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1 | 2505-2508 | During the electrolysis of aqueous
sodium chloride solution, the products are NaOH, Cl2 and H2 In this
case besides Na+ and Cl– ions we also have H+ and OH– ions along with
the solvent molecules, H2O At the cathode there is competition between the following reduction
reactions:
Na+ (aq) + e– ® Na (s)
(
)
o
Ecell
= – 2 71 V
H+ (aq) + e– ® ½ H2 (g)
(
)
o
Ecell
= 0 |
1 | 2506-2509 | In this
case besides Na+ and Cl– ions we also have H+ and OH– ions along with
the solvent molecules, H2O At the cathode there is competition between the following reduction
reactions:
Na+ (aq) + e– ® Na (s)
(
)
o
Ecell
= – 2 71 V
H+ (aq) + e– ® ½ H2 (g)
(
)
o
Ecell
= 0 00 V
The reaction with higher value of Eo is preferred and therefore, the
reaction at the cathode during electrolysis is:
H+ (aq) + e– ® ½ H2 (g)
(2 |
1 | 2507-2510 | At the cathode there is competition between the following reduction
reactions:
Na+ (aq) + e– ® Na (s)
(
)
o
Ecell
= – 2 71 V
H+ (aq) + e– ® ½ H2 (g)
(
)
o
Ecell
= 0 00 V
The reaction with higher value of Eo is preferred and therefore, the
reaction at the cathode during electrolysis is:
H+ (aq) + e– ® ½ H2 (g)
(2 33)
but H+ (aq) is produced by the dissociation of H2O, i |
1 | 2508-2511 | 71 V
H+ (aq) + e– ® ½ H2 (g)
(
)
o
Ecell
= 0 00 V
The reaction with higher value of Eo is preferred and therefore, the
reaction at the cathode during electrolysis is:
H+ (aq) + e– ® ½ H2 (g)
(2 33)
but H+ (aq) is produced by the dissociation of H2O, i e |
1 | 2509-2512 | 00 V
The reaction with higher value of Eo is preferred and therefore, the
reaction at the cathode during electrolysis is:
H+ (aq) + e– ® ½ H2 (g)
(2 33)
but H+ (aq) is produced by the dissociation of H2O, i e ,
H2O (l ) ® H+ (aq) + OH– (aq)
(2 |
1 | 2510-2513 | 33)
but H+ (aq) is produced by the dissociation of H2O, i e ,
H2O (l ) ® H+ (aq) + OH– (aq)
(2 34)
Therefore, the net reaction at the cathode may be written as the sum
of (2 |
1 | 2511-2514 | e ,
H2O (l ) ® H+ (aq) + OH– (aq)
(2 34)
Therefore, the net reaction at the cathode may be written as the sum
of (2 33) and (2 |
1 | 2512-2515 | ,
H2O (l ) ® H+ (aq) + OH– (aq)
(2 34)
Therefore, the net reaction at the cathode may be written as the sum
of (2 33) and (2 34) and we have
H2O (l ) + e– ® ½H2(g) + OH–
(2 |
1 | 2513-2516 | 34)
Therefore, the net reaction at the cathode may be written as the sum
of (2 33) and (2 34) and we have
H2O (l ) + e– ® ½H2(g) + OH–
(2 35)
At the anode the following oxidation reactions are possible:
Cl– (aq) ® ½ Cl2 (g) + e–
(
)
o
Ecell
= 1 |
1 | 2514-2517 | 33) and (2 34) and we have
H2O (l ) + e– ® ½H2(g) + OH–
(2 35)
At the anode the following oxidation reactions are possible:
Cl– (aq) ® ½ Cl2 (g) + e–
(
)
o
Ecell
= 1 36 V
(2 |
1 | 2515-2518 | 34) and we have
H2O (l ) + e– ® ½H2(g) + OH–
(2 35)
At the anode the following oxidation reactions are possible:
Cl– (aq) ® ½ Cl2 (g) + e–
(
)
o
Ecell
= 1 36 V
(2 36)
2H2O (l ) ® O2 (g) + 4H+(aq) + 4e–
(
)
o
Ecell
= 1 |
1 | 2516-2519 | 35)
At the anode the following oxidation reactions are possible:
Cl– (aq) ® ½ Cl2 (g) + e–
(
)
o
Ecell
= 1 36 V
(2 36)
2H2O (l ) ® O2 (g) + 4H+(aq) + 4e–
(
)
o
Ecell
= 1 23 V
(2 |
1 | 2517-2520 | 36 V
(2 36)
2H2O (l ) ® O2 (g) + 4H+(aq) + 4e–
(
)
o
Ecell
= 1 23 V
(2 37)
The reaction at anode with lower value of E o is preferred and
therefore, water should get oxidised in preference to Cl– (aq) |
1 | 2518-2521 | 36)
2H2O (l ) ® O2 (g) + 4H+(aq) + 4e–
(
)
o
Ecell
= 1 23 V
(2 37)
The reaction at anode with lower value of E o is preferred and
therefore, water should get oxidised in preference to Cl– (aq) However,
on account of overpotential of oxygen, reaction (2 |
1 | 2519-2522 | 23 V
(2 37)
The reaction at anode with lower value of E o is preferred and
therefore, water should get oxidised in preference to Cl– (aq) However,
on account of overpotential of oxygen, reaction (2 36) is preferred |
1 | 2520-2523 | 37)
The reaction at anode with lower value of E o is preferred and
therefore, water should get oxidised in preference to Cl– (aq) However,
on account of overpotential of oxygen, reaction (2 36) is preferred Thus,
the net reactions may be summarised as:
NaCl (aq)
H O
2
→
Na+ (aq) + Cl– (aq)
Cathode:
H2O(l ) + e– ® ½ H2(g) + OH– (aq)
Anode:
Cl– (aq) ® ½ Cl2(g) + e–
Net reaction:
NaCl(aq) + H2O(l) ® Na+(aq) + OH–(aq) + ½H2(g) + ½Cl2(g)
The standard electrode potentials are replaced by electrode potentials
given by Nernst equation (Eq |
1 | 2521-2524 | However,
on account of overpotential of oxygen, reaction (2 36) is preferred Thus,
the net reactions may be summarised as:
NaCl (aq)
H O
2
→
Na+ (aq) + Cl– (aq)
Cathode:
H2O(l ) + e– ® ½ H2(g) + OH– (aq)
Anode:
Cl– (aq) ® ½ Cl2(g) + e–
Net reaction:
NaCl(aq) + H2O(l) ® Na+(aq) + OH–(aq) + ½H2(g) + ½Cl2(g)
The standard electrode potentials are replaced by electrode potentials
given by Nernst equation (Eq 2 |
1 | 2522-2525 | 36) is preferred Thus,
the net reactions may be summarised as:
NaCl (aq)
H O
2
→
Na+ (aq) + Cl– (aq)
Cathode:
H2O(l ) + e– ® ½ H2(g) + OH– (aq)
Anode:
Cl– (aq) ® ½ Cl2(g) + e–
Net reaction:
NaCl(aq) + H2O(l) ® Na+(aq) + OH–(aq) + ½H2(g) + ½Cl2(g)
The standard electrode potentials are replaced by electrode potentials
given by Nernst equation (Eq 2 8) to take into account the concentration
effects |
1 | 2523-2526 | Thus,
the net reactions may be summarised as:
NaCl (aq)
H O
2
→
Na+ (aq) + Cl– (aq)
Cathode:
H2O(l ) + e– ® ½ H2(g) + OH– (aq)
Anode:
Cl– (aq) ® ½ Cl2(g) + e–
Net reaction:
NaCl(aq) + H2O(l) ® Na+(aq) + OH–(aq) + ½H2(g) + ½Cl2(g)
The standard electrode potentials are replaced by electrode potentials
given by Nernst equation (Eq 2 8) to take into account the concentration
effects During the electrolysis of sulphuric acid, the following processes
are possible at the anode:
2H2O(l) ® O2(g) + 4H+(aq) + 4e–
(
)
o
Ecell
= +1 |
1 | 2524-2527 | 2 8) to take into account the concentration
effects During the electrolysis of sulphuric acid, the following processes
are possible at the anode:
2H2O(l) ® O2(g) + 4H+(aq) + 4e–
(
)
o
Ecell
= +1 23 V
(2 |
1 | 2525-2528 | 8) to take into account the concentration
effects During the electrolysis of sulphuric acid, the following processes
are possible at the anode:
2H2O(l) ® O2(g) + 4H+(aq) + 4e–
(
)
o
Ecell
= +1 23 V
(2 38)
Rationalised 2023-24
54
Chemistry
2SO4
2– (aq) ® S2O8
2– (aq) + 2e–
(
)
o
Ecell
= 1 |
1 | 2526-2529 | During the electrolysis of sulphuric acid, the following processes
are possible at the anode:
2H2O(l) ® O2(g) + 4H+(aq) + 4e–
(
)
o
Ecell
= +1 23 V
(2 38)
Rationalised 2023-24
54
Chemistry
2SO4
2– (aq) ® S2O8
2– (aq) + 2e–
(
)
o
Ecell
= 1 96 V
(2 |
1 | 2527-2530 | 23 V
(2 38)
Rationalised 2023-24
54
Chemistry
2SO4
2– (aq) ® S2O8
2– (aq) + 2e–
(
)
o
Ecell
= 1 96 V
(2 39)
For dilute sulphuric acid, reaction (2 |
1 | 2528-2531 | 38)
Rationalised 2023-24
54
Chemistry
2SO4
2– (aq) ® S2O8
2– (aq) + 2e–
(
)
o
Ecell
= 1 96 V
(2 39)
For dilute sulphuric acid, reaction (2 38) is preferred but at higher
concentrations of H2SO4, reaction (2 |
1 | 2529-2532 | 96 V
(2 39)
For dilute sulphuric acid, reaction (2 38) is preferred but at higher
concentrations of H2SO4, reaction (2 39) is preferred |
1 | 2530-2533 | 39)
For dilute sulphuric acid, reaction (2 38) is preferred but at higher
concentrations of H2SO4, reaction (2 39) is preferred Any battery (actually it may have one or more than one cell connected
in series) or cell that we use as a source of electrical energy is basically
a galvanic cell where the chemical energy of the redox reaction is
converted into electrical energy |
1 | 2531-2534 | 38) is preferred but at higher
concentrations of H2SO4, reaction (2 39) is preferred Any battery (actually it may have one or more than one cell connected
in series) or cell that we use as a source of electrical energy is basically
a galvanic cell where the chemical energy of the redox reaction is
converted into electrical energy However, for a battery to be of practical
use it should be reasonably light, compact and its voltage should not
vary appreciably during its use |
1 | 2532-2535 | 39) is preferred Any battery (actually it may have one or more than one cell connected
in series) or cell that we use as a source of electrical energy is basically
a galvanic cell where the chemical energy of the redox reaction is
converted into electrical energy However, for a battery to be of practical
use it should be reasonably light, compact and its voltage should not
vary appreciably during its use There are mainly two types of batteries |
1 | 2533-2536 | Any battery (actually it may have one or more than one cell connected
in series) or cell that we use as a source of electrical energy is basically
a galvanic cell where the chemical energy of the redox reaction is
converted into electrical energy However, for a battery to be of practical
use it should be reasonably light, compact and its voltage should not
vary appreciably during its use There are mainly two types of batteries In the primary batteries, the reaction occurs only once and after use
over a period of time battery becomes dead and cannot be reused
again |
1 | 2534-2537 | However, for a battery to be of practical
use it should be reasonably light, compact and its voltage should not
vary appreciably during its use There are mainly two types of batteries In the primary batteries, the reaction occurs only once and after use
over a period of time battery becomes dead and cannot be reused
again The most familiar example of this type is the dry
cell (known as Leclanche cell after its discoverer) which is
used commonly in our transistors and clocks |
1 | 2535-2538 | There are mainly two types of batteries In the primary batteries, the reaction occurs only once and after use
over a period of time battery becomes dead and cannot be reused
again The most familiar example of this type is the dry
cell (known as Leclanche cell after its discoverer) which is
used commonly in our transistors and clocks The cell
consists of a zinc container that also acts as anode and
the cathode is a carbon (graphite) rod surrounded by
powdered manganese dioxide and carbon (Fig |
1 | 2536-2539 | In the primary batteries, the reaction occurs only once and after use
over a period of time battery becomes dead and cannot be reused
again The most familiar example of this type is the dry
cell (known as Leclanche cell after its discoverer) which is
used commonly in our transistors and clocks The cell
consists of a zinc container that also acts as anode and
the cathode is a carbon (graphite) rod surrounded by
powdered manganese dioxide and carbon (Fig 2 |
1 | 2537-2540 | The most familiar example of this type is the dry
cell (known as Leclanche cell after its discoverer) which is
used commonly in our transistors and clocks The cell
consists of a zinc container that also acts as anode and
the cathode is a carbon (graphite) rod surrounded by
powdered manganese dioxide and carbon (Fig 2 8) |
1 | 2538-2541 | The cell
consists of a zinc container that also acts as anode and
the cathode is a carbon (graphite) rod surrounded by
powdered manganese dioxide and carbon (Fig 2 8) The
space between the electrodes is filled by a moist paste of
ammonium chloride (NH4Cl) and zinc chloride (ZnCl2) |
1 | 2539-2542 | 2 8) The
space between the electrodes is filled by a moist paste of
ammonium chloride (NH4Cl) and zinc chloride (ZnCl2) The
electrode reactions are complex, but they can be written
approximately as follows :
Anode:
Zn(s) ¾® Zn2+ + 2e–
Cathode:
MnO2+ NH4
++ e–¾® MnO(OH) + NH3
In the reaction at cathode, manganese is reduced
from the + 4 oxidation state to the +3 state |
1 | 2540-2543 | 8) The
space between the electrodes is filled by a moist paste of
ammonium chloride (NH4Cl) and zinc chloride (ZnCl2) The
electrode reactions are complex, but they can be written
approximately as follows :
Anode:
Zn(s) ¾® Zn2+ + 2e–
Cathode:
MnO2+ NH4
++ e–¾® MnO(OH) + NH3
In the reaction at cathode, manganese is reduced
from the + 4 oxidation state to the +3 state Ammonia
produced in the reaction forms a complex with Zn2+ to give
[Zn (NH3)4]2+ |
1 | 2541-2544 | The
space between the electrodes is filled by a moist paste of
ammonium chloride (NH4Cl) and zinc chloride (ZnCl2) The
electrode reactions are complex, but they can be written
approximately as follows :
Anode:
Zn(s) ¾® Zn2+ + 2e–
Cathode:
MnO2+ NH4
++ e–¾® MnO(OH) + NH3
In the reaction at cathode, manganese is reduced
from the + 4 oxidation state to the +3 state Ammonia
produced in the reaction forms a complex with Zn2+ to give
[Zn (NH3)4]2+ The cell has a potential of nearly 1 |
1 | 2542-2545 | The
electrode reactions are complex, but they can be written
approximately as follows :
Anode:
Zn(s) ¾® Zn2+ + 2e–
Cathode:
MnO2+ NH4
++ e–¾® MnO(OH) + NH3
In the reaction at cathode, manganese is reduced
from the + 4 oxidation state to the +3 state Ammonia
produced in the reaction forms a complex with Zn2+ to give
[Zn (NH3)4]2+ The cell has a potential of nearly 1 5 V |
1 | 2543-2546 | Ammonia
produced in the reaction forms a complex with Zn2+ to give
[Zn (NH3)4]2+ The cell has a potential of nearly 1 5 V Mercury cell, (Fig |
1 | 2544-2547 | The cell has a potential of nearly 1 5 V Mercury cell, (Fig 2 |
1 | 2545-2548 | 5 V Mercury cell, (Fig 2 9) suitable for low current devices
like hearing aids, watches, etc |
1 | 2546-2549 | Mercury cell, (Fig 2 9) suitable for low current devices
like hearing aids, watches, etc consists of zinc – mercury
amalgam as anode and a paste of HgO and carbon as the
cathode |
1 | 2547-2550 | 2 9) suitable for low current devices
like hearing aids, watches, etc consists of zinc – mercury
amalgam as anode and a paste of HgO and carbon as the
cathode The electrolyte is a paste of KOH and ZnO |
1 | 2548-2551 | 9) suitable for low current devices
like hearing aids, watches, etc consists of zinc – mercury
amalgam as anode and a paste of HgO and carbon as the
cathode The electrolyte is a paste of KOH and ZnO The
electrode reactions for the cell are given below:
Anode:
Zn(Hg) + 2OH– ¾® ZnO(s) + H2O + 2e–
Cathode:
HgO + H2O + 2e– ¾® Hg(l) + 2OH–
2 |
1 | 2549-2552 | consists of zinc – mercury
amalgam as anode and a paste of HgO and carbon as the
cathode The electrolyte is a paste of KOH and ZnO The
electrode reactions for the cell are given below:
Anode:
Zn(Hg) + 2OH– ¾® ZnO(s) + H2O + 2e–
Cathode:
HgO + H2O + 2e– ¾® Hg(l) + 2OH–
2 6 Batteries
2 |
1 | 2550-2553 | The electrolyte is a paste of KOH and ZnO The
electrode reactions for the cell are given below:
Anode:
Zn(Hg) + 2OH– ¾® ZnO(s) + H2O + 2e–
Cathode:
HgO + H2O + 2e– ¾® Hg(l) + 2OH–
2 6 Batteries
2 6 Batteries
2 |
1 | 2551-2554 | The
electrode reactions for the cell are given below:
Anode:
Zn(Hg) + 2OH– ¾® ZnO(s) + H2O + 2e–
Cathode:
HgO + H2O + 2e– ¾® Hg(l) + 2OH–
2 6 Batteries
2 6 Batteries
2 6 Batteries
2 |
1 | 2552-2555 | 6 Batteries
2 6 Batteries
2 6 Batteries
2 6 Batteries
2 |
1 | 2553-2556 | 6 Batteries
2 6 Batteries
2 6 Batteries
2 6 Batteries
2 |
1 | 2554-2557 | 6 Batteries
2 6 Batteries
2 6 Batteries
2 6 |
1 | 2555-2558 | 6 Batteries
2 6 Batteries
2 6 1 Primary
Batteries
Fig |
1 | 2556-2559 | 6 Batteries
2 6 1 Primary
Batteries
Fig 2 |
1 | 2557-2560 | 6 1 Primary
Batteries
Fig 2 8: A commercial dry cell
consists of a graphite
(carbon) cathode in a
zinc container; the latter
acts as the anode |
1 | 2558-2561 | 1 Primary
Batteries
Fig 2 8: A commercial dry cell
consists of a graphite
(carbon) cathode in a
zinc container; the latter
acts as the anode Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
2 |
1 | 2559-2562 | 2 8: A commercial dry cell
consists of a graphite
(carbon) cathode in a
zinc container; the latter
acts as the anode Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
2 10 If a current of 0 |
1 | 2560-2563 | 8: A commercial dry cell
consists of a graphite
(carbon) cathode in a
zinc container; the latter
acts as the anode Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
2 10 If a current of 0 5 ampere flows through a metallic wire for 2 hours,
then how many electrons would flow through the wire |
1 | 2561-2564 | Intext Questions
Intext Questions
Intext Questions
Intext Questions
Intext Questions
2 10 If a current of 0 5 ampere flows through a metallic wire for 2 hours,
then how many electrons would flow through the wire 2 |
1 | 2562-2565 | 10 If a current of 0 5 ampere flows through a metallic wire for 2 hours,
then how many electrons would flow through the wire 2 11 Suggest a list of metals that are extracted electrolytically |
1 | 2563-2566 | 5 ampere flows through a metallic wire for 2 hours,
then how many electrons would flow through the wire 2 11 Suggest a list of metals that are extracted electrolytically 2 |
1 | 2564-2567 | 2 11 Suggest a list of metals that are extracted electrolytically 2 12 Consider the reaction: Cr2O7
2– + 14H+ + 6e– ® 2Cr3+ + 7H2O
What is the quantity of electricity in coulombs needed to reduce 1 mol
of Cr2O7
2– |
1 | 2565-2568 | 11 Suggest a list of metals that are extracted electrolytically 2 12 Consider the reaction: Cr2O7
2– + 14H+ + 6e– ® 2Cr3+ + 7H2O
What is the quantity of electricity in coulombs needed to reduce 1 mol
of Cr2O7
2– Rationalised 2023-24
55
Electrochemistry
Fig |
1 | 2566-2569 | 2 12 Consider the reaction: Cr2O7
2– + 14H+ + 6e– ® 2Cr3+ + 7H2O
What is the quantity of electricity in coulombs needed to reduce 1 mol
of Cr2O7
2– Rationalised 2023-24
55
Electrochemistry
Fig 2 |
1 | 2567-2570 | 12 Consider the reaction: Cr2O7
2– + 14H+ + 6e– ® 2Cr3+ + 7H2O
What is the quantity of electricity in coulombs needed to reduce 1 mol
of Cr2O7
2– Rationalised 2023-24
55
Electrochemistry
Fig 2 10: The Lead storage battery |
1 | 2568-2571 | Rationalised 2023-24
55
Electrochemistry
Fig 2 10: The Lead storage battery The overall reaction is represented by
Zn(Hg) + HgO(s) ¾® ZnO(s) + Hg(l)
The cell potential is approximately
1 |
1 | 2569-2572 | 2 10: The Lead storage battery The overall reaction is represented by
Zn(Hg) + HgO(s) ¾® ZnO(s) + Hg(l)
The cell potential is approximately
1 35 V and remains constant during its
life as the overall reaction does not
involve any ion in solution whose
concentration can change during its life
time |
1 | 2570-2573 | 10: The Lead storage battery The overall reaction is represented by
Zn(Hg) + HgO(s) ¾® ZnO(s) + Hg(l)
The cell potential is approximately
1 35 V and remains constant during its
life as the overall reaction does not
involve any ion in solution whose
concentration can change during its life
time A secondary cell after use can be recharged by passing current
through it in the opposite direction so that it can be used again |
1 | 2571-2574 | The overall reaction is represented by
Zn(Hg) + HgO(s) ¾® ZnO(s) + Hg(l)
The cell potential is approximately
1 35 V and remains constant during its
life as the overall reaction does not
involve any ion in solution whose
concentration can change during its life
time A secondary cell after use can be recharged by passing current
through it in the opposite direction so that it can be used again A
good secondary cell can undergo a large number of discharging
and charging cycles |
1 | 2572-2575 | 35 V and remains constant during its
life as the overall reaction does not
involve any ion in solution whose
concentration can change during its life
time A secondary cell after use can be recharged by passing current
through it in the opposite direction so that it can be used again A
good secondary cell can undergo a large number of discharging
and charging cycles The most important secondary cell is the lead
storage battery (Fig |
1 | 2573-2576 | A secondary cell after use can be recharged by passing current
through it in the opposite direction so that it can be used again A
good secondary cell can undergo a large number of discharging
and charging cycles The most important secondary cell is the lead
storage battery (Fig 2 |
1 | 2574-2577 | A
good secondary cell can undergo a large number of discharging
and charging cycles The most important secondary cell is the lead
storage battery (Fig 2 10) commonly used in automobiles and
invertors |
1 | 2575-2578 | The most important secondary cell is the lead
storage battery (Fig 2 10) commonly used in automobiles and
invertors It consists of a lead anode and a grid of lead packed with
lead dioxide (PbO2 ) as cathode |
1 | 2576-2579 | 2 10) commonly used in automobiles and
invertors It consists of a lead anode and a grid of lead packed with
lead dioxide (PbO2 ) as cathode A 38% solution of sulphuric acid
is used as an electrolyte |
1 | 2577-2580 | 10) commonly used in automobiles and
invertors It consists of a lead anode and a grid of lead packed with
lead dioxide (PbO2 ) as cathode A 38% solution of sulphuric acid
is used as an electrolyte The cell reactions when the battery is in use are given below:
Anode:
Pb(s) + SO4
2–(aq) ® PbSO4(s) + 2e–
Cathode:
PbO2(s) + SO4
2–(aq) + 4H+(aq) + 2e– ® PbSO4 (s) + 2H2O (l)
i |
1 | 2578-2581 | It consists of a lead anode and a grid of lead packed with
lead dioxide (PbO2 ) as cathode A 38% solution of sulphuric acid
is used as an electrolyte The cell reactions when the battery is in use are given below:
Anode:
Pb(s) + SO4
2–(aq) ® PbSO4(s) + 2e–
Cathode:
PbO2(s) + SO4
2–(aq) + 4H+(aq) + 2e– ® PbSO4 (s) + 2H2O (l)
i e |
1 | 2579-2582 | A 38% solution of sulphuric acid
is used as an electrolyte The cell reactions when the battery is in use are given below:
Anode:
Pb(s) + SO4
2–(aq) ® PbSO4(s) + 2e–
Cathode:
PbO2(s) + SO4
2–(aq) + 4H+(aq) + 2e– ® PbSO4 (s) + 2H2O (l)
i e , overall cell reaction consisting of cathode and anode reactions is:
Pb(s) + PbO2(s) + 2H2SO4(aq) ® 2PbSO4(s) + 2H2O(l)
On charging the battery the reaction is reversed and PbSO4(s) on
anode and cathode is converted into Pb and PbO2, respectively |
1 | 2580-2583 | The cell reactions when the battery is in use are given below:
Anode:
Pb(s) + SO4
2–(aq) ® PbSO4(s) + 2e–
Cathode:
PbO2(s) + SO4
2–(aq) + 4H+(aq) + 2e– ® PbSO4 (s) + 2H2O (l)
i e , overall cell reaction consisting of cathode and anode reactions is:
Pb(s) + PbO2(s) + 2H2SO4(aq) ® 2PbSO4(s) + 2H2O(l)
On charging the battery the reaction is reversed and PbSO4(s) on
anode and cathode is converted into Pb and PbO2, respectively Fig |
1 | 2581-2584 | e , overall cell reaction consisting of cathode and anode reactions is:
Pb(s) + PbO2(s) + 2H2SO4(aq) ® 2PbSO4(s) + 2H2O(l)
On charging the battery the reaction is reversed and PbSO4(s) on
anode and cathode is converted into Pb and PbO2, respectively Fig 2 |
1 | 2582-2585 | , overall cell reaction consisting of cathode and anode reactions is:
Pb(s) + PbO2(s) + 2H2SO4(aq) ® 2PbSO4(s) + 2H2O(l)
On charging the battery the reaction is reversed and PbSO4(s) on
anode and cathode is converted into Pb and PbO2, respectively Fig 2 9
Commonly used
mercury cell |
1 | 2583-2586 | Fig 2 9
Commonly used
mercury cell The
reducing agent is
zinc and the
oxidising agent is
mercury (II) oxide |
1 | 2584-2587 | 2 9
Commonly used
mercury cell The
reducing agent is
zinc and the
oxidising agent is
mercury (II) oxide 2 |
1 | 2585-2588 | 9
Commonly used
mercury cell The
reducing agent is
zinc and the
oxidising agent is
mercury (II) oxide 2 6 |
1 | 2586-2589 | The
reducing agent is
zinc and the
oxidising agent is
mercury (II) oxide 2 6 2 Secondary
Batteries
Rationalised 2023-24
56
Chemistry
Positive plate
Separator
Negative plate
Another important secondary
cell is the nickel-cadmium cell
(Fig |
1 | 2587-2590 | 2 6 2 Secondary
Batteries
Rationalised 2023-24
56
Chemistry
Positive plate
Separator
Negative plate
Another important secondary
cell is the nickel-cadmium cell
(Fig 2 |
1 | 2588-2591 | 6 2 Secondary
Batteries
Rationalised 2023-24
56
Chemistry
Positive plate
Separator
Negative plate
Another important secondary
cell is the nickel-cadmium cell
(Fig 2 11) which has longer life
than the lead storage cell but
more expensive to manufacture |
1 | 2589-2592 | 2 Secondary
Batteries
Rationalised 2023-24
56
Chemistry
Positive plate
Separator
Negative plate
Another important secondary
cell is the nickel-cadmium cell
(Fig 2 11) which has longer life
than the lead storage cell but
more expensive to manufacture We shall not go into details of
working of the cell and the
electrode reactions during
charging and discharging |
1 | 2590-2593 | 2 11) which has longer life
than the lead storage cell but
more expensive to manufacture We shall not go into details of
working of the cell and the
electrode reactions during
charging and discharging The overall reaction during
discharge is:
Cd (s) + 2Ni(OH)3 (s) ® CdO (s) + 2Ni(OH)2 (s) + H2O (l )
Production of electricity by thermal plants is not a very efficient method
and is a major source of pollution |
1 | 2591-2594 | 11) which has longer life
than the lead storage cell but
more expensive to manufacture We shall not go into details of
working of the cell and the
electrode reactions during
charging and discharging The overall reaction during
discharge is:
Cd (s) + 2Ni(OH)3 (s) ® CdO (s) + 2Ni(OH)2 (s) + H2O (l )
Production of electricity by thermal plants is not a very efficient method
and is a major source of pollution In such plants, the chemical energy
(heat of combustion) of fossil fuels (coal, gas or oil) is first used for
converting water into high pressure steam |
1 | 2592-2595 | We shall not go into details of
working of the cell and the
electrode reactions during
charging and discharging The overall reaction during
discharge is:
Cd (s) + 2Ni(OH)3 (s) ® CdO (s) + 2Ni(OH)2 (s) + H2O (l )
Production of electricity by thermal plants is not a very efficient method
and is a major source of pollution In such plants, the chemical energy
(heat of combustion) of fossil fuels (coal, gas or oil) is first used for
converting water into high pressure steam This is then used to run
a turbine to produce electricity |
1 | 2593-2596 | The overall reaction during
discharge is:
Cd (s) + 2Ni(OH)3 (s) ® CdO (s) + 2Ni(OH)2 (s) + H2O (l )
Production of electricity by thermal plants is not a very efficient method
and is a major source of pollution In such plants, the chemical energy
(heat of combustion) of fossil fuels (coal, gas or oil) is first used for
converting water into high pressure steam This is then used to run
a turbine to produce electricity We know that a galvanic cell directly
converts chemical energy into electricity and is highly efficient |
1 | 2594-2597 | In such plants, the chemical energy
(heat of combustion) of fossil fuels (coal, gas or oil) is first used for
converting water into high pressure steam This is then used to run
a turbine to produce electricity We know that a galvanic cell directly
converts chemical energy into electricity and is highly efficient It is
now possible to make such cells in which reactants are fed continuously
to the electrodes and products are removed continuously from the
electrolyte compartment |
1 | 2595-2598 | This is then used to run
a turbine to produce electricity We know that a galvanic cell directly
converts chemical energy into electricity and is highly efficient It is
now possible to make such cells in which reactants are fed continuously
to the electrodes and products are removed continuously from the
electrolyte compartment Galvanic cells that are designed to convert
the energy of combustion of fuels like hydrogen, methane, methanol,
etc |
1 | 2596-2599 | We know that a galvanic cell directly
converts chemical energy into electricity and is highly efficient It is
now possible to make such cells in which reactants are fed continuously
to the electrodes and products are removed continuously from the
electrolyte compartment Galvanic cells that are designed to convert
the energy of combustion of fuels like hydrogen, methane, methanol,
etc directly into electrical energy are called fuel cells |
1 | 2597-2600 | It is
now possible to make such cells in which reactants are fed continuously
to the electrodes and products are removed continuously from the
electrolyte compartment Galvanic cells that are designed to convert
the energy of combustion of fuels like hydrogen, methane, methanol,
etc directly into electrical energy are called fuel cells One of the most successful fuel cells
uses the reaction of hydrogen with oxygen
to form water (Fig |
1 | 2598-2601 | Galvanic cells that are designed to convert
the energy of combustion of fuels like hydrogen, methane, methanol,
etc directly into electrical energy are called fuel cells One of the most successful fuel cells
uses the reaction of hydrogen with oxygen
to form water (Fig 2 |
1 | 2599-2602 | directly into electrical energy are called fuel cells One of the most successful fuel cells
uses the reaction of hydrogen with oxygen
to form water (Fig 2 12) |
1 | 2600-2603 | One of the most successful fuel cells
uses the reaction of hydrogen with oxygen
to form water (Fig 2 12) The cell was
used for providing electrical power in the
Apollo space programme |
1 | 2601-2604 | 2 12) The cell was
used for providing electrical power in the
Apollo space programme The water
vapours produced during the reaction
were condensed and added to the
drinking water supply for the astronauts |
1 | 2602-2605 | 12) The cell was
used for providing electrical power in the
Apollo space programme The water
vapours produced during the reaction
were condensed and added to the
drinking water supply for the astronauts In the cell, hydrogen and oxygen are
bubbled through porous carbon
electrodes into concentrated aqueous
sodium hydroxide solution |
1 | 2603-2606 | The cell was
used for providing electrical power in the
Apollo space programme The water
vapours produced during the reaction
were condensed and added to the
drinking water supply for the astronauts 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 |
1 | 2604-2607 | The water
vapours produced during the reaction
were condensed and added to the
drinking water supply for the astronauts 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 |
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