour

+

+clear;

+clc;

+

+printf("\t Example 5.18\n");

+

+//(a)

+V=5.2;//volume, L

+T=47+273;

+n=3.5;

+R=0.0821;//universal Gas constant, L.atm/K.mol

+P=n*R*T/V;

+

+printf("\t the pressure of NH3 gas from ideal gas equation is : %4.1f atm\n",P);

+

+//(b)

+a=4.17;//constant, atm.L2/mol2

+b=0.0371;//constant, L/mol

+Pc=a*n^2/V^2;//pressure correction term, atm

+Vc=n*b;//volume correction term, L

+P=n*R*T/(V-Vc)-Pc;//from van der waals equation, pressure, atm

+

+printf("\t the pressure of NH3 gas from van der waals equation is : %4.1f atm\n",P);

+

+//End

diff --git a/884/CH5/EX5.2/Example5_2.sce b/884/CH5/EX5.2/Example5_2.sce
new file mode 100755
index 000000000..6edf423fb
--- /dev/null
+++ b/884/CH5/EX5.2/Example5_2.sce
@@ -0,0 +1,14 @@
+//Pressure Units

+

+clear;

+clc;

+

+printf("\t Example 5.2\n");

+

+Pbaro=732;//pressure in mm Hg

+Patm=Pbaro/760;//pressure in atm

+P=Patm*1.01325*10^2;//pressure in kilo Pascal

+

+printf("\t the presuure in kilo pascals is : %4.1f kPa\n",P);

+

+//End

diff --git a/884/CH5/EX5.3/Example5_3.sce b/884/CH5/EX5.3/Example5_3.sce
new file mode 100755
index 000000000..6a2466d47
--- /dev/null
+++ b/884/CH5/EX5.3/Example5_3.sce
@@ -0,0 +1,17 @@
+//Ideal Gas Equation

+

+clear;

+clc;

+

+printf("\t Example 5.3\n");

+

+V=5.43;//volume, L

+t=69.5;//temperature, C

+T=t+273;//temperature, K

+n=1.82;//moles

+R=0.0821;//universal gas constant, L.atm/(K.mol)

+P=n*R*T/V;//pressure, atm

+

+printf("\t the presuure in atmospheres is : %4.2f atm\n",P);

+

+//End

diff --git a/884/CH5/EX5.4/Example5_4.sce b/884/CH5/EX5.4/Example5_4.sce
new file mode 100755
index 000000000..b2d8c91c3
--- /dev/null
+++ b/884/CH5/EX5.4/Example5_4.sce
@@ -0,0 +1,19 @@
+//Ideal Gas Equation

+

+clear;

+clc;

+

+printf("\t Example 5.4\n");

+

+m=7.4;//mass of NH3, g

+

+//at STP for NH3 for 1mole of NH3

+V1=22.41;// volume, L

+NH3=17.03;//molar mass of NH3, g

+

+n=m/NH3;//moles of NH3

+V=n*V1;//volume, L

+

+printf("\t the volume of NH3 under given conditions is : %4.2f L\n",V);

+

+//End

diff --git a/884/CH5/EX5.5/Example5_5.sce b/884/CH5/EX5.5/Example5_5.sce
new file mode 100755
index 000000000..907c107b1
--- /dev/null
+++ b/884/CH5/EX5.5/Example5_5.sce
@@ -0,0 +1,18 @@
+//Ideal Gas Equation

+

+clear;

+clc;

+

+printf("\t Example 5.5\n");

+

+V1=0.55;//volume, L

+P1=1;//pressure at sea level, atm

+P2=0.4;//pressurea at 6.5km height, atm

+

+//n1=n2 and T1=T2 given hence P1V1=P2V2

+

+V2=P1*V1/P2;

+

+printf("\t the volume of He balloon at height 6.5km above sea level is : %4.1f L\n",V2);

+

+//End

diff --git a/884/CH5/EX5.6/Example5_6.sce b/884/CH5/EX5.6/Example5_6.sce
new file mode 100755
index 000000000..b2ec2e6fc
--- /dev/null
+++ b/884/CH5/EX5.6/Example5_6.sce
@@ -0,0 +1,17 @@
+//Ideal Gas Equation

+

+clear;

+clc;

+

+printf("\t Example 5.6\n");

+

+P1=1.2;// pressure initial, atm

+T1=18+273;//temperature initial, K

+T2=85+273;//temperature final, K

+//volume is constant

+

+P2=P1*T2/T1;// pressure final,atm

+

+printf("\t the final pressure is : %4.2f atm\n",P2);

+

+//End

diff --git a/884/CH5/EX5.7/Example5_7.sce b/884/CH5/EX5.7/Example5_7.sce
new file mode 100755
index 000000000..f07f83750
--- /dev/null
+++ b/884/CH5/EX5.7/Example5_7.sce
@@ -0,0 +1,18 @@
+//Ideal Gas Equation

+

+clear;

+clc;

+

+printf("\t Example 5.7\n");

+

+P1=6.4;// pressure initial, atm

+P2=1.0;// pressure final, atm

+T1=8+273;//temperature initial, K

+T2=25+273;//temperature final, K

+V1=2.1;//volume initial, mL

+

+V2=P1*V1*T2/(T1*P2);// volume final, mL

+

+printf("\t the final volume is : %4.0f mL\n",V2);

+

+//End

diff --git a/884/CH5/EX5.8/Example5_8.sce b/884/CH5/EX5.8/Example5_8.sce
new file mode 100755
index 000000000..0f6400836
--- /dev/null
+++ b/884/CH5/EX5.8/Example5_8.sce
@@ -0,0 +1,28 @@
+//Density Calulations

+

+clear;

+clc;

+

+printf("\t Example 5.8\n");

+

+//taking 1 mole of CO2

+n=1;

+R=0.0821;//universal gas constant, L. atm/K.mol

+t=55;//temperature, C

+T=t+273;//temperature, K

+P=0.99;//.pressure, atm

+M=44.01;//molar mass of CO2, g

+d1=P*M/(R*T);//density of CO2, g/L

+

+printf("\t the density of CO2 is : %4.2f g/L\n",d1);

+

+//altenate method

+//taking 1 mole of CO2

+mass=M;//mass of CO2 in g =mol mass since we are considering 1 mole of CO2

+V=n*R*T/P;//volume, L

+d2=mass/V;//density=mass/volume, g/L

+

+

+printf("\t (Alternate Method)the density of CO2 is : %4.2f g/L\n",d2);

+

+//End

diff --git a/884/CH5/EX5.9/Example5_9.sce b/884/CH5/EX5.9/Example5_9.sce
new file mode 100755
index 000000000..c22a7f8ae
--- /dev/null
+++ b/884/CH5/EX5.9/Example5_9.sce
@@ -0,0 +1,24 @@
+//Computation of Molar Mass of Gaseous substance

+

+clear;

+clc;

+

+printf("\t Example 5.9\n");

+

+d=7.71;// density, g/mL(given)

+R=0.0821;//universal gas constant, L. atm/K.mol

+T=36+273;// temp, K

+P=2.88;//pressure, atm

+M1=d*R*T/P;// mol. mass, g/mol

+printf("\t the molecular mass of given compound is : %4.1f g/mol\n",M1);

+

+//alternate method

+//considering 1 L of compound

+V=1;//volume, L

+n=P*V/(R*T);//no of moles

+m=7.71;//mass per 1 L, g

+M2=m/n;// mol. mass, g/mol

+

+printf("\t {alternate method} the molecular mass of given compound is : %4.1f g/mol\n",M2);

+printf("\t the molecular formula can be only found by trial and error method as given in the book \n");

+//End