Chapter One
Chemistry 1st Paper
States of Matter
1.What do you understand by intermolecular force? Explain the effect of temperature on this force and also explain how the physical properties of matters depend upon this force.
2.What is gas? What are the characteristics of gases? How many gas laws are there and what are they?
3.Write down Charles’s law and give its mathematical explanation.
Or,Write down the law concerning the effect of pressure on the volume of any fixed mass of gas ,at constant temperature and also establish a mathematical equation for this law?
4.Show that at –273oC temperature the volume of any gas id theoretically zero
Or ,Show that volume of all gases becomes theoretically zero at absolute zero temperature .
5.What do you understand by absolute zero temperature? Explain how the absoluter temperature scale could be establishes from Charle’s law.
Or, Explain how the absolute temperature scale is obtained from Charle:s law.
6.Deduce the ideal gas equation from Boyle’s, Charle’s and Avogadro’s law (PV = nRT).
Or, Deduce the ideal gas equation by combining the gas laws.
Or, Deduce the ideal gas equation by combination of Boyle’s and Charle’s law.
6.Show that for 1 mole of an ideal gas PV=RT ( where the symbol has their conventional meaning).
Or, Show that PV/T = K ( constant ) for an ideal gas.
7. State
8. Write down
9. What is partial pressure ? how the relationship between the partial pressure of a constituent gas of a gas mixture, its le fraction and the total pressure of the mixture.
10.Two containers of volume V1and V2 contains two different gases and their pressure is P1 and P2 respectively. What is the pressure of the gas mixture when the two containers id joined with each other by a tube and is allowed to intermix ?
11.Deduce the combined law (P1V1/T1=P2V2/T2 ) of Boyel’s law.
12.Statr and explain Graham’s diffusion law.
13. State and explain Graham’s diffusion law.
Or,( Deduce the equation fir funding the molecular mass of any gas sing Graham’s diffusion law).
13. Write down the postulate if kinetic theory of gases ? Write down the equation for kinetic theory of gases.
14. Deduce the following laws from the equation if kinetic theory if gasses;
a) Boyle’s law
b) Charke’s Law.
c) Avogadrow’s Law
d) Graham’s law.
15. Explain the causes if deviation of real gases from ideal behavior.
Or, Deduce the Van der Waal’s equation for real gases.
16. Write down the important of critical temperature in liquefaction of gases.
17. What do you understand by the vapour pressure of liquid substance?
18. What do you understand by the unit cell of crystals?
19. Incase if crystals of metals explain:
a) Hexagonal closest parched structure, h.c.p.
b) Face centered cubic close parched structure, f.c.c
c) Body centered cubic close parched structure, b.c.c.
20. Which class does the crystal structure if Na+Cl- belongs ? Discuss the crystal structure if NaCl which its diagram. What is the co-operation in it ?
21. a) Discuss the crystalline structure of Cs+Cl- with diagram which class does it belongs and what is the co-ordination if it ?
b) discuss briefly t he crystalline structure of NaCl.
22. a) What is the unit of pressure and volume of gas in S.I. system ?
b) What do you mean by STP and SATP?
23. What is the equation of ideal gas ? Give two uses of it.
24. a) What is molar gas constant ?
b) Explain the dimension and significance of R ?
c) Find out the value of R in litre-atmosphere.
d) Find out the value of R in S.I. unit.
e) Calculate the value of R in C.G.S unit.
f) What is Boltzmann constant ?
25. a) Deduce Dalton’s partial pressure Law.
b) What do you mean by partial of gas ?
26. a) deduce the Graham’s diffusion law.
b) What do you mean diffusion and effusion ?
c) Whose rate of diffusion is more on between NH3 (g) and HCL (g) and why ?
27. What kinetic theory of gases? Write ors postulates.
28. a) What do you mean by average velocity of gases and root mean square velocity of gases?
b) Write the equation of the relation between RMS velocity, temperature and molecular mass.
29.a) What are ideal and real gas?
b) Write down the equation of Van der Waal’s for ‘n’ mole if real gas.
c) Write down the Joule- Thomson effect?
30. a) What is critical temperature? What is the critical temperature of CO2?
b)What is critical pressure?
c) What do you mean by the critical temperature o fCO2 is 31.10C?
31. What are the differences between gas and vapour ?
32. What is the unit cell of solid substance ?
33. Na+Cl- are the unit belong to which crystal ?
34. Explain the following:
a) real gases at high temperature and at low pressure behave like ideal gases.
b) Generally temperature decreases in Joule- Thomson effect.
35. Write down short motes on the following:
a) Joule- Thomson effect. b) Critical temperature.
36. Why does the temperature of gas fall at all time of Joule Thomson effect ?
Mathematical problems
01.The volume if gas with a solid substance is 100 L at 270C temperature. If temperature is raised to 540C the pressure increases as double and the volume with the solid substance becomes 59.3 L. What is the volume of the solid substance ? [Ans:1055 L]
02. a) At 170C temperature and 99.99 Kpa pressure, 0.058 m3 H2 gas is collected over water . If steam pressure or 3.27 or3.30 Kpa at 170C temperature then what will be the volume an mass of the gas at S.T.P ? [Ans. Volume 0.0521 m3mass 4.69 g ]
b) At 170 C temperature and 0.95 atm pressure 580 ml H2 gas was collected over water, Calculate the volume of H2 gas at STP ( the vapour pressure at 17C is 3.26 kpa )
03. At 270 C temperature in a container of 2000 L N2 O2 are mixed .If the volume of O2 ( mixed)is 16.8 L at S.T.P. then find out the partial pressure of O2 in the mixture. [ Ans: 0.7015 cm Hg ]
04. 600 ml if O2 gas is collected over water at 170 C temperature and 770 mm (Hg) pressure. What is the volume and mass of that gas at S.TP.? Vapour pressure of water at 170 C temperature is 14.5 m (Hg)
Equation 4: P1/T2D1=P2/T2D2
05. Find out the number of molecules present in 0.001 m3 of So2 ( or 0.0011 m3 of H2 ) at 2700 C temperature and98.66 *103 NM-2 pressures. [Ans;2.382x1022 ]
06. There is a container of0.001 m3 which contains O2, at 00 C temperature and at 1.01 x 10-10 pa pressure. How many molecules of o2 are there in the container ? [Ans: 4.45 x 10-17 mole; 2.6 x107 molecule]
Equation 6:PV=g/M RT (Ideal gas equation)
07. At 170 temperature and 740 mm pressure a gas if 0.842 g occupies 400 ml volume. Find the molecular mass if that gas. [Ans; 52 ]
08. Vapour density if a gas is 15. At 298 k temperature and 101.3 Kpa pressure find out the volume if 5.6 g of that gas ? [Ans: 4.568]
09. A gas ‘A’ of 100 cm3 needs 292 second ti diffuse through a tiny pore. At the same condition co2 need 230 second. What is the molecular mass of ‘A’? [Ans.70.92]
10. At constant temperature, 1.3. L hydrogen gas (H2) at 95 kpa pressure, 0.6 L nitrogen gas (N2) at 99 kpa pressure and 1.4 L oxygen gas (o2) at 75 kpa pressure are accumulated into a 1.5 L container .Find our the total pressure of the gas mixture.[And: 191.93]
11. At constant remperatuere,250 ml nitrogen gas at pressure 1 atm and 500 ml oxygen gas at pressure 600 mm(Hg) are mixed in a flask, whose volume is ! L . calculate the total pressure in the gas mixture.
Equation 10: C= √3RT/M
12.At 270 C temperature and 101.325 kpa pressure, what is the the Root Mean square (RMS) velocity of nitrogen gas (N2)?[Ans:517.01 m/s]
13.a)Find out the root mean square (RMS) velocity of o2 .
b) Calculate the the mean root velocity of N2 at 00 C.
14. At S.T.P. the density of nitrogen gas (N2) is 1.25 kgm-3 . Calculate the root mean square (RMS) velocity of nitrogen molecules at that temperature . [Ans:493.197 m/s]
15. Find out the Root Mean square (RMS) velocity of oxygen (o2) molecule at 270 c temperature .[Ans:483.62 ms-1]
16. At what temperature (in degree celsius) the ( RMS) velocity of CO2 become equal to the RMS velocity of Cl2 at 293 K temperature .
Equation 11: P1/T1=P2/T2
17. An oxygen cylinder can endure 250 atn or 300 atm pressure . At 125 atm or 150 atm pressure and 270 C temperature the cylinder has filled O2. At what temperature the cylinder will explode? [ Ans:3270 c]
Equation 12: P1= px
18. Calculate the kinetic energy of 5 g O2 at temperature.[Ans:584.72] End
Chapter Two
Broad Question
01. Write down the postulates of
02. a) What are fundamental particles ? Write down the characteristics of fundamental particles.
b) Describe three permanent fundamental particles.
03. How do you prove that, atom contains nucleus?
04. Describe the experiment of
05. a) Describe the atomic model of
.b) Mention the limitation of
06.a) Describe Bohr’s postulates of related structure of atom.
Or, Write down the main assumption of Bohr’s atom .
b) Mention the limitations of Bohr’s atom model.
07.a) Describe the quantum numbers which are use to describe an electron on an atom.
b) What is quantum number? Describe the significance of quantum numbers.
c) Why four quantum numbers are used to identify an electron completely of an atom?
d) What is quantum number?
e) Give describe of magnetic quantum number.
08. a) What is Pauli’s exclusion principle? According to this principle, calculate the highest numbers of electrons that are present in L Shell.
b) Describe puli’s exclusion principle with example.
c) What is pauli’s exclusion principle? According to this principle how many electrons can present in ‘d’ subshell ?
09. a) What is Aufbau principle ? Explain the electronic configuration of atoms with the help if this principle.
b) Calculate the value of I m and find the number of electrons present in 4th energy level.
c) Calculate I and m for 3rd shell.
10.a) What is orbit and orbital ?
b) Write the differences between orbit and orbital.
11. a)What is ionization potential ? Give examples.
b) Why the 2nd ionization of mg is less than that of Na ?
12. a) What do you mean by electron affinity ? Explain .
b) Why the electron affinity of fluorine is less than that chlorine ?Explain it.
c) Why the ionization potential of N is more than O.
13. Calculate and show the charge of an electron .
14. a) What do you mean by radioactivity and radioactive isotope ?
b) Write the uses if radioactive isotope .
15.What changes occur in the nucleus due to the scattering of α,β,γ rays of radioactive isotope ?
b) What is radioactivity ? the change which is occurred by the scattering if radioactive alpha particles, explain that with examples.
c) What is radioactivity ? What changes occur in radioactive β particle ? Show with examples.
d) What is nuclear reaction ? Write down the difference between nuclear reaction and chemical reaction
e) What do you mean by radioactivity and radioactive isotopes ?
f) What is radioactivity ? Explain the nuclear fusion reaction with example .
16. a) Atomic number and atomic mass number .
b) Isotope
c) Isobar
d) Subsidiary quantum no.
e) Isotone [Ans:2.14]
f)Magnetic quantum number
g)
h) Pauli exclusion principle
i) Ionization potential
k) Electron affinity
l) Radioactive isotope and their uses
m) What is radioactivity ? characteristics if scattering if radioactive rays .
n) What is nuclear fusion and write with the examples.
o) Write four differences between nuclear fission and nuclear fusion.
Short Question:
01. Calculate the values of I and m and find out the total numbers of orbitals and electrons present in 3rd energy level.
02. Which are possible and impossible of the following ?
a) 4p, 2d, 3d, 1p, 5f
b) 1p, 2s, 2d,3f
03. a) What is Hund’s rule ? Write the electronic configuration of N. p and O or S according ti this rule.
b) What is Hunds rule ? Electronic configuration if N obey Hund’s rule- explain.
04. a) Explain why the last electron of K enters to 4s orbitals , instead if 3d orbital.
b) Why the electronic configuration Cu is different.
05. Show the electronic configuration of following element and ions-
a) Mg(12), Al+3(13)
b) P(15), P3-(15)
c) S(16), S2-16)
d) Cl(17), Cl-(17)
e) K(19), K+(19)
f) Ca(20), Ca2+(20)
g) Sc(21)
h) Cr(24)
i) Fe(24) Fe2+(26), Fe3+(26)
j) Cu(29), Cu2+(29)
k) Zn(30), Zn2+(30)
l) I(53), I-(53)
m) Ni2+(28)
n) N
o) O
06. Compete and write the correct symbols of the followings;
a) 7N14 + ? → 6C11 + 2He4
b) 8O16 + 0n1 → ? + 1H1
c) 7N14 + 1H1 → ? + 2He4
d) 13Al27 + 0n1 → ? + 1H1
e) 1H2 +1H3 → 2He4 + ?
f) 92U236 + 0n1 → ? + 36Kr92 + 3 0n1
g) When α ray scatter from 90Th234 then what happens.
h) 7N17 + ? → 6C11 + 2He4
i) 92U236 + 0n1 → 56Ba141 + 3 0n1 + ?
07. What happens when Bray is radiated from 90Th262 ?
08.Write down the difference between isotope and isobar ?
09. Why the 2nd ionization potential if every element is greater than that if first ionization potential ?
10. Why d-orbital is absent in 2nd energy layer ?
11. Draw the orbital figure I of and p.
End
Chapter Three
Broad Question
01. Write down the limitations or defects of Mendeleef’s periodic table.
02. a) Write down he modern periodic law.
b) Write down the characteristics if modern periodic table.
03. a) “ the periodicity of element is dependent on the electronic configuration of the elements” – put arguments in favour of this statement.
b) “ Electronic configuration is he real basis if the periodic table” – Explain.
04. Discuss the classification if elements in the light of electronic configuration.
05. a) Hydrogen is placed in both Group –ⅠA and ⅦA. Explain positions.
b) Describe the position of H2 in the periodic table.
06. a) What are inert gases ? Discuss the position of inert gases in the periodic table.
b) Write down the modern periodic law . Discuss the position of inert gases in the periodic table.
c) Explain the inertness if noble gases.
Short Question:
01. Write down the electronic configuration of the following element . From the electronic configuration find the position of these elements and discuss the type of elements. They areas follows:
a. K(19) b. Sc (21) c. Cr (24) d. Fe (26) e. Cu (29) f. Zn (30)
02. a) How many group and periods are present in the modern periodic table. ?
03. write short notes on:
a) Transition metals.
04. “Every element occupies a single position table” -explain it.
05. Write short note on the following :
a) s- block element.
b) p- block element.
c) d- block element.
06. a) Define transition elements. Write two general properties of transition elements .
b)Write down the differences between transition elements and d- block elements .
c) ‘ All transition elements are d- block elements but all d –block element are not transition elements – explain it.
d) Why Na is called transition alkali metal.
07. Write down 3 defects relationship in the periodic table.
08. Discuss the diagonal relationship in the periodic table.
09. What are s-block and p-block elements. Write down their characteristic.
Chapter Four
Board Questions:
01. Write short notes:
a) Standard solution .
b) Primary and Secondary standard substance.
c) Indicator.
d) Molar solution
02. Define empirical and molecular formula. Differentiate empirical and molecular formula with examples.
03. How can we determine the empirical formula if a compound and molecular formula from it.
04. What id molarity, molality and normality of solution ? Give examples. Which one if them depends on temperature and why ?
05. Show that:
a) Molar solution is a standard solution .
b) Decimolar (or semimolar) solution is a standard solution.
c) Why H2SO4 is not called primary standard substance.
06. What are primary and secondary standard substance ? Give explaination.
Short Question
07. What is mole ? Explain with example.
08. What is Avogadro’s number ? Give example .
09. What is molarity and molar volume ?
10. What is molarity and molality ? Which one of them is influenced by temperature ?
11. How atoms are present in one gram of carbon ?
12. Calculate the mass of H2SO4 dissolved in 500 ml decimolar solution if it .
13. What is molar solution and indicator ?
14. What is Standard solution ?
15. Why the molarity and normality is equal in HCl ?
Mathematical Problems :
01. Specific gravity of sea water id 1.03 . By vaporiding 1.0 dm3 of sea water 36.4 g dry salt is obtained . Calculate the percentage composition of solid substance in sea water. [Ans:3.534%]
02. 30 g sugar is dissolved in 500 g water . Calculate the mole fraction of water and sugar in the solution. [Ans:Mole fraction of water and sugar is 0.97 and 0.031 respectively.]
03. In a compound there are C = 54.54%, H = 9.09% and O = 71.06%. If the vapour density if the compound is 45 then calculate its molecular formula. [Ans:C4H8O2]
04. In a compound there are C = 26.7%, H = 2.24% and O = 71.06%. If the vapour density if the compound is 45 then calculate is molecular formula. [Ans;C2H2O4]
05. A compound contains 26.7% C and 2.24% hydrogen. Determine the empirical formula if the compound.
Equation Related problems:
01. How much g of quick lime (CaO) will be obtained when 8.15 g pure ZnO is reduced by carbon reduction process? [Ans:6.551]
02. What amount of quick lone (CaO) will be obtained when 200 g of 95% pure limestone (CaCO3) os completely decomposed in heating and calculate the volume of produced carbon dioxide at S.T.P. [Ans:106.4 g, 42.56 litre]
03. How much caustic soda will be needed when the amount liberated carbon dioxide from 20 g of CaCO3 of completely converted to Na2CO3. [Ans:16.0g]
04. A sample of limestone contains 96% CaCO .How much litre of CO2 will be obtained at S.T.P. when 150 g of limestone is dissolved in dilute hydrochloric acid solution ?
05. 12.5 g of limestone reacts with hydrochloric (HCL) production 2.53 dm3 of at 270 C temperature and 99.99 Kpa pressure . What is the percentage of CaCO3 in that limestone ?[Ans:78.52]
06. There is a magnetite ore which contains 60% ferrous ferric oxide . What amount of iron will be obtained from 500 Kg of ore ?[Ans:217.08]
07. A sample of limestone contains 98% CaCO3 how much gram of limestone will be needed to prepare 40 L of carbon dioxide at 300C temperature and 780 mm if pressure ? [Ans:168.49g]
08. When 1.84 g mixture of CaCO3 and MgCO3 is heated then a residue of 0.96 g is obtained . Calculate the percentage of CaCO3 and MgCO3 present on the mixture ?
09. when NaCl is heated with concentrated H2SO4 then a complete salt and HCL ate produced . In this process- a) What amount of HCl is produced from 100g if NaCl ?
b) How much gram of H2SO4 reacts with 100 g of NaCl ?
:Avogadro’s Hypothesis Related if Hydrogen :
01. a) What number if molecule an atom remain in 1.0 g if Oxygen ? [Ans:1.882 × 1022 and 3.764 x 1022]
b) What number of atom of hydrogen and oxygen of present in 5 g of water ? [Ans:3.34 x 1023 H Ans 1.67 x 1023 O ]
c) What number if molecule if SO2 present in 1.0 dm3 at 270C temperature and 740 mm pressure ? [Ans:2.38 x 1022]
d) What is the number of methane molecule is present on 2.0 g methane (CH4) ?[Ans:7.529 x 1022]
e) What number of molecule is present in 250 ml nitrogen at S.T.P. [Ans:6.72 x 10]
d) What number of molecule is present in 1.0 ml at 300C temperature and 750 mm atm pressure ?
f) What number of molecule are present in 0.1 ml if hydrogen at 270 temperature and 0.987 atm pressure ?
g) What number if mole and molecule are present in 90 g if water ?[Ans: 50 mol, 3.0115 x 1024 no. if molecule]
1) How many molecules are there in 1 ml if nitrogen at normal temperature and pressure ?
Mathematical problems related to Acidimetry and Alkalimetry;
01. How much grams of Na2CO3 will be needed to make a- a . molar, b. decimolar 250 cm3 Na2CO3 solution ? [Ans:23.50 g, 2.66 g]
02. How much cm3 of decimolar solution can be prepared by 100 cm3 0.5 M Na2CO3 solution ?[Ans:253.33 cm3]
03. Find out the concentration in molarity of a 10% Na2CO3 solution ?[Ans:0.943]
04. A 200 cm3 solution is prepared by mixing water with 2.7 g monoacidic base. 65.5 cm3 1M HCl solution was needed ti neutralise that . What was the molecular weight of that base ? [Ans:40]
05. The volume of the solution of sample if 1.881 g Na2CO3 with impurities was made 250 cm3 of this solution neutralize 24.05 cm3 M/10 HCl solutions. Find the % of impurity in Na2CO3 . [Ans:32.23%]
06. The volume of the solution of a sample of Na2CO3 with 0.89 g impurities was made 250 cm3 .25 cm3 of this solution neutralize 22.05 cm3M/10 HCl solutions. Find the % of impurity in Na2CO3. [Ans:43.23%]
07. 20 cm3 0.5 M Na2CO3 was mixed with 30 cm3 HCL solution. 20 cm3 0.1 M NaOH was needed to neutralize the remaining acid solution . What is the concentration of acid solution .[Ans:0.733M]
08. To neutralize 25 ml NaOH ,10ml 0.1 M HCl was added. But to neutralize properly 8 ml 0.15 HCl solution was needed .What is the concentration of the NaOH solution ? How much NaOH is there in 1 L if this solution ? [Ans:0.088 M,3.52 g]
09. 10.2 ml 0.05 M H2SO4 solution is needed to neutralize 25 ml Na2CO3 solution. What is the concentration o f the Na2CO3 solution ?
10. If 12.0 g CaCO3 is soluted in HCL some CO2 gas is extracted . 650ml NaOH is necessary to make this gas NaCO3 .what is the molarity of the basic solution ? [Ans:0.369]
11. 10 cm3 Na2CO3 was partially neutralized by 20 cm3 0.1 M HCl .more 16 cm3 0.15 M HCl was necessary to neutralized it fully . What is the concentration of the Na2CO3 solution . [Ans:0.22 M]
12. 20 ml of 0.5 M Na2CO3 solution is added to 30 ml HCl solution and then further 20 ml of 0.1 M NaOH solution is needed to neutralize the acid solution completely . Determine the concentration of the acid solution . [Ans:0.733 M]
Chapter Five
Broad Question
01. “Oxidation- reduction takes place simultaneously “ – explain with example.
02. Describe oxidation – reduction with example according to electronic concept .
03. Discuss with example about the rules which are used for balancing chemical equation of oxidation - reduction.
04. a) Briefly discuss the basic principles if Redox Titration.
b) describe basic principle for the determination of amount of ferrous iron using standard KmnO4 solution.
05. a) Define oxidation and reduction with example . discuss electronic concept.
b) What do you means by Iodimetry and Iodimetry Titration .
06. a) Fe2+ is oxidized by acidic KmnO4 solution.
b) H2S is oxidized by acidic by KmnO4 in dilute H2SO4 solution .
c) KI reacts with K2CrO7 in acid solution .(HCl) .
d) Oxalic acid is oxidized by KmnO4 in acid solution.
e) KI is oxidized by H2SO4 mixed solution of KmnO4.
07. Calculate the oxidation number of underline elements in the following compound:
a) H2SO4 [Ans:5.8] b) Na2S2O3 c) K2Cr2O7
d) H2SO3 e) H3PO3 f) K4[Fe(CN)6]
g) [Fe(CN)6] h) [Cu(NH3)4]2+ I) [Cu(NH3)4]SO4
08. Explain the following :
a) Electron transferred in oxidation- reaction .
b) Electrolysis is a oxidation – reduction reaction.
Problem:
09. Balanced the following equation using half equation method:
a) I2 (s) + S2O32- → I- + S4O62
09. Complete and Balance the following equation ( Write half equation):
a) Cr2O72- + 14 H+ + 6I- → 2C3+ + ? + ?
c) K2Cr2 + H2SO4 +H2S → ?
d) 6Fe2+ + Cr2O72- + 14H+ → 6Fe3+ + 2Cr3+ + 7H2O
e) MnO4- + H+ +C2O42- → Mn2+ H2O + CO2
10. Express the following equation in Redox half equation. Find out the oxidant and Reductant.
a) 6Fe2+ + 14H+ + Cr2O72- → 6Fe3+ + 2Cr3+ + 7H2O
b) 2MnO4- + 16H+ + 5Cr2O42- → 2Mn2+ 8H2O + 10CO2
Short Question:
01. What is Redox reaction ? Give example
02. What is oxidation number.
03. What is oxidation half equation and reduction half equation ? Give example.
04. Fe3+ → Fe2+ By adding electron balance the equation.
05. Determine the oxidation number if Fe and Cu in [Fe(Cu)6]3- and [Cu(NH3)4]2+ ion respectively .
06. Write three differences between valency and oxidation number .
07. Complete the following reaction:
S2O32- + I2 → ? + 2I-
Mathematical Problems:
01. a) A sample of 25 cm3 of H2O2 is oxidized by 15 cm3 of 0.3 M KmnO4 solution in dilute H2SO4. Determine the molar concentration of the sample of H2O2. [ans:0.45M]
b)10 cm3 of a KmnO4 solution is needed to oxidize 25 cm3 of 0.03 M H2O2 in presence of dilute H2SO4 .Determine the molar concentration of KmnO4 solution . [Ans:0.03M]
02. a piece of iron is dissolved in dilute H2SO4. 98.5 (or95)cm3 of 0.02 (or0.01) M KmnO4 solution is needed to oxidized the solution completely. What is the mass of iron piece ?[Ans:0.552 g ]
03. 45.02 (or 27.5) cm3 of 0.03 M KmnO4 or (0.03M K2Cr2O7) solution is needed to oxidized a solution which is obtained when a piece of iron is dissolved in dilute H2SO4 solution .What is the mass of iron piece ?[ans:0.377 g]
04. 1.5 g of iron ore is dissolved in H2SO4 to prepare 100ml solution .22.5ml of 0.02 MKMO4 solution is needed to titrate 25 ml of the solution . Calculate the percentage of iron in the ore. [Fe = 55.85] [Ans:Fe=0.50265 g and 33.5%]
05. What volume of 0.05 M K2Cr2O7 solution will be needed to liberate chlorine will be produced. [Ans:51.00 cm3, 0.728 g]
06. 5 ml of 0.05 M KMnO4 solution is needed to oxidized 0.5 g impure green vitriol. What is the percentage if impurities of green vitriol ?[ans:30.45%]
07. How much ram of pure K2Cr2O7 will be needed to oxidize 10 g of FeSO4.[Ans:3.23 g]
08. How much gram of KMnO4 will be needed to oxidize 2.40 g of FeSO4 in H2SO4 solution ? [Fe=55.85, Mn=54.94, K=39.1] [Ans:0.5 g]
09. 35 ml of0.15 M Na2SO3 solution is needed to titrate the liberated iodine from the reaction of 50 ml of CuSO4 With excess KI solution. Calculate the amount of Cu2+ in the solution . [Ex-7] [Ans:0.333 g Cu2+]
10. A 15 ml solution of 0.3 M KMnO4 mixed with dilute H2SO4 can oxidize 25 ml of H2SO4 solution . Calculate the molar concentration of H2SO4 solution .
11. How much gram of pure K2Cr2O7 will be needed to oxidize 10 gm ferrous sulphate.
Chapter six
Broad Question
01. What os ionic bond ? How it is formed , explain with examples.
02. Define convalent bond. Discuss covalent bond with examples.
03. Explain the structure of co-ordinate covalent bond with examples.
04. a) Compare the characteristics between ionic and covalent bond.
c) Discuss the ionic characteristics of covalent bond and covalent characteristics of ionic bond.]
05. What is metallic bond ? How the metallic bond explain the characteristics of metals ?
06. Define sigma (s) and pie (p) bond . Explain the characteristics of metals ?
07. What is hybridization ? Explain with examples sp sp2 and sp3 hybridization.
08. What do you mean by hydrogen bonding ? Explain it .
09. What is hydrogen bond ? Explain with example how this bond is formed ?
10. Describe the significance of hydrogen in the formation of ice .
11. Write Short Notes
a) Fazan’s rule
b) Covalent characteristics of ionic bond and ionic characteristics of covalent bond. [Ans:6.19, 6.20]
c) Metallic bond
d) Pie bond]
e) Hybridization
f) Delocalization of electrons
g) Hydrogen bond
h) Vander Waal’s force.
i) Sigma Bond.
12. What types of bond are present in the following compounds? Explain with electronic configuration :
a) CaCl2 b) CH4 c) NH3 d) NH4Cl e) [Cu(NH3)4] SO4
f) K3[Fe(CN)6] g) NH4+ h)KF I)K4[Fe(CN)6]
13. Describe the shape of the following compounds: [Ans:6.24]
a) H2O b) CH4 c) CCl4 d) BeCl2 e) XeF2 g) XeF4
Explain the following :
14.At normal temperature, H2S is gas but H2S is liquid. Why ?
16. Explain that sigma and pie bond is covalent bond.
17. NaCl can carry electricity but CCl4 can not .
18. Graphite is a conductor of electricity but diamond is not ?
19. Though ethyl alcohol is an organic compound but soluble in water. Why ?
20. NaCl is soluble in water in kerosene and alcohonl.
21. Though HCl is a covalent compound but solube in water .
22. Carbon and silicon both belongs to group ⅳA but at normal temperature CO2 is gas but silicon is solid. Why ?
23. Though AlF3 is an ionic compound but AlCl3 has string covalent character. Explain.
24.
25. AgF is soluble in water but AgCl is not Soluble, why ?
26. HF is a polar compound: explain
27. Which one is more covalent between CaCl2 and AlCl3 ?
28. Ice floats in water .Why ?
29. Why the angle of ⌊HNH in NH3 is 1070 ?
30. Why BeCl2 atom is linear ?
31. At normal temperature CO2 is gas but SiO2 is solid ?
32. NCl5 doesn’t exits but PCl5 exits? Why?
33. Which one is more ionic between Kcl and CaCl2 ?
34. Which one is more covalent between MgCl2 and AlCl3 and why ?
35. Which one is soluble in water among the halides of silver and why ?
36. The melting point of FeCl2 is grate than that of FeCl3 –Why?
37. HCl is a polar compound_ Explain
Short Question:
01. What is polar compound ? What is dipole .
02. What is the angle present in H2O and NH3 ?
03. What are do you mean by polarization ?
04. What is pie bond ?
05. What is co – ordinate bond ?
06. What is ionic bond ?
07. Why the angle of HOH in H2O is 104.50 ? explain it .
08. What do you mean by delocalized electron ?
Chapter Seven
Board Question
01. What are exothermic and endothermic reactions. Explain with example .
02. Prove that heat of reaction at constant pressure s equal to the change of enthalpy .
03. Describe with explanation and example of Hess’s law of heat summation .
04. Describe an experimental method of determining heat of neutralization of strong acid and strong base.
05. What is standard enthalpy if formation? How enthalpy of reaction can be calculated from enthalpy of formation ?
06. What is heat neutralization ? Heat of neutralization of strong acid and strong base is always constant explain with example.
07. Why the heat of neutralization of NaOH is greater than that of constant value- explain it.
08. Why the heat of neutralization of week acid or week base is less than the constant value ? Explain it.
Short note:
01. a) Heat of neutralization .
b) Heat of solution
c) Hess’s law of heat of summation .
Short Question:
01. What is enthalpy ?
02. What is thermochemical equation ?
03. What is combustion enthalpy ?
04. Express Hess’s law with the help of mathematical equation.
05. What is enthalpy of neutralization ?
Mathematical problems:
01. The heat combustion of CS2, C and S are –1109.17Kjmol-, -394.55 Kj mol and –297.39 Kjmol-1then find the value heat of formation of CS2. [Ans:+119.84 kj mol-1]
02. Standard heat of combustion of Acetic acid , carbon and hydrogen are –871.5 kj/mol-1 and –2/85.85 kj/mol respectively. Calculate the heat of formation of acetic acid . [Ans:-487.2 kj mol-1]
03. Heat of combustion of methane is –890.3 Kj-1. To produce 1335.45 kj heat how much gram of methane is required.
