1. What is the Raoult’s law of lowering of vapour pressure? Explain it.
2. Give the application and limitation of Raoult’s law.
3. Explain and deduce the Raoult’s law of lowering of vapour pressure in case of liquid- liquid solution.
4. What is ideal solution ? Mention its characteristics .
5. Show the graphical representation of how vapour pressure of ideal solution changes with the composition of its components .
6. What are the conditions to prepare an ideal of liquid- liquid solution? Explain the vapour pressure versus composition graph.
7. Explain the graph of vapour pressure versus composition of non- ideal solution showing positive deviation from Raoult’s.
8.Discuss the causes of positive deviation of liquid-liquid solution from Raoult’s law?
09. Explain the graph of vapour pressure versus composition of non-ideal liquid-liquid solution showing negative deviation Raoult’s law.
10. Explain with diagram the deviation of non-ideal solution from ideal condition.
11. When does the ideal solution behave like a non-ideal solution?
12. What do you mean by fractional distillation .
13. Explain the principle if fractional distillation
Short Question:
01. Why its is not necessary to mention temperature in Raoult’s law ?
01. What is ideal solution? What are its condition and characteristics ?
02. What is non-ideal solution ? What are its condition and characteristics ?
03. What is mole fraction ?
04. What is azeotropic mixture ? Give two examples .
05. Why components of azeotropic mixture cannot be separated by fractional distillation method?
06. what is fractional distillation? Write down the principles of faction distillation.
Mathematical problem:
01. Benzene and toluene makes an ideal solution .At a definite temperature the vapour pressure of pure benzene and toluene are 20.0 Kpa and 6067 Kpa. Find out total vapour pressure of the solution in which the amount (weight) of benzene and toluene is equal . [Ans:13.884 kPa]
02. At a definite temperature, vapour pressure of methanol and ethanol are 22 Kpa and 16.66 Kpa respectively. What will be the total vapour pressure if the solution when 57.5 g of ethanol is mixed with 80 g if methanol to prepare a solution . [Ans;20.24 Kpa]
Chapter Nine
Chemical equilibrium
Broad Question
01. What is equilibrium ? Describe static equilibrium and dynamic equilibrium with example .
02. What are reversible and irreversible reaction ? Give example .
03. Explain the characteristic of chemical of equilibrium with example.
04. What is the law of mass action ? Explain with example .
05. What do you understand by equilibrium constant ? What are Kp and Kc ?
06. Derive the expression for gas constant using the law of mass action,
07. Deduce Kp expression term by using ;aw of mass action .
[ A + B = C, determine the expression term Kp for this reaction ]
08. Establish the relation between Kp and Kc
09. Proof with an experiment “at equilibrium state all reaction is dynamic “.
10. What is Le Chatelier principle ? Explain .
11. Describe with example effect of temperature , pressure and concentration on the equilibrium .
12. What is Le Chatelier’s principle ? using this principle describe the effect of temperature on the equilibria of an reversible reaction .
13. a) What is equilibrium constant ? If the degree of dissociation of PCL5 is ‘α’ then deduce the expression of Kp for the equilibrium reaction below .
14. PCl5 (g)⇌ PCl3 (g) + Cl2 (g)
b)Deduce the expression of Kc for the reaction :
PCl5 (g) ⇌ PCl3 (g) + Cl2 (g)
C) Derive the expression of equilibrium constant for the reaction 2NH3 N2+3H using the law of mass action
15. What do you understand by chemical equilibrium? Explain the effect of temperature and pressure on the equilibrium reaction in the light of Le- Chatelier’s principle:
a)N2 (g) + O2(g) ⇌ 2NO(g) –Heat
b) N2(g) + 3H2(g) ⇌ 2NH3 (g); ∆H=-92.4K
a) 2SO2 (g) + O2(g) ⇌ 2SO3 (g) +Heat
b) A2 (g) +3B2(g) ⇌ 2AB3(g)+ Heat
c) N2O4⇌ 2NO2
d) 2NH3 (g) ⇌ N2+3H2
Explanation :
01.Explain – ‘All chemical equations move towards equilibrium .’
02.Explain – ‘Chemical equilibrium is always dynamic .’
03.Equilibrium constant will never be zero or infinite – Explain it.
Short Questions:
01.What is Le Chatelier’s principle?
02. How can you transform a reversible reaction to irreversible reaction ?
03. What is chemical equilibrium ?
04. Write down the three characteristics of chemical equilibrium .
Mathematical problems:
01. If a mixture of 15 mol I2 are heated then 10.0 mol HI is produced . Calculate the equilibrium constant of the reaction .
02. At 4450 C temperature , a mixture of 41.4 g hydrogen and 125.88 g iodine vapour is heated. As a result , 1308.16 g hydrogen iodide is produced. Calculate the equilibrium constant for the reaction. (H=1.0, I=126.9) [Ans:61.56]
03. At 300 temperature and 1.5 atm pressure , 15.6% PCl5 dissociates . Calculate the value of Kp for the dissociation reaction. [Asn:3.74 x 10-2]
04. At 4500C temperature 1 mol hydrogen and 1 mol iodine react together in a container of volume 2 L and reaches to equilibria . If the the amount of hydrogen iodide at equilibria is 1.56 mol then at the same temperature what is the value of Kp for the reaction. [Asn:50.28]
05. At 298 k temperature , in case of dissociation of N2O4, the partial pressure of N2O4 is 0.8 atm and Kp of the reaction is 0.008 atm . Find out Kc and partial pressure of NO2 for the reaction .
06. At 4250C temperature , when 4.2 mol H2 and 4.75 mol I2 are reacted in a container of volume 1 L, then 6.70 mol of HI is produced . Find the equilibrium constant Kp ans Kc according to the reaction following:
H2 + I2 ⇌ 2HI [Ans:Kp=Kc=35.627]
07.At 250C temperature and 3 atm pressure , 80% of PCl5 dissociate to PCL3 and Cl2.Ca;cu;ate the partial pressure pf PCl3 and Cl2 and also determine Kp.[Ans: ppcl3 = 1.332 atm and Kp= 5.332atm]
08. 18.5% of N2O4is dissociated at 25 0C temperature and 1.0 atm pressure. Determine the Kp of the dissociation. [ans:0.142]
Chapter Ten
Acid base equilibrium
Broad Question
01 .Explain with examples the definitions of acids and bases according to Bronsted Lowry’s concept (or protonic concept).
01. a)according to Bronsted Lowry’s theory acid are classified into how many classes ? mention the class with examples.
b) What are conjugated acid and conjugate base ? Explain with examples. What is the nature of conjugate acid and conjugate base of weak base and weak alkali ? Write with examples.
02. Explain the strength of acid and base. Arrange the following acid according to their strength and explain the reasons – HClO4 H2SO4, HNO3, H2SO4, H3PO4 and H2CO3
03. What is Oswald’s dilution law ? Prove that the degree of dissociation of a weak base or acid is inversely proportional to the square root of the concentration.
04. What is the dissociation of an acid ? What is the value of dissociation constant of strong acid and strong base ? Write few names of strong acid and strong base.
05. What is PH ? Write the mathematical expression of PH . Describe the advantages ( With examples) of expressing the concentration of acid solution with the help of PH.
06. a) What is POH? Write with examples .
b) Show that water acts as both acid and base that is a amphoteric substance.
07. Describe the main theory of acid base titration.
08. a) What is indicator ? Write some name of acid base indicator . What color they gain in acid and base solution ?
b) how indicator works to determine the neutralization point of acid base titration?
Or : How it changes its color in acid base titration?
10.How is the nature of following substances in aqueous solution ? – Explain
a) FeCl3 b) CuSO4
11.Describe the nature if the graph of changing of PH in different acid base titration.
12.What is buffer solution ? Describe the application of buffer solution in the field of industry , agriculture , human body and chemical analysis.
14. What do you mean by buffer solution? Works in the control of PH ?
15. a) Describe how buffer solution in made at a definite degree of PH? Deduce
b) Establish the equation for measuring PH of basic buffer solution .
c) Describe the mechanism of acidic buffer solution .
16. What is the ionic product of water ? Will there any change of water if acid or base is added differently in water ?
17. How the scale of PH can be determined from on product if water?
18. Give the differences between bases and alkli. Explain the statement , ‘All alkalis are base but base are not alkali”.
Explanation:
01. a) Carbon (CO32-) is a base explain.
b) Show that HCO3 ion behaves both as acid and base.
d) Show that water acts as both acid and base.
e) Ionic product of water.
Short Question:
01. What do you mean by conjugate acid and base ? Indicate the conjugate acid base in following reaction – HCL + H2O ⇌ H3O+ + Cl-
02. What is ionic product of water .
03. Write the mathematical expression of Oswald’s dilution law.
04. What is indicator ?
05. What are conjugate acid and base if HSO4- ion?
06. What is buffer solution ?
07. What is the dissociation constant of acid Ka and dissociation of constant base Kb ? What is its unit ?
08. What is the conjugate acid of following :
KCO3-, NO3-, SO3H+, H2PO3- , H2O, HSO4
09. indicate the conjugate acid and base of following reaction-
a) HNO3 +
b) H2SO4 +H2O ⇌ SO42- + H3O+
c) HSO-4 +H2O ⇌ SO2-4 +H3O+
10. a) What is the acidity of Al2O3?
b) What is the acidity of Fe2O3?
d) The acidity of CaO is two- Explain it .
11. What is buffer solution , butter reaction?
12. Write a name of indicator which is used to neutralize strong base and weak acid.
13. What is indicator ? In the titration of a strong acid by weak base, which indicator is to be used?
14. Which one is stronger between H3PO4 and HClO4?
15. Which one is stronger between HNO3 and H3PO4 and why ?
16. Complete the following reaction:
HSO-4 +
17. What is PH ?
18. Why the value of PH in aqueous solution of Al2(SO4)3 is less than that of 7 ?
Mathematical problem:
01. Calculate PH of the following solution which ionized completely
a) M/100 NaOH [Ans:12]
b) 10-3 M NaOH [Ans:11]
c) 0.02 M NaOH solution ( 2.0 x 10-2 M basic solution ) [ans:12.3]
d) 0.01 M HCl Solution [Ans:2.0]
e) Solution of
f) What is the PH of 0.2 m HCL Solution ?
g) 0.5 M H2SO4 Solution [Ans:0]
h) 0.1 M ethanoic acid . [Pka = 4.744]
i) 2 x 10-3 mL-1 basic soln
j) 0.005 M H2SO4
k) 0.05 M H2SO4
02. What will be the PH of 0.1 mol acetic acid and 0.1 mol sodium acetate solution ? (Ka=1.0x10-5) [Ans:5.0]
03. To prepare a buffer solution of 4.0 pH on 60 cubic cm o.o5 M formic acid solution what amount of cubic cm of 0.1 M sodium format solution is to be added ? [ PKHCOOH =3.8] [ans:47.55 cm3]
Chapter –11
Electrolysis
Board Question
01. What do you understand by electric conductor and non-electric conductor ? Give examples.
02. “Electrolysis in an oxidation- reduction process” – Explain with examples.
03. Discuss faraday’s two of electrolysis.
04. Explain the 2nd law of faraday.
05. What do you mean by one Faraday?
06. Calculate the charge of electron from Faraday’s Law.
07. How blister copper can be purified by electrolysis process ?
08. What is electroplating ? For what purpose it is done?
09. Describe the extraction of Aluminum metal from electrolysis of pure alumina.
Short Question:
01.What is electroplating ? Write down its uses.
02. What do you mean by one faraday ?
04. Describe Faraday’s 2nd law of electrolysis . How charge of electron and be calculated from this ?
Explanation:
01. Write short notes :
a) Electro-refining copper metal
b) Electrochemical equivalent .
Mathematical problems:
01.What amount of copper will be deposited at cathode due to the electrolysis, if 0.5 a current is passed for 10 min through CuSO4 solution?
02. When electricity is passed through H2SO4mixed water with the help of Pt electrode then 500 ml of H2 gas is obtained at S.T.P. Calculate the amount of electricity passed through the solution . [Ans:4308 Coulomb]
03. When 0.2 A current is passed through the electrodes of a cell for 50 min then 0.1978 g of Cu is deposited at cathode . Calculate the electrochemical equivalent of copper.
04. What amount of copper will be deposited in cathode if a current of 5A is passed through aqueous solution of blue vitriol for 15 minutes ?
05. What amount of copper will be deposited if a current of 5A is passed fopr 60 minutes through a solution of CuSO4. [Cu=63.5]
Chapter – 12
Electrochemical Cell
Broad Question
01. a) What is electrochemical cell ? Describe the structure of a Daniel Cell with figure.
c) Write down the differences between the electrolytic cell and Galvanic cell.
02. What is half cell? How many types of half cell are there and what are they ? what is half cell reaction ? Give example .
03. What is electromotive force and how it can be determined ?
04. What is corrosion ? Write down the role of electrode potential in the prevention of corrosion.
05. Describe the structure of standard hydrogen electrode.
06. What is dry cell ? With the help of figure , describe the dry cell.
07. What is storage cell? Describe its structure. How electricity is stored in storage cell ? Describe it with equations .
08. Write down the reaction with take place in the following cell:
a) Zn/ZnSO4 (aq) ‖ CuSO4 (aq)/Cu
b) Write down the reactions and cell made by Zn/Zn2+ and Ag/Ag+
c) Zn (s)/Zn2+ (aq) ‖ H+ (aq) /H2 (g), pt
d) What is salt bridge ? Write down its role. [Ans:12.16]
Short Note:
01. a) Standard hydrogen electrode .
b) Standard electrode potential.
d)
Explanation:
02. a) Potential of standard hydrogen electrode is Zero explain it.
b) “ The potential of standard copper electrode is 0.3394 V. “Explain it.
c) Corrosion of metal is a chemical reaction- Why?
Short Question:
01. What is electrode ?
02. What is oxidation potential ?
03. What is reduction potential?
04. What is standard electrode potential ?
05. What is salt bridge ? Write down its role.
06. Give an example if a half cell reaction .
07. What is E.M.F.?
08. What is electrochemical cell?
09. What is electromotive force ?
10. What is reference electrode.
Mathematical problems:
01. Represent the electric cell in which the below reactions fakes place.
a) Zn (s) + H2SO4 (aq) → ZnSO4 (aq) + H2 (g) [Ans:Zn/ZnSO4ll H2SO4/H2, pt;
02. The standard oxidation electrode potential of the reaction Zn (s) = Zn2+ +2e- and Cu (S) = Cu2+ + 2e- are + 0.337 V respectively . Mention with explanation that this reaction Zn (s) + Cu2+ → Zn2+ + Cu (s) is possible or not.
03. The following reaction happens in an electric cell oxidation otential of zn/Zn++ and Ag/Ag++ electrodes of the electric cell are + 0.76 V and –0.799 v respectively.
Zn + 2Ag+ = Zn2+ + 2Ag [Ans:ETotal = 1.559V]
04. Which of te following reaction happens spontaneously
a) Zn +CuSO4→ ZnSO4(aq) + Cu (s) [Asn:Ni (s) + 2Ag+ (aq) = Ni2+ (aq) + Ag (s)]
05. Does it can keep Fe2+ Solution in Zinc container ? Explain wit statement.
Zn/Zn2+; E0ox = +0.54V
Fe/Fe2+; E0ox = +0.44V
06. Can a FeSO4 Solution be kept in copper container?
Given that , E0cu/cu2+ = -0.34V and F0Fe/Fe2+ = +0.44 V
Chapter – 13
Chemical kinetics
Broad Questions
01. What do you understand by rat of chemical reaction?
02. Give the definition if “rate constant” of chemical reaction.
03. a) Discuss the effect if concentration of reactants in the rate of reaction .
b) Discuss the effect of temperature on rate of reaction.
c) Show by Arrhenius equation, rate of reaction increases with the increase in temperature.
Or) Explain the effect of temperature on the rate of reaction with the help of Arrhenius equation.
e) Describe the effect of surface area of the reactant on the rate of reaction.
05. a) What do you understand by order of reaction ?
b) Write down the differences between Molecularity and order of reaction .
a) What do you understand by zero order reaction? Give an example.
b) Deduce zero order rate constant equation and mention its characteristics.
06. a) What is first order reaction ? Deduce first order rate constant equation.
Or, A → product. Deduce ate constant equation of the reaction.
b) What is half – life of reaction? Show that the time required for completion of halt-life of first order or, a definite part does depend on the initial concentration of the reactant.
c) Show that, first order reaction never ends completely.
07. a) 2A → product; Deduce constant rate constant equation for this type of reaction.
b) What is half-life? Show that half-life of second order reaction is inversely proportional to the initial concentration of reactant.. Give mathematical explanation.
08. a) Describe molecular collision theory by activation energy is related with the rate of reaction?
b)What do you understand by activation energy and activated complex compound?
c) What is activation energy ? How activation energy is related with the rate of reaction?
09. Give definition of catalyst poison and catalyst promoter.
10. a) Write down the uses o catalyst in industry with examples.
b) What is auto catalysis? Give example.
c) What is induced catalysis? Give example.
e) What is catalyst poison? Give example.
11. What is enzyme? How does it work?
Short Questions:
01. What is rate or reaction ? Write down the mathematical equation for rare of reaction.
02. What is meant by order and Molecularity of a reaction?
03. Write down two examples if zero order reactions.
04. What is the unit of rate constant of zero order reaction and first order reaction ?
05. What is pseudo-unimolecular reaction ? Explain with example.
06. State the names of the factors which influence the rate of reaction.
07. a) What od you understand by activation energy ?
b) How activation energy influence rate of reaction ?
Or, Describe the relation between rate of reaction and activation energy .
08. What is the relationship between activation energy and rate constant of reaction ?
09. What is enzyme ?
10. What is heterogeneous catalysis ? Give example.
11. What is zero order reaction? Give example.
Mathematical Problems:
01. Time required for the completion of 75% of the reaction. [Ans. a) K = 9.59 x 10-3 min-1, b) t1/2 = 72.26 min, c) t = 1.44.58 min]
02. Half of the reactants of any first order reaction is dissociated at 400 seconds .After what time, from the starting of reaction will remain one-eight of the reactant? [ans:1202 second]
03. The relative rate of reaction of a first order reaction is 10-3 s-1. Calculate the time requride to decrease 2.5 from 10 g of the reactant . [ans:4 min 47.7 second]
04. In a first order reaction, initial concentration of the reactant is 0.6 mol/dm3 from the initial concentration of the reactant . What is the rate constant of the reaction? (or, 1 x 10-3 s-1) [Ans:1.325 x 10-3 s-1]
05. The rate constant of a first order reaction is 2 x 10-3 s-1. Calculate the half-life of the reaction. [Ans:346.5 second]
06. If the rate constant of a first order reaction is 4.6 x 10-2 min-1 then what is the half-life of this reaction? [Ans:15.06 min]
07. In a first order reaction initial concentration to the reactant is 0.6 mol/dm3 and 5 minute is required to decrease its initial concentration to 0.2 mol/dm3. Find the rate constant of the reaction?
08. Half-life of a first order reaction is 15 minute . Find out the rate constant of the reaction. [ans:0.0462 min]
09. What time is needed to complete 75% of a first order reaction if half life if that reaction is 50 second? [ans:1 min, 40.03 s]
Chapter- 14
Periodic properties of elements
Broad Question
01. What do you understand by periodic property?
02. How does atomic radius change in the same group and period in periodic table, explain with reasons.
03. a) What so you understand by ionization potential?
b) What is ionization potential of elements ? Discuss about its change in same group and period.
c) How does ionization potential of alkaline metals change with the increase in atomic number?
e) What is ionization potential ? Explain, why does ionization potential increase with the increase of atomic number in a period in periodic table .
04. a) What do you understand by electron affinity of an elements ?
b) Discuss how electron affinity of elements changes in periods and groups.
05. What are the differences between electron affinity and electronegativity ?
06. a) What do you understand by electronegativity of elements ?
b) Explain how electronegativity changes for elements in the same period and same group in periodic table .
Short Question ;
01. Explain the followings:
a) Why ionization potential of potassium is less than that of sodium ?
b) Why the 1st ionization potential of Boron is less than that of Beryllium ?
c) Why the 1st ionization potential of Nitrogen is greater than that of oxygen ?
d) At normal condition, why Na+ is formed but Na+2 dos not formed?
e) At normal condition, Why Magnesium doesn’t forms, Mg3+ ion but it forms Mg2+ ion?
f) Why does electronegativity of elements decreases with the increase of atomic number in any period if periodic table.
g) Why Fluorine is the most electronegative element ?
h) Why electronegativity of Chlorine is greater than that of Bromine?
i) Why electron affinity of Fluorine is less than that of chlorine ?
j) What is electron affinity? How electron affinity of the elements in a group in the periodic table changes?
Chapter – 15
Inert Gas
Broad Question
01. a) What is inert gas ?
b) How many inert gases are there ? Mention them. Give their electronic configuration .
Explanation:
01. What are the inert gases? Explain the causes of inertness of inert gases.
02. All inert gases are mono atomic –why ?
03. “The valence of inert gases are zero” – explain it?
04. Generally inert gases are inert even they can form some compounds- explain with examples.
Short Question:
01. Write the uses of inert gases,
02. Write two uses of Neon.
03. Give the geometrical shape XeF2, XeF4, XeF6.
04. Write two uses of argon.
05. Write two uses of Helium .
06. Why xenon can make more compounds than argon?
07. Describe the formation of coordinate compound by inert gases.
08. What is clatherate compound?
Chapter – 16
Chemistry of group IA and IIA
Broad Question
01. What are the elements called base metals ? How atomic radius and ionization potential changes with the increase of atomic number ?
02. What is brine? Describe the manufacture of NaOH and cl2 from Brine .
03. Write down four uses of sodium hydroxide.
04. write down the principle with reactions of the manufacture of soda ash ( or washing soda) (Na2CO3) by solvay process . [Ammonia soda process]
Short Question :
01. Why the group IA elements are called as alkali metals ?
02. Why Ca is called alkaline earth metals ?
03. What do you mean by s- block elements ? Why their oxdation no is + 1 or + 2 ?
04. Why metals of group IA and IIA’s oxidation number are constant ?
05. Why sodium is called alkali metal ?
06. Write the symbols of the followings.
a) Rock salt b) Chili salt petre c) Natrone d) Borax e) Carnalite f) Magnetite g) Dolomite
h) Epson salt I) Gypsum j) globar salt k) Phosphorate l) Write vitriol m) Bleaching powder
07. Be (OH)2 is insoluble in water but Ca(OH)2 is soluble why ?
08. Whate forms if we heat the following compounds
09. LiNO3 b) KNO3 c) Mg(NO3)2 e) Na2CO3
10. Why Concentrated HCL is used in flame test ?
11. Discuss the diagonal relationship between the lithium and magnesium .
12. What do you mean by diagonal relationship ? Explain with examples.
13. a) Mg3N2 + H2O → ?
b) AgNO3 (aq) + NaOH (aq)→ ?
c)AlCl3 + NaOH →?
d) NaOH + Cl2 15 c→ ?
e) SO2 + NaOH → ?
14. Wht the aqueous solution of Na2CO3 is basic ?
15. Why Na can not be kept in open air ?
16. What happens when N2 gas is passed over heated Mg and the produced compound is added to the water?
17. How will you identify Na+ in solution?
Chapter – 17
Chemistry of group IIA and IIIA
Broad Question
01. Write down the similarities between boron and silicon .
02. Write down four similarities and dissimilarities between carbon and silicon.
