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Chapter 1 Some Basic Concepts of Chemistry Chemistry Worksheet for Class 11
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Class 11 Chemistry Chapter 1 Some Basic Concepts of Chemistry Worksheet Pdf
Question. The dimensions of pressure are the same as that of
(a) force per unit volume
(b) energy per unit volume
(c) force
(d) energy
Answer. B
Question. Given the numbers : 161 cm, 0.161 cm, 0.0161 cm. The number of significant figures for the three numbers is
(a) 3, 3 and 4 respectively
(b) 3, 4 and 4 respectively
(c) 3, 4 and 5 respectively
(d) 3, 3 and 3 respectively.
Answer. D
Question. Equal masses of H2, O2 and methane have been taken in a container of volume V at temperature 27 °C in identical conditions. The ratio of the volumes of gases H2 : O2 : methane would be
(a) 8 : 16 : 1
(b) 16 : 8 : 1
(c) 16 : 1 : 2
(d) 8 : 1 : 2
Answer. C
Question. What volume of oxygen gas (O2) measured at 0°C and 1 atm, is needed to burn completely 1 L of propane gas (C3H8) measured under the same conditions?
(a) 5 L
(b) 10 L
(c) 7 L
(d) 6 L
Answer. A
Question. 0.24 g of a volatile gas, upon vaporisation, gives 45 mL vapour at NTP. What will be the vapour density of the substance? (Density of H2 = 0.089 g/L)
(a) 95.93
(b) 59.93
(c) 95.39
(d) 5.993
Answer. B
Question. The molecular weight of O2 and SO2 are 32 and 64 respectively. At 15°C and 150 mmHg pressure, one litre of O2 contains ‘N’ molecules. The number of molecules in two litres of SO2 under the same conditions of temperature and pressure will be
(a) N/2
(b) N
(c) 2 N
(d) 4 N
Answer. C
Question. What is the weight of oxygen required for the complete combustion of 2.8 kg of ethylene?
(a) 2.8 kg
(b) 6.4 kg
(c) 9.6 kg
(d) 96 kg
Answer. C
Question. An element, X has the following isotopic composition : 200X : 90% 199X : 8.0% 202X : 2.0%
The weighted average atomic mass of the naturally occurring element X is closest to
(a) 201 amu
(b) 202 amu
(c) 199 amu
(d) 200 amu
Answer. D
Question. Boron has two stable isotopes, 10B(19%) and 11B(81%). Calculate average at. wt. of boron in the periodic table.
(a) 10.8
(b) 10.2
(c) 11.2
(d) 10.0
Answer. A
Question. Which one of the followings has maximum number of atoms?
(a) 1 g of Ag(s) [Atomic mass of Ag = 108]
(b) 1 g of Mg(s) [Atomic mass of Mg = 24]
(c) 1 g of O2(g) [Atomic mass of O = 16]
(d) 1 g of Li(s) [Atomic mass of Li = 7]
Answer. D
Question. In which case is number of molecules of water maximum?
(a) 18 mL of water
(b) 0.18 g of water
(c) 0.00224 L of water vapours at 1 atm and 273 K
(d) 10–3 mol of water
Answer. A
Question. Suppose the elements X and Y combine to form two compounds XY2 and X3Y2. When 0.1 mole of XY2 weighs 10 g and 0.05 mole of X3Y2 weighs 9 g, the atomic weights of X and Y are
(a) 40, 30
(b) 60, 40
(c) 20, 30
(d) 30, 20
Answer. A
Question. If Avogadro number NA, is changed from 6.022 × 1023 mol–1 to 6.022 × 1020 mol–1, this would change
(a) the mass of one mole of carbon
(b) the ratio of chemical species to each other in a balanced equation
(c) the ratio of elements to each other in a compound
(d) the definition of mass in units of grams.
Answer. A
Question. The number of water molecules is maximum in
(a) 1.8 gram of water
(b) 18 gram of water
(c) 18 moles of water
(d) 18 molecules of water.
Answer. C
Question. A mixture of gases contains H2 and O2 gases in the ratio of 1 : 4 (w/w). What is the molar ratio of the two gases in the mixture?
(a) 16 : 1
(b) 2 : 1
(c) 1 : 4
(d) 4 : 1
Answer. D
Question. Which has the maximum number of molecules among the following?
(a) 44 g CO2
(b) 48 g O3
(c) 8 g H2
(d) 64 g SO2
Answer. C
Question. The number of atoms in 0.1 mol of a triatomic gas is
(NA = 6.02 × 1023 mol–1)
(a) 6.026 × 1022
(b) 1.806 × 1023
(c) 3.600 × 1023
(d) 1.800 × 1022
Answer. B
Question. The maximum number of molecules is 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.
Answer. A
Question. Which has maximum molecules?
(a) 7 g N2
(b) 2 g H2
(c) 16 g NO2
(d) 16 g O2
Answer. B
Question. Specific volume of cylindrical virus particle is 6.02 × 10–2 cc/g whose radius and length are 7 Å and 10 Å respectively. If NA = 6.02 × 1023, find molecular weight of virus.
(a) 15.4 kg/mol
(b) 1.54 × 104 kg/mol
(c) 3.08 × 104 kg/mol
(d) 3.08 × 103 kg/mol
Answer. A
Question. The number of atoms in 4.25 g of NH3 is approximately
(a) 4 × 1023
(b) 2 × 1023
(c) 1 × 1023
(d) 6 × 1023
Answer. D
Question. Haemoglobin contains 0.334% of iron by weight. The molecular weight of haemoglobin is approximately 67200. The number of iron atoms (Atomic weight of Fe is 56) present in one molecule of haemoglobin is
(a) 4
(b) 6
(c) 3
(d) 2
Answer. A
Question. The number of moles of oxygen in one litre of air containing 21% oxygen by volume, under standard conditions, is
(a) 0.0093 mol
(b) 2.10 mol
(c) 0.186 mol
(d) 0.21 mol
Answer. A
Question. The total number of valence electrons in 4.2 g of N3– ion is (NA is the Avogadro’s number)
(a) 2.1 NA
(b) 4.2 NA
(c) 1.6 NA
(d) 3.2 NA
Answer. C
Question. The number of gram molecules of oxygen in 6.02 × 1024 CO molecules is
(a) 10 g molecules
(b) 5 g molecules
(c) 1 g molecule
(d) 0.5 g molecules.
Answer. B
Question. Ratio of Cp and Cv of a gas ‘X’ is 1.4. The number of atoms of the gas ‘X’ present in 11.2 litres of it at NTP will be
(a) 6.02 × 1023
(b) 1.2 × 1023
(c) 3.01 × 1023
(d) 2.01 × 1023
Answer. A
Question. The number of oxygen atoms in 4.4 g of CO2 is
(a) 1.2 × 1023
(b) 6 × 1022
(c) 6 × 1023
(d) 12 × 1023
Answer. A
Question. 1 cc N2O at NTP contains
(a) 1. 8/224 ×1022 atoms
(b) 6.02/22400 ×1023 molecules
(c) 1.32/224 ×1023 electrons
(d) all of the above.
Answer. D
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) CHO
(b) CH4O
(c) CH3O
(d) CH2O
Answer. C
Question. Percentage of Se in peroxidase anhydrous enzyme is 0.5% by weight (at. wt. = 78.4) then minimum molecular weight of peroxidase anhydrous enzyme is
(a) 1.568 × 104
(b) 1.568 × 103
(c) 15.68
(d) 2.136 × 104
Answer. A
Question. Which of the following fertilizers has the highest nitrogen percentage?
(a) Ammonium sulphate
(b) Calcium cyanamide
(c) Urea
(d) Ammonium nitrate
Answer. C
Question. The number of moles of hydrogen molecules required to produce 20 moles of ammonia through Haber’s process is
(a) 40
(b) 10
(c) 20
(d) 30
Answer. D
Question. The density of 2 M aqueous solution of NaOH is 1.28 g/cm3. The molality of the solution is [Given that molecular mass of NaOH = 40 g mol–1]
(a) 1.20 m
(b) 1.56 m
(c) 1.67 m
(d) 1.32 m
Answer. C
Question. A mixture of 2.3 g formic acid and 4.5 g oxalic acid is treated with conc. H2SO4. The evolved gaseous mixture is passed through KOH pellets. Weight (in g) of the remaining product at STP will be
(a) 1.4
(b) 3.0
(c) 2.8
(d) 4.4
Answer. C
Question. What is the mass of the precipitate formed when 50 mL of 16.9% solution of AgNO3 is mixed with 50 mL of 5.8% NaCl solution?
(Ag = 107.8, N = 14, O = 16, Na = 23, Cl = 35.5)
(a) 3.5 g
(b) 7 g
(c) 14 g
(d) 28 g
Answer. B
Question. 20.0 g of a magnesium carbonate sample decomposes on heating to give carbon dioxide and 8.0 g magnesium oxide. What will be the percentage purity of magnesium carbonate in the sample?
(At. wt. of Mg = 24)
(a) 96
(b) 60
(c) 84
(d) 75
Answer. C
Question. When 22.4 litres of H2(g) is mixed with 11.2 litres of Cl2(g), each at STP, the moles of HCl(g) formed is equal to
(a) 1 mol of HCl(g)
(b) 2 mol of HCl(g)
(c) 0.5 mol of HCl(g)
(d) 1.5 mol of HCl(g)
Answer. A
Question. 1.0 g of magnesium is burnt with 0.56 g O2 in a closed vessel. Which reactant is left in excess and how much? (At. wt. Mg = 24, O = 16)
(a) Mg, 0.16 g
(b) O2, 0.16 g
(c) Mg, 0.44g
(d) O2, 0.28 g
Answer. A
Question. 6.02 × 1020 molecules of urea are present in 100 mL of its solution. The concentration of solution is
(a) 0.001 M
(b) 0.1 M
(c) 0.02 M
(d) 0.01 M
Answer. D
Question. In an experiment it showed that 10 mL of 0.05 M solution of chloride required 10 mL of 0.1 M solution of AgNO3, which of the following will be the formula of the chloride (X stands for the symbol of the element other than chlorine)?
(a) X2Cl2
(b) XCl2
(c) XCl4
(d) X2Cl
Answer. B
Question. 25.3 g of sodium carbonate, Na2CO3 is dissolved in enough water to make 250 mL of solution. If sodium carbonate dissociates completely, molar concentration of sodium ion, Na+ and carbonate ions, CO32– are respectively
(Molar mass of Na2CO3 = 106 g mol–1)
(a) 0.955 M and 1.910 M
(b) 1.910 M and 0.955 M
(c) 1.90 M and 1.910 M
(d) 0.477 M and 0.477 M
Answer. B
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) 3 mol
(b) 4 mol
(c) 1 mol
(d) 2 mol
Answer. B
Question. How many moles of lead(II) chloride will be formed from a reaction between 6.5 g of PbO and 3.2 g HCl?
(a) 0.011
(b) 0.029
(c) 0.044
(d) 0.333
Answer. B
Question. The mass of carbon anode consumed (giving only carbon dioxide) in the production of 270 kg of aluminium metal from bauxite by the Hall process is
(a) 270 kg
(b) 540 kg
(c) 90 kg
(d) 180 kg
(Atomic mass : Al = 27)
Answer. C
Question. Molarity of liquid HCl, if density of solution is 1.17 g/cc is
(a) 36.5
(b) 18.25
(c) 32.05
(d) 42.10
Answer. C
Question. Volume of CO2 obtained by the complete decomposition of 9.85 g of BaCO3 is
(a) 2.24 L
(b) 1.12 L
(c) 0.84 L
(d) 0.56 L
Answer. B
Question. In the reaction,
4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(l)
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. A
Question. The amount of zinc required to produce 224 mL of H2 at STP on treatment with dilute H2SO4 will be
(a) 65 g
(b) 0.065 g
(c) 0.65 g
(d) 6.5 g
Answer. C
Question. At STP the density of CCl4 vapour in g/L will be nearest to
(a) 6.87
(b) 3.42
(c) 10.26
(d) 4.57
Answer. A
CBSE Class 11 Chemistry Chapter 1 Some Basic Concepts of Chemistry Very Short Answer
CBSE Class 11 Chemistry Chapter 1 Some Basic Concepts of Chemistry Short Answer
Question. Define chemistry?
Answer. The branch of the science that studies the preparation, properties, structures and reactions of the material substances. It is the science of the molecules and their transformations. It is the science not so much of the one hundred elements but of the infinite variety of the molecules that may be built from them.
Question. Distinguish between mixture and pure substances?
Answer. 1. Mixtures are made up of several substances that are not chemically bonded whereas pure substances are made of only one matter.
2. Mixture is the categorized as homogeneous and heterogeneous whereas pure substances can be categorized as gas, liquid and solid.
Question. What is the use of physical properties and chemical properties?
Answer. Physical properties are those that can be observed without changing the identity of the substance. Physical properties are used to observe and describe matter. Physical properties include: appearance, texture, color, odor, melting point, boiling point, density, solubility, polarity etc..
A chemical property is a characteristic of a substance that may be observed when it participates in a chemical reaction. Chemical properties include flammability, toxicity, chemical stability, and heat of combustion.
Question. Define volume and density?
Answer. Volume: Volume is the amount of the space occupied by a substance. It is the quantity of three-dimensional space occupied by a liquid, solid, or gas. It has the units of length3 and in SI system the volume units is m3.
Density: The density of a substance is the relationship between the mass of the substance and the space it takes place. The mass of atoms, their size, and how they are arranged determine the density of a substance. Density equals the mass of the substance divided by its volume.
Question. What do you mean by uncertainty in measurement?
Answer. The uncertainty in measurements all measurements have a degree of uncertainty regardless of precision and accuracy. This is caused by two factors, the limitation of
the measuring instrument and the skill of the experimenter making the measurements.
CBSE Class 11 Chemistry Chapter 1 Some Basic Concepts of Chemistry Long Answer
Question. Explain the importance of chemistry?
Answer. Chemistry is important because whatever we do is chemistry. Our body is also made up of the chemicals. Chemical reactions occur when you breathe, eat, or just sit there reading. All matter is made of chemicals, so the importance of chemistry is that it's the study of everything. Chemistry contributes in a big manner to the national economy. Chemistry many of our daily activities are achieved. Soaps, detergents, pills, plastics, clothes, food, colors, and many others are some of the products of chemistry. A biological organism made up of various bio chemicals like carbohydrates, proteins, vitamins, lipids etc. Our biological processes like digestion, respiration, cellular metabolism, reproduction, and many others are accomplished by biochemical reactions. Chemistry contributes to a large extent in the development and the growth of the nation. Chemicals have helped greatly in increasing the yield of fruits, vegetables, and other crops. Chemicals have greatly helped to preserve food products for a longer period. It has given methods to test the presence of adulterants. This ensures the supply of pure foodstuff. Chemistry provided mankind with a large number of life-saving drugs.
Question. Explain nature of matter and states of matter?
Answer. Anything that occupies space and has mass is known as matter. Everything around us is a form of matter. Atoms that have protons, neutrons, electrons and a nucleus consist of matter. It generally exists in four states i.e. liquid, solid, and gaseous state.
States of matter:
1. Solid: Solid matter is composed of tightly packed particles. A solid will retain its shape; the particles are not free to move around. In solids the atoms are bonded fairly firmly together, though they do move about a bit. We do not need to put a solid in a container, it stays where it is because its atoms are locked tightly into a definite shape that, ordinarily, does not change. If a solid is reasonably soft and we press it, we can make it change shape by pushing its atoms into new positions.
2. Liquids: A liquid is one of the states of matter. The liquid state of a material has a definite volume, but it does not have a definite shape and takes the shape of the container. The particles in a liquid are free to flow, so while a liquid has a definite volume, it does not have a definite shape. Liquids consist of atoms or molecules that are connected by intermolecular bonds.
3. Gaseous: The gaseous state is considered one of the simplest states of matter. A slight increase in the physical conditions of temperature or pressure can be easily observed. Gas is a state of matter that has no fixed shape and no fixed volume. Gases have lower density than other states of matter, such as solids and liquids.
Question. Difference between mass and weight?
Answer. 1. Mass is the measure of the amount of matter in a body whereas weight is the measure of the amount of force acting on a mass due to the acceleration due to gravity.
2. Mass is a scalar quantity whereas weight is a vector quantity.
3. Mass is not affected by gravity whereas weight is affected by the gravity.
4. Mass can usually measure in grams and kilograms whereas weight can usually measures in newton.
5. Mass value cannot be zero whereas weight can be zero if no gravity is observed.
Question. Write short note on volume, density and temperature?
Answer.
Volume: Volume is the quantity of three-dimensional space occupied by a liquid, solid,and gas. Volume is measured as the amount of space that matter occupies. It has the units of (length) 3. The volume of an object is a measure of the amount of space occupied by that object. When we have to measure the volume of the liquid then the SI unit id liter. A volumetric flask is used to prepare a known volume of a solution.
Density: The density of a substance is the relationship between the mass of the substance and how much space it takes up (volume). The mass of atoms, their size, and how they are arranged determine the density of a substance. Density equals the mass of the substance divided by its volume, D = m/v.
Temperature: Temperature is the property of matter which reflects the quantity of energy of motion of the component particles. It is a comparative measure of how hot or cold a material is. The coldest theoretical temperature is called absolute zero. The basic unit of temperature in the SI is the Kelvin. It has the symbol K.
Question. Explain about significant figures in chemistry?
Answer. Significant figures are any non-zero digits or trapped zeros. They do not include leading or trailing zeros. When going between decimal and scientific notation, maintain the same number of significant figures. Precision refers to the closeness of the various measurements for the same quantity. The accuracy is the agreement of a particular value to the true value of the result, for example: 91 have two significant figures (9 and 1), while 123.45 has five significant figures (1, 2, 3, 4 and 5). Zeros appearing anywhere between two non-zero digits are significant: 101.1203 have seven significant figures: 1, 0, 1, 1, 2, 0 and 3. The rules for determining the number of the significant figures these are:
1. All non- zero digits are significant.
2. Zeros proceeding to first non- zero digits are not significant, such zero indicates the position of the decimal point.
3. Zeros between two non-zero digits are significant.
4. Zeros at the end of right of a number are significant provided they are on the right side of the decimal point.
5. Counting the numbers if the object.
Chapter 1 Some Basic Concepts of Chemistry CBSE Class 11 Chemistry Worksheet
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