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CBSE And NCERT Solutions:

NCERT Books Solutions for Class 10 Science english Medium 1. Chemical Reactions and Equations

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NCERT SolutionsClass 10th Science Chapter 1. Chemical Reactions and Equations
Page 3 of 5

1. Chemical Reactions and Equations

 

Exercise Chap. 1

 

Exercise (chap-1, NCERT Text Book)

Q1. Which of the statements about the reaction below are incorrect?

2PbO(s) + C(s) → 2Pb(s) + CO2(g)

(a) Lead is getting reduced.

(b) Carbon dioxide is getting oxidised.

(c) Carbon is getting oxidised.

(d) Lead oxide is getting reduced.

(i) (a) and (b)

(ii) (a) and (c)

(iii) (a), (b) and (c)

(iv) all

Ans:  (ii) (a) and (c)

Q2.  Fe2O3 + 2Al → Al2O3 + 2Fe

The above reaction is an example of a

(a) combination reaction.

(b) double displacement reaction.

(c) decomposition reaction.

(d) displacement reaction.

Ans:  (d) displacement reaction.

Q3. What happens when dilute hydrochloric acid is added to iron fillings? Tick the correct answer.

(a) Hydrogen gas and iron chloride are produced.

(b) Chlorine gas and iron hydroxide are produced.

(c) No reaction takes place.

(d) Iron salt and water are produced.

Ans: (a) Hydrogen gas and iron chloride are produced.

Q4. What is a balanced chemical equation? Why should chemical equations be balanced?

Ans: The total mass of the elements present in the products of a chemical reaction has to be equal to the total mass of the elements present in the reactants. Such a chemical equation is called balanced chemical equation.  A chemical equation is  balanced to satisfy the law of conservation of mass.

Q5. Translate the following statements into chemical equations and then balance them.

(a) Hydrogen gas combines with nitrogen to form ammonia.

(b) Hydrogen sulphide gas burns in air to give water and sulpur dioxide.

(c) Barium chloride reacts with aluminium sulphate to give aluminium chloride and a precipitate of barium sulphate.

(d) Potassium metal reacts with water to give potassium hydroxide and hydrogen gas.

Ans:     

(a) N2(g) + ____  H3(g) → ____ NH3 (g)

Sol: N2(g) +  3H3(g) → 2 NH3 (g)

(b) ____ H2S(g) + ___ O3 (g) → ____ H2O(i) + ____ SO2 (g)

Sol: 2H2S(g) + 3O3 (g) → 2H2O(i) + 2SO2 (g)

(c) ____ BaCl2 + Al2(SO4)3 → _____ BaSO4 + _____ AlCl3

Sol: 3BaCl2 + Al2(SO4)3 → 3BaSO4 + 3AlCl3

(d) ____ K + ____ H2O → _____ KOH + H2(g)

Sol: 2K +  2H2O → 2KOH + H2(g)

Q6. Balance the following chemical equations.

(a) HNO3 + Ca(OH)2 → Ca(NO3)2 + H2O

(b) NaOH + H2SO4 → Na2SO4 +H2O

(c) NaCl + AgNO3 → AgCl + NaNO3

(d) BaCl2 + H2SO4 → BaSO4 + HCl

Ans :

(a) ___ HNO3 + ____ Ca(OH)2 → ____ Ca(NO3)2 + ____ H2O

Sol: 2HNO3 + Ca(OH)2 → Ca(NO3)2 + 2H2O

(b) ___NaOH + ____ H2SO4 → ____ Na2SO4 + ___ H2O

Sol: 2NaOH +  H2SO4 → Na2SO4 + 2H2O

(c) ___NaCl + ____ AgNO3 → ____ AgCl + ____ NaNO3

Sol: NaCl + AgNO3 →  AgCl +  NaNO3

(d) ___BaCl2 + ____ H2SO4 → ____ BaSO4 + ___ HCl

Sol: BaCl2 +  H2SO4 → BaSO4 + 2HCl

Q7. Write the balanced chemical equations for the following reactions.

(a) Calcium hydroxide + Carbon dioxide → Calcium carbonate + Water

(b) Zinc + Silver nitrate → Zinc nitrate + Silver

(c) Aluminium + Copper chloride → Aluminium chloride + Copper

(d) Barium chloride + Potassium sulphate → Barium sulphate + Potassium chloride

Ans:     

(a) Calcium hydroxide + Carbon dioxide → Calcium carbonate + Water

Sol: Ca(OH)2 + CO2 → CaCO3 + H2O

    Ca(OH)2 + CO2 → CaCO3 + H2O (Already Balanced)

(b) Zinc + Silver nitrate → Zinc nitrate + Silver

Sol: Zn +  AgNO3  →  Zn (NO3)2 + Ag

   Zn + 2AgNO3  →  Zn (NO3)2 +  2Ag balanced)

(c) Aluminium + Copper chloride → Aluminium chloride + Copper

Sol:  Al + CuCl2 → AlCl3 + Cu2

       Al + 3CuCl→ 2AlCl3 + 3Cu (balanced)

(d) Barium chloride + Potassium sulphate → Barium sulphate + Potassium chloride

Sol: BaCl2 + K2SO4 → BaSO4  + KCl

    BaCl2 + K2SO4 → BaSO4  + 2KCl     (balanced)

Q8. Write the balanced chemical equation for the following and identify the type of reaction in each case.

(a) Potassium bromide(aq) + Barium iodide(aq) → Potassium iodide(aq) + Barium bromide(s)

(b) Zinc carbonate(s) → Zinc oxide(s) + Carbon dioxide(g)

(c) Hydrogen(g) + Chlorine(g) → Hydrogen chloride(g)

(d) Magnesium(s) + Hydrochloric acid(aq) → Magnesium chloride(aq) + Hydrogen(g)

Ans:  

(a) Potassium bromide(aq) + Barium iodide(aq) → Potassium iodide(aq) + Barium bromide(s)

Sol: KBr(aq) + BaI2(aq) → KI (aq) + BaBr2 (aq)

2KBr(aq) + BaI2(aq) → 2KI (aq) + BaBr2 (aq)  (balanced)

Type of Reaction is double displacement.

(b) Zinc carbonate(s) → Zinc oxide(s) + Carbon dioxide(g)

Sol: ZnCO3(s) → ZnO(s) + CO2(g)

     ZnCO3(s) → ZnO(s) + CO2(g)   (Already balanced)

Type of Reaction is decomposition reaction.

(c) Hydrogen(g) + Chlorine(g) → Hydrogen chloride(g)

Sol: H2(g) + Cl2(g) →   HCl (g)

     H2(g) + Cl2(g) → 2HCl (g)  (balanced)         

Type of Reaction is combination reaction.

(d) Magnesium(s) + Hydrochloric acid(aq) → Magnesium chloride(aq) + Hydrogen(g)

Sol: Mg (s) + HCl (aq) → MgCl2(aq) + H2(g)

    Mg (s) + 2HCl (aq) → MgCl2(aq) + H2(g) (balanced)

Q9. What does one mean by exothermic and endothermic reactions? Give examples.

Ans:

Exothermic Reaction: Reactions in which heat is released along with the formation of products are called exothermic chemical reactions.

Like;

(i) Burning of coal

C(s) + O2(g) → CO2(g) (energy)

Other examples of exothermic reactions are –

(i) Burning of natural gas

CH4(g) + 2O2 (g) → CO2 (g) + 2H2O (g) (energy)

Endothermic Reaction: Reactions in which energy is absorbed are known as endothermic reactions.

Q10. Why is respiration considered an exothermic reaction? Explain.

Ans: Our body requires energy to support life. Our body obtains energy from food that we eat. During digestion, body mechanisms breaks down complex energy molecules of food into simpler substances such as glucose. This glucose is used with oxygen during the cellular respiration and gives energy. The releasing of energy carries on during the whole process. That is why the respiration is considered as an exothermic reaction. 

Q11. Why are decomposition reactions called the opposite of combination reactions? Write equations for these reactions.

Ans: In decomposition reactions a compound breaks down to form two or more substances. These reactions require a source of energy to proceed. Thus, they are the exact opposite of combination reactions. In the combination reaction, two or more substances combine to give a new substance with the releasing of energy.

Example of decomposition reaction: 

2H2O(l)  Electrolysis → 2H2(g) + O2(g)

Example of combination reaction : 

2H2(g) + O2(g) → 2H2O(l) + Energy 

Q12. Write one equation each for decomposition reactions where energy is supplied in the form of heat, light or electricity.

Ans: 

Q13. What is the difference between displacement and double displacement reactions? Write equations for these reactions.

Ans: 

In a displacement reaction a more reactive element replace a less reactive element from its compound. 

General equation for displacement reaction: 

A + Bx  → Ax + B 

Here, A is more reactive element and B is less reactive element. 

For example: 

CuSO4(aq) + Zn  →  ZnSO4(aq) + Cu 

In double displacement reaction, the exchanging of ions are taken place. 

General equation for this reaction: 

ABx + CDx → CBx + ADx 

For exampe: 

Na2SO4(aq) + BaCl2(aq) → BaSO4(s) + 2NaCl(aq)

Q14. In the refining of silver, the recovery of silver from silver nitrate solution involved displacement by copper metal. Write down the reaction involved.

Ans: 2AgNO3(aq)  + Cu(s) → Cu(NO3)2(aq)  + 2Ag(s) 

(silver nitrate)           (copper)       (copper nitrate)        (Silver) 

Q15. What do you mean by a precipitation reaction? Explain by giving examples.

Ans: A reaction in which precipitate (an insoluble substance) is formed is called a precipitation reaction.

Example (1).

Na2SO4(aq) + BaCl2(aq) → BaSO4(s) + 2NaCl(aq)

The white precipitate of BaSO4 is formed by this reaction. 

Example (2). 

Na2CO3(aq) + CaCl2(aq)  →  CaCO2(S) + 2NaCl(aq) 

In this reaction, calcium carbonate is obtained as a precipitate. Hence, it is a precipitation reaction.

Q16. Explain the following in terms of gain or loss of oxygen with two examples each.

(a) Oxidation

(b) Reduction

Ans:

(a) Oxidation:  if a substance gains oxygen or loses hydrogen during a reaction, it is oxidised.€‹ Such reaction is known as oxidation. Here copper gains oxygen and gets oxidised.

2Cu + O2 heat → 2CuO

(b) Reduction

CuO  + H2 heat → Cu + H2O

ZnO + C   Zn + CO

Ans: 

(a) Oxidation: if a substance gains oxygen or loses hydrogen during a reaction, it is oxidised.€‹ Such reaction is known as oxidation.

Example1:  Copper gains oxygen and gets oxidised. 

Example2: Hydrogen gains oxygen and gets oxidised. 

(b) Reduction: If a substance loses oxygen or gains hydrogen during a reaction, it is reduced.€‹ Such reaction is called reduction.

Example1:

Here Copper loses oxygen and gets reduced. 

Example2: Here zinc loses oxygen and it gets reduced. 

ZnO + C → Zn + CO

Q17. A shiny brown coloured element ‘X’ on heating in air becomes black in colour.

Name the element ‘X’ and the black coloured compound formed.

Ans: X is copper and black coloured compound is copper oxide

Q18. Why do we apply paint on iron articles?

Ans: We apply paint on iron articles to prevent corrosion. Paints or oil keeps away iron surfaces by contacting with air or air moisture.

Q19. Oil and fat containing food items are flushed with nitrogen. Why?

Ans: Nitrogen is an anti-oxydising agent (antioxidant). It reduces the possibility of getting oxidised of food items. So Oil and fat containing food items are flushed with nitrogen. 

Q20. Explain the following terms with one example each.

(a) Corrosion :

(b) Rancidity

Ans: 

(a) Corrosion: When a metal is attacked by substances around it such as moisture, acids, etc., it is said to corrode and this process is called corrosion.€‹ Corrosion is a process of a term corrode in which metal loses in metal surface. 

Example: Rusting of iron surfaces and loses of copper's rod surface when it comes in contact of air and forms black compound copper oxide.

(b) Rancidity: When fats and oils are oxidised, they become rancid and their smell and taste change.€‹ The process of oxidising such a food material is known as Rancidity.

Example : Any oily food items which are left for a long time they get rancid. 

 

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