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1 | 2605-2608 | In the cell, hydrogen and oxygen are
bubbled through porous carbon
electrodes into concentrated aqueous
sodium hydroxide solution Catalysts like
finely divided platinum or palladium
metal are incorporated into the electrodes
for increasing the rate of electrode
reactions The electrode reactions are
given below:
Cathode:
O2(g) + 2H2O(l) + 4e–¾® 4OH–(aq)
Anode:
2H2 (g) + 4OH–(aq) ¾® 4H2O(l) + 4e–
Overall reaction being:
2H2(g) + O2(g) ¾® 2H2O(l )
The cell runs continuously as long as the reactants are supplied Fuel cells produce electricity with an efficiency of about 70 % compared
Fig |
1 | 2606-2609 | Catalysts like
finely divided platinum or palladium
metal are incorporated into the electrodes
for increasing the rate of electrode
reactions The electrode reactions are
given below:
Cathode:
O2(g) + 2H2O(l) + 4e–¾® 4OH–(aq)
Anode:
2H2 (g) + 4OH–(aq) ¾® 4H2O(l) + 4e–
Overall reaction being:
2H2(g) + O2(g) ¾® 2H2O(l )
The cell runs continuously as long as the reactants are supplied Fuel cells produce electricity with an efficiency of about 70 % compared
Fig 2 |
1 | 2607-2610 | The electrode reactions are
given below:
Cathode:
O2(g) + 2H2O(l) + 4e–¾® 4OH–(aq)
Anode:
2H2 (g) + 4OH–(aq) ¾® 4H2O(l) + 4e–
Overall reaction being:
2H2(g) + O2(g) ¾® 2H2O(l )
The cell runs continuously as long as the reactants are supplied Fuel cells produce electricity with an efficiency of about 70 % compared
Fig 2 11
A rechargeable
nickel-cadmium cell
in a jelly roll
arrangement and
separated by a layer
soaked in moist
sodium or potassium
hydroxide |
1 | 2608-2611 | Fuel cells produce electricity with an efficiency of about 70 % compared
Fig 2 11
A rechargeable
nickel-cadmium cell
in a jelly roll
arrangement and
separated by a layer
soaked in moist
sodium or potassium
hydroxide 2 |
1 | 2609-2612 | 2 11
A rechargeable
nickel-cadmium cell
in a jelly roll
arrangement and
separated by a layer
soaked in moist
sodium or potassium
hydroxide 2 7 Fuel Cells
2 |
1 | 2610-2613 | 11
A rechargeable
nickel-cadmium cell
in a jelly roll
arrangement and
separated by a layer
soaked in moist
sodium or potassium
hydroxide 2 7 Fuel Cells
2 7 Fuel Cells
2 |
1 | 2611-2614 | 2 7 Fuel Cells
2 7 Fuel Cells
2 7 Fuel Cells
2 |
1 | 2612-2615 | 7 Fuel Cells
2 7 Fuel Cells
2 7 Fuel Cells
2 7 Fuel Cells
2 |
1 | 2613-2616 | 7 Fuel Cells
2 7 Fuel Cells
2 7 Fuel Cells
2 7 Fuel Cells
Fig |
1 | 2614-2617 | 7 Fuel Cells
2 7 Fuel Cells
2 7 Fuel Cells
Fig 2 |
1 | 2615-2618 | 7 Fuel Cells
2 7 Fuel Cells
Fig 2 12: Fuel cell using H2 and O2 produces electricity |
1 | 2616-2619 | 7 Fuel Cells
Fig 2 12: Fuel cell using H2 and O2 produces electricity Rationalised 2023-24
57
Electrochemistry
Fig |
1 | 2617-2620 | 2 12: Fuel cell using H2 and O2 produces electricity Rationalised 2023-24
57
Electrochemistry
Fig 2 |
1 | 2618-2621 | 12: Fuel cell using H2 and O2 produces electricity Rationalised 2023-24
57
Electrochemistry
Fig 2 13: Corrosion of iron in atmosphere
Oxidation: Fe (s)® Fe2+ (aq) +2e–
Reduction: O2
Atomospheric (g) + 4H+(aq) +4e– ® 2H2O(l)
oxidation: 2Fe2+(aq) + 2H2O(l) + ½O2(g) ® Fe2O3(s) + 4H+(aq)
to thermal plants whose efficiency is about 40% |
1 | 2619-2622 | Rationalised 2023-24
57
Electrochemistry
Fig 2 13: Corrosion of iron in atmosphere
Oxidation: Fe (s)® Fe2+ (aq) +2e–
Reduction: O2
Atomospheric (g) + 4H+(aq) +4e– ® 2H2O(l)
oxidation: 2Fe2+(aq) + 2H2O(l) + ½O2(g) ® Fe2O3(s) + 4H+(aq)
to thermal plants whose efficiency is about 40% There has been
tremendous progress in the development of new electrode materials,
better catalysts and electrolytes for increasing the efficiency of fuel cells |
1 | 2620-2623 | 2 13: Corrosion of iron in atmosphere
Oxidation: Fe (s)® Fe2+ (aq) +2e–
Reduction: O2
Atomospheric (g) + 4H+(aq) +4e– ® 2H2O(l)
oxidation: 2Fe2+(aq) + 2H2O(l) + ½O2(g) ® Fe2O3(s) + 4H+(aq)
to thermal plants whose efficiency is about 40% There has been
tremendous progress in the development of new electrode materials,
better catalysts and electrolytes for increasing the efficiency of fuel cells These have been used in automobiles on an experimental basis |
1 | 2621-2624 | 13: Corrosion of iron in atmosphere
Oxidation: Fe (s)® Fe2+ (aq) +2e–
Reduction: O2
Atomospheric (g) + 4H+(aq) +4e– ® 2H2O(l)
oxidation: 2Fe2+(aq) + 2H2O(l) + ½O2(g) ® Fe2O3(s) + 4H+(aq)
to thermal plants whose efficiency is about 40% There has been
tremendous progress in the development of new electrode materials,
better catalysts and electrolytes for increasing the efficiency of fuel cells These have been used in automobiles on an experimental basis Fuel
cells are pollution free and in view of their future importance, a variety
of fuel cells have been fabricated and tried |
1 | 2622-2625 | There has been
tremendous progress in the development of new electrode materials,
better catalysts and electrolytes for increasing the efficiency of fuel cells These have been used in automobiles on an experimental basis Fuel
cells are pollution free and in view of their future importance, a variety
of fuel cells have been fabricated and tried Corrosion slowly coats the surfaces of metallic objects with oxides or
other salts of the metal |
1 | 2623-2626 | These have been used in automobiles on an experimental basis Fuel
cells are pollution free and in view of their future importance, a variety
of fuel cells have been fabricated and tried Corrosion slowly coats the surfaces of metallic objects with oxides or
other salts of the metal The rusting of iron, tarnishing of silver,
development of green coating on copper and bronze are some of the
examples of corrosion |
1 | 2624-2627 | Fuel
cells are pollution free and in view of their future importance, a variety
of fuel cells have been fabricated and tried Corrosion slowly coats the surfaces of metallic objects with oxides or
other salts of the metal The rusting of iron, tarnishing of silver,
development of green coating on copper and bronze are some of the
examples of corrosion It causes enormous damage to
buildings, bridges, ships and to all objects made of
metals especially that of iron |
1 | 2625-2628 | Corrosion slowly coats the surfaces of metallic objects with oxides or
other salts of the metal The rusting of iron, tarnishing of silver,
development of green coating on copper and bronze are some of the
examples of corrosion It causes enormous damage to
buildings, bridges, ships and to all objects made of
metals especially that of iron We lose crores of rupees
every year on account of corrosion |
1 | 2626-2629 | The rusting of iron, tarnishing of silver,
development of green coating on copper and bronze are some of the
examples of corrosion It causes enormous damage to
buildings, bridges, ships and to all objects made of
metals especially that of iron We lose crores of rupees
every year on account of corrosion In corrosion, a metal is oxidised by loss of electrons
to oxygen and formation of oxides |
1 | 2627-2630 | It causes enormous damage to
buildings, bridges, ships and to all objects made of
metals especially that of iron We lose crores of rupees
every year on account of corrosion In corrosion, a metal is oxidised by loss of electrons
to oxygen and formation of oxides Corrosion of iron
(commonly known as rusting) occurs in presence of
water and air |
1 | 2628-2631 | We lose crores of rupees
every year on account of corrosion In corrosion, a metal is oxidised by loss of electrons
to oxygen and formation of oxides Corrosion of iron
(commonly known as rusting) occurs in presence of
water and air The chemistry of corrosion is quite
complex but it may be considered
essentially as an electrochemical
phenomenon |
1 | 2629-2632 | In corrosion, a metal is oxidised by loss of electrons
to oxygen and formation of oxides Corrosion of iron
(commonly known as rusting) occurs in presence of
water and air The chemistry of corrosion is quite
complex but it may be considered
essentially as an electrochemical
phenomenon At a particular spot
(Fig |
1 | 2630-2633 | Corrosion of iron
(commonly known as rusting) occurs in presence of
water and air The chemistry of corrosion is quite
complex but it may be considered
essentially as an electrochemical
phenomenon At a particular spot
(Fig 2 |
1 | 2631-2634 | The chemistry of corrosion is quite
complex but it may be considered
essentially as an electrochemical
phenomenon At a particular spot
(Fig 2 13) of an object made of iron,
oxidation takes place and that spot
behaves as anode and we can write
the reaction
Anode: 2 Fe (s) ¾® 2 Fe2+ + 4 e–
o
(Fe2+
/Fe)
E
= – 0 |
1 | 2632-2635 | At a particular spot
(Fig 2 13) of an object made of iron,
oxidation takes place and that spot
behaves as anode and we can write
the reaction
Anode: 2 Fe (s) ¾® 2 Fe2+ + 4 e–
o
(Fe2+
/Fe)
E
= – 0 44 V
Electrons released at anodic spot move through the metal and go
to another spot on the metal and reduce oxygen in the presence of H+
(which is believed to be available from H2CO3 formed due to dissolution
of carbon dioxide from air into water |
1 | 2633-2636 | 2 13) of an object made of iron,
oxidation takes place and that spot
behaves as anode and we can write
the reaction
Anode: 2 Fe (s) ¾® 2 Fe2+ + 4 e–
o
(Fe2+
/Fe)
E
= – 0 44 V
Electrons released at anodic spot move through the metal and go
to another spot on the metal and reduce oxygen in the presence of H+
(which is believed to be available from H2CO3 formed due to dissolution
of carbon dioxide from air into water Hydrogen ion in water may also
be available due to dissolution of other acidic oxides from the
atmosphere) |
1 | 2634-2637 | 13) of an object made of iron,
oxidation takes place and that spot
behaves as anode and we can write
the reaction
Anode: 2 Fe (s) ¾® 2 Fe2+ + 4 e–
o
(Fe2+
/Fe)
E
= – 0 44 V
Electrons released at anodic spot move through the metal and go
to another spot on the metal and reduce oxygen in the presence of H+
(which is believed to be available from H2CO3 formed due to dissolution
of carbon dioxide from air into water Hydrogen ion in water may also
be available due to dissolution of other acidic oxides from the
atmosphere) This spot behaves as cathode with the reaction
Cathode: O2(g) + 4 H+(aq) + 4 e– ¾® 2 H2O (l)
o
|
|
+
2
2
H
O
H O
=1 |
1 | 2635-2638 | 44 V
Electrons released at anodic spot move through the metal and go
to another spot on the metal and reduce oxygen in the presence of H+
(which is believed to be available from H2CO3 formed due to dissolution
of carbon dioxide from air into water Hydrogen ion in water may also
be available due to dissolution of other acidic oxides from the
atmosphere) This spot behaves as cathode with the reaction
Cathode: O2(g) + 4 H+(aq) + 4 e– ¾® 2 H2O (l)
o
|
|
+
2
2
H
O
H O
=1 23 V
E
The overall reaction being:
2Fe(s) + O2(g) + 4H+(aq) ¾® 2Fe2 +(aq) + 2 H2O (l)
o
E(cell)
=1 |
1 | 2636-2639 | Hydrogen ion in water may also
be available due to dissolution of other acidic oxides from the
atmosphere) This spot behaves as cathode with the reaction
Cathode: O2(g) + 4 H+(aq) + 4 e– ¾® 2 H2O (l)
o
|
|
+
2
2
H
O
H O
=1 23 V
E
The overall reaction being:
2Fe(s) + O2(g) + 4H+(aq) ¾® 2Fe2 +(aq) + 2 H2O (l)
o
E(cell)
=1 67 V
The ferrous ions are further oxidised by atmospheric oxygen to
ferric ions which come out as rust in the form of hydrated ferric oxide
(Fe2O3 |
1 | 2637-2640 | This spot behaves as cathode with the reaction
Cathode: O2(g) + 4 H+(aq) + 4 e– ¾® 2 H2O (l)
o
|
|
+
2
2
H
O
H O
=1 23 V
E
The overall reaction being:
2Fe(s) + O2(g) + 4H+(aq) ¾® 2Fe2 +(aq) + 2 H2O (l)
o
E(cell)
=1 67 V
The ferrous ions are further oxidised by atmospheric oxygen to
ferric ions which come out as rust in the form of hydrated ferric oxide
(Fe2O3 x H2O) and with further production of hydrogen ions |
1 | 2638-2641 | 23 V
E
The overall reaction being:
2Fe(s) + O2(g) + 4H+(aq) ¾® 2Fe2 +(aq) + 2 H2O (l)
o
E(cell)
=1 67 V
The ferrous ions are further oxidised by atmospheric oxygen to
ferric ions which come out as rust in the form of hydrated ferric oxide
(Fe2O3 x H2O) and with further production of hydrogen ions Prevention of corrosion is of prime importance |
1 | 2639-2642 | 67 V
The ferrous ions are further oxidised by atmospheric oxygen to
ferric ions which come out as rust in the form of hydrated ferric oxide
(Fe2O3 x H2O) and with further production of hydrogen ions Prevention of corrosion is of prime importance It not only saves
money but also helps in preventing accidents such as a bridge collapse
or failure of a key component due to corrosion |
1 | 2640-2643 | x H2O) and with further production of hydrogen ions Prevention of corrosion is of prime importance It not only saves
money but also helps in preventing accidents such as a bridge collapse
or failure of a key component due to corrosion One of the simplest
methods of preventing corrosion is to prevent the surface of the metallic
object to come in contact with atmosphere |
1 | 2641-2644 | Prevention of corrosion is of prime importance It not only saves
money but also helps in preventing accidents such as a bridge collapse
or failure of a key component due to corrosion One of the simplest
methods of preventing corrosion is to prevent the surface of the metallic
object to come in contact with atmosphere This can be done by covering
the surface with paint or by some chemicals (e |
1 | 2642-2645 | It not only saves
money but also helps in preventing accidents such as a bridge collapse
or failure of a key component due to corrosion One of the simplest
methods of preventing corrosion is to prevent the surface of the metallic
object to come in contact with atmosphere This can be done by covering
the surface with paint or by some chemicals (e g |
1 | 2643-2646 | One of the simplest
methods of preventing corrosion is to prevent the surface of the metallic
object to come in contact with atmosphere This can be done by covering
the surface with paint or by some chemicals (e g bisphenol) |
1 | 2644-2647 | This can be done by covering
the surface with paint or by some chemicals (e g bisphenol) Another
simple method is to cover the surface by other metals (Sn, Zn, etc |
1 | 2645-2648 | g bisphenol) Another
simple method is to cover the surface by other metals (Sn, Zn, etc ) that
are inert or react to save the object |
1 | 2646-2649 | bisphenol) Another
simple method is to cover the surface by other metals (Sn, Zn, etc ) that
are inert or react to save the object An electrochemical method is to
provide a sacrificial electrode of another metal (like Mg, Zn, etc |
1 | 2647-2650 | Another
simple method is to cover the surface by other metals (Sn, Zn, etc ) that
are inert or react to save the object An electrochemical method is to
provide a sacrificial electrode of another metal (like Mg, Zn, etc ) which
corrodes itself but saves the object |
1 | 2648-2651 | ) that
are inert or react to save the object An electrochemical method is to
provide a sacrificial electrode of another metal (like Mg, Zn, etc ) which
corrodes itself but saves the object 2 |
1 | 2649-2652 | An electrochemical method is to
provide a sacrificial electrode of another metal (like Mg, Zn, etc ) which
corrodes itself but saves the object 2 8
2 |
1 | 2650-2653 | ) which
corrodes itself but saves the object 2 8
2 8
2 |
1 | 2651-2654 | 2 8
2 8
2 8
2 |
1 | 2652-2655 | 8
2 8
2 8
2 8
2 |
1 | 2653-2656 | 8
2 8
2 8
2 8 Corrosion
Corrosion
Corrosion
Corrosion
Corrosion
Rationalised 2023-24
58
Chemistry
The Hydrogen Economy
The Hydrogen Economy
The Hydrogen Economy
The Hydrogen Economy
The Hydrogen Economy
At present the main source of energy that is driving our economy is fossil fuels
such as coal, oil and gas |
1 | 2654-2657 | 8
2 8
2 8 Corrosion
Corrosion
Corrosion
Corrosion
Corrosion
Rationalised 2023-24
58
Chemistry
The Hydrogen Economy
The Hydrogen Economy
The Hydrogen Economy
The Hydrogen Economy
The Hydrogen Economy
At present the main source of energy that is driving our economy is fossil fuels
such as coal, oil and gas As more people on the planet aspire to improve their
standard of living, their energy requirement will increase |
1 | 2655-2658 | 8
2 8 Corrosion
Corrosion
Corrosion
Corrosion
Corrosion
Rationalised 2023-24
58
Chemistry
The Hydrogen Economy
The Hydrogen Economy
The Hydrogen Economy
The Hydrogen Economy
The Hydrogen Economy
At present the main source of energy that is driving our economy is fossil fuels
such as coal, oil and gas As more people on the planet aspire to improve their
standard of living, their energy requirement will increase In fact, the per
capita consumption of energy used is a measure of development |
1 | 2656-2659 | 8 Corrosion
Corrosion
Corrosion
Corrosion
Corrosion
Rationalised 2023-24
58
Chemistry
The Hydrogen Economy
The Hydrogen Economy
The Hydrogen Economy
The Hydrogen Economy
The Hydrogen Economy
At present the main source of energy that is driving our economy is fossil fuels
such as coal, oil and gas As more people on the planet aspire to improve their
standard of living, their energy requirement will increase In fact, the per
capita consumption of energy used is a measure of development Of course, it
is assumed that energy is used for productive purpose and not merely wasted |
1 | 2657-2660 | As more people on the planet aspire to improve their
standard of living, their energy requirement will increase In fact, the per
capita consumption of energy used is a measure of development Of course, it
is assumed that energy is used for productive purpose and not merely wasted We are already aware that carbon dioxide produced by the combustion of fossil
fuels is resulting in the ‘Greenhouse Effect’ |
1 | 2658-2661 | In fact, the per
capita consumption of energy used is a measure of development Of course, it
is assumed that energy is used for productive purpose and not merely wasted We are already aware that carbon dioxide produced by the combustion of fossil
fuels is resulting in the ‘Greenhouse Effect’ This is leading to a rise in the
temperature of the Earth’s surface, causing polar ice to melt and ocean levels
to rise |
1 | 2659-2662 | Of course, it
is assumed that energy is used for productive purpose and not merely wasted We are already aware that carbon dioxide produced by the combustion of fossil
fuels is resulting in the ‘Greenhouse Effect’ This is leading to a rise in the
temperature of the Earth’s surface, causing polar ice to melt and ocean levels
to rise This will flood low-lying areas along the coast and some island nations
such as Maldives face total submergence |
1 | 2660-2663 | We are already aware that carbon dioxide produced by the combustion of fossil
fuels is resulting in the ‘Greenhouse Effect’ This is leading to a rise in the
temperature of the Earth’s surface, causing polar ice to melt and ocean levels
to rise This will flood low-lying areas along the coast and some island nations
such as Maldives face total submergence In order to avoid such a catastrope,
we need to limit our use of carbonaceous fuels |
1 | 2661-2664 | This is leading to a rise in the
temperature of the Earth’s surface, causing polar ice to melt and ocean levels
to rise This will flood low-lying areas along the coast and some island nations
such as Maldives face total submergence In order to avoid such a catastrope,
we need to limit our use of carbonaceous fuels Hydrogen provides an ideal
alternative as its combustion results in water only |
1 | 2662-2665 | This will flood low-lying areas along the coast and some island nations
such as Maldives face total submergence In order to avoid such a catastrope,
we need to limit our use of carbonaceous fuels Hydrogen provides an ideal
alternative as its combustion results in water only Hydrogen production must
come from splitting water using solar energy |
1 | 2663-2666 | In order to avoid such a catastrope,
we need to limit our use of carbonaceous fuels Hydrogen provides an ideal
alternative as its combustion results in water only Hydrogen production must
come from splitting water using solar energy Therefore, hydrogen can be used
as a renewable and non polluting source of energy |
1 | 2664-2667 | Hydrogen provides an ideal
alternative as its combustion results in water only Hydrogen production must
come from splitting water using solar energy Therefore, hydrogen can be used
as a renewable and non polluting source of energy This is the vision of the
Hydrogen Economy |
1 | 2665-2668 | Hydrogen production must
come from splitting water using solar energy Therefore, hydrogen can be used
as a renewable and non polluting source of energy This is the vision of the
Hydrogen Economy Both the production of hydrogen by electrolysis of water
and hydrogen combustion in a fuel cell will be important in the future |
1 | 2666-2669 | Therefore, hydrogen can be used
as a renewable and non polluting source of energy This is the vision of the
Hydrogen Economy Both the production of hydrogen by electrolysis of water
and hydrogen combustion in a fuel cell will be important in the future And
both these technologies are based on electrochemical principles |
1 | 2667-2670 | This is the vision of the
Hydrogen Economy Both the production of hydrogen by electrolysis of water
and hydrogen combustion in a fuel cell will be important in the future And
both these technologies are based on electrochemical principles Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
2 |
1 | 2668-2671 | Both the production of hydrogen by electrolysis of water
and hydrogen combustion in a fuel cell will be important in the future And
both these technologies are based on electrochemical principles Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
2 13 Write the chemistry of recharging the lead storage battery, highlighting
all the materials that are involved during recharging |
1 | 2669-2672 | And
both these technologies are based on electrochemical principles Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
2 13 Write the chemistry of recharging the lead storage battery, highlighting
all the materials that are involved during recharging 2 |
1 | 2670-2673 | Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
2 13 Write the chemistry of recharging the lead storage battery, highlighting
all the materials that are involved during recharging 2 14 Suggest two materials other than hydrogen that can be used as fuels in
fuel cells |
1 | 2671-2674 | 13 Write the chemistry of recharging the lead storage battery, highlighting
all the materials that are involved during recharging 2 14 Suggest two materials other than hydrogen that can be used as fuels in
fuel cells 2 |
1 | 2672-2675 | 2 14 Suggest two materials other than hydrogen that can be used as fuels in
fuel cells 2 15 Explain how rusting of iron is envisaged as setting up of an
electrochemical cell |
1 | 2673-2676 | 14 Suggest two materials other than hydrogen that can be used as fuels in
fuel cells 2 15 Explain how rusting of iron is envisaged as setting up of an
electrochemical cell Summary
Summary
Summary
Summary
Summary
An electrochemical cell consists of two metallic electrodes dipping in electrolytic
solution(s) |
1 | 2674-2677 | 2 15 Explain how rusting of iron is envisaged as setting up of an
electrochemical cell Summary
Summary
Summary
Summary
Summary
An electrochemical cell consists of two metallic electrodes dipping in electrolytic
solution(s) Thus an important component of the electrochemical cell is the ionic
conductor or electrolyte |
1 | 2675-2678 | 15 Explain how rusting of iron is envisaged as setting up of an
electrochemical cell Summary
Summary
Summary
Summary
Summary
An electrochemical cell consists of two metallic electrodes dipping in electrolytic
solution(s) Thus an important component of the electrochemical cell is the ionic
conductor or electrolyte Electrochemical cells are of two types |
1 | 2676-2679 | Summary
Summary
Summary
Summary
Summary
An electrochemical cell consists of two metallic electrodes dipping in electrolytic
solution(s) Thus an important component of the electrochemical cell is the ionic
conductor or electrolyte Electrochemical cells are of two types In galvanic cell,
the chemical energy of a spontaneous redox reaction is converted into electrical
work, whereas in an electrolytic cell, electrical energy is used to carry out a non-
spontaneous redox reaction |
1 | 2677-2680 | Thus an important component of the electrochemical cell is the ionic
conductor or electrolyte Electrochemical cells are of two types In galvanic cell,
the chemical energy of a spontaneous redox reaction is converted into electrical
work, whereas in an electrolytic cell, electrical energy is used to carry out a non-
spontaneous redox reaction The standard electrode potential for any electrode
dipping in an appropriate solution is defined with respect to standard electrode
potential of hydrogen electrode taken as zero |
1 | 2678-2681 | Electrochemical cells are of two types In galvanic cell,
the chemical energy of a spontaneous redox reaction is converted into electrical
work, whereas in an electrolytic cell, electrical energy is used to carry out a non-
spontaneous redox reaction The standard electrode potential for any electrode
dipping in an appropriate solution is defined with respect to standard electrode
potential of hydrogen electrode taken as zero The standard potential of the cell
can be obtained by taking the difference of the standard potentials of cathode and
anode (
(
)
o
Ecell
= Eocathode – Eoanode) |
1 | 2679-2682 | In galvanic cell,
the chemical energy of a spontaneous redox reaction is converted into electrical
work, whereas in an electrolytic cell, electrical energy is used to carry out a non-
spontaneous redox reaction The standard electrode potential for any electrode
dipping in an appropriate solution is defined with respect to standard electrode
potential of hydrogen electrode taken as zero The standard potential of the cell
can be obtained by taking the difference of the standard potentials of cathode and
anode (
(
)
o
Ecell
= Eocathode – Eoanode) The standard potential of the cells are
related to standard Gibbs energy (DrGo = –nF
(
)
o
Ecell
) and equilibrium constant
(DrGo = – RT ln K) of the reaction taking place in the cell |
1 | 2680-2683 | The standard electrode potential for any electrode
dipping in an appropriate solution is defined with respect to standard electrode
potential of hydrogen electrode taken as zero The standard potential of the cell
can be obtained by taking the difference of the standard potentials of cathode and
anode (
(
)
o
Ecell
= Eocathode – Eoanode) The standard potential of the cells are
related to standard Gibbs energy (DrGo = –nF
(
)
o
Ecell
) and equilibrium constant
(DrGo = – RT ln K) of the reaction taking place in the cell Concentration dependence
of the potentials of the electrodes and the cells are given by Nernst equation |
1 | 2681-2684 | The standard potential of the cell
can be obtained by taking the difference of the standard potentials of cathode and
anode (
(
)
o
Ecell
= Eocathode – Eoanode) The standard potential of the cells are
related to standard Gibbs energy (DrGo = –nF
(
)
o
Ecell
) and equilibrium constant
(DrGo = – RT ln K) of the reaction taking place in the cell Concentration dependence
of the potentials of the electrodes and the cells are given by Nernst equation The conductivity, k, of an electrolytic solution depends on the concentration
of the electrolyte, nature of solvent and temperature |
1 | 2682-2685 | The standard potential of the cells are
related to standard Gibbs energy (DrGo = –nF
(
)
o
Ecell
) and equilibrium constant
(DrGo = – RT ln K) of the reaction taking place in the cell Concentration dependence
of the potentials of the electrodes and the cells are given by Nernst equation The conductivity, k, of an electrolytic solution depends on the concentration
of the electrolyte, nature of solvent and temperature Molar conductivity, Lm, is
defined by = k/c where c is the concentration |
1 | 2683-2686 | Concentration dependence
of the potentials of the electrodes and the cells are given by Nernst equation The conductivity, k, of an electrolytic solution depends on the concentration
of the electrolyte, nature of solvent and temperature Molar conductivity, Lm, is
defined by = k/c where c is the concentration Conductivity decreases but molar
conductivity increases with decrease in concentration |
1 | 2684-2687 | The conductivity, k, of an electrolytic solution depends on the concentration
of the electrolyte, nature of solvent and temperature Molar conductivity, Lm, is
defined by = k/c where c is the concentration Conductivity decreases but molar
conductivity increases with decrease in concentration It increases slowly with
decrease in concentration for strong electrolytes while the increase is very steep
for weak electrolytes in very dilute solutions |
1 | 2685-2688 | Molar conductivity, Lm, is
defined by = k/c where c is the concentration Conductivity decreases but molar
conductivity increases with decrease in concentration It increases slowly with
decrease in concentration for strong electrolytes while the increase is very steep
for weak electrolytes in very dilute solutions Kohlrausch found that molar
conductivity at infinite dilution, for an electrolyte is sum of the contribution of the
Rationalised 2023-24
59
Electrochemistry
molar conductivity of the ions in which it dissociates |
1 | 2686-2689 | Conductivity decreases but molar
conductivity increases with decrease in concentration It increases slowly with
decrease in concentration for strong electrolytes while the increase is very steep
for weak electrolytes in very dilute solutions Kohlrausch found that molar
conductivity at infinite dilution, for an electrolyte is sum of the contribution of the
Rationalised 2023-24
59
Electrochemistry
molar conductivity of the ions in which it dissociates It is known as law of
independent migration of ions and has many applications |
1 | 2687-2690 | It increases slowly with
decrease in concentration for strong electrolytes while the increase is very steep
for weak electrolytes in very dilute solutions Kohlrausch found that molar
conductivity at infinite dilution, for an electrolyte is sum of the contribution of the
Rationalised 2023-24
59
Electrochemistry
molar conductivity of the ions in which it dissociates It is known as law of
independent migration of ions and has many applications Ions conduct electricity
through the solution but oxidation and reduction of the ions take place at the
electrodes in an electrochemical cell |
1 | 2688-2691 | Kohlrausch found that molar
conductivity at infinite dilution, for an electrolyte is sum of the contribution of the
Rationalised 2023-24
59
Electrochemistry
molar conductivity of the ions in which it dissociates It is known as law of
independent migration of ions and has many applications Ions conduct electricity
through the solution but oxidation and reduction of the ions take place at the
electrodes in an electrochemical cell Batteries and fuel cells are very useful
forms of galvanic cell |
1 | 2689-2692 | It is known as law of
independent migration of ions and has many applications Ions conduct electricity
through the solution but oxidation and reduction of the ions take place at the
electrodes in an electrochemical cell Batteries and fuel cells are very useful
forms of galvanic cell Corrosion of metals is essentially an electrochemical
phenomenon |
1 | 2690-2693 | Ions conduct electricity
through the solution but oxidation and reduction of the ions take place at the
electrodes in an electrochemical cell Batteries and fuel cells are very useful
forms of galvanic cell Corrosion of metals is essentially an electrochemical
phenomenon Electrochemical principles are relevant to the Hydrogen Economy |
1 | 2691-2694 | Batteries and fuel cells are very useful
forms of galvanic cell Corrosion of metals is essentially an electrochemical
phenomenon Electrochemical principles are relevant to the Hydrogen Economy 2 |
1 | 2692-2695 | Corrosion of metals is essentially an electrochemical
phenomenon Electrochemical principles are relevant to the Hydrogen Economy 2 1
Arrange the following metals in the order in which they displace each other
from the solution of their salts |
1 | 2693-2696 | Electrochemical principles are relevant to the Hydrogen Economy 2 1
Arrange the following metals in the order in which they displace each other
from the solution of their salts Al, Cu, Fe, Mg and Zn |
1 | 2694-2697 | 2 1
Arrange the following metals in the order in which they displace each other
from the solution of their salts Al, Cu, Fe, Mg and Zn 2 |
1 | 2695-2698 | 1
Arrange the following metals in the order in which they displace each other
from the solution of their salts Al, Cu, Fe, Mg and Zn 2 2
Given the standard electrode potentials,
K+/K = –2 |
1 | 2696-2699 | Al, Cu, Fe, Mg and Zn 2 2
Given the standard electrode potentials,
K+/K = –2 93V, Ag+/Ag = 0 |
1 | 2697-2700 | 2 2
Given the standard electrode potentials,
K+/K = –2 93V, Ag+/Ag = 0 80V,
Hg2+/Hg = 0 |
1 | 2698-2701 | 2
Given the standard electrode potentials,
K+/K = –2 93V, Ag+/Ag = 0 80V,
Hg2+/Hg = 0 79V
Mg2+/Mg = –2 |
1 | 2699-2702 | 93V, Ag+/Ag = 0 80V,
Hg2+/Hg = 0 79V
Mg2+/Mg = –2 37 V, Cr3+/Cr = – 0 |
1 | 2700-2703 | 80V,
Hg2+/Hg = 0 79V
Mg2+/Mg = –2 37 V, Cr3+/Cr = – 0 74V
Arrange these metals in their increasing order of reducing power |
1 | 2701-2704 | 79V
Mg2+/Mg = –2 37 V, Cr3+/Cr = – 0 74V
Arrange these metals in their increasing order of reducing power 2 |
1 | 2702-2705 | 37 V, Cr3+/Cr = – 0 74V
Arrange these metals in their increasing order of reducing power 2 3
Depict the galvanic cell in which the reaction
Zn(s)+2Ag+(aq) ®Zn2+(aq)+2Ag(s) takes place |
1 | 2703-2706 | 74V
Arrange these metals in their increasing order of reducing power 2 3
Depict the galvanic cell in which the reaction
Zn(s)+2Ag+(aq) ®Zn2+(aq)+2Ag(s) takes place Further show:
(i) Which of the electrode is negatively charged |
1 | 2704-2707 | 2 3
Depict the galvanic cell in which the reaction
Zn(s)+2Ag+(aq) ®Zn2+(aq)+2Ag(s) takes place Further show:
(i) Which of the electrode is negatively charged (ii) The carriers of the current in the cell |
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