Chemistry
Chemistry HSC Maharastra Board Multiple Choice Question With Answer
1) The following types of solids contain molecules as constituent particles?
A) Molecular solidsB) Lonic solidsC) Metallic solidsD) Covalent network solids
Ans : Molecular solids
2) The following crystal systems contain 4 Bravais lattices?
A) CubicB) TetragonalC) OrthorhombicD) Monoclinic
Ans : Orthorhombic
3) An octahedral void is surrounded by ________.
A) 4 spheresB) 3 spheresC) 8 spheresD) 6 spheres
Ans : 6 spheres
4) Which of the following is an amorphous solid?
A) Copper sulphateB) MagnesiumC) TarD) Diamond
Ans : Tar
5) A paired cation-anion vacancy is called _______.
A) Schottky defectB) Frenkel defectC) Impurity defectD) Vacancy defect
Ans : Schottky defect
6) The unit cell of a simple cubic system has atoms at the eight corners. Hence, number of atoms in a unit cell is ______.
A) 8B) 3C) 1D) 2
Ans : 1
7) In crystal lattice formed by primitive unit cell, the space occupied by particles is ______.
A) 47.6%B) 52.4%C) 32%D) 68%
Ans : 52.4%
8) The coordination number of spheres in hcp lattice in three dimension is ______.
A) 2B) 6C) 4D) 12
Ans : 6
9) A compound is made up of two elements X and Y and crystallizes in bcc structure. Atoms of X are present at the corners of the cube. Atoms of Y are present at the centre of the cube. The formula of the compound is ______.
A) X2YB) XYC) XY2D) X2Y3
Ans : XY
10) Sodium crystallizes in bcc structure. If the edge length of unit cell is 4.3 × 10-8 cm, the radius of Na atom is ______.
A) 1.86 × 10-8 cmB) 1.52 × 10-8 cmC) 2.15 × 10-8 cmD) 4.3 × 10-8 cm
Ans : 1.86 × 10-8 cm
11) Sugar dissolves in water because ______.
A) Sugar is nonpolarB) Water is polarC) It forms hydrogen bonding with waterD) Sugar and water are both polar
Ans : It forms hydrogen bonding with water
12) The solubility of a gas in water ______.
A) Decreases with increase in temperatureB) Increases with increase in temperatureC) Decreases with decrease in temperatureD) Is not affected by temperature
Ans : Decreases with increase in temperature
13) The units of Henry’s law constant are ______.
A) Bar dm3 mol–1B) Mol L–1 bar–1C) L mol–1 bar–1D) Bar L–1 mol–1
Ans : Mol L–1 bar–1
14) The colligative properties of solutions _______.
A) Depend on nature of solute particlesB) Do not depend on number of solute particlesC) Do not depend on dissociation of solute in solventD) Depend on number of solute particles
Ans : Depend on number of solute particles
15) The following solution/solvent has maximum vapour pressure _______.
A) 1 M copper sulphate solutionB) Pure solvent waterC) 0.5 M copper sulphate solutionD) 2 M copper sulphate solution
Ans : Pure solvent water
16) According to Raoult’s law, relative lowering of vapour pressure of solution containing dissolved nonvolatile solute _______.
A) Is equal to mole fraction of solventB) Is equal to mole fraction of soluteC) Does not depend on mole fraction of soluteD) Is equal to molality of solution
Ans : Is equal to mole fraction of solute
17) Freezing point depression constant of a solvent is _______.
A) Inversely proportional to molality of solutionB) Directly proportional to molarity of solutionC) Dependent on molality of solutionD) Xpressed in K kg mol–1
Ans : Xpressed in K kg mol–1
18) The theory which explain amphoteric nature of water is ______.
A) Arrhenius theoryB) Lewis theoryC) Ostwald theoryD) Bronsted-Lowry theory
Ans : Bronsted-Lowry theory
19) An intensive property amongst the following is ______.
A) MassB) VolumeC) Number of molesD) Temperature
Ans : Temperature
20) The value of 1dm3 bar is ______.
A) 10 JB) 102 JC) 103 JD) 10-2 J
Ans : 102 J
21) The work done in the dm3 bar when 200 mL of ethylene gas and 150 mL of HCl gas were allowed to react at 1 bar pressure is ______.
A) 0.10B) 0.15C) 0.20D) 0.2
Ans : 0.15
22) The work done in vacuum when 300 m mole of an ideal gas expands until its volume is increased by 2.3 dm3 at 1 bar pressure is ______ mole.
A) ZeroB) OneC) TwoD) Three
Ans : Zero
23) For an Isothermal process
A) W = - QB) ∆U = WC) ∆U = Q + WD) ∆U = Q
Ans : W = - Q
24) For an Isochoric process
A) ∆U = 0B) ∆V = 0C) ∆P = 0D) Q = 0
Ans : ∆V = 0
25) Kohlrausch law is applicable for the solution _______.
A) At infinite dilutionB) A concentrated solutionC) Concentrated as well as dilute solutionD) Aqueous solution
Ans : At infinite dilution
26) SI unit of conductivity is _______.
A) Ω-1 m-1B) Ω cm-1C) Ω m-1D) Ω-1 m2 mol-1
Ans : Ω-1 m-1
27) In construction of Standard Hydrogen Electrode, platinum acts as ______.
A) Inert electrodeB) Positive ion producing electrodeC) Negative ion producing electrodeD) Null electrode
Ans : Inert electrode
28) When molten ionic compound is electrolyzed, a metal is formed at _______.
A) Negative electrodeB) Positive electrodeC) Salt bridgeD) Electrolyte
Ans : Negative electrode
29) A First order reaction is 50% complete in 69.3 minutes. Time required for 90% completion for the same reaction is _______.
A) 230.3 minB) 100 minC) 230 minD) 125 min
Ans : 230.3 min
30) Rate constant of a reaction is 3.6 × 10–3 s–1. The order of reaction is ______.
A) FirstB) SecondC) ThirdD) Zero
Ans : First
32) The rate law relates to the rate of a chemical reaction in terms of _______.
A) Concentration of catalystB) TemperatureC) Potential energyD) Mol/L of reactants
Ans : Mol/L of reactants
33) Order of reaction for which unit of rate constant is mol dm–3 s–1 is _______.
A) 1B) 3C) 0D) 2
Ans : 0
34) The rate of catalysed reaction is large than the uncatalysed reaction as _______.
A) Ea is largerB) Ea is lowerC) Ea is sameD) Threshold energy is absent
Ans : Ea is lower
35) Effect of catalyst in a chemical reaction is to change the _______.
A) Activation energyB) Equilibrium concentrationC) Final productsD) Heat of a reaction
Ans : Activation energy
36) In chlorous acid, oxidation state of chlorine is _______.
A) +2B) +4C) +3D) +7
Ans : +3
37) Acidic strength of halogen acids increases in the order of _______.
A) HF > HCl > HBr > HIB) HCl > HF > HBr > HIC) HBr > HCl > HF > HID) HI > HBr > HCl > HF
Ans : HI > HBr > HCl > HF
38) Sulfur dioxide reacts with sodium hydroxide solution to form _______.
A) Sodium sulfiteB) Sodium sulfateC) Sodium hydrogen sulfiteD) Sodium hydrogen sulfate
Ans : Sodium sulfite
39) The gas evolved when sulfuric acid reacts with copper metal _______.
A) Sulfur dioxideB) Sulfur trioxideC) Nitrogen dioxideD) Nitrogen trioxide
Ans : Sulfur dioxide
40) Hot and concentrated alkali NaOH reacts with chlorine to form _______.
A) Only chlorateB) Only hypochloriteC) Chloride and chlorateD) Chloride and hypochlorite
Ans : Chloride and chlorate
41) When SO2 is passed through an aqueous solution of I2, the solution becomes _______.
A) Ruby redB) ColourlessC) VioletD) Yellowish green
Ans : Colourless
42) O2 molecule is ______.
A) FerromagneticB) DiamagneticC) ParamagneticD) Ferrimagnetic
Ans : Paramagnetic
43) The number of covalent bonds present in sulfuric acid:
A) 4B) 6C) 8D) 2
Ans : 6
44) In interhalogen compounds, which of the following halogens is never the central atom?
A) IB) ClC) BrD) F
Ans : F
45) Transition elements have more tendency to form interstitial compounds because _______.
A) Of defect in their crystal latticeB) They have reducing propertyC) They have low ionization enthalpyD) They have same atomic size
Ans : Of defect in their crystal lattice
46) Zinc does NOT show variable valency because of ______.
A) Complete 4s subshellB) Complete d subshellC) Incomplete d subshellD) Incomplete S subshell
Ans : Complete d subshell
47) The atomic number of transuranium elements starts from _______.
A) 89 – 103B) 90 – 103C) 91 – 103D) 93 – 103
Ans : 93 – 103
48) The following pair of elements has half-filled d-orbitals.
A) Chromium and cobaltB) Manganese and nickelC) Chromium and manganeseD) Cobalt and nickel
Ans : Chromium and manganese
49) Amongst the following, the ambidentate ligand is ____________
A) Ethylene diamineB) Oxalate ionC) Chloride ionD) Cyanide ion
Ans : Cyanide ion
50) The IUPAC name of Na3[AlF6] is _____________
A) Hexa fluorosodiumaluminateB) Sodium hexafluoroaluminate(III)C) Sodium hexafluoroaluminate(II)D) Sodium hexafluoroaluminium(III)
Ans : Sodium hexafluoroaluminate(III)