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After tremendous success of our last year Important Questions Bank for Maharashtra HSC Board Exam 2016, we have also created a list of Most Important Questions Bank for Maharashtra HSC Board Exam 2017 which are likely to appear in HSC Board Exams this year.
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Chemistry Important Question Bank 2017
Q1 Write the structural formula and IUPAC names of all possible isomers of the compounds with molecular formula C3 H8 O.
Write ‘two’ uses of phenol.
What happens when glucose is treated with –
(a) Bromine water
(b) Dilute nitric acid
(c) Hydrogen cyanide (HCN)
Q2 What is the action of the following reagents on aniline?
(a) Bromine water
(b) Acetic anhydride
( C ) Hot and conc. Sulphuric acid
Q3. What is ‘boiling Point’?
Derive a relation between ΔH and ΔU for a chemical reaction. Draw neat labeled diagram of calomel electrode. Resistance and conductivity of a cell containing 0.001 M KCL solution at 298K are 1500Ω and 1.46 x 10 -4 S.cm -1 respectively. What is the cell constant?
Q 4. Distinguish between crystalline solid and amorphous solid.
Q5. (a) Explain with reason sign conventions of ΔS in the following reactions:
- N2(g) + 3H2(g) → 2NH3(g)
- CO2(g) → CO2(g)
(b). Explain the following terms:
( c ) Gold occurs as face centered cube and has a density of 19.30 Kg dm -3. Calculate atomic radius of gold. (Molar mass of Au = 197)
Q6. (I) write a short note on Hoffmann bromamide degradation.
(II) Explain the mechanism of action of hydroiodic acid on 3-methylbutan-2-ol.
(III) Mention ‘two’ uses of propan-2-one.
Q7. Write the different oxidation states of manganese. Why + 2 oxidation state of manganese is more stable?
Q8. Define antioxidants and mention two examples.
Q9. Calculate the mole fraction and molality of HNO3 in a solution containing 12.2 % HNO3. (Give – atomic masses: H = 1, N = 14, O = 16)
Q10. Face centered cubic crystal lattice of copper has density of 8.966 g. cm -3. Calculate the volume of the unit cell. Given molar mass of copper is 63.5 g.mol -1 and Avogadro number NA is 6.022 x 10 23 mol -1.
Q11. State the first and second law of electrolysis.
Q12. 1.0 x 10 -3 Kg of urea when dissolved in 0.0985 Kg of a solvent, decreases freezing point of the solvent by 0.211 K. 1.6 x 10 -3 kg of another non – electrolyte solute when dissolved in 0.086 Kg of the same solvent depresses the freezing point by 0.34 K. Calculate the molar mass of the another solute. (Give molar mass of urea = 60)
Q13. Calculate E cell and ΔG for the following at 28˚C: Mg(s) + Sn 2+ (0.04M) → Mg 2+ (0.06M) → Sn(s) E˚cell = 2.23 V. Is the reaction spontaneous?
Q14. How is carbolic acid prepared from the following compounds:
II] Chlorobenzene and steam at 698K?
Draw structure of DDT. Write its environmental effects.
Q15. A liquid rises to a height of 5 cm in a glass capillary of radius 0.02 cm. what will be the height of the same liquid in a glass capillary of radius 0.04 cm?
Q16. State any ‘six’ assumptions on which the kinetic theory of glass is based. Define three moduli of elasticity. State their formulae. State Kirchhoff’s law of radiation and prove its theoretically.
Q17. The period of simple pendulum is found to increase by 50% when the length of the pendulum is increased by 0.6 m. calculate the initial length and initial period of oscillation at a place where g = 9.8 m/s2
Q18. An object of mass 2 kg attached to a wire of length 5 m is revolved in a horizontal circle. If it makes 60 r.p.m. find its (a) angular speed, (b) linear speed, (c) centripetal acceleration, (d) centripetal force.
Q19. Describe how an artificial satellite is launched in an orbit around the earth. Explain the nature of all the possible orbits of a satellite with the help of a suitable diagram.
Q20. A heated metal ball is placed in cooler surroundings. Its rate of cooling is 2˚C per minute. When its temperature is 60˚C and 1.2˚C per minute when its temperature is 52˚C. determine the temperature of the surroundings and the rate of cooling when the temperature of the ball is 48˚C. Also find the temperature at which, rate of cooling is 0.6 ˚C per minute.
Q21. Which specific heat of a gas is greater? Why?
Q22. In a Melde’s experiment when 6 gram weights are added to pan, the number of loops in 5 and when 10.5 gram weight are added to the pan, the number of loop is 4. Find the number of loops when there are no weight in that pan.
Q23. Write the following methods to protect metals from corrosion:
A] Galvanization b] Passivation
Q24. Define cell constant. Draw a neat and well labeled diagram of primary reference electrode.
Q 25. Calculate C-Cl bond enthalpy from following reaction:
CH3Cl(g) + Cl2(g) → CH2Cl2(g) + HCl(g) ΔH˚ = – 104 KJ
If C-H, Cl – Cl and H-Cl bond enthalpies are 414. 243 and 431 KJ-Mol-1 respectively
Q26. Write four points of difference between properties of nitrogen and other elements of group 15.
Explain the structure of CIF3
Conductivity of a solution is 6.23 x 10-5Ω -1 cm -1 and its resistance is 13710Ω. If the electrodes are 0.7cm apart, calculate the cross sectional area of electrode.
Why is molatity of a solution independent of temperature?
Q 27. What is the action of dioxygen on – a] Calcium b] Iron c] Carbon disulphide?
Q28. What is the effect of temperature on solubility of a gas in a liquid?
Explain refining of nickel by Mond process.
State kohlrausch’s law of independent migration of ions.
Silver crystallizes in F.C.C. (face- centred cubic crystal) structure. The edge length of the unit cell is found to be 408.7 pm. Calculate density of the unite cell.[Give: Molar mass of sliver is 108 g.mol -1]
Q29. What is the hybridization of carbon atom in diamond and graphite? 0.1 mole of buckminsterfullerene contains how many kg of carbon? [Atomic mass of carbon = 12]
Q 30. Draw structures of (A) chlorine trifluoride (B) chlorine pentafluoride.
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