Chapter 1 Chemical Reactions and Equations
These
are the solutions of chapter 1 chemical reactions and equations of class 10
science of RBSE (Rajasthan education board). These solutions have been prepared
by experienced teachers.
If
you are preparing for RBSE class 10 board exams, then these solutions of intext
and end exercise questions will help you a lot.
These
solutions cover a complete syllabus and
will let you solve homework and assignments in an easy way.
Board |
RBSE |
Subject |
Science |
Chapter |
Chemical Reactions and Equations |
No. of Intext questions |
|
No. of End exercise questions |
20 |
|
|
TEXT BOOK QUESTIONS:
Answers of questions of page 6
Q.1 Why should magnesium ribbon be cleaned before burning in
air?
Ans.Magnesium
ribbon reacts with atmospheric Oxygen and form a oxide layer of Magnesium oxide
which does not allow Magnesium to burn.
That’s why Magnesium ribbon should be
cleaned before burning to remove the layer of Magnesium oxide [MgO].
Q.2 Write the balanced equation for the following chemical
reactions:
(i)Hydrogen
+Chloride→HydrogenChloride
(ii)Barium
chloride+Aluminium sulphate→Barium sulphate +Aluminium chloride
(iii)Sodium +water→Sodium
hydroxide+ Hydrogen
Ans. Balanced
equations for the reactions are as follows:
(i)H2 + Cl2→2HCl
(ii)3BaCl2+Al2Cl3→3BaSO4+2AlCl3
(iii)2Na+2H2O→2NaOH+H2
Q.3 Write a balanced chemical equation with state symbols for
the following reactions:
(i) Solutions of barium chloride and sodium sulphate in water react to
give insoluble barium sulphate
and the solution of sodium
chloride.
(ii) Sodium hydroxide solution (in water) reacts with hydrochloric acid
solution (in water) to produce sodium
chloride and water.
Ans. Balanced
chemical equations with state symbols for the reactions are as follows:
(i)BaCl2(aq) +Na2SO4(aq)→BaSO4(aq)+
NaCl(aq)
(ii) NaOH(aq)+HCl(aq)→NaCl(aq)+H2O
Answers of questions of page 10
Q.1 A solution of a substance ‘X’ is used for white washing
(i) Name the
substance ‘X’ and write its formula.
(ii) Write the reaction
of the substance ‘X’ named in (i) above with water.
Ans.
(i)In white washing the wall a solution of
quick lime is used.so substance ‘X’ is quick lime and its formula is CaO.
(ii) Substance ‘X’ [CaO] reacts with water
to form calcium hydroxide (slaked lime).
Q.2 Why is the amount of gas collected in one of the test
tubes in activity 1.7 double of the amount collected in the other? Name this
gas.
Ans. Water (H2O) contains two parts hydrogen and one
part oxygenduring electrolysis of water, on passing current water
decomposes to form hydrogen and oxygen gases. The
amountof hydrogen and oxygen produced during electrolysis of water is in a 2:1
ratio.
Electrolysis
H2O(l) ----------- →
2H2(g) + O2(g)
In
the above reaction, the balanced equation shows that during electrolysis of
water 1 mole of oxygen gas and 2 moles of hydrogen gas are produced. That’s
why, the amount of gas is double in one of the test tubes and it is hydrogen
gas.
Answers of questions of page 13
Q.1 Why does the colour of copper sulphate solution change,
when an iron nail is dipped in it?
Ans. Iron
is more active element than copper. Copper sulphate (CuSO4) solution
is of blue colour, Iron (Fe) displaces copper from its compound copper sulphate
(CuSO4) and changes to iron sulphate (FeSO4) which is green
in colour. That’s why blue colour of copper sulphate solution changes.
Fe+CuSO4→FeSO4 +Cu
Q.2 Give an example of a double displacement reaction other
than the one given in above activity 1.10
Ans. The
other example of a double displacement reaction is – mixing of solutions of
sodium carbonate and calcium chloride and in this reaction calcium carbonate
and sodium chloride are formed.
Na2CO3(aq)+CaCl2(aq)→CaCO3(s)+2NaCl(aq)
Q.3 Identify the substances oxidized and the substances
reduced in the following reactions:
(i)4Na(s)+ O2(g)
→2Na2O(s)
(ii)CuO(s) +H2→Cu+H2O
Ans .
(i).Sodium gains oxygen so it gets
oxidized and on the other hand oxygen gets reduced.
(ii)Copper oxide is reduced to copper and
hydrogen gets oxide to water.
Reaction
|
Substance
oxidised |
Substance
reduced |
(i) (ii) |
Na H2 |
O2 CuO |
Answers of EXERCISES questions
Q.1 Which of the statement 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.
Correct Ans. (i) a and b.
Q.2 Fe2O3 +2Al→Al2O3+2Fe
The above reaction is an example of
(a) Combination
reaction
(b) Double displacement
reaction
(c) Decomposition
reaction
(d) Displacement
reaction
Correct Ans. (d) Displacement reaction
Q.3 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
Correct
Ans. (a) Hydrogen gas and iron chloride are produced.
Fe(s)+dil. 2HCl(aq)→FeCl2(aq)+H2↑
Q.4 What is a balanced chemical equation? Why should the
chemical equation be balanced?
Ans. The
total numbers of atoms of reactants and products are equal in a balanced
chemical equation.
On the basis of the ‘ Law of Conservation
of mass’ – Mass can neither be created nor destroyed. So, the
total mass of reactants should be equal to the total mass of the products. That’s
why chemical equations should be balanced.
Q.5 Translate the following statements in to 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 sulphur dioxide.
(c) Barium chloride
reacts with aluminum sulphate to give aluminum chloride and precipitate of
barium sulphate.
(d) Potassium metal
reacts with water to give potassium hydroxide and hydrogen gas.
Ans. First
of all , find the reactants and products in the given statement.
(a) Following reactants and products are
given in the statement
Reactants
|
Hydrogen
and nitrogen |
Products
|
Ammonia
|
N2(g)+H2(g)→2NH3(g)
(b) Following reactants and products are
given in the statement
Reactants
|
Hydrogen
sulphide and air (oxygen) |
Products
|
Water
and sulphur di oxide |
H2S(g)+3O2(g)→2H2O(l)+SO2(g)
(c) Following reactants and products are
given in the statement
Reactants
|
Barium
chloride and aluminium sulphate |
Products
|
Barium
sulphate and Ammonium chloride |
3BaCl2(s)+Al2(SO4)3(aq) →3BaSO4↓ + AlCl3
(d) Following reactants and products are
given in the statement
Reactants
|
Potassium
and water |
Products
|
Potassium
hydroxide and hydrogen |
2K(s)+2H2O(l)→2KOH(l)+H2(g)
Q.6 Balance the following chemical equations:
(i)HNO3+Ca(OH)2→Ca(NO3)2+H2O
(ii)NaOH+H2SO4→Na2SO4+H2O
(iii)NaCl+AgNO3→BaSO4+HCl
(iv)BaCl2+H2SO4→BaSO4+HCl
Answer – Following
are the balanced chemical equations
(i)2HNO3+Ca(OH)2→Ca(NO3)2+2H2O
(ii)2NaOH+H2SO4→Na2SO4+2H2O
(iii)NaCl+AgNO3→BaSO4+HCl
(iv)BaCl2+H2SO4→BaSO4+2HCl
Q.7 Write the balanced chemical equations for the following
reactions:
(a)Calcium hydroxide +Carbon
di oxide→ 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
Answer – Write the chemical formula of
reactants and products then write the balanced chemical equation.
(a)
Reactants |
Product |
Calcium
hydroxide – Ca(OH)2 |
Calcium
carbonate - CaCO3 |
Carbon
dioxide – CO2 |
Water
– H2O |
Ca(OH)2+CO2 →CaCO3 + H2O
(b)
Reactants |
Product |
Zinc –
Zn |
Zinc nitrate
– ZnNO3 |
Silver
nitrate – AgNO3 |
Silver
- Ag |
Zn +2AgNO3 →ZnNO3+2Ag
(c)
Reactants |
Product |
Aluminium
- Al |
Aluminium
chloride- AlCl3 |
Copper
chloride – CuCl2 |
Copper
- Cu |
2Al+3CuCl2 →2AlCl3+3Cu
(d)
Reactants |
Product |
Barium
chloride- BaCl2 |
Barium
sulphate – BaSO4 |
Potassium
sulphate – K2SO4 |
Potassium
chloride - KCl |
BaCl2+K2SO4
→ BaSO4 +2KCl
Q.8 Write the balanced chemical equations for the following
reactions and identify the type of reaction:
(a)Potassium
bromide(aq)+Barium iodide(aq)→Potssium iodide(aq)+Barium bromide(aq)
(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)
Answer
(a)2KBr(aq)+BaI2(aq) →2KI(aq)BaBr2(aq)
This is a double displacement reaction.
(b)ZnCO3(s) →ZnO(s)+CO2(g)
This is a decomposition reaction.
(c)H2(g)+Cl2(g) →2HCl(g)
This is a combination reaction.
(d)Mg(s)+HCl(aq)
→MgCl2(aq)+H2(g)
This is a displacement reaction.
Q.9 What does one mean by exothermic and endothermic
reactions? Give examples.
Ans.
C + O2 → CO2
+395kJ
Endothermic reaction -Chemical reaction in which energy is absorbed or gained i is
called exothermic reaction.
N2 + O2
+180.5kJ →2NO
Q.10 Why is respiration considered as an exothermic reaction?
Explain.
Ans. Energy is essential for different life process and this energy is obtained from the food that we eat.
During digestion, large molecules of food are broken down into simpler substancessuch as glucose. Glucose combines with oxygen in the cells and in thisprocess energy is released.
The name of this reaction is
respiration. Since energy is released in the whole process, it is an exothermic
process.
Q.11 Why are decomposition reactions called opposite of combination reaction?Write equations for these reactions.
Ans.In a combination reaction two
or more substances (elements and compounds) combine to form a single substance,
whereas in a decomposition reaction one substance (compound) changes to two or
more simpler substances (elements or compounds). That’s why; a decomposition
reaction is called opposite of combination reaction.
Combination reaction
2H2 + O2→2H2O
Decomposition reaction
Electric
current
2H2O
-----------→2H2 + O2
Q.12 Write one equation each for decomposition reactions where
energy is supplied in the form of heat, light or electricity.
Ans. For
decomposition reaction, energy is required in the form of heat, light or electricity.
(i)Decomposition of lime stone (Calcium
Carbonate) into lime (calcium oxide) and carbon dioxide is carried out by
supplying heat. This is called thermal decomposition.
heat
CaCO3 ------→CaO +CO2
(ii)Decomposition of silver bromide into
silver and bromine takes place on exposure to light.This is called photolysis.
light
2AgBr-----------
→ 2Ag Br
(iii)Decomposition of water in hydrogen
and oxygen gases takes place by supplying electricity.This is called
electrolysis.
Electric current
H2O(l) ----------- → 2H2(g) + O2(g)
Q.13 What is the difference between the displacement and
double displacement reactions? Write equations for these reactions.
Ans. Displacement
reaction- more reactive element
replaces a less reactive element froma compound.
Displacement
reaction |
Double displacement reaction |
A more
reactive element displaces a less reactive element from a compound. |
There
is a mutual exchange of ions between two compounds. |
Zn+ CuSO4→ZnSO4+Cu |
BaCl2+K2SO4→BaSO4 +2KCl |
Q.14 In the refining of silver, the recovery of silver from
silver nitrate solution involved displacement by copper metal. Write down the
reaction involved.
Ans. In
the refining of silver from silver nitrate solution by copper metal, the
reaction is as follows:
Cu+2AgNO3(aq)→Cu(NO3)2(aq)
+2Ag
Q.15 What do you mean by precipitation reaction? Explain
giving examples.
Ans. A reaction in which an insoluble solid substance is formed ,
it is called precipitate and the reaction
is called a precipitation reaction.
BaCl2+Na2SO4→BaSO42NaCl
Q.16 Explain the following in terms of gain or loss of oxygen
with two examples each:
(a) Oxidation (b) reduction
Ans.
Oxidation - In this process addtion of oxygen to a
substnace
C+O2 →CO2
2Mg+O2 →2MgO
Reduction – In this process loss of oxygen
from a substance
2H2O →2H2 +O2
2MgO →2Mg +O2
Q.17 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. When
air is passed over heated copper powder, it reacts with oxygen of air to form
copper (II) oxide which is of black colour.
Element ‘X’ is copper and black coloured
compound is copper (II) oxide
Q.18 Why do we apply paint on iron articles?
Ans. For
rusting of iron articles, their open surface, oxygen and moisture are
essentially required. Applying paint, surface is covered and moreover oxygen of
air is not contact of surface of metal. Iron articles get rusted when come in
contact of air and moisture but whenthey are painted, thecontact of iron
articles from moisture and air is cut off. Hence, rusting is prevented.
Q.19 Oil and fat containing food items are flushed with
nitrogen. Why?
Ans. When
food items kept open and unprotected for some time, they give unpleasant smell
and taste of become rancid, this process is called rancidity. This happens because of oxidation of food items. Nitrogen is an inert gas and does not easily react with
these substances. That’s why bags used in packing food items are flushed with
nitrogen gas to remove oxygen inside the pack.
Q.20 Explain the following terms with an example each:
(a) Corrosion (b) rancidity
Ans. (a).
Corrosion is
defined as a process where materials, usually metals, deteriorate as a resultof
a chemical reaction with air, moisture, chemicals, etc.
Eg. - In the presence of moisture, Iron reacts
with oxygen to form hydrated iron oxide.
This hydrated iron oxide is
rust.
(b). Rancidity- The process
of oxidation of fats and oils containing food items and their smell and taste
get changed, this process is known as rancidity. For example - The taste and
smell of butter changes when kept for long.
We hope these RBSE class 10
science chapter 1 solutions will help you securing good marks in board exams.
Related Topics
Chapter | Chapter Name |
1 | |
2 | |
3 | |
4 | |
5 | |
6 | |
7 | How do Organisms Reproduce? |
8 | Heredity |
9 | Light – Reflection and Refraction |
10 | The Human Eye and the Colourful World |
11 | Electricity |
12 | Magnetic Effects of Electric Current |
13 | Our Environment |
No comments:
Post a Comment