Tamil Nadu Board of Secondary EducationHSC Science Class 11th

# Tamil Nadu Board Samacheer Kalvi solutions for Class 11th Chemistry Volume 1 and 2 Answers Guide chapter 1 - Basic Concepts of Chemistry and Chemical Calculations [Latest edition]

## Chapter 1: Basic Concepts of Chemistry and Chemical Calculations

Choose the best answer [Pages 29 - 33]

### Tamil Nadu Board Samacheer Kalvi solutions for Class 11th Chemistry Volume 1 and 2 Answers Guide Chapter 1 Basic Concepts of Chemistry and Chemical CalculationsChoose the best answer [Pages 29 - 33]

Choose the best answer | Q I. 1. | Page 29

40 ml of methane is completely burnt using 80 ml of oxygen at room temperature The volume of gas left after cooling to room temperature is

• 40 ml CO2 gas

• 40 ml CO2 gas and 80 ml H2O gas

• 60 ml CO2 gas and 60 ml H2O gas

• 120 ml CO2 gas

Choose the best answer | Q I. 2. | Page 29

An element X has the following isotopic composition 200X = 90%, 199X = 8% and 202X = 2%. The weighted average atomic mass of the element X is closest to

• 201 u

• 202 u

• 199 u

• 200 u

Choose the best answer | Q I. 3. | Page 29

Assertion: Two mole of glucose contains 12.044 × 1023 molecules of glucose

Reason: Total number of entities present in one mole of any substance is equal to 6.02 × 1022

• both assertion and reason are true and the reason is the correct explanation of assertion

• both assertion and reason are true but reason is not the correct explanation of assertion

• assertion is true but reason is false

• both assertion and reason are false

Choose the best answer | Q I. 4. | Page 29

Carbon forms two oxides, namely carbon monoxide and carbon dioxide. The equivalent mass of which element remains constant?

• Carbon

• oxygen

• both carbon and oxygen

• neither carbon nor oxygen

Choose the best answer | Q I. 5. | Page 29

The equivalent mass of a trivalent metal element is 9 g eq-1 the molar mass of its anhydrous oxide is

• 102 g

• 27 g

• 270 g

• 78 g

Choose the best answer | Q I. 6. | Page 30

The number of water molecules in a drop of water weighing 0.018 g is

• 6.022 × 1026

• 6.022 × 1023

• 6.022 × 1020

• 9.9 × 1022

Choose the best answer | Q I. 7. | Page 30

1 g of an impure sample of magnesium carbonate (containing no thermally decomposable impurities) on complete thermal decomposition gave 0.44 g of carbon dioxide gas. The percentage of impurity in the sample is

• 0%

• 4.4%

• 16%

• 8.4%

Choose the best answer | Q I. 8. | Page 30

When 6.3 g of sodium bicarbonate is added to 30 g of acetic acid solution, the residual solution is found to weigh 33 g. The number of moles of carbon dioxide released in the reaction is

• 3

• 0.75

• 0.075

• 0.3

Choose the best answer | Q I. 9. | Page 30

When 22.4 litres of H2 (g) is mixed with 11.2 litres of Cl2 (g), each at 273 K at 1 atm the moles of HCl (g), formed is equal to

• 2 moles of HCl (g)

• 0.5 moles of HCl (g)

• 1.5 moles of HCl (g)

• 1 mole of HCl (g)

Choose the best answer | Q I. 10. | Page 30

Hot concentrated sulphuric acid is a moderately strong oxidising agent. Which of the following reactions does not show oxidising behaviour?

• $\ce{Cu + 2H2SO4 -> CuSO4 + SO2 + 2HO2}$

• $\ce{C + 2H2SO4 -> CO2 + 2SO2 + 2H2O}$

• $\ce{BaCl2 + H2SO4 -> BaSO4 + 2HCl}$

• none of the above

Choose the best answer | Q I. 11. | Page 30

Choose the disproportionation reaction among the following redox reactions.

• $\ce{3Mg_{(s)} + N2_{(g)} -> Mg3N2_{(s)}}$

• $\ce{P4_{(s)} + 3NaOH + 3H2O -> PH3_{(g)} + 3NaH2PO2_{(aq)}}$

• $\ce{Cl2_{(g)} + 2Kl_{(aq)} -> 2KCl_{(aq)} + I2}$

• $\ce{Cr2O3_{(s)} + 2Al_{(s)} -> Al2O3_{(s)} + 2Cr_{(s)}}$

Choose the best answer | Q I. 12. | Page 31

The equivalent mass of potassium permanganate in alkaline medium is $\ce{MnO^-_4 + 2H2O + 3e^- -> MnO2 + 4OH^-}$

• 31.6

• 52.7

• 79

• None of these

Choose the best answer | Q I. 13. | Page 31

Which one of the following represents 180 g of water?

• 5 Moles of water

• 90 moles of water

• (6.022 xx 10^23)/180 molecules of water

• 6.022 × 1024 molecules of water

Choose the best answer | Q I. 14. | Page 31

7.5 g of a gas occupies a volume of 5.6 litres at 0° C and 1 atm pressure. The gas is

• NO

• N2O

• CO

• CO2

Choose the best answer | Q I. 15. | Page 31

Total number of electrons present in 1.7 g of ammonia is

• 6.022 × 1023

• (6.022 xx 10^22)/1.7

• (6.022 xx 10^24)/1.7

• (6.022 xx 10^23)/1.7

Choose the best answer | Q I. 16. | Page 31

The correct increasing order of the oxidation state of sulphur in the anions $\ce{SO^2-_4, SO^2-_3, S2O^2-_4, S2O^2-_6}$ is

• $\ce{SO^2-_3 < SO^2-_4 < S2O^2-_4 < S2O^2-_6}$

• $\ce{SO^2-_4 < S2O^2-_4 < S2O^2-_6 < SO^2-_3}$

• $\ce{S2O^2-_4 < SO^2-_3 < S2O^2-_6 < SO^2-_4}$

• $\ce{S2O^2-_6 < S2O^2-_4 < SO^2-_4 < SO^2-_3}$

Choose the best answer | Q I. 17. | Page 31

The equivalent mass of ferrous oxalate is

• "molar mass of ferrous oxalate"/1

• "molar mass of ferrous oxalate"/2

• "molar mass of ferrous oxalate"/3

• none of these

Choose the best answer | Q I. 18. | Page 31

If the Avogadro number were changed from 6.022 × 1023 to 6.022 × 1020, this would change

• the ratio of chemical species to each other in a balanced equation

• the ratio of elements to each other in a compound

• the ratio of elements to each other in a compound

• the mass of one mole of carbon

Choose the best answer | Q I. 19. | Page 32

Two 22.4 litre containers A and B contains 8 g of O2 and 8 g of SO2 respectively at 273 K and 1 atm pressure, then

• Number of molecules in A and B are same

• Number of molecules in B is more than that in A.

• The ratio between the number of molecules in A to number of molecules in B is 2 : 1

• Number of molecules in B is three times greater than the number of molecules in A.

Choose the best answer | Q I. 20. | Page 32

What is the mass of precipitate formed when 50 ml of 8.5% solution of AgNO3 is mixed with 100 ml of 1.865% potassium chloride solution?

• 3.59 g

• 7 g

• 14 g

• 28 g

Choose the best answer | Q I. 21. | Page 32

The mass of a gas that occupies a volume of 612.5 ml at room temperature and pressure (25° C and 1 atm pressure) is 1.1 g. The molar mass of the gas is

• 66.25 g mol-1

• 44 g mol-1

• 24.5 g mol-1

• 662.5 g mol-1

Choose the best answer | Q I. 22. | Page 32

Which of the following contains the same number of carbon atoms as in 6 g of carbon-12.

• 7.5 g ethane

• 8 g methane

• both 7.5 g ethane and 8 g methane

• none of these

Choose the best answer | Q I. 23. | Page 32

Which of the following compound(s) has/have a percentage of carbon same as that in ethylene (C2H4).

• propene

• ethyne

• benzene

• ethane

Choose the best answer | Q I. 24. | Page 32

Which of the following is/are true with respect to carbon-12.

• relative atomic mass is 12 u

• oxidation number of carbon is +4 in all its compounds.

• 1 mole of carbon-12 contain 6.022 × 1022 carbon atoms.

• all of these

Choose the best answer | Q I. 25. | Page 33

Which one of the following is used as a standard for atomic mass.

• 6C12

• 7C12

• 6C13

• 6C14

Write brief answer to the following questions [Pages 33 - 35]

### Tamil Nadu Board Samacheer Kalvi solutions for Class 11th Chemistry Volume 1 and 2 Answers Guide Chapter 1 Basic Concepts of Chemistry and Chemical CalculationsWrite brief answer to the following questions [Pages 33 - 35]

Write brief answer to the following questions | Q II. 1) | Page 33

Define relative atomic mass.

Write brief answer to the following questions | Q II. 2) | Page 33

What do you understand by the term mole?

Write brief answer to the following questions | Q II. 3) | Page 33

Define equivalent mass.

Write brief answer to the following questions | Q II. 4) | Page 33

What do you understand by the term oxidation number?

Write brief answer to the following questions | Q II. 5) | Page 33

Distinguish between oxidation and reduction.

Write brief answer to the following questions | Q II. 6) i) | Page 33

Calculate the molar mass of the following compound.

Urea [CO(NH2)2]

Write brief answer to the following questions | Q II. 6) ii) | Page 33

Calculate the molar mass of the following compound.

Acetone [CH3COCH3]

Write brief answer to the following questions | Q II. 6) iii) | Page 33

Calculate the molar mass of the following compound.

Boric acid [H3BO3]

Write brief answer to the following questions | Q II. 6) iv) | Page 33

Calculate the molar mass of the following compound.

Sulphuric acid [H2SO4]

Write brief answer to the following questions | Q II. 7) | Page 33

The density of carbon dioxide is equal to 1.965 kgm3 at 273 K and 1 atm pressure. Calculate the molar mass of CO2.

Write brief answer to the following questions | Q II. 8) | Page 33

Which contains the greatest number of moles of oxygen atoms

1. 1 mol of ethanol
2. 1 mol of formic acid
3. 1 mol of H2O
Write brief answer to the following questions | Q II. 9) | Page 33

Calculate the average atomic mass of naturally occurring magnesium using the following data.

 Isotope Isotopic atomic mass Abundance (%) Mg24 23.99 78.99 Mg25 24.99 10.00 Mg26 25.98 11.01
Write brief answer to the following questions | Q II. 10) (a) | Page 34

In a reaction $\ce{x + y + z2 -> xyz2}$ identify the Limiting reagent if any, in the following reaction mixture.

200 atoms of x + 200 atoms of y + 50 molecules of z2

Write brief answer to the following questions | Q II. 10) (b) | Page 34

In a reaction $\ce{x + y + z2 -> xyz2}$ identify the Limiting reagent if any, in the following reaction mixture.

1 mol of x + 1 mol of y + 3 mol of z2

Write brief answer to the following questions | Q II. 10) (c) | Page 34

In a reaction $\ce{x + y + z2 -> xyz2}$ identify the Limiting reagent if any, in the following reaction mixture.

50 atoms of x + 25 atoms of y + 50 molecules of z2

Write brief answer to the following questions | Q II. 10) (d) | Page 34

In a reaction $\ce{x + y + z2 -> xyz2}$ identify the Limiting reagent if any, in the following reaction mixture.

2.5 mol of x + 5 mol of y + 5 mol of z2

Write brief answer to the following questions | Q II. 11) | Page 34

Mass of one atom of an element is 6.645 × 10−23 g. How many moles of element are there in 0.320 kg.

Write brief answer to the following questions | Q II. 12) i) | Page 34

What is the empirical formula of the following?

Fructose (C6H12O6) found in honey.

Write brief answer to the following questions | Q II. 12) ii) | Page 34

What is the empirical formula of the following?

Caffeine (C8H10N4O2) a substance found in tea and coffee.

Write brief answer to the following questions | Q II. 13) | Page 34

The reaction between aluminium and ferric oxide can generate temperatures up to 3273 K and is used in welding metals.
(Atomic mass of Al = 27 u Atomic mass of O = 16 u)
$\ce{2Al + Fe2O3 -> Al2O3 + 2Fe}$; If, in this process, 324 g of aluminium is allowed to react with 1.12 kg of ferric oxide.

1. Calculate the mass of Al2O3 formed.
2. How much of the excess reagent is left at the end of the reaction?
Write brief answer to the following questions | Q II. 14) | Page 34

How many moles of ethane is required to produce 44 g of $\ce{CO2_{(g)}}$ after combustion.

Write brief answer to the following questions | Q II. 15) | Page 34

Hydrogen peroxide is an oxidising agent. It oxidises ferrous ion to ferric ion and reduced itself to water. Write a balanced equation.

Write brief answer to the following questions | Q II. 16) | Page 34

Calculate the empirical and molecular formula of a compound containing 76.6% carbon, 6.38% hydrogen and rest oxygen its vapour density is 47.

Write brief answer to the following questions | Q II. 17) | Page 35

A Compound on analysis gave Na = 14.31% S = 9.97% H = 6.22% and O = 69.5% calculate the molecular formula of the compound if all the hydrogen in the compound is present in combination with oxygen as water of crystallization. (molecular mass of the compound is 322).

Write brief answer to the following questions | Q II. 18) i) | Page 35

Balance the following equation by the oxidation number method.

$\ce{K2Cr2O7 + Kl + H2SO4 -> K2SO4 + Cr2(SO4)3 + I2 + H2O}$

Write brief answer to the following questions | Q II. 18) ii) | Page 35

Balance the following equation by the oxidation number method.

$\ce{KMnO4 + Na2SO3 -> MnO2 + Na2SO4 + KOH}$

Write brief answer to the following questions | Q II. 18) iii) | Page 35

Balance the following equation by the oxidation number method.

$\ce{Cu + HNO3 -> Cu(NO3)2 + NO2 + H2O}$

Write brief answer to the following questions | Q II. 18) iv) | Page 35

Balance the following equation by the oxidation number method.

$\ce{KMnO4 + H2C2O4 + H2SO4 -> K2SO4 + MnSO4 + CO2 + H2O}$

Write brief answer to the following questions | Q II. 19) i) | Page 35

Balance the following equation by the ion electron method.

$\ce{KMnO4 + SnCl2 + HCl -> MnCl2 + SnCl4 + H2O + KCl}$

Write brief answer to the following questions | Q II. 19) ii) | Page 35

Balance the following equation by the ion electron method.

$\ce{C2O^2-_4 + Cr2O^2-_7 -> Cr^3+ + CO2}$ (in acid medium)

Write brief answer to the following questions | Q II. 19) iii) | Page 35

Balance the following equation by the ion electron method.

$\ce{Na2S2O3 + I2 -> Na2S4O6 + NaI}$

Write brief answer to the following questions | Q II. 19) iv) | Page 35

Balance the following equation by the ion electron method.

$\ce{Zn + NO^-_3 ->Zn^2+ + NO}$ (in acid medium)

## Tamil Nadu Board Samacheer Kalvi solutions for Class 11th Chemistry Volume 1 and 2 Answers Guide chapter 1 - Basic Concepts of Chemistry and Chemical Calculations

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Concepts covered in Class 11th Chemistry Volume 1 and 2 Answers Guide chapter 1 Basic Concepts of Chemistry and Chemical Calculations are Redox Reactions, Chemistry - the Centre of Life, Classification of Matter, Atomic and Molecular Masses, Mole Concept, Gram Equivalent Concept, Empirical Formula and Molecular Formula, Stoichiometry.

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