JEE Chemistry Some Basic Concepts Of Chemistry MCQs Set B

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MCQ for Full Syllabus Chemistry Some Basic Concepts Of Chemistry

Full Syllabus Chemistry students should refer to the following multiple-choice questions with answers for Some Basic Concepts Of Chemistry in Full Syllabus.

Some Basic Concepts Of Chemistry MCQ Questions Full Syllabus Chemistry with Answers

 

 

Question: The mass of 1 mole of electrons is

  • a) 0.55 mg
  • b) 9.1 × 10–28g
  • c) 1.008 mg
  • d) 9.1 × 10–27 g

Answer: 0.55 mg

 

Question: 10 g of hydrogen and 64 g of oxygen were filled in a steel vessel and exploded. Amount of water produced in this reaction will be:

  • a) 4 mol
  • b) 2 mol
  • c) 3 mol
  • d) 1 mol

Answer: 4 mol

 

Question: Which has the maximum number of molecules among the following ?

  • a) 8 g H2
  • b) 44 g CO2
  • c) 48 g O3
  • d) 64 g SO2

Answer: 8 g H2

 

Question: The weight of one molecule of a compound C60H122 is

  • a)

  • b)

  • c)

  • d) None of these

Answer:

 

Question:  The simplest formula of a compound containing 50% of element X (atomic mass 10) and 50% of element Y (atomic mass 20) is

  • a) X2Y
  • b) XY
  • c) XY3
  • d) None of these

Answer: X2Y

 

Question: Empirical formula of hydrocarbon containing 80% carbon and 20% hydrogen is

  • a) CH3
  • b) CH
  • c) CH4
  • d) CH2

Answer: CH3

 

Question: The empirical formula of a compound is CH2. One mole of this compound has a mass of 42 grams. Its molecular formula is

  • a) C3H6
  • b) CH2
  • c) C3H8
  • d) C2H2

Answer: C3H6

 

Question: A compound contains 54.55 % carbon, 9.09% hydrogen , 36.36% oxygen. The empirical formula of this compound is

  • a) C2H4O
  • b)

  • c)

  • d)

Answer: C2H4O

 

Question: In a hydrocarbon, mass ratio of hydrogen and carbon is 1:3, the empirical formula of hydrocarbon is

  • a) CH4
  • b) C2H
  • c) CH2
  • d) CH3

Answer: CH4

 

Question: 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) CH3O
  • b) CHO
  • c) CH2O
  • d) CH4O

Answer: CH3O

 

Question: A hydrocarbon is composed of 75% carbon. The empirical formula of the compound is

  • a) CH4
  • b) CH3
  • c) CH2
  • d) C2H5

Answer:  CH4

 

Question: 12 gm of Mg (atomic mass 24) will react completely with hydrochloric acid to give

  • a) 1/2 mol of H2
  • b) One mol of H2
  • c) 2/3 mol of O2
  • d) both 1/2 mol of H2 and 1/2 mol of O2

Answer: 1/2 mol of H2

 

 More Questions...............................

 

Question: 20.0 kg of N2(g) and 3.0 kg of H2(g) are mixed to produce NH3(g). The amount of NH3(g) formed is

  • a) 17 kg
  • b) 20 kg
  • c) 34 kg
  • d) 3 kg

Answer: 17 kg

 

Question: 20.0 kg of H2(g) and 32 kg of O2(g) are reacted to produce H2O(l). The amount of H2O (l) formed after completion of reaction is

  • a) 72 kg
  • b) 62 kg
  • c) 38 kg
  • d) 42 kg

Answer: 72 kg

 

Question: What is the weight of oxygen required for the complete combustion of 2.8 kg of ethylene ?

  • a) 9.6 kg
  • b) 2.8 kg
  • c) 6.4 kg
  • d) 96 kg

Answer: 9.6 kg

 

Question: In the reaction

When 1 mole of ammonia and 1 mole of O2 are made to react to completion.

  • a) all the oxygen will be consumed
  • b) 1.0 mole of NO will be produced
  • c) 1.0 mole of H2O is produced
  • d) all the ammonia will be consumed

Answer: all the oxygen will be consumed

 

Question: What is the molarity of 0.2N Na2CO3 solution?

  • a) 0.1 M
  • b) 0.4 M
  • c) 0 M
  • d) 0.2 M

Answer: 0.1 M

 

Question: The molar solution of H2SO4 is equal to

  • a) N/2 solution
  • b) 2N solution
  • c) N solution
  • d) 3N solution

Answer: N/2 solution

 

Question: Volume of water needed to mix with 10 mL 10N HNO3 to get 0.1 N HNO3 is :

  • a) 990 mL
  • b) 10 mL
  • c) 1000 mL
  • d) 1010 mL

Answer: 990 mL

 

Question: One kilogram of a sea water sample contains 6 mg of dissolved O2. The concentration of O2 in the sample in ppm is

  • a) 6.0
  • b) 16.0
  • c) 0.6
  • d) 60.0

Answer: 6.0

 

Question: A 5 molar solution of H2SO4 is diluted from 1 litre to a volume of 10 litres, the normality of the solution will be

  • a) 1N
  • b) 5N
  • c) 0.1N
  • d) 0.5N

Answer: 1N

 

Question: With increase of temperature, which of these changes?

  • a) Molarity
  • b) Molality
  • c) Weight fraction of solute
  • d) Mole fraction

Answer:  Molarity

 

Question: 6.02 × 1020 molecules of urea are present in 100 ml of its solution. The concentration of urea solution is

  • a) 0.01 M
  • b) 0.1 M
  • c) 0.02 M
  • d) 0.001 M

Answer: 0.01 M

 

Question:  Two solutions of a substance (non electrolyte) are mixed in the following manner. 480 ml of 1.5 M first solution + 520 ml of 1.2 M second solution. What is the molarity of the final mixture?

  • a) 1.344 M
  • b) 1.20 M
  • c) 2.70 M
  • d) 1.50 M

Answer: 1.344 M

 

Question: Which of the following statements are correct ?

(i) Both solids and liquids have definite volume.
(ii) Both liquids and gases do not have definite shape.
(iii) Both solids and gases take the shape of the container

  • a) (i) and (ii)
  • b) (i) and (iii)
  • c) (ii) and (iii)
  • d) (i), (ii) and (iii)

Answer: (i) and (ii)

 

Question: Choose correct option based on following statements. Here T stands for true statement and F for false statement.

(i) Homogeneous mixture has uniform composition throughout.
(ii) All components of a heterogeneous mixture are observable to naked eyes.
(iii) All solutions are homogeneous in nature.
(iv) Air is an example of heterogeneous mixture.

  • a) TFTF
  • b) TFFF
  • c) TTFF
  • d) FFTT

Answer: TFTF

 

Question:  Read the following and choose the incorrect statements.

(i) Both weight and mass are same quantities used for measurement of amount of matter present in a substance
(ii) Mass and weight of a substance vary from one place to another due to change in gravity.
(iii) SI unit of mass is kilogram and while SI unit of weight is gram.

  • a) All of these
  • b) (ii) and (iii)
  • c) (i) and (iii)
  • d) (i) and (ii)

Answer: All of these

 

Question: Moon takes 27.3 days to complete one orbit around the

Earth. Now read the following statements and choose the correct code. Here T is for true statement and F is for ‘False statement’.
(i) Moon takes 655.2 hours to complete one orbit around the Earth.
(ii) Moon takes 39312 seconds to complete one orbit around the earth.
(iii) Moon takes 1638 minutes to complete one orbit around the Earth

  • a) T F F
  • b) F T F
  • c) T F T
  • d) T T T

Answer: T F F

 

Question: Give the correct order of initials T or F for following statements. Use T if statement is true and F if it is false.

(i) Gay-Lussac’s law of gaseous volumes is actually the law of definite proportion by volume.
(ii) Law of conservation of mass is true for physical change, but not for chemical change.
(iii) The percentage of oxygen in H2O2 is different from that in H2O. Hence, it violates law of definite proportions.
(iv) Fixed mass of A reacts with two different masses of B (say x and y), then the ratio of x/y can be any positive integer.
(v) At STP, 5 mL of N2 and H2 have different no. of molecules.

  • a) TFFTF
  • b) TTFTF
  • c) FTTFT
  • d) TFTTF

Answer: TFFTF

 

Question: Consider the following statements.

(i) Atoms of H, O, N and C have identical properties but different mass.
(ii) Matter is divisible into atoms which are further indivisible.
(iii) The ratio of N: H in NH3 is 1 : 3 and N : O in nitric oxide is 2 : 1.
(iv) Dalton’s atomic theory support law of conservation of mass.

Which of the following pairs of statements is true according to Dalton’s atomic theory ?

  • a) (ii) and (iv)
  • b) (i) and (ii)
  • c) (ii) and (iii)
  • d) (i) and (iv)

Answer: (ii) and (iv)

 

Question: Choose the correct option based on following statements. Here ‘T’ stands for true and ‘F’ stands for false statement.

(i) Molecular mass of cane sugar (C12H22O11) is 182 amu.
(ii) 1 mole of cane sugar contains 6.022 × 1023 molecules of cane sugar.
(iii) 34.20 g of cane sugar contains 6.022 × 1021 molecules of cane sugar

  • a) FTF
  • b) TTF
  • c) TFT
  • d) FTT

Answer: FTF

 

Question: Match the items of Column I, II and III appropriately and choose the correct option from the codes given below

  • a) A – (s), (ii); B – (r), (i); C – (p), (iii); D – (q), (iv)
  • b) A – (p), (ii); B – (q), (iii); C – (r), (i); D – (s), (iv)
  • c) A – (q), (iv); B – (p), (ii); C – (p), (i); D – (r), (iii)
  • d) A – (r), (iii); B – (p), (ii); C – (s), (i); D – (q), (iv)

Answer:  A – (s), (ii); B – (r), (i); C – (p), (iii); D – (q), (iv)

 

Question: Match the columns

  • a) A – (t), B – (p), C – (s), D – (r), E – (q)
  • b) A – (r), B – (q), C – (t), D – (p), E – (s)
  • c) A – (p), B – (t), C – (s), D – (r), E – (q)
  • d) A – (t), B – (s), C – (r), D – (q), E – (p)

Answer:  A – (t), B – (p), C – (s), D – (r), E – (q)

 

Question:

  • a) A – (s), B – (r), C – (p), D – (q)
  • b) A – (p), B – (r), C – (s), D – (q)
  • c) A – (r), B – (p), C – (s), D – (q)
  • d) A – (q), B – (s), C – (r), D – (p)

Answer: A – (s), B – (r), C – (p), D – (q)

 

Question:

  • a) A – (r), B – (s), C – (p), D – (q)
  • b) A – (p), B – (r), C – (q), D – (s)
  • c) A – (r), B – (p), C – (q), D – (s)
  • d) A – (r), B – (q), C – (s), D – (p)

Answer: A – (r), B – (s), C – (p), D – (q)

 

Question:

  • a) A – (q), B – (r), C – (p), D – (t), E – (s)
  • b) A – (r), B – (q), C – (p), D – (t), E – (s)
  • c) A – (q), B – (p), C – (r), D – (t), E – (s)
  • d) A – (q), B – (r), C – (p), D – (s), E – (t)

Answer: A – (q), B – (r), C – (p), D – (t), E – (s)

 

Question: Match the mass of elements given in Column I with the number of moles given in Column II and mark the appropriate choice. Choose the correct codes formt he options given below.

  • a) A – (q), B – (p), C – (s), D – (r)
  • b) A – (r), B – (q), C – (p), D – (s)
  • c) A – (p), B – (r), C – (q), D – (s)
  • d) A – (s), B – (r), C – (q), D – (p)

Answer:  A – (q), B – (p), C – (s), D – (r)

 

Question:

  • a) A – (r), B – (q), C – (p), D – (s)
  • b) A – (q), B – (r), C – (p), D – (s)
  • c) A – (r), B – (q), C – (s), D – (p)
  • d) A – (r), B – (p), C – (q), D – (s)

Answer: A – (r), B – (q), C – (p), D – (s)

 

Question:

Assertion : Significant figures for 0.200 is 3 whereas for 200 it is 1.
Reason : Zero at the end or right of a number are significant provided they are not on the right side of the decimal point.

  • a) Assertion is correct, reason is incorrect
  • b) Assertion is incorrect, reason is correct
  • c) Assertion is correct, reason is correct; reason is not a correct explanation for assertion
  • d) Assertion is correct, reason is correct; reason is a correct explanation for assertion

Answer: Assertion is correct, reason is incorrect

 

Question:

Assertion : One atomic mass unit is defined as one twelfth of the mass of one carbon - 12 atom.
Reason : Carbon-12 isotope is the most abundunt isotope of carbon and has been chosen as standard.

  • a) Assertion is correct, reason is correct; reason is not a correct explanation for assertion
  • b) Assertion is correct, reason is correct; reason is a correct explanation for assertion
  • c) Assertion is correct, reason is incorrect
  • d) Assertion is incorrect, reason is correct

Answer: Assertion is correct, reason is correct; reason is not a correct explanation for assertion

 

Question:

Assertion : Volume of a gas is inversely proportional to the number of moles of gas.
Reason : The ratio by volume of gaseous reactants and products is in agreement with their mole ratio

  • a) Assertion is incorrect, reason is correct
  • b) Assertion is correct, reason is incorrect
  • c) Assertion is correct, reason is correct; reason is not a correct explanation for assertion
  • d) Assertion is correct, reason is correct; reason is a correct explanation for assertion

Answer: Assertion is incorrect, reason is correct

 

Question:

Assertion : Equal moles of different substances containsame number of constituent particles.
Reason : Equal weights of different substances contain the same number of constituent particles

  • a) Assertion is correct, reason is incorrect
  • b) Assertion is incorrect, reason is correct
  • c) Assertion is correct, reason is correct; reason is not a correct explanation for assertion
  • d) Assertion is correct, reason is correct; reason is a correct explanation for assertion

Answer: Assertion is correct, reason is incorrect

 

Question:

Assertion : The empirical mass of ethene is half of its molecular mass.
Reason : The empirical formula represents the simplest whole number ratio of various atoms present in a compound

  • a) Assertion is correct, reason is correct; reason is a correct explanation for assertion
  • b) Assertion is correct, reason is correct; reason is not a correct explanation for assertion
  • c) Assertion is correct, reason is incorrect
  • d) Assertion is incorrect, reason is correct

Answer: Assertion is correct, reason is correct; reason is a correct explanation for assertion

 

Question: What are the significant figure(s) in a broken “ruler” show below?

  • a) A, B, D
  • b) A and B
  • c) A, B and C
  • d) A only

Answer: A, B, D

 

Question: Which one of the following sets of compounds correctly illustrate the law of reciprocal proportions?

  • a)

  • b)

  • c)

  • d) None of these

Answer:

 

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) decrease twice
  • b) increase two fold
  • c) remain unchanged
  • d) be a function of the molecular mass of the substance

Answer: decrease twice

 

Question: The maximum number of molecules are present in

  • a) 15 L of H2 gas at STP
  • b) 0.5 g of H2 gas
  • c) 5 L of N2 gas at STP
  • d) 10 g of O2 gas

Answer: 15 L of H2 gas at STP

 

Question: How many moles of magnesium phosphate, Mg3(PO4)2 will contain 0.25 mole of oxygen atoms?

  • a) 3.125 × 10–2
  • b) 2.5 × 10–2
  • c) 1.25 × 10–2
  • d) 0.02

Answer: 3.125 × 10–2

 

Question: Volume occupied by one molecule of water

  • a) 3.0 × 10–23 cm3
  • b) 9.0 × 10–23 cm3
  • c) 6.023 × 10– 23 cm3
  • d) None of these

Answer: 3.0 × 10–23 cm3

 

Question: The number of atoms in 0.1 mol of a triatomic gas is :

(NA = 6.02 ×1023 mol–1)

  • a) 1.806 × 1023
  • b) 1.800 × 1022
  • c) 6.026 × 1022
  • d) 3.600 × 1023

Answer: 1.806 × 1023

 

Question: 1 c.c. N2O at NTP contains

  • a) All of the above
  • b)

  • c)

  • d)

Answer: All of the above

 

Question: How much time (in hours) would it take to distribute one  Avogadro number of wheat grains if 1020 grains are distributed each second ?

  • a) 1.673
  • b) 167.3
  • c) 0.1673
  • d) 16.73

Answer: 1.673

 

Question: Arrange the following in the order of increasing mass (atomic mass: O = 16, Cu = 63, N = 14)

I. one atom of oxygen
II. one atom of nitrogen
III. 1 × 10–10 mole of oxygen
IV. 1 × 10–10 mole of copper

  • a) II < I < III < IV
  • b) III < II < IV < I
  • c) I < II < III < IV
  • d) IV < II < III < I

Answer: II < I < III < IV

 

Question: If 1.5 moles of oxygen combines with Al to form Al2O3, the mass of Al in g [Atomic mass of Al = 27] used in the reaction is

  • a) 54
  • b) 81
  • c) 2.7
  • d) 40.5

Answer: 54

 

Question: Which one of the following is the lightest?

  • a) 0.1 g of silver
  • b) 6.023 × 1022 molecules of nitrogen
  • c) 0.1 mole of oxygen gas
  • d) 0.2 mole of hydrogen gas

Answer: 0.1 g of silver

 

Question: In a compound C, H and N atoms are present in 9 : 1 : 3.5 by weight. Molecular weight of compound is 108. Molecular formula of compound is

  • a) C6H8N2
  • b) C2H6N2
  • c) None of these
  • d) C3H4N

Answer: C6H8N2

 

Question: The empirical formula of an acid is CH2O2, the probable molecular formula of acid may be :

  • a) CH2O2
  • b) C3H6O4
  • c) CH2O
  • d) None of these

Answer: CH2O2

 

Question: A gaseous hydrocarbon gives upon combustion 0.72 g of water and 3.08 g. of CO2. The empirical formula of the hydrocarbon is

  • a) C7H8
  • b) C3H4
  • c) C2H4
  • d) None of these

Answer: C7H8

 

Question:  Which of the following is the correct empirical and molecular formulae of a compound, if the molecular mass of a compound is 80 and compound contains 60% of C, 5% of H and 35% of N ?

  • a)

  • b)

  • c)

  • d)

Answer:

 

Question: Which of the following is the correct empirical and molecular formulae of a compound, if the molecular mass of a compound is 93 and compound containing 77.43% of C, 7.53% of H and 15.05% of N ?

  • a)

  • b)

  • c)

  • d)

Answer:

 

Question:

  • a) 84 L
  • b) 11.2 L
  • c) 74 L
  • d) 22.4 L

Answer: 84 L

 

Question: Assuming fully decomposed, the volume of CO2 released at STP on heating 9.85 g of BaCO3 (Atomic mass, Ba = 137) will be

  • a) 1.12 L
  • b) 2.24 L
  • c) 4.96 L
  • d) 0.84 L

Answer: 1.12 L

 

Question: The mass of BaCO3 produced when excess CO2 is bubbled through a solution of 0.205 mol Ba(OH)2 is

  • a) 40.5 g
  • b) 162 g
  • c) 81 g
  • d) 20.25 g

Answer: 40.5 g

 

Question:

  • a) 67.2 dm3
  • b) 22.4 dm3
  • c) 11.2 dm3
  • d) 44.8 dm3

Answer: 67.2 dm3

 

Question: How many moles of lead (II) chloride will be formed from a reaction between 6.5 g of PbO and 3.2 g of HCl ?

  • a) 0.029
  • b) 0.333
  • c) 0.044
  • d) 0.011

Answer: 0.029

 

Question: Fat is an important source of energy and water, this is important for the desert animals like camel which store fat in its hump and provide water and energy. How many grams and moles of H2O are produced from the combustion of fat C57H110O6 from 450 gram of fat stored in hump of camel ?

  • a) 500.56 , 27.80
  • b) 580, 25.0
  • c) 450, 26.80
  • d) 400, 26.6

Answer: 500.56 , 27.80

 

Question: Which of the following option represents correct limiting reagents in reactions (i), (ii) and (iii) respectively.

  • a)

  • b)

  • c)

  • d)

Answer:

 

Question: 10 mL of 2(M) NaOH solution is added to 200 mL of 0.5 (M) of NaOH solution. What is the final concentration ?

  • a) 0.57 (M)
  • b) 11.4 (M)
  • c) 5.7 (M)
  • d) 1.14 (M)

Answer: 0.57 (M)

 

Question: If maximum fluoride ion presence was set to be 4 ppm number of moles of fluoride in 10 ml drinking water ?

  • a) 2.10 × 10–3
  • b) 3.10 × 10–3
  • c) 2.10 × 10–2
  • d) 3.3 × 10–2

Answer: 2.10 × 10–3

 

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