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Question Paper - Chemistry 2014 - 2015-H.S.C-12th Board Exam Maharashtra State Board (MSBSHSE)

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Marks: 70
Q: 1 | Select and write the most appropriate answer from the given alternatives for each sub-question [7]
Q: 1.1[1]

p - type semi-conductors are made by mixing silicon with impurities of-

  1. germanium
  2. boron
  3. arsenic  
  4. antimony
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Q: 1.2[1]

Amongst the following identify the criterion for a process to be at equilibrium -

  1. ΔG < 0
  2. ΔG > 0
  3. ΔStotal=0
  4. ΔS < 0
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Q: 1.3[1]

Colligative property depends only on ........................ in a solution.

  1. Number of solute particles.
  2. Number of solvent particles.
  3. Nature of solute particles.
  4. Nature of solvent particles.
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Q: 1.4[1]

The charge of how many coulomb is required to deposit 1.0 g of sodium metal (molar mass 23.0 g mol-1) from sodium ions is -

  1. 2098
  2. 96500
  3. 193000
  4. 4196
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Q: 1.5[1]

What is the chemical composition of malachite?

  1. CuO . CuC03
  2. Cu(OH)2 CuC03
  3. CuO.Cu(OH)2         
  4. Cu2O . Cu(OH)2
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Q: 1.6[1]

The element that does NOT exhibit allotropy is

  1. As
  2. Sb
  3. Bi
  4. N
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Q: 1.7[1]

The integrated rate equation for first order reaction is A → products

(a) ``

(b) `k=-1/tl_n[A]_t/[A]_0`

(c) `k=2.303/t log_10 ([A]_t/[A]_0 )`

(d) `k=l/tl_n[A]_t/[A]_0`

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Q: 2 | Answer any SIX of the following [12]
Q: 2.1[2]

Define the Enthalpy of fusion

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Define the Enthalpy of atomization

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Q: 2.2[2]

Derive van’t Hoff general solution equation

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Q: 2.3[2]

Explain impurity defect in stainless steel with diagram

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Q: 2.4[2]

Derive the relation between half life and rate constant for a first order reaction

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Q: 2.5[2]

Draw neat and labelled diagram of dry cell.

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Q: 2.6[2]

Explain the structure of sulphur dioxide.

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Q: 2.7[2]

What is calcination?

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Explain calcination with reactions.

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Q: 2.8[2]

Arrange the following reducing agents in the order of increasing strength under standard state conditions. Justify the answer 

Element

Al(s)

Cu(s)

Cl(aq)

Ni(s)

 

Eo

-1.66V

0.34V

1.36V

-0.26V

 

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Q: 3 |  Answer any THREE of the following [9]
Q: 3.1[3]

Determine whether the reactions with the following ΔH and ΔS values are spontaneous or non-spontaneous. State whether the reactions are exothermic or endothermic.

(a) ΔH = -110kJ, ΔS = + 40JK-1 at 400 K

(b) ΔH = + 40kJ, ΔS = -120JK-1 at 250K

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Q: 3.2[3]

1.0 x10-3Kg of urea when dissolved in 0.0985 Kg of a solvent, decreases freezing point of the solvent by 0.211 k.

1.6x10 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. (Given molar mass of urea = 60)

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Q: 3.3[3]

Sucrose decomposes in acid solution into glucose and fructose according to the first order rate law with t1/2= 3 hours. What fraction of the sample of sucrose remains after 8 hours?

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Q: 3.4[3]

Explain how does nitrogen exhibit anomalous behaviour amongst group 15 elements.

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Q: 4 | Answer any one of the following :[7]
Q: 4.1[7]

Niobium crystallises as body centred cube (BCC) and has density of 8.55 Kg / dm-3 . Calculate the attomic radius of niobium.

(Given : Atomic mass of niobium = 93).

 

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Write one statement of first law of thermodyamics and its mathematical expression.

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Write the reactions involved in th'e zone of reduction in blast furnace during extraction of iron.

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Q: 4.2[7]

Write molecular formulae and structures of Dithionic acid

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Write molecular formulae and structures of the Peroxy monosulphuric acid

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Write molecular formulae and structures of the Pyrosulphuric acid 

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Write molecular formulae and structures of the Dithionous acid

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Calculate E and AG for the following at 28°C:

Mg(s) + Sn2+(0.04M) → Mg2+(0.06M) + Sn(s)

Ecell = 2.23V

Is the reaction spontaneous?

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Q: 5 | Select and write the most appropriate answers from the given alternatives for each sub-question [7]
Q: 5.1[1]

Identify the product ‘D’ in the following sequence of reactions:

`H3C-CH2-CH2-Cl (Alc)/(KOH)'B'(HBr)/()'C'(Na)/(Ether)’D'`

  1. 2,2 - dimethyl butane  
  2. 2,3- dimethylbutane
  3. hexane                           
  4. 2,4 - dimethylpentane
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Q: 5.2[1]

Which of the following complexes will give a white precipitate on treatment with a solution of barium nitrate?

  1. [Cr(NH3)4SO4] Cl
  2. [Co(NH3)4Cl2] NO2
  3. [Cr(NH3)4Cl2]SO4
  4. [CrCl2(H2O)4]Cl
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Q: 5.3[1]

What is the geometry of chromate ion?

  1. Tetrahedral                    
  2. Octahedral
  3. Trigonal planer              
  4. Linear
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Q: 5.4[1]

Primary and secondary nitroalcanes containing α - H atom show property of -

  1. chain isomerism
  2. tautomerism
  3. optical isomerism
  4. geometrical isomerism
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Q: 5.5[1]

In phenol carbon atom attached to -OH group undergoes -

  1. SP3 hybridisation          
  2. SP hybridisation
  3. SP2 hybridisation
  4. No hybridisation
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Q: 5.6[1]

Identify the strongest acid amongst the followings:

  1. Chloroacetic acid          
  2. Acetic acid
  3. Trichloroacetic acid
  4. Dichloroaceticacid
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Q: 5.7[1]

Which of the following vitamins is water soluble?

  1. A
  2. D
  3. E
  4. B
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Q: 6 | Answer any SIX of the following :[12]
Q: 6.1[2]

Write a note on Friedel Craft’s acylation.

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Q: 6.2[2]

How is ethyl amine prepared from methyl iodide?

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Q: 6.3[2]

What are antibiotics? Give ‘two’ examples

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Q: 6.4[2]

Explain, why are boiling points of carboxylic acids higher than corresponding alcohols

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Q: 6.5[2]

How are proteins classified on the basis of molecular shapes?

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Q: 6.6[2]

Explain Interstitial compounds

What are interstitial compounds?

What are interstitial compounds? Why are such compounds well known for transition metals?

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Why do interstitial compounds have higher melting points than corresponding pure metals?

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Q: 6.7[2]

Write the structures and IUPAC names of the :Adipic acid compound

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Write the structures and IUPAC names of the α - methyl butyraldehyde.

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Q: 6.8[2]

Explain with examples, branched and linear polymers.

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Q: 7 | Answer any THREE of the following :[9]
Q: 7.1[3]

On the basis of valence bond theory explain the nature of bonding in [CoF6]3 ion.

 

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Write the IUPAC name of [Co(N02)3(NH3)3].

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Q: 7.2[3]

Define lanthanoid contraction. Explain its effects.

What is lanthanoid contraction? What are the consequences of lanthanoid contraction?

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Q: 7.3[3]

Write mechanism of Aldol addition reaction.

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Q: 7.4[3]

Define carbohydrates.

What are carbohydrates?

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What are reducing and non-reducing sugars?

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Q: 8 | Answer any ONE of the following [7]
Q: 8.1[7]

Write a note on Gabriel phthalimide synthesis.

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What are biodegradable polymers and non-biodegradable polymers? Write ‘one example’ of each.

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Explain cationic detergents.

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Q: 8.2[7]

How is carbolic acid prepared from the following compounds :

(1) Aniline

(2) Chlorobenzene and steam at 698K?

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Draw structure of DDT. Write its environmental effects

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Mention ‘two’ physical properties of carbolic acid.

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