Please refer to MCQ Questions Chapter 1 Some Basic Concepts of Chemistry Class 11 Chemistry with answers provided below. These multiple-choice questions have been developed based on the latest NCERT book for class 11 Chemistry issued for the current academic year. We have provided MCQ Questions for Class 11 Chemistry for all chapters on our website. Students should learn the objective based questions for Chapter 1 Some Basic Concepts of Chemistry in Class 11 Chemistry provided below to get more marks in exams.
Chapter 1 Some Basic Concepts of Chemistry MCQ Questions
Please refer to the following Chapter 1 Some Basic Concepts of Chemistry MCQ Questions Class 11 Chemistry with solutions for all important topics in the chapter.
MCQ Questions Answers for Chapter 1 Some Basic Concepts of Chemistry Class 11 Chemistry
Question. Which one of the following set of units represents the smallest and largest amount of energy respectively ?
(a) J and erg
(b) erg and cal
(c) cal and eV
(d) eV and L-atm
Question. The system that contains the maximum number of atoms is
(a) 4.25 g of NH3
(b) 8 g of O2
(c) 2g of H2
(d) 4 g of He
Question. Number of molecules in 1 L of water is close to
(a) 18/22.4 X 1023
(b) 55.5 X 6.023 X 1023
(c) 6·023 x 1023
(d) 18 x 6.023 x 1023
Question. One mole of CO2 contains
(a) 3 g atoms of CO2
(b) 18.1 x 1023 molecules of CO2
(c) 6.02 x 1023 atoms of O
(d) 6.02 x 1023 atoms of C
Question. Which has the highest weight ?
(a) 1 m 3 of water
(b) A normal adult man
(c) 10 L of Hg
(d) All have same weight
Question. The number of hydrogen atoms present in 25.6 g of sucrose (C12H22O11) which has a molar mass of 342.3 g is
(a) 22 X 1023
(b) 9.91 X 1023
(c) 11 X 1023
(d) 44 X 1023
Question. The number of fonnula units of calcium fluoride, CaF2 present in 146.4 g of CaF2 (the molar mass of CaF2 is 78.08 g/mol) is
(a) 1.129 X 1024 CaF2
(b) 1.146 X 1024 CaF2
(c) 7.808 x 1024 CaF2
(d) l.877 x 1024 CaF2
Question. Mass of0.1 mole of methane is
Question. 80 g of oxygen contains as many atoms as in
(a) 80 g of hydrogen
(b) 1 g of hydrogen
(c) 10 g of hydrogen
(d) 5 g of hydrogen
Question. 0.1 mole of a carbohydrate with empirical formula CH2O contains 1 g of hydrogen. What is its molecular formula?
Question. Which one of the following has maximum number of atoms of oxygen ?
(a) 2 g of carbon monoxide
(b) 2 g of carbon dioxide
(c) 2 g of sulphur dioxide
(d) 2 g of water
Question. Gram molecular volume of oxygen at STP is
(a) 3200 cm3
(b) 5600 cm3
(c) 22400 cm3
(d) 11200 cm3
Question. Which has maxinmm number of atoms ?
(a) 24 g ofC
(b) 56 g of Fe
(d) 108 g of Ag
Question. Law of constant composition is same as the law of
(a) conservation of mass
(b) conservation of energy
(c) multiple proportion
(d) definite proportion
Question. The maximum number of molecules are present in
(a) 15 L of H2 gas at STP
(b) 5 L of N2 gas at STP
(c) 0.5 g of H2 gas
(d) 10 g of O2 gas
Question. The value of amu is which of the following ?
(a) 1.57 x 10-24 kg
(b) 1.66 x 10-24 kg
(c) 1.99 X 10-23 kg
(d) 1.66 x 10-27 kg
Question. The mass of 1 mole of electrons is
(a) 9.1 x 10-23 g
(d) 9.1 x 10-27 g
Question. Which of the following is correct for
C (graphite) +O2(g) → CO2, Heat = – 348kJ ?
(a) Heat absorbed
(b) Mass of product> Mass of reactant
(c) Mass of product < Mass ofreactant
( d) Mass of product = Mass of reactant
Question. A signature, written in carbon pencil weighs 1 mg. What is the number of carbon atoms present in the signature ?
(a) 5.02 X 1023
(b) 5.02 X 1020
(c) 6.02x 1020
(d) 0.502x 1020
Question. How many moles of Al2(SO4)3 h would be in 50 g of the substance ?
(a) 0.083 mol
(c) 0.481 mol
(b) 0.952 mol
(d) 0.140 mo!
Question. The number of molecules of CO2 present in 44 g of CO2 is
(a) 6.0x 1023
(b) 3 X 1023
(c) 12x 1023
(d) 3x 1010
Question. 0.56 g of a gas occupies 280cm3 at NTP, then its molecular mass is
Question. In the disproportionation reaction,
3HCIO3 → HC1O4 + Cl2 + 202 + H2O,
the equivalent mass of the oxidising agent is (molar mass of HClO3 = 84.45)
Question. The equivalent weight of KMnO4 for acid solution is
Question. Given, that the abundances of isotopes 54Fe, 56Fe and 57Fe are 5%, 90% and 5%, respectively, the atomic mass of Fe is
Question. The percentage of an element M is 53 in its oxide of molecular formula M2O3 . Its atomic mass is about
Question. An unknown element forms an oxide. What will be the equivalent weight of the element if the oxygen content is 20% by weight ?
Question. 1.520 g of hydroxide of a metal on ignition gave 0.995 g of ox.ide. The equivalent weight of metal is
Question. For the reaction,
Na2CO3 + 2HCI → 2NaCI + H2O+ CO2
Equivalent weight of Na2CO3 is
Question. KMnO4 (mo!. wt. = 158) oxidises oxalic acid in acidic medium to CO2 and water as follows
5C2O42- t + 2MnO4 + 16H+
→ I0CO2 + 2Mn2+ + 8H2O
What is the equivalent weight of KMnO 4 ?
Question. In the equation, H2S+ 2HNO3 → 2H2O + 2NO2 + S The equivalent weight of hydrogen sulphide is
Question. If we consider that 1/6 , in place of 1/12 ,mass of carbon atom is taken to be the relative atomic mass unit, the mass of one mole of a substance will
(a) be a function of the molecular mass or the substance
(b) remain unchanged
(c) increase two fold
(d) decrease twice
Question. The equivalent weight of a certain trivalent element is 20. Molecular weight of its oxide is
Question. An organic compound on analysis was found to contain 10.06% carbon, 0.84% hydrogen and 89.10% chlorine. What will be the empirical fom1ula of the substance?
Question. If two compounds have the same empirical formula but ilifferent molecular formulae, they must have
(a) different percentage composition
(b) different molecular weights
(c) same viscosity
( d) same vapour density
Question. In a compound C, H and N are present in 9 : l : 3.5 by weight. If molecular weight of the compound is 108, then the molecular formula of the compound is
Question. For the reaction represented by the equation,
ex4 + 202 → CO2 + 2X2O
9.0 g of CX4 completely reacts with 1.74 g ofoxygen. The approxin1ate molar mass of X will be
Question. A 5.82 g silver coin is ilissolved in nitric acid. When soilium chloride is added to the solution, all the silver is precipitated as AgCl. The AgCl precipitate weighs 7 .20 g. The percentage of silver in the coin is
Question. If 20 g of CaCO3 is treated with 100 mL of 20% HCl solution, the amount of CO2 produced is
(a) 22.4 L
(b) 8.80 g
(c) 4.40 g
(d) 2.24 L
Question. 5 moles ofBa(OHh are treated with excess of CO2. How much BaCO3 will be formed?
(a) 39.4 g
(b) 197 g
(c) 591 g
(d) 985 g
Question. 20 mL of methane is completely burnt using 50 mL of oxygen. The volume of the gas left after cooling at room temperature is
(a) 40 mL
(b) 60 mL
(c) 30 mL
(d) 80 mL
Question. A mixture of CaCI2 and NaCl weighing 4.44 g is treated with sodium carbonate solution to precipitate all the Ca2+ ions as calcium carbonate. The calcium carbonate so obtained is heated strongly to get 0.56 g of CaO. The percentage of NaCl in the mixture ( atomic mass of Ca= 40) is
Question. An aqueous solution containing 6.5 g of NaCl of 90% purity was subjected to electrolysis. After the complete electrolysis, the solution was evaporated to get solid NaOH. The volume of 1 M acetic acid required to neutralise NaOH obtained above is
(a) I 000 cm3
(b) 2000 cm3
(c) I 00 cm3
(d) 200 cm3
Question. Acidified KMnO4 oxidises oxalic acid to CO2 . What is the volume (in litres) of 10-4 M KMnO4 required to completely oxidise 0. 5 L of 10-2 M oxalic acid in acidic medium ?
Question. The ratio of amounts of H2S needed to precipitate all the metal ions from 100 mL of 1 M AgNO3 and 100 mL of CuSO4 , will be
(d) None of these
Question. For the reaction, Fe2O3 + 3CO~ 2Fe + 3CO2 , the volume of carbon monoxide required to reduce one mole of fen-ic oxide is
(d) l l.2dm3
Question. 1 mole of methylamine on reaction with nitrous acid gives at NTP
(a) 1.0 L of nitrogen
(c) 11.2 L ofnitrogen
(b) 22.4 L of nitrogen
(d) 5.6 L of nitrogen
Question. Air contains 20% O2 by volume. How much volume of air will be required for 100 cc of acetylene ?
(a) 500 cc
(b) 1064 cc
(c) 212.8 cc
(d) 1250 cc
Question. 2 g of mixture of CO and CO2 on reaction with excess I2O5 produced 2.54 g of I2. What would be the mass % of CO2 in the original mixture ?
Question. What amount of bromine will be required to convert 2 g of phenol into 2, 4, 6-tribromophenol ?
(a) 20.44 g
(b) 6.00 g
(d) l 0.22g
Question. Sodium bicarbonate on heating decomposes to form sodium carbonate, CO2 and water. If 0.2 moles of sodium bicarbonate is completely decomposed, how many moles of sodium carbonate is formed ?
33. 100 g of CaCO3 is treated with I L of 1 N HCI. What would be the weight of CO2 liberated after the completion of the reaction? Question
(e) 44 g
Question. x grams of calcium carbonate was completely bwnt in air. The weight of the solid residue formed is 28 g. What is the value of x (in grams)?
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