Important Exam Question Papers are included Unit-wise in the Probable Q&A Section.
In the Probable Q&A Section of CHSE Board test Preparation, unit-wise inclusion of question papers provides important insight into test trends and curriculum covering. Students can study and refresh their understanding of each topic more effectively if questions are organized into units. This strategy allows for more targeted review, assisting students in identifying their strengths and areas for growth. Additionally, unit-specific question papers provide for a more thorough assessment of preparation, allowing students to judge their competency level across different parts of the curriculum. Finally, using unit-specific question papers improves test preparation and builds confidence in attaining success on the CHSE Board Exams.
Topic: Solutions
2/3- Marks important exam questions
1.If 20 gm of NaOH is dissolved in 500 mL of solution. What is the normality.
2.Define Molality of a solution. What is the effect of temperature on Molality?
3.What are the factors on which the solubility of a gas in liquid depends?
4.Define vapour pressure of a liquid. What is the SI unit?
5.What are the characteristics of ideal solutions?
6.Define a non-ideal solution.
7.State and Explain Roult’s Law.
8.Define colligative properties of a solution. Give examples.
9.What is depression of freezing point? How to find out molecular mass of solute using?
10.Define osmosis. How it differs from diffusion?
11.Derive Vant-Hoff’s equation for dilute solution.
7 Mark questions
1.Explain the effect on the boiling point and freezing point when non-volatile solute is dissolved in a solvent.
2.State Roult’s law. Derive its mathematical expression for a solution of a non-volatile solute in a volatile solvent.
3.What is Vant-Hoff factor? How it helps in the determination of degree of dissociation.
Topic- Electrochemistry
2 / 3 Mark important exam questions
1.What is the use of salt bridge in galvanic cell?
2.Define electrode potential.
3.State and explain Kohlrausch’s law.
4.State and explain Faraday’s laws of electrolysis.
5.Differentiate between fuel cell and batteries.
6.What are the different types of fuel cells.
7.Give the relationship between equivalent conductance and molar conductance of a given solution.
Topic-Chemical Kinetics
2/3-Marks important exam questions
1.Define rate of reaction write its unit.
2.Define order and molecularity with examples.
3.Define activation energy. Explain with diagram.
4.Derive the relation between rate constant and half-life of a first order reaction.
5.The half-life period of a first order reaction is 100 sec. What is the rate constant?
6.What are the differences between order and molecularity with example?
7.Define effective collision.
8.What is zero order reaction give one example?
9.What is Threshold and Activation energy? Explain with examples.
10.What is the effect of temperature on rate of reaction?
Long Questions
1.Derive an expression for the rate constant of a first order reaction. What is the relation between half-life and rate constant?
2.Derive an expression for zero order rates constant. Derive an expression for half-life of a zero-order reaction.
3.(a) Difference between order and molecularity with example.
(b) Derive Arrhenius equation of reaction rate.
d and f – block elements
2/3- marks important exam question:
1.How do your account for the variable oxide on state of transition elements?
2.Why transition metal compounds are colored?
3.Silver atom has completely filled outermost orbit in its ground state. Why it is a transition element?
4.How would you account for the irregular variation of ionization enthalpy is in the first- row transition series?
5.Why is the highest oxidation state of a metal exhibited in its Oxides or Fluorides? Why?
6.What are the Oxidation states exhibited by Lanthanoids?
7.Lanthanides have variable oxidation state. Why?
8.The enthalpies of atomization of the transition metals are high.
9.The ‘d’ configuration in very unstable. Explain.
11.What is Lanthanide contraction?
10.What is meant by disproportionation of an oxidation state? Give an example.
Long Questions
1.Define Transition element. Discuss three Characteristics of transition element.
2.(a)Why the transition metal form compose compound?
(b)What is Effective atomic number rule?
(c)What are interstitial compounds?
3.Give reasons of the following:
(i)The lowest oxide of transition metal is basic whereas the highest oxide is. amphoteric or acidic.
(ii)The highest oxidation is exhibited in oxo-anions of a metal.
(iii)The generally the transition metal compound are colored.
Haloalkanes and Haloarenes
2/ 3- Mark important exam Questions:
1.How can you prepare diethyl ether from ethyl chloride? Give equation.
2.What happens when silver acetate is treated with bromine? Give equation.
3.Explain, why alkyl halide of lower alkane when treated with metallic sodium give higher alkanes?
4.Convert Toluene to benzyl alcohol.
5.How can you convert aniline to chlorobenzene?
6.How will you distinguish between benzyl bromide and p-bromotoluene?
7.Explain, chlorine present in chlorobenzene is ortho and para –directing.
8.How can you convert Benzene to 4 – Bromonitrobenzene?
9.Complete the reaction:
Long Questions
1.How can you prepare chlorobenzene from
(a)benzene diazonium chloride
(b)benzene
What happens when chlorobenzene reacts with
(a)aq. NaOH at 3000C under pressure
(b)Cl2 in presence of Anhydrous FeCl3
2.Write state notes on
(a)Wurtz – Filtig reaction
(b)Ullaman reaction
3.Bring about the following conversion.
(i)Methane to Methyl cyanide
(ii)Ethane to Ethyl alcohol
(iii)Methyl alcohol to Acetic acid
4.Give two examples for the electrophilic substitution in chlorobenzene. Also write the mechanism of reaction.
Alcohols, Phenols & Ethers
Two- or Three-Mark Questions:
1.Write the equations, what happens when ethyl alcohol vapour is passed over reduced copper at 3000C.
2.Explain, why ethanol is less acidic than phenol?
3.What is Reimer –Tiemann Reaction?
4.Explain acidity of Phenol. How substituents affect acidity of phenol.
5.Convert phenol to picric acid.
6.Predict the product A and B:
Long Questions:
1.How can you distinguish between 10, 20 and 30 alcohol by oxidation method?
2.(a) Write down the preparation of ethyl alcohol from ethylene.
(b)What happens when ethyl alcohol is heated with (i) iodine/NaOH (ii) PCl5 (iii) CH3COOH
3.Describe the preparation of phenol from benzene sulphonic acid. How phenol reacts with?
- Sulphuric acid (conc.)
- HNO3
- CH3Cl in presence of AlCl3
Aldehyde, Ketones & Carboxylic acid
Two/Three Mark Question
1.Discuss Reimer – Tiemann reactions.
2.Write the uses of Benzoic acid.
3.What is Cannizzaros reaction?
4.Discuss Iodoform recation.
5.What happens when benzaldehyde is treated with Fehling solution and why?
6.Give two test to distinguish between HCOOH & CH3COOH.
7.Why aldehyde are more reactive than ketone?
8.Explain Clemmension’s reduction with examples.
9.Convert Benzene to Benzoic acid.
10.How Benzoic acid converted to Benzaldehyde?
11.How benzoic acid is prepared (any three)?
12.Discuss Etard’s reaction.
13.How tert. Butyl alcohol is prepared from CH3COOH?
14.What happens when CH3CHO react with iodine in dil. NaOH. Give equation.
15.How will you prepare phenyl hydrazone of acetone? Indicate with equations.
16.Ol is Why Methanal is a gas but Methan It is necessary to control the PH of medium during the reaction of aldehyde and ketone with Ammonia derivative. Explain.
LONG QUESTIONS
1.An organic compound (A) molecular formula C8H16O2 was hydrolyzed with dil. H2SO4 to a give Carboxylic acid (B) and on alcohol (C) oxidation of ‘C’ with Chromic acid produce (B). (C) On hydration gives butene. Write the equation for the reaction involved.
2.Compound A(C6H12O2) on reduction with LiAlH4 yielded two compounds ‘B’ and ‘C’. The compound ‘B’ an oxidation gave ‘D’ which when treated with aqueous alkali and subsequent
3.Discuss the reaction used to distinguish between Aldehyde & Ketone. Write the order of reactivity of HCHO, CH3CHO, CH3COCH3.
4.What happens when
(a)Acetyl chloride treated with H2 in presence of Pd/BaSO4
(b)Mixture of Calcium acetate and Calcium formate is heated
(c)Propyne treated with dil. H2SO4 in presence of HgSO4
(d)HCHO treated with NH3.
5.Discuss the following Name reaction
(a)Rosenmond reduction
(b)Stephen reduction
(c)Clemmenson’s reduction
(d)Wolf-kishner reduction
(e)HVZ reaction
(f)Kolbe’s reaction
(g)Schmidt reaction
Physics Important Exam Questions:
7 Mark Questions
All topics
(i) Define an electric dipole.
(ii) Define an electric dipole moment.
(iii) Derive an expression for electric field intensity at a point due
due to an electric dipole.
(a)an axial line.
(b)an equatorial line.
- Derive the laws for connection:
(a)In Series
(b)In Parallel
- (i)What is Capacitance?
(ii)Define derive an expression for capacity of a parallel plate capacitor.
(iii)What happens to the capacity if dielectric is taken between the plates?
4.(i)State Biot Savart’s law.
(ii)State Ampere’s law.
(iii)Derive an expression for magnetic field intensity at a point due to along
Straight conductor carrying current by using Biot Savart’s law/Ampere’s Law.
5.State Kirchoff’s laws of electric network. Derive the condition for balance in
Whitestone bridge.
6.Write an expression for energy stored in a capacitor. Also find its energy Density.
7.Derive an expression for a charge in an uniform magnetic field also found
It’s fire rotation, time period and radius of path.
8.What is a cycloform? Derive for it’s frequency and explain the Biot Savart law.
9.Derive and expression for magnetic field due to a straight carrying conductor.
Also find an expression for an infinite conductor.
- derive an expression for torque and a current loop when a magnetic field is in
the place of the laws?
11.Explain principal construction working of an A.C generated?
- Discuss Gauss’s law and apply it to calculate the electric field due to various charge distributions, including point charges, charged conductors, and infinite planes.
- Explain the concept of electric potential and derive expressions for the electric potential due to point charges and charged conductors.
14.Describe the behaviour of capacitors in circuits, including their charging and discharging processes, energy stored, and time constants.
14.Discuss the first and second laws of thermodynamics and apply them to analyse heat engines, refrigerators, and heat pumps.
15.Explain the concept of entropy and discuss its significance in thermodynamic processes, including reversible and irreversible processes.
16.Analyze the behaviour of ideal gases using the kinetic theory of gases, including the derivation of the ideal gas law and its applications.
17.Explain the properties of waves, including wavelength, frequency, amplitude, and wave velocity.
18.Discuss wave interference, diffraction, and polarization.
19.Describe the behaviour of light, including reflection, refraction, and the formation of images by mirrors and lenses.
20.Discuss the theory of special relativity, including time dilation, length contraction, and the relativistic addition of velocities.
21.Explain the basic principles of quantum mechanics, including the wave-particle duality of matter and the uncertainty principle.
22.Describe the structure of the atom, including the Bohr model and the quantum mechanical model, and discuss atomic spectra and transitions.
2 Mark Question
ALL TOPICS
1.State Ohm’s law.
2.Define electric potential.
3.State Fleming’s left-hand rule.
4.Define magnetic field strength.
5.Define capacitance.
6.Define specific heat capacity.
7.State the first law of thermodynamics.
8.Define adiabatic process.
9.Define entropy.
10.State the zeroth law of thermodynamics
11.Define frequency.
12.State Huygen’s principle.
13.Define critical angle.
14.State the law of reflection.
15.Define diffraction.
16.Define photon.
17.State Planck’s quantum theory.
18.Define radioactive decay.
19.Define half-life.
20.Define photoelectric effect.
3 Mark Questions
ALL TOPICS
1.Calculate the resistance of a wire if a current of 2 A flows through it when a voltage of 12 V is applied.
2.Explain the difference between series and parallel circuits.
3.State Gauss’s law and its application to find the electric field due to a point charge.
4.Calculate the force experienced by a charged particle of charge 5 μC placed in an electric field of intensity 100 N/C.
5.Define magnetic flux and Faraday’s law of electromagnetic induction.
6.Calculate the change in internal energy of a gas if 100 J of heat is added to it, and 50 J of work is done on it.
7.Explain the difference between isothermal and adiabatic processes.
8.Define entropy and discuss its relation to the second law of thermodynamics.
9.Calculate the efficiency of a heat engine operating between temperatures of 500 K and 300 K.
10.Define specific heat capacity and its relation to heat transfer.
11.Calculate the frequency of a wave with a wavelength of 0.2 m traveling at a speed of 300 m/s.
12.Explain the difference between constructive and destructive interference.
13.Calculate the angle of refraction when light passes from air into water, given the angle of incidence is 30 degrees.
14.Define polarization and discuss its significance in optics.
15.Calculate the focal length of a converging lens with a refractive index of 1.5 and a radius of curvature of 0.1 m.
16.Explain the concept of quantization of energy in quantum theory.
17.Calculate the de Broglie wavelength of an electron with a kinetic energy of 100 eV.
18.State Heisenberg’s uncertainty principle and discuss its implications.
19.Define the terms alpha decay, beta decay, and gamma decay.
20.Calculate the energy released in a nuclear reaction if the mass defect is 0.02 atomic mass units.
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