1 / Write the Chemical equations for the steps involved in rusting of iron. Give one method to prevent rusting of iron.
2 / For the galvanicCell
Mg(s) + 2Ag+ (0.0001M Mg2+ (0.1M) + 2Ag(s) E0Mg2+/Mg = -2.36V, E0Ag+/Ag = 0.81V
Calculate ECell,E0Cell. Write Cell representation. Will the reaction be spontaneous?
3 / a)Calculate the eq. Const. for the reaction Zn + Cd2+ Zn2+ + Cd
E0Cd2+/Cd = -0.403V, E0Zn2+/Zn = -0.763V
(b) When a Current of 0.75A is passed through a CuSO4 solution for 25 min.
0.369 g of Cu is deposited at the Cathode. Calculate atomic mass of Cu
(C) Tarnished Ag Contains Ag2S Can this tarnish be removed by placing tarnished Ag ware in an Al pan Containing an electrolytic solution such as NaCl. The E0 for half
reactions are
Ag2S + 2e 2Ag + S2- is –0.17V
Al3+ +3e Al is -1.66V
4 / (a) Calculate ∆G0 for the following reaction at 250C
Au + Ca2+(0.1M) Au3+(1M) + Ca ( E0Au3+/Au = +1.5V, E0Cd2+/Cd = -0.403V)
Predict whether the reaction will be spontaneous or not at 250C .Which of the
above two half Cells will act as an O.A. & which one will be a R.A.
(b)The Conductivity of 0.001M acetic acid is 4 x 10 –5 S/Cm Calculate the
dissociation Const. of acetic acid if limiting molar Conductivity for acetic acid
is 390.5 SCm2/mol
5 / Molar Conductivityvs square root of Conc. is given
(a ) What Can you say about the nature of the two electrolytes A & B
(b) How do you account for the increases in molar Conductivity for strong electrolyte A & weak electrolyte B on dilution.
6 / (a) A Current of 1.5 A was passed through an electrolyticCell Containing AgNO3 soln. With an inert electrodes. The weight of Ag deposited was 1.5 g How long did the Current flow?
(b)Write the reaction s taking place at the anode & Cathode in the above Cell.
(C)Give reaction s taking place at the two electrodes if these are made up of Ag.
7 / Conductivity of 0.00241M acetic acid solution is 7.896x10 –5 S Cm-1Calculate its molar Conductivity in this soln. If limiting molar Conductivity for acetic acid be 390.5SCm2mol-1 What would be its dissociation Constant?
8 / Three electrolyticCells A, B, CContaining soln. of ZnSO4, AgNO3, CuSO4 resp. are Connected in series A steady Current of 1.5 A was passed through them until 1.45 g of Ag was deposited at the Cathode of Cell B How long did the Current flow? What mass of Cu & what mass of Zn were deposited in the Concerned Cell?(Ag = 108, Zn = 65.4 ,Cu =63.5)
9 / (a) What is primary Cell? Give one example
(b) The Conductivity of a 0.2M soln. of KCl at 298 K is 0.0248 SCm-1. Calculate its molar Conductivity.
10 / Formulate the galvanicCell in which the following reaction tale place
Zn + 2Ag+ Zn2+ + 2Ag
(i)Which one of its electrodes is negatively charged?
(ii)The reaction taking place at each of its electrode
(iii)The Carriers of Current within & out side this Cell.
11 / (a)Express the relation between Conductivity & molar Conductivity of a soln.
(b) The resistance of Cond. Cell Containing 0.001 M KCl soln. at 298 K is 1500 ohm What is the Cell Const. if the Conductivity of 0.001 M soln. at 298 K is 0.146 x 10 –3 S Cm-1
12 / Illustrate with the help of diagram how the molar Conductivities of a (i)strong electrolyte (ii) weak electrolyte vary with dilution of soln. Give reason for this variation
13 / Calculate E0Cell for the following.
2Cr + 3Cd2+ 2Cr3+ + 3Cd Calculate ∆G0 & eq. Const. K of the above reaction at 25 0C (E0Cd2+/Cd = -0.40V, E0Cr3+/Cr = -0.74V)
14 / (a) Explain why electrolysis of an aq. Soln. of NaCl gives H2 at Cathode & Cl2 at anode. (E0Na+/Na = -2.71V, E0H2O/H2 = -0.83V, E0Cl2/2Cl- = +1.36V E02H+/1/2O2/H2O = +1.23V)
(b)The resistance of Conductivity Cell Containing 0.05 M soln of an electrolyte X at 400C is 100 ohm The same Cell is filled with 0.01M soln. of electrolyte. Y has a resistance of 50 ohm . The Conductivity of 0.05 M soln of electrolyte X is 1.0 x 10 –4 SCm-1 .Calculate
(i)Cell Const. (ii) Conductivity of 0.01 M Y soln.(iii) molar Conductivity of 0.01M Y soln.
15 / (a) State Kohlrausch law of independent migration of ions. How can the degree of dissociation of acetic acid in a soln. to be calculated from its molar conductivity data.
(b)(i) Formulate the galvanic cell 2Cr + 3Fe2+ 2Cr3+ + 3Fe
(ii)Calculate E0cell. (E0Cr3+/Cr = -0.74V , E0Fe2+/Fe = -0.44V)
(iii)Calculate E cell at 250C if [Cr3+] = 0.1M , [Fe2+] = 0.01 M
16 / What type of cell is a lead storage battery? Write the anode & cathode reaction & the overall reactions occurring in the use of a lead storage battery.
17 / Two half cell reactions of an electrochemical cells are given below.
MnO4- + 8H++ 5 e Mn2+ + 4H2O E0 = +1.51V
Sn2+Sn4+ + 2e E0 =+0.15V
Construct the redox equation from the two half cell reactions & predict if this reaction favours formation of reactants or product shown in the equation.
18 / A Cu-Ag cell is set up. The Cu 2+ concentration in it is 0.1M The Ag+ concentration is not known. The cell potential measured 0.422V Determine concentration of Ag+ in the cell.
Given: (E0Ag+/Ag = 0.80V,E0Cu2+/Cu = +0.80V)
19 / A voltaic cell is set up at 25 0C with the following half cells
Al/Al 3+ (0.001M) & Ni/Ni 2+ (0.5M)
Write the equation for the cell reaction that occurs when the cell generates an electric current & determine the cell potential. (E0Ni2+/Ni = -0.25V, E0Al3+/Al = -1.66V)
20 / (a) Define molar conductivity of a substance & describe how far weak &strong electrolyte, molar cond. Changes with conc. of solute. How is such change? Explain.
(b) A voltaic cell is set up at 25 0C with the following half cells
Ag+ (0.001M)/Ag & Cu 2+ (0.1M)/Cu
What would be the voltage of this cell? (E0cell. + 0.46V)
21 / a) State the relationship amongst cell const. of a cell, resistance of the soln. in the cell & conductivity of soln. How is molar conductivity of a solute related to conductivity of its soln.
(b) Calculate K for the reaction Fe+ Cd2+ Fe2+ + Cd
(E0Fe2+/Fe = -0.44V, E0Cd2+/Cd = -0.40V)
22 / (a) Define molar conductivity. How is it related to conductivity Of the related soln.
(b)One half cell in voltaiccell is constructedfrom a silver wire dipped in AgNO3 soln. of unknown conc.Its other half cell consists of a Znelectrode dipping in 1.0 M soln. of Zn(NO3)2.A voltage of 1.48V is measured for this cell. Calculate [Ag+ ]
(E0Zn2+/Zn = -0.76V, E0Ag+/Ag = 0.80V)
23 / (a) Corrosion is essentially an electrochemical phenomenon. Explain the reactions occurring during the corrosion of iron kept in an open atmosphere.
(b) Calculate K for the reaction Fe+ Cd2+ Fe2+ + Cd
(E0Fe2+/Fe = -0.44V, E0Cd2+/Cd = -0.40V)
24 / (a)Calculate emf for the given cell at 5 0C Cr/Cr3+(0.1M)//Fe2+ (0.01M)/Fe
(E0Fe2+/Fe = -0.44V, E0Cr3+/Cr = -0.74V)
(b)Calculate the strength of current required to deposit 1.2 g Mg from molten MgCl2 in 1 hour. [1F =96500C/mol at.mass Mg =24]
25 / (a)What is meant by Limiting molar conductivity?
(b) Given that E0 of metals are K+/K = -2.93V,Ag+/Ag = 0.80V,
Cu2+/Cu = 0.34V,Mg2+/Mg = -2.37V,Cr3+/Cr = -0.74V,Fe2+/Fe = -0.44V.
Arrange these metals in increasing order of their reducing power.
26 / Write the anode and cathode reactions occurring in a commonly used Hg –
cell. How is the overall reaction represented?
27 / One Half cell in a voltaic cell is constructed from Ag wire dipped in AgNO3 solution of unknown concentration .The other half cell consists of Zn electrode in 0.1M solution of Zn(NO3)2.A voltage of 1.48V is measured for this cell. Calculate concentration of AgNO3 solution. (Given E0Ag+/Ag = 0.80V, E0Zn2+/Zn = - 0.763V)
28 / A voltaic cell is set up at 250C with the following half cells Al3+ (0.001M) and Ni2+ (0.5M) Write equation and determine Ecell. (Given E0Al3+/Al = -1.66 V, E0Ni2+/Ni = - 0.25V)
29 / (i) Write the product obtained at anode on electrolysis of conc. H2SO4 using Pt electrode.
(ii) For a weak electrolyte molar conductance in dilute solution increases sharply as the concentration in solution is decreased. Give reason.
(iii)Write overall cell reaction for lead storage battery when the battery is being charged.
30 / (a)Calculate the charge in Coulombs required for oxidation of 2 moles of water to oxygen.(1 F = 96500 C/mol)
(b) Zn/Hg oxide cell is used in hearing aids and electric watches.The following reactions occur
Zn(s) Zn2+ + 2 e E0Zn2+/Zn = - 0.76V)
Hg2O+H2O + 2e 2Hg + 2OH- E0Hg+/Hg = - 0.344V)
Calculate (i) standard potential of the cell(ii ) standard Gibb’s energy
31 / (a)Describe the construction of a H2 –O2 fuel cell and the reactions taking place in it.
(b) Define the terms given below- (a)Conductivity (b) molar conductivity
What are their units?
32 / Give reasons:
(a)Why does an alkaline medium inhibit the rusting of iron?
(b) Why does a dry cell become dead after a long time even if it has not been used?
(c) Why is Zn better than Sn in protecting iron from corrosion?
33 / (a) Two electrolytic cells containing AgNO3 solution and dil. HCl solution were connected in series A steady current of 2.5 A was passed through them till 1.078 g of Ag was deposited. [Ag = 107.8 g/mol, 1F = 96500 C]
(i)How much electricity was consumed?
(ii)What was the weight of O2 gas liberated?
(b)Give reasons:
(i)Rusting of iron pipe can be prevented by joining it with a piece of Mg
(ii)Conductivity of an electrolyte solution decreases with the decrease in concentration.
34 / (a) What is a fuel cell? What is the main advantage?
(b) What are the reactions occurring at the cathode and anode of a Lachlanche cell?
(c)In a button cell widely used for watches and other devices the following reactions takes place
Zn(s)+Hg2O+H2O 2Hg + 2OH- + Zn2+
Give the cell representation and determine the value of Kc for the above reactions using the following data. Zn(s) Zn2+ + 2 e E0Zn2+/Zn = - 0.76V)
Hg2O+H2O + 2e 2Hg + 2OH- (E0Hg+/Hg = - 0.344V)
Zn2+ + 2 e Zn(s) ( E0Zn2+/Zn = - 0.76V)
35 / (a) What type of cell is a lead storage battery? Write the anode & cathode reaction & the overall reactions occurring in the use of a lead storage battery.
(b ) Calculate the potential for half cell containing 0.1M K2Cr2O7 (aq) , 0.2M Cr3+(aq)and
1.0 x 10 -4 M H+. The half cell reaction is
Cr2O72- (aq) + 14 H+(aq) + 6 e 2 Cr3+(aq) + 7 H2O(l)
And the standard electrode potential is given as E0 = 1.33V
36 / (a) How many moles of Hg will be produced by electrolyzing 1M Hg(NO3)2 solution with a current of 2 A for 3 hours? [Hg(NO3)2 = 200.6 g/mol]
(b) A voltaic cell is set up at 250C with the following half cells Al3+ (0.001M) and
Ni2+ (0.5M) Write equation and determine Ecell.
(Given E0Al3+/Al = -1.66 V, E0Ni2+/Ni = - 0.25V)
37 / (a) Explain why electrolysis of aq. solution of NaCl gives H2 at cathode and Cl2 at anode. Write overall reaction. ( E0 Na+/Na = - 2.71 V,E0 H2O/H2 = - 0.83 V, E0 Cl2/Cl- = + 1.36V, E0 H+/H2/H2O = + 1.23V)
(b ) The resistance of a conductivity cell containing 0.001 M KCl solution at 298K
is 1500 Ω Calculate the cell constant if conductivity of 0.001M KCl solution at
298 K is 0.146 x 10 -3 S/cm.
38 / (a) Calculate the emf for the given cell at 250C.
Cr/Cr 3+ (0.1M)//Fe2+(0.01M)/Fe (E0 Cr3+/Cr = -0.74V , E0 Fe2+ /Fe = -0.44 V)
(b ) Calculate the strength of the current required to deposit 1.2 g of Mg from
molten MgCl2 in 1 hour.( 1F = 96500 C / mol , Mg = 24)
39 / What is nickel-cadmium cell? State its one merit and one demerit over lead storage cell. Write the overall reaction that occurs during discharging of this cell.
40 / State and explain Kohlrausch law of independent migration of ions. How can the degree of dissociation of acetic acid be calculated from its molar conductivity data.
41 / The electrical resistance of a column of 0.05 M NaOH solution of diameter 1 cm length 50 cm is 5.55 x 10 3 ohm. Calculate its resistivity, conductivity and molar conductivity.
12 / A voltaic cell is set up at 25 0C with the following half cells Al 3+ (0.001 M) and Ni2+ (0.5 M) Write the cell reaction and determine the cell potential.
(E0 Ni2+/Ni =- 0.258V , E0 Al3+ /Al = -1.66 V)
43 / (a) Define molar conductivity of a solution and explain how molar conductivity changes with change in concentration of a solution for a weak and a strong electrolyte.
(b)A strip of nickel metal is placed in a 1 molar solution of Ni(NO3)2 and a strip of silver metal is placed in a 1 molar solution of AgNO3.Anelectrochemical cell is created when the two solutions are connected by a salt bridge and the two strips are connected by wires to volt meter.
(i)Write the balanced equation for the overall reaction occurring in the cell and calculate the cell potential.
(ii)Calculate the cell potential,E at 250C for the cell, if the initial concentration of Ni(NO3)2 is 0.1 molar and the initial concentration of AgNO3 is 1 molar.
(E0 Ag+/Ag = +0.80V , E0 Ni2+/Ni = - 0.25V)
44 / The standard electrode potential (E0) for Daniel cell is +1.1 V. Calculate the ∆G 0 for the reaction Zn(s) + Cu 2+ Zn2+ + Cu(s) ( 1F = 96500 C mol-1)
45 / Calculate emf of the following cell at 250C
Ag(s) /Ag+ (10-3M)// Cu2+ (10-1 M)/Cu (s) (Given E0 Cell= + 0.46 V and log 10 n = n)
Chemical Kinetics
1 / For a chemical reaction variation in the [R] t ( graph ln log [R] t )
(i)What is the order of reaction
(ii)What are the units of rate constant k
(iii)Give the relationship between k & t ½
(iv)What does the slope of the above line indicate?
(v)Draw a plot log [R0]/[R] t
2 / The reaction A+2B 2C+D
Expt. / [A]0 / [B]0 / Initial rate
1 / 0.3 / 0.3 / 0.96
2 / 0.6 / 0.3 / 0.384
3 / 0.3 / 0.6 / 0.192
4 / 0.6 / 0.6 / 0.768
(i)Derive the order of reaction w.r.t. both reactants [A] & [B]
(ii)Write the rate law
(iii)Write the expression for the rate of reaction in terms of A & B
3 / Consider the reaction AP (graph [R] t is given)
(i)Predict the order of reaction
(ii)Derive expression for the integrated rate law for the reaction
4 / (a) 2N2O5 4NO2 + O2 is first order reaction with rate constant of 5x10-4 s-1.If initial concentration of N2O5 is 0.25M. Calculate its concentration after 2 min. Also calculate half life for decomposition of N2O5
(b)2A +B 3C The rate of appearance of C at time t is 1.3x10-4 mol/L/s. Calculate at this time (i)rate of reaction (ii) rate of disappearance of A
5 / (i)The decomposition reaction ofNH3 gas on Pt surface has a rate const. K = 2.5x10-4 mol /L/s. What is the order of reaction?
(ii) What is molecularity of the reaction Cl (g) ½ Cl2(g)
6 / (i) Graph of log[Ro]/[R] t is given for a reaction
(a) What is the relation between slope of this line & rate const.
(b) Calculate the rate const. Of the above reaction if the slope is2x10-4 s-1
(ii) Derive the relation between half life of a first order reaction & its rate const.
7 / (i)Define the term order of reaction for chemical reaction
(ii)A first order decomposition reaction takes 40 min. for 30% decomposition Calculate its t1/2 value.
8 / What is meant by the rate const. ’k’ of a reaction. If the concentration be expressed in mol/L units & time in sec. What would be the units for k (i) for a zero order reaction (ii) for a first order reaction
9 / (a) Derive the general form of the expression for the half life of a first order reaction
(b) The decomposition of NH3 on Pt surface is a zero order reaction What are the rates of production of N2 & H2 if k = 2.5x10-4 mol/L/s
10 / (a) List the factors on which the rate of a chemical reaction depends?
(b) The half life for decay of radioactive C-14 is 5730 years. An archeological artifact containing wood has only 80% of C-14 activity is found in living trees. Calculate the age of the artifact.
11 / (i) A reaction is second order w.r.t. A How is the rate of this reaction altered if the concentration of A is (i) doubled (ii) reduced to half
(ii)The rate of reaction increases to four times when the temp. is raised from 300K to320K Calculate Ea of this reaction (R = 8.314J/mol/K)
12 / (i)Distinguish between order & molecularity of a reaction When could order & molecularity of a reaction be the same.
(ii)The decomposition of PH3 - 4PH3 P4 + 6H2 has the rate law r = 6.0x10-4 s-1 & Ea is 3.05 x 105 J/mol. Calculate k at 310 K (R = 8.314J/mol/K)
13 / (i)Define order of reaction. How will you prove that a chemical reaction is of first order?
(ii) For a chemical reaction what is the effect of catalyst on the following
(i)activation energy of the reaction
(ii)rate const. of the reaction
14 / For the reaction 2N2O5 4NO2 + O2 at 298 K
Sr.no. / [N2O5] mol/L / Rate of disappearance of N2O5(mol/L/min)
1 / 1.13 x10-2 / 34 x 10-5
2 / 0.84 x10-2 / 25 x 10-5
3 / 0.62 x10-2 / 18 x 10-5
Determine (i) order of reaction (ii)rate const. (iii)rate law
15 / A first order reaction has a rate const. of 0.0051 min-1 If we begin with 0.10 M concentration of reactant. What concentration of reactant will be left over after 3 hours?
16 / For a decomposition reaction the values of rate const. k at two different temp. are given below
K1 = 2.15 x 10-8 L /mol/s at 650K, K2= 2.39 x 10-7 L/mol/s at 700K.Calculate Ea for this reaction (R = 8.314J/mol/K)
17 / (i)Why does the rate of a reaction not remain const. throughout the reaction process?
(ii) Explain the term order of a reaction. Derive the unit for first order rate const.
(iii) Show that for a first order reaction,the time required for half life period is independent of initial concentration.
18 / (a) Explain the terms: (i) Rate of reaction (ii) Activation energy of a reaction
(b) The decomposition of PH3 proceeds according to the following equation.
4PH3 P4 + 6H2 It is found that the reaction follows the following rate equation
Rate = k [PH3] The half life of PH3 is 39.9 s at120 0C
(i) How much time is required for 3/4th of PH3 to decompose?
(ii) What fraction of the original sample of PH3 remains behind after one minute.
19 / (a) Explain the terms: (i) Order of reaction (ii) molecularity of a reaction
(b) The rate of reaction increases four times when the temperature changes from 300K to 320 K Calculate Ea, assuming that it does not change with temperature. ( R = 8.314J/K/mol)
20 / A reaction is of first order in reactant A and second order in reactant B. How is the rate of this reaction affected when (i) [B] alone is increased to three times (ii) [A] as well as [B] are doubled.
21 / The rate constant for a reaction of zero order is 0.003mol/L/s. How long will it take for the initial concentration of A to fall from 0.1M to 0.075M?
22 / For the reaction N2 + 3H22NH3 If ∆[NH3]/ ∆t = 4 x 10 -8 mol/L/s what is the value of -∆[H2]/ ∆t?
23 / Sucrose decomposes in acid solution into glucose and fructose according to the first order rate law with t1/2 = 3 hrs. Calculate the fraction of sucrose which remains after 8 hrs.
24 / The rate constant of a reaction at 500K and 700K are 0.02 /s and 0.07 /s resp. Calculate value of activation energy for the reaction (R = 8.314 J/mol/K)
25 / (a) For the reaction C12H22O11 + H2O C6H12O6 + C6H12O6
Write (i) Rate of reaction expression( ii) Rate law equation( iii) molecularity ( iv) order of reaction
(b) The following data were obtained during the first order thermal decomposition of SO2Cl2 at const. volume.
SO2Cl2 (g) SO2(g) + Cl2(g)
experiment / Time (s) / Total press. (atm)
1 / 0 / 0.5
2 / 100 / 0.6
Calculate the rate of reaction when total press. Is 0.65 atm.
26 / (a) Illustrate graphically the effect of catalyst on activation energy
(b) Catalysts have no effect on equilibrium const. why?
(c) The decomposition of A into product has value of K as 4.5 x 10 3 /s at 10 0 C and activation energy is 60 KJ/mol.Calculate the temp. at which the value of K be 1.5 x 10 4 /s
27 / Consider the decomposition of H2O2 in alkaline medium which is ctalysed by iodide ions.
2H2O2 2H2O + O2
This reaction takes place in two steps as given below
Step I H2O2 + I- H2O + IO-
Step II H2O2 + IO-H2O + I- +O2
(a)Write the rate law expression and determine the order of reaction w.r.t. H2O2
(b)What is the molecularity of each individual step?
28 / In a hydrolysis reaction 5 g ethyl acetate is hydrolysed in presence of dil. HCl in 300 min. If the reaction is of 1st order and the initial concentration of ethyl acetate 22 mol/L, Calculate the rate const. of the reaction.
29 / The thermal decomposition of HCOOH is first order reaction with a rate const. of 2.4x10 -3 /s at a certain temp. Calculate how long it will take for 3 /4th of initial quantity of HCOOH to decompose. (log 0.25 = -0.6021)
(a) Distinguish between rate expression and rate constant of a reaction.
(b)2N2O5 4NO2 +O2
The first order reaction was allowed to proceed at 400Cand the data below were collected.
[N2O5] M / 0.4 / 0.289 / 0.209 / 0.151 / 0.109
Time (min) / 0 / 20 / 40 / 60 / 80
(a)Calculate the rate constant. Include units with your answer.
(b)What will be the concentration of N2O5 after 100 min?
(c)Calculate the initial rate of reaction.
30 / (i)Why does rate of reaction not remain constant throughout the reaction Process?
(ii)Explain the term order of reaction Derive the unit for first order rate constant.
(iii)Show that for the first order reaction the time required for half life period is independent of initial concentration.
31 / (a) Explain difference between the average rate and instantaneous rate of Reaction.
(b ) In pseudo first order hydrolysis of ester in water, the following results are obtained.
Time in seconds / 0 / 30 / 60 / 90
[Ester] M / 0.55 / 0.31 / 0.17 / 0.085
(i)Calculate the average rate of reaction between time interval 30 to 60 seconds
(ii)Calculate the pseudo first order rate constant for the hydrolysis of ester.
32 / (a) Distinguish between molecularity and order of reaction
(b)The activation energy for the reaction 2 HI H2 + I2 is 209.5 kJ/mol at 581K.Calculate the fraction of molecules having energy equal to or greater than activation energy (R= 8.31 J/mol/K)
33 / For the reaction 2NO + Cl22NOClThe following data were collected .All the measurements were taken at 263K
Expt no. / Initial [NO](M) / Initial [Cl]2 (M) / Initial rate of disappearance of Cl2 (M/min)
1 / 0.15 / 0.15 / 0.60
2 / 0.15 / 0.30 / 1.20
3 / 0.30 / 0.15 / 2.40
4 / 0.25 / 0.25 / ?
(a)Write the expression for rate law.
(b)Calculate the value of rate constant and specify its units.
(c)What is the initial rate of disappearance of Cl2 in expt.4?
34 / Consider the reaction 2A + B C+ D
Following results were obtained in experiments designed to study the rate
of reaction .
Expt. No. / Initial concentration (mol/L) / Initial rate of formation