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Some Basic Concepts Of Chemistry Class 11 MCQs Questions with Answers
Calculate the number of oxygen atoms in 50 g of CaCO3
(a) 6.033×1023 atoms
(b) 9.033×1023 atoms
(c) 8.033×1023 atoms
(d) 3.033×1023 atoms
Answer: (b) 9.033×1023 atoms
Which of the following pairs have the same number of atoms?
(a) 16 g of O2(g) and 4 g of H2(g)
(b) 16 g of O2 and 44 g of CO2
(c) 28 g of N2 and 32 g of O2
(d) 12 g of C(s) and 25 g of Na(s)
Answer: (c) 28 g of N2 and 32 g of O2
Which of the following statements about a compound is incorrect?
(a) A molecule of a compound has atoms of different elements.
(b) A compound cannot be separated into its constituent elements by physical methods of separation.
(c) A compound retains the physical properties of its constituent elements.
(d) The ratio of atoms of different elements in a compound is fixed
Answer: (c) A compound retains the physical properties of its constituent elements.
How many mL of water must be added to 200 mL of .65 M HCL to dilute the solution to .20 M
(a) 450 mL
(b) 400 mL
(c) 350 mL
(d) 500 mL
Answer: (a) 450 mL
Which of the following has the largest number of atoms
(a) 0.5 g-atoms of Cu
(b) 0.635 g Cu
(c) 0.25 moles of Cu atoms
(d) 1g of Cu
Answer: (a) 0.5 g-atoms of Cu
A measured temperature on Fahrenheit scale is 200°F. What will this reading be on Celsius scale?
(a) 40°C
(b) 94°C
(c) 93.3°C
(d) 30°C
Answer: (c) 93.3°C
Which of the following reactions is not correct according to the law of conservation of mass
(a) 2Mg(s)+O2(g)→2MgO(s)
(b) C3H8(g)+O2(g)→CO2(g)+H2O(g)
(c) P4(s)+5O2(g)→P4O10(s)P4(s)+5O2(g)→P4O10(s)
(d) CH4(g)+2O2(g)→CO2(g)+2H2O(g)
Answer: (b) C3H8(g)+O2(g)→CO2(g)+H2O(g)
The number of gram molecules of oxygen in 6.02×1024 CO molecules is
(a) 10 gm-molecules
(b) 5 gm-molecules
(c) 1 gm -molecules
(d) .5 gm-molecules
Answer: (b) 5 gm-molecules
The number of significant figures for the three numbers 161 cm, 0.161 cm, 0.0161 cm are
(a) 3,3 and 3 respectively
(b) 3,4 and 4 respectively
(c) 3,4 and 5 respectively
(d) 3,3 and 4 respectively
Answer: (a) 3,3 and 3 respectively
Calculate the standard molar volume of oxygen gas. The density of O2 gas at NTP is 1.429g/L.
(a) 22.39 Litres
(b) 21.2 Litres
(c) 24 Litres
(d) None of the above
Answer: (a) 22.39 Litres
81.4 g sample of ethyl alcohol contains 0.002 g of water. The amount of pure ethyl alcohol to the proper number of significant figures is
(a) 81.398 g
(b) 71.40 g
(c) 91.4 g
(d) 81 g
Answer: (a) 81.398 g
What is the concentration of nitrate ions if equal volumes of 0.1 MAgNO3 and 0.1 M NaCl are mixed together
(a) 0.1 M
(b) 0.2 M
(c) 0.05 M
(d) 0.25 M
Answer: (c) 0.05 M
An atom is 10 times heavier than 1/12th of mass of a carbon atom (C – 12). The mass of the atom in a.m.u. is
(a) 10
(b) 120
(c) 1.2
(d) 12
Answer: (a) 10
Haemoglobin contains 0.33% of iron by weight. The molecular weight of haemoglobin is approximately 67200. The number of iron atoms (At. wt. of Fe = 56) present in one molecule of haemoglobin is
(a) 6
(b) 1
(c) 4
(d) 2
Answer: (c) 4
Approximate atomic weight of an element is 26.89. If its equivalent weight is 8.9, the exact atomic weight of element would be
(a) 26.89
(b) 8.9
(c) 17.8
(d) 26.7
Answer: (a) 26.89
One mole of calcium phosphide on reaction with excess of water gives
(a) One mole of phosphine
(b) Two moles of phosphoric acid
(c) Two moles of phosphine
(d) One mole of phosphorous pentoxide
Answer: (c) Two moles of phosphine
Irrespective of the source, pure sample, of water always yields 88.89% mass of oxygen and 11.11% mass of hydrogen. This is explained by the law of
(a) Conservation of Mass
(b) Multiple Proportions
(c) Constant Composition
(d) Constant Volume
Answer: (c) Constant Composition
An aqueous solution of 6.3 g of oxalic acid dihydrate is made upto 250 ml. The volume of 0.1 N NaOH required to completely neutralise 10 ml of this solution is
(a) 40 ml
(b) 20 ml
(c) 10 m
(d) 4 ml
Answer: (a) 40 ml
Under similar conditions of pressure and temperature, 40 ml of slightly moist hydrogen chloride gas is mixed with 20 ml of ammonia gas, the final volume of gas at the same temperature and pressure will be
(a) 100 ml
(b) 20 ml
(c) 40 ml
(d) 60 ml
Answer: (b) 20 ml
The percentage of nitrogen in urea is about
(a) 46
(b) 85
(c) 18
(d) 28
Answer: (a) 46
Which of the following weighs the most?
(a) One g – atom of nitrogen
(b) One mole of water
(c) One mole of sodium
(d) One molecule of H2SO4
Answer: (c) One mole of sodium
The total number of ions present in 111 g of CaCl2 is
(a) One Mole
(b) Two Mole
(c) Three Mole
(d) Four Mole
Answer: (c) Three Mole
Which of the following is a homogeneous mixture?
(a) Mixture of soil and water
(b) Sugar solution
(c) Mixture of sugar, salt and sand
(d) Iodised table salt
Answer: (b) Sugar solution
The prefix 1018 is
(a) giga
(b) exa
(c) kilo
(d) mega
Answer: (b) exa
Which of the following contains same number of carbon atoms as are in 6.0 g of carbon (C – 12)?
(a) 6.0 g Ethane
(b) 8.0 g Methane
(c) 21.0 g Propane
(d) 28.0 g CO
Answer: (b) 8.0 g Methane
The number of significant figures in 6.02 x 1023 is
(a) 23
(b) 3
(c) 4
(d) 26
Answer: (b) 3
An organic compound contains carbon , hydrogen and oxygen. Its elemental analysis gave C, 38.71% and H, 9.67%. The empirical formula of the compound would be
(a) CHO
(b) CH4O
(c) CH3O
(d) CH2O
Answer: (c) CH3O
Which of the following cannot give iodometric titrations
(a) Fe3+
(b) Cu2+
(c) Pb2+
(d) Ag+
Answer: (c) Pb2+
A symbol not only represents the name of the element but also represents
(a) Atomic Mass
(b) Atomic Number
(c) Atomicity
(d) Atomic Volume
Answer: (c) Atomicity
The sulphate of a metal M contains 9.87% of M. This sulphate is isomorphous with ZnSO4.7H2O. The atomic weight of M is
(a) 40.3
(b) 36.3
(c) 24.3
(d) 11.3
Answer: (c) 24.3
Difference in density is the basis of
(a) gravity separation
(b) molecular sieving
(c) ultrafiltration
(d) molecular attraction
Answer: (a) gravity separation
Which of the following substances cannot be separated in
(a) Solid glucose
(b) Salt and sugar
(c) Sugar and water solution
(d) None of these
Answer: (a) Solid glucose
7.5 grams of a gas occupy 5.6 litres of volume at STP. The gas is
(a) NO
(b) N2O
(c) CO
(d) CO2
Answer: (a) NO
Which one of the following set of units represents the smallest and largest amount of energy respectively?
(a) eV and L-atm
(b) erg and cal
(c) J and erg
(d) cal and eV
Answer: (a) eV and L-atm
An atom is 10 times heavier than 1/12th of mass of a carbon atom (C – 12). The mass of the atom in a.m.u. is
(a) 10
(b) 120
(c) 1.2
(d) 12
Answer: (a) 10
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