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1 | 1805-1808 | 2
Electrochemistry
Unit
Unit
Unit
Unit2Unit
Electrochemistry
Rationalised 2023-24
32
Chemistry
Cu
Eext >1 1
e
–
Current
Cathode
+ve
Anode
–ve
Zn
Fig 2 2
Functioning of Daniell
cell
when
external
voltage Eext opposing the
cell potential is applied |
1 | 1806-1809 | 1
e
–
Current
Cathode
+ve
Anode
–ve
Zn
Fig 2 2
Functioning of Daniell
cell
when
external
voltage Eext opposing the
cell potential is applied We had studied the construction and functioning of Daniell cell
(Fig |
1 | 1807-1810 | 2 2
Functioning of Daniell
cell
when
external
voltage Eext opposing the
cell potential is applied We had studied the construction and functioning of Daniell cell
(Fig 2 |
1 | 1808-1811 | 2
Functioning of Daniell
cell
when
external
voltage Eext opposing the
cell potential is applied We had studied the construction and functioning of Daniell cell
(Fig 2 1) |
1 | 1809-1812 | We had studied the construction and functioning of Daniell cell
(Fig 2 1) This cell converts the chemical energy liberated during the
redox reaction
Zn(s) + Cu2+(aq) ® Zn2+(aq) + Cu(s)
(2 |
1 | 1810-1813 | 2 1) This cell converts the chemical energy liberated during the
redox reaction
Zn(s) + Cu2+(aq) ® Zn2+(aq) + Cu(s)
(2 1)
to electrical energy and has an electrical
potential equal to 1 |
1 | 1811-1814 | 1) This cell converts the chemical energy liberated during the
redox reaction
Zn(s) + Cu2+(aq) ® Zn2+(aq) + Cu(s)
(2 1)
to electrical energy and has an electrical
potential equal to 1 1 V when concentration
of Zn2+ and Cu2+ ions is unity (1 mol dm–3)* |
1 | 1812-1815 | This cell converts the chemical energy liberated during the
redox reaction
Zn(s) + Cu2+(aq) ® Zn2+(aq) + Cu(s)
(2 1)
to electrical energy and has an electrical
potential equal to 1 1 V when concentration
of Zn2+ and Cu2+ ions is unity (1 mol dm–3)* Such a device is called a galvanic or a
voltaic cell |
1 | 1813-1816 | 1)
to electrical energy and has an electrical
potential equal to 1 1 V when concentration
of Zn2+ and Cu2+ ions is unity (1 mol dm–3)* Such a device is called a galvanic or a
voltaic cell If an external opposite potential is applied
in the galvanic cell [Fig |
1 | 1814-1817 | 1 V when concentration
of Zn2+ and Cu2+ ions is unity (1 mol dm–3)* Such a device is called a galvanic or a
voltaic cell If an external opposite potential is applied
in the galvanic cell [Fig 2 |
1 | 1815-1818 | Such a device is called a galvanic or a
voltaic cell If an external opposite potential is applied
in the galvanic cell [Fig 2 2(a)] and increased
slowly, we find that the reaction continues to
take place till the opposing voltage reaches
the value 1 |
1 | 1816-1819 | If an external opposite potential is applied
in the galvanic cell [Fig 2 2(a)] and increased
slowly, we find that the reaction continues to
take place till the opposing voltage reaches
the value 1 1 V [Fig |
1 | 1817-1820 | 2 2(a)] and increased
slowly, we find that the reaction continues to
take place till the opposing voltage reaches
the value 1 1 V [Fig 2 |
1 | 1818-1821 | 2(a)] and increased
slowly, we find that the reaction continues to
take place till the opposing voltage reaches
the value 1 1 V [Fig 2 2(b)] when, the reaction
stops altogether and no current flows through
the cell |
1 | 1819-1822 | 1 V [Fig 2 2(b)] when, the reaction
stops altogether and no current flows through
the cell Any further increase in the external
potential again starts the reaction but in the
opposite direction [Fig |
1 | 1820-1823 | 2 2(b)] when, the reaction
stops altogether and no current flows through
the cell Any further increase in the external
potential again starts the reaction but in the
opposite direction [Fig 2 |
1 | 1821-1824 | 2(b)] when, the reaction
stops altogether and no current flows through
the cell Any further increase in the external
potential again starts the reaction but in the
opposite direction [Fig 2 2(c)] |
1 | 1822-1825 | Any further increase in the external
potential again starts the reaction but in the
opposite direction [Fig 2 2(c)] It now functions
as an electrolytic cell, a device for using
electrical energy to carry non-spontaneous
chemical reactions |
1 | 1823-1826 | 2 2(c)] It now functions
as an electrolytic cell, a device for using
electrical energy to carry non-spontaneous
chemical reactions Both types of cells are
quite important and we shall study some of
their salient features in the following pages |
1 | 1824-1827 | 2(c)] It now functions
as an electrolytic cell, a device for using
electrical energy to carry non-spontaneous
chemical reactions Both types of cells are
quite important and we shall study some of
their salient features in the following pages *Strictly speaking activity should be used instead of concentration |
1 | 1825-1828 | It now functions
as an electrolytic cell, a device for using
electrical energy to carry non-spontaneous
chemical reactions Both types of cells are
quite important and we shall study some of
their salient features in the following pages *Strictly speaking activity should be used instead of concentration It is directly proportional to concentration |
1 | 1826-1829 | Both types of cells are
quite important and we shall study some of
their salient features in the following pages *Strictly speaking activity should be used instead of concentration It is directly proportional to concentration In dilute
solutions, it is equal to concentration |
1 | 1827-1830 | *Strictly speaking activity should be used instead of concentration It is directly proportional to concentration In dilute
solutions, it is equal to concentration You will study more about it in higher classes |
1 | 1828-1831 | It is directly proportional to concentration In dilute
solutions, it is equal to concentration You will study more about it in higher classes 2 |
1 | 1829-1832 | In dilute
solutions, it is equal to concentration You will study more about it in higher classes 2 1
2 |
1 | 1830-1833 | You will study more about it in higher classes 2 1
2 1
2 |
1 | 1831-1834 | 2 1
2 1
2 1
2 |
1 | 1832-1835 | 1
2 1
2 1
2 1
2 |
1 | 1833-1836 | 1
2 1
2 1
2 1 Electrochemical
Electrochemical
Electrochemical
Electrochemical
Electrochemical
Cells
Cells
Cells
Cells
Cells
Fig |
1 | 1834-1837 | 1
2 1
2 1 Electrochemical
Electrochemical
Electrochemical
Electrochemical
Electrochemical
Cells
Cells
Cells
Cells
Cells
Fig 2 |
1 | 1835-1838 | 1
2 1 Electrochemical
Electrochemical
Electrochemical
Electrochemical
Electrochemical
Cells
Cells
Cells
Cells
Cells
Fig 2 1: Daniell cell having electrodes of zinc and
copper dipping in the solutions of their
respective salts |
1 | 1836-1839 | 1 Electrochemical
Electrochemical
Electrochemical
Electrochemical
Electrochemical
Cells
Cells
Cells
Cells
Cells
Fig 2 1: Daniell cell having electrodes of zinc and
copper dipping in the solutions of their
respective salts salt
bridge
Zn
Cu
anode
cathode
current
ZnSO4
CuSO4
E
<
ext 1 |
1 | 1837-1840 | 2 1: Daniell cell having electrodes of zinc and
copper dipping in the solutions of their
respective salts salt
bridge
Zn
Cu
anode
cathode
current
ZnSO4
CuSO4
E
<
ext 1 1V
e
-ve
+ve
I=0
Zn
Cu
ZnSO4
CuSO4
E
ext=
1 |
1 | 1838-1841 | 1: Daniell cell having electrodes of zinc and
copper dipping in the solutions of their
respective salts salt
bridge
Zn
Cu
anode
cathode
current
ZnSO4
CuSO4
E
<
ext 1 1V
e
-ve
+ve
I=0
Zn
Cu
ZnSO4
CuSO4
E
ext=
1 1V
When Eext < 1 |
1 | 1839-1842 | salt
bridge
Zn
Cu
anode
cathode
current
ZnSO4
CuSO4
E
<
ext 1 1V
e
-ve
+ve
I=0
Zn
Cu
ZnSO4
CuSO4
E
ext=
1 1V
When Eext < 1 1 V
(i) Electrons flow from Zn rod to
Cu rod hence current flows
from Cu to Zn |
1 | 1840-1843 | 1V
e
-ve
+ve
I=0
Zn
Cu
ZnSO4
CuSO4
E
ext=
1 1V
When Eext < 1 1 V
(i) Electrons flow from Zn rod to
Cu rod hence current flows
from Cu to Zn (ii) Zn dissolves at anode and
copper deposits at cathode |
1 | 1841-1844 | 1V
When Eext < 1 1 V
(i) Electrons flow from Zn rod to
Cu rod hence current flows
from Cu to Zn (ii) Zn dissolves at anode and
copper deposits at cathode When Eext = 1 |
1 | 1842-1845 | 1 V
(i) Electrons flow from Zn rod to
Cu rod hence current flows
from Cu to Zn (ii) Zn dissolves at anode and
copper deposits at cathode When Eext = 1 1 V
(i) No flow of
electrons or
current |
1 | 1843-1846 | (ii) Zn dissolves at anode and
copper deposits at cathode When Eext = 1 1 V
(i) No flow of
electrons or
current (ii) No chemical
reaction |
1 | 1844-1847 | When Eext = 1 1 V
(i) No flow of
electrons or
current (ii) No chemical
reaction When Eext > 1 |
1 | 1845-1848 | 1 V
(i) No flow of
electrons or
current (ii) No chemical
reaction When Eext > 1 1 V
(i) Electrons flow
from Cu to Zn
and current flows
from Zn to Cu |
1 | 1846-1849 | (ii) No chemical
reaction When Eext > 1 1 V
(i) Electrons flow
from Cu to Zn
and current flows
from Zn to Cu (ii) Zinc is deposited
at the zinc
electrode and
copper dissolves at
copper electrode |
1 | 1847-1850 | When Eext > 1 1 V
(i) Electrons flow
from Cu to Zn
and current flows
from Zn to Cu (ii) Zinc is deposited
at the zinc
electrode and
copper dissolves at
copper electrode (a)
(b)
(c)
Rationalised 2023-24
33
Electrochemistry
As mentioned earlier a galvanic cell is an electrochemical cell that
converts the chemical energy of a spontaneous redox reaction into
electrical energy |
1 | 1848-1851 | 1 V
(i) Electrons flow
from Cu to Zn
and current flows
from Zn to Cu (ii) Zinc is deposited
at the zinc
electrode and
copper dissolves at
copper electrode (a)
(b)
(c)
Rationalised 2023-24
33
Electrochemistry
As mentioned earlier a galvanic cell is an electrochemical cell that
converts the chemical energy of a spontaneous redox reaction into
electrical energy In this device the Gibbs energy of the spontaneous
redox reaction is converted into electrical work which may be used for
running a motor or other electrical gadgets like heater, fan,
geyser, etc |
1 | 1849-1852 | (ii) Zinc is deposited
at the zinc
electrode and
copper dissolves at
copper electrode (a)
(b)
(c)
Rationalised 2023-24
33
Electrochemistry
As mentioned earlier a galvanic cell is an electrochemical cell that
converts the chemical energy of a spontaneous redox reaction into
electrical energy In this device the Gibbs energy of the spontaneous
redox reaction is converted into electrical work which may be used for
running a motor or other electrical gadgets like heater, fan,
geyser, etc Daniell cell discussed earlier is one such cell in which the following
redox reaction occurs |
1 | 1850-1853 | (a)
(b)
(c)
Rationalised 2023-24
33
Electrochemistry
As mentioned earlier a galvanic cell is an electrochemical cell that
converts the chemical energy of a spontaneous redox reaction into
electrical energy In this device the Gibbs energy of the spontaneous
redox reaction is converted into electrical work which may be used for
running a motor or other electrical gadgets like heater, fan,
geyser, etc Daniell cell discussed earlier is one such cell in which the following
redox reaction occurs Zn(s) + Cu2+(aq) ® Zn2+ (aq) + Cu(s)
This reaction is a combination of two half reactions whose addition
gives the overall cell reaction:
(i) Cu2+ + 2e– ® Cu(s)
(reduction half reaction)
(2 |
1 | 1851-1854 | In this device the Gibbs energy of the spontaneous
redox reaction is converted into electrical work which may be used for
running a motor or other electrical gadgets like heater, fan,
geyser, etc Daniell cell discussed earlier is one such cell in which the following
redox reaction occurs Zn(s) + Cu2+(aq) ® Zn2+ (aq) + Cu(s)
This reaction is a combination of two half reactions whose addition
gives the overall cell reaction:
(i) Cu2+ + 2e– ® Cu(s)
(reduction half reaction)
(2 2)
(ii) Zn(s) ® Zn2+ + 2e–
(oxidation half reaction)
(2 |
1 | 1852-1855 | Daniell cell discussed earlier is one such cell in which the following
redox reaction occurs Zn(s) + Cu2+(aq) ® Zn2+ (aq) + Cu(s)
This reaction is a combination of two half reactions whose addition
gives the overall cell reaction:
(i) Cu2+ + 2e– ® Cu(s)
(reduction half reaction)
(2 2)
(ii) Zn(s) ® Zn2+ + 2e–
(oxidation half reaction)
(2 3)
These reactions occur in two different portions of the Daniell cell |
1 | 1853-1856 | Zn(s) + Cu2+(aq) ® Zn2+ (aq) + Cu(s)
This reaction is a combination of two half reactions whose addition
gives the overall cell reaction:
(i) Cu2+ + 2e– ® Cu(s)
(reduction half reaction)
(2 2)
(ii) Zn(s) ® Zn2+ + 2e–
(oxidation half reaction)
(2 3)
These reactions occur in two different portions of the Daniell cell The reduction half reaction occurs on the copper electrode while the
oxidation half reaction occurs on the zinc electrode |
1 | 1854-1857 | 2)
(ii) Zn(s) ® Zn2+ + 2e–
(oxidation half reaction)
(2 3)
These reactions occur in two different portions of the Daniell cell The reduction half reaction occurs on the copper electrode while the
oxidation half reaction occurs on the zinc electrode These two portions
of the cell are also called half-cells or redox couples |
1 | 1855-1858 | 3)
These reactions occur in two different portions of the Daniell cell The reduction half reaction occurs on the copper electrode while the
oxidation half reaction occurs on the zinc electrode These two portions
of the cell are also called half-cells or redox couples The copper
electrode may be called the reduction half cell and the zinc electrode,
the oxidation half-cell |
1 | 1856-1859 | The reduction half reaction occurs on the copper electrode while the
oxidation half reaction occurs on the zinc electrode These two portions
of the cell are also called half-cells or redox couples The copper
electrode may be called the reduction half cell and the zinc electrode,
the oxidation half-cell We can construct innumerable number of galvanic cells on the pattern
of Daniell cell by taking combinations of different half-cells |
1 | 1857-1860 | These two portions
of the cell are also called half-cells or redox couples The copper
electrode may be called the reduction half cell and the zinc electrode,
the oxidation half-cell We can construct innumerable number of galvanic cells on the pattern
of Daniell cell by taking combinations of different half-cells Each half-
cell consists of a metallic electrode dipped into an electrolyte |
1 | 1858-1861 | The copper
electrode may be called the reduction half cell and the zinc electrode,
the oxidation half-cell We can construct innumerable number of galvanic cells on the pattern
of Daniell cell by taking combinations of different half-cells Each half-
cell consists of a metallic electrode dipped into an electrolyte The two
half-cells are connected by a metallic wire through a voltmeter and a
switch externally |
1 | 1859-1862 | We can construct innumerable number of galvanic cells on the pattern
of Daniell cell by taking combinations of different half-cells Each half-
cell consists of a metallic electrode dipped into an electrolyte The two
half-cells are connected by a metallic wire through a voltmeter and a
switch externally The electrolytes of the two half-cells are connected
internally through a salt bridge as shown in Fig |
1 | 1860-1863 | Each half-
cell consists of a metallic electrode dipped into an electrolyte The two
half-cells are connected by a metallic wire through a voltmeter and a
switch externally The electrolytes of the two half-cells are connected
internally through a salt bridge as shown in Fig 2 |
1 | 1861-1864 | The two
half-cells are connected by a metallic wire through a voltmeter and a
switch externally The electrolytes of the two half-cells are connected
internally through a salt bridge as shown in Fig 2 1 |
1 | 1862-1865 | The electrolytes of the two half-cells are connected
internally through a salt bridge as shown in Fig 2 1 Sometimes, both
the electrodes dip in the same electrolyte solution and in such cases we
do not require a salt bridge |
1 | 1863-1866 | 2 1 Sometimes, both
the electrodes dip in the same electrolyte solution and in such cases we
do not require a salt bridge At each electrode-electrolyte interface there is a tendency of metal
ions from the solution to deposit on the metal electrode trying to make
it positively charged |
1 | 1864-1867 | 1 Sometimes, both
the electrodes dip in the same electrolyte solution and in such cases we
do not require a salt bridge At each electrode-electrolyte interface there is a tendency of metal
ions from the solution to deposit on the metal electrode trying to make
it positively charged At the same time, metal atoms of the electrode
have a tendency to go into the solution as ions and leave behind the
electrons at the electrode trying to make it negatively charged |
1 | 1865-1868 | Sometimes, both
the electrodes dip in the same electrolyte solution and in such cases we
do not require a salt bridge At each electrode-electrolyte interface there is a tendency of metal
ions from the solution to deposit on the metal electrode trying to make
it positively charged At the same time, metal atoms of the electrode
have a tendency to go into the solution as ions and leave behind the
electrons at the electrode trying to make it negatively charged At
equilibrium, there is a separation of charges and depending on the
tendencies of the two opposing reactions, the electrode may be positively
or negatively charged with respect to the solution |
1 | 1866-1869 | At each electrode-electrolyte interface there is a tendency of metal
ions from the solution to deposit on the metal electrode trying to make
it positively charged At the same time, metal atoms of the electrode
have a tendency to go into the solution as ions and leave behind the
electrons at the electrode trying to make it negatively charged At
equilibrium, there is a separation of charges and depending on the
tendencies of the two opposing reactions, the electrode may be positively
or negatively charged with respect to the solution A potential difference
develops between the electrode and the electrolyte which is called
electrode potential |
1 | 1867-1870 | At the same time, metal atoms of the electrode
have a tendency to go into the solution as ions and leave behind the
electrons at the electrode trying to make it negatively charged At
equilibrium, there is a separation of charges and depending on the
tendencies of the two opposing reactions, the electrode may be positively
or negatively charged with respect to the solution A potential difference
develops between the electrode and the electrolyte which is called
electrode potential When the concentrations of all the species involved
in a half-cell is unity then the electrode potential is known as standard
electrode potential |
1 | 1868-1871 | At
equilibrium, there is a separation of charges and depending on the
tendencies of the two opposing reactions, the electrode may be positively
or negatively charged with respect to the solution A potential difference
develops between the electrode and the electrolyte which is called
electrode potential When the concentrations of all the species involved
in a half-cell is unity then the electrode potential is known as standard
electrode potential According to IUPAC convention, standard
reduction potentials are now called standard electrode potentials |
1 | 1869-1872 | A potential difference
develops between the electrode and the electrolyte which is called
electrode potential When the concentrations of all the species involved
in a half-cell is unity then the electrode potential is known as standard
electrode potential According to IUPAC convention, standard
reduction potentials are now called standard electrode potentials In a
galvanic cell, the half-cell in which oxidation takes place is called anode
and it has a negative potential with respect to the solution |
1 | 1870-1873 | When the concentrations of all the species involved
in a half-cell is unity then the electrode potential is known as standard
electrode potential According to IUPAC convention, standard
reduction potentials are now called standard electrode potentials In a
galvanic cell, the half-cell in which oxidation takes place is called anode
and it has a negative potential with respect to the solution The other
half-cell in which reduction takes place is called cathode and it has a
positive potential with respect to the solution |
1 | 1871-1874 | According to IUPAC convention, standard
reduction potentials are now called standard electrode potentials In a
galvanic cell, the half-cell in which oxidation takes place is called anode
and it has a negative potential with respect to the solution The other
half-cell in which reduction takes place is called cathode and it has a
positive potential with respect to the solution Thus, there exists a
potential difference between the two electrodes and as soon as the
switch is in the on position the electrons flow from negative electrode
to positive electrode |
1 | 1872-1875 | In a
galvanic cell, the half-cell in which oxidation takes place is called anode
and it has a negative potential with respect to the solution The other
half-cell in which reduction takes place is called cathode and it has a
positive potential with respect to the solution Thus, there exists a
potential difference between the two electrodes and as soon as the
switch is in the on position the electrons flow from negative electrode
to positive electrode The direction of current flow is opposite to that of
electron flow |
1 | 1873-1876 | The other
half-cell in which reduction takes place is called cathode and it has a
positive potential with respect to the solution Thus, there exists a
potential difference between the two electrodes and as soon as the
switch is in the on position the electrons flow from negative electrode
to positive electrode The direction of current flow is opposite to that of
electron flow 2 |
1 | 1874-1877 | Thus, there exists a
potential difference between the two electrodes and as soon as the
switch is in the on position the electrons flow from negative electrode
to positive electrode The direction of current flow is opposite to that of
electron flow 2 2 Galvanic Cells
2 |
1 | 1875-1878 | The direction of current flow is opposite to that of
electron flow 2 2 Galvanic Cells
2 2 Galvanic Cells
2 |
1 | 1876-1879 | 2 2 Galvanic Cells
2 2 Galvanic Cells
2 2 Galvanic Cells
2 |
1 | 1877-1880 | 2 Galvanic Cells
2 2 Galvanic Cells
2 2 Galvanic Cells
2 2 Galvanic Cells
2 |
1 | 1878-1881 | 2 Galvanic Cells
2 2 Galvanic Cells
2 2 Galvanic Cells
2 2 Galvanic Cells
Rationalised 2023-24
34
Chemistry
The potential difference between the two electrodes of a galvanic
cell is called the cell potential and is measured in volts |
1 | 1879-1882 | 2 Galvanic Cells
2 2 Galvanic Cells
2 2 Galvanic Cells
Rationalised 2023-24
34
Chemistry
The potential difference between the two electrodes of a galvanic
cell is called the cell potential and is measured in volts The cell
potential is the difference between the electrode potentials (reduction
potentials) of the cathode and anode |
1 | 1880-1883 | 2 Galvanic Cells
2 2 Galvanic Cells
Rationalised 2023-24
34
Chemistry
The potential difference between the two electrodes of a galvanic
cell is called the cell potential and is measured in volts The cell
potential is the difference between the electrode potentials (reduction
potentials) of the cathode and anode It is called the cell electromotive
force (emf) of the cell when no current is drawn through the cell |
1 | 1881-1884 | 2 Galvanic Cells
Rationalised 2023-24
34
Chemistry
The potential difference between the two electrodes of a galvanic
cell is called the cell potential and is measured in volts The cell
potential is the difference between the electrode potentials (reduction
potentials) of the cathode and anode It is called the cell electromotive
force (emf) of the cell when no current is drawn through the cell It
is now an accepted convention that we keep the anode on the left and
the cathode on the right while representing the galvanic cell |
1 | 1882-1885 | The cell
potential is the difference between the electrode potentials (reduction
potentials) of the cathode and anode It is called the cell electromotive
force (emf) of the cell when no current is drawn through the cell It
is now an accepted convention that we keep the anode on the left and
the cathode on the right while representing the galvanic cell A galvanic
cell is generally represented by putting a vertical line between metal
and electrolyte solution and putting a double vertical line between
the two electrolytes connected by a salt bridge |
1 | 1883-1886 | It is called the cell electromotive
force (emf) of the cell when no current is drawn through the cell It
is now an accepted convention that we keep the anode on the left and
the cathode on the right while representing the galvanic cell A galvanic
cell is generally represented by putting a vertical line between metal
and electrolyte solution and putting a double vertical line between
the two electrolytes connected by a salt bridge Under this convention
the emf of the cell is positive and is given by the potential of the half-
cell on the right hand side minus the potential of the half-cell on the
left hand side i |
1 | 1884-1887 | It
is now an accepted convention that we keep the anode on the left and
the cathode on the right while representing the galvanic cell A galvanic
cell is generally represented by putting a vertical line between metal
and electrolyte solution and putting a double vertical line between
the two electrolytes connected by a salt bridge Under this convention
the emf of the cell is positive and is given by the potential of the half-
cell on the right hand side minus the potential of the half-cell on the
left hand side i e |
1 | 1885-1888 | A galvanic
cell is generally represented by putting a vertical line between metal
and electrolyte solution and putting a double vertical line between
the two electrolytes connected by a salt bridge Under this convention
the emf of the cell is positive and is given by the potential of the half-
cell on the right hand side minus the potential of the half-cell on the
left hand side i e ,
Ecell = Eright – Eleft
This is illustrated by the following example:
Cell reaction:
Cu(s) + 2Ag+(aq) ¾® Cu2+(aq) + 2 Ag(s)
(2 |
1 | 1886-1889 | Under this convention
the emf of the cell is positive and is given by the potential of the half-
cell on the right hand side minus the potential of the half-cell on the
left hand side i e ,
Ecell = Eright – Eleft
This is illustrated by the following example:
Cell reaction:
Cu(s) + 2Ag+(aq) ¾® Cu2+(aq) + 2 Ag(s)
(2 4)
Half-cell reactions:
Cathode (reduction): 2Ag+(aq) + 2e– ® 2Ag(s)
(2 |
1 | 1887-1890 | e ,
Ecell = Eright – Eleft
This is illustrated by the following example:
Cell reaction:
Cu(s) + 2Ag+(aq) ¾® Cu2+(aq) + 2 Ag(s)
(2 4)
Half-cell reactions:
Cathode (reduction): 2Ag+(aq) + 2e– ® 2Ag(s)
(2 5)
Anode (oxidation): Cu(s) ® Cu2+(aq) + 2e–
(2 |
1 | 1888-1891 | ,
Ecell = Eright – Eleft
This is illustrated by the following example:
Cell reaction:
Cu(s) + 2Ag+(aq) ¾® Cu2+(aq) + 2 Ag(s)
(2 4)
Half-cell reactions:
Cathode (reduction): 2Ag+(aq) + 2e– ® 2Ag(s)
(2 5)
Anode (oxidation): Cu(s) ® Cu2+(aq) + 2e–
(2 6)
It can be seen that the sum of (3 |
1 | 1889-1892 | 4)
Half-cell reactions:
Cathode (reduction): 2Ag+(aq) + 2e– ® 2Ag(s)
(2 5)
Anode (oxidation): Cu(s) ® Cu2+(aq) + 2e–
(2 6)
It can be seen that the sum of (3 5) and (3 |
1 | 1890-1893 | 5)
Anode (oxidation): Cu(s) ® Cu2+(aq) + 2e–
(2 6)
It can be seen that the sum of (3 5) and (3 6) leads to overall reaction
(2 |
1 | 1891-1894 | 6)
It can be seen that the sum of (3 5) and (3 6) leads to overall reaction
(2 4) in the cell and that silver electrode acts as a cathode and copper
electrode acts as an anode |
1 | 1892-1895 | 5) and (3 6) leads to overall reaction
(2 4) in the cell and that silver electrode acts as a cathode and copper
electrode acts as an anode The cell can be represented as:
Cu(s)|Cu2+(aq)||Ag+(aq)|Ag(s)
and we have Ecell = Eright – Eleft = EAg+úAg – ECu2+úCu
(2 |
1 | 1893-1896 | 6) leads to overall reaction
(2 4) in the cell and that silver electrode acts as a cathode and copper
electrode acts as an anode The cell can be represented as:
Cu(s)|Cu2+(aq)||Ag+(aq)|Ag(s)
and we have Ecell = Eright – Eleft = EAg+úAg – ECu2+úCu
(2 7)
The potential of individual half-cell cannot be measured |
1 | 1894-1897 | 4) in the cell and that silver electrode acts as a cathode and copper
electrode acts as an anode The cell can be represented as:
Cu(s)|Cu2+(aq)||Ag+(aq)|Ag(s)
and we have Ecell = Eright – Eleft = EAg+úAg – ECu2+úCu
(2 7)
The potential of individual half-cell cannot be measured We can
measure only the difference between the two half-cell potentials that
gives the emf of the cell |
1 | 1895-1898 | The cell can be represented as:
Cu(s)|Cu2+(aq)||Ag+(aq)|Ag(s)
and we have Ecell = Eright – Eleft = EAg+úAg – ECu2+úCu
(2 7)
The potential of individual half-cell cannot be measured We can
measure only the difference between the two half-cell potentials that
gives the emf of the cell If we arbitrarily choose the potential of one
electrode (half-cell) then that of the other can be determined with respect
to this |
1 | 1896-1899 | 7)
The potential of individual half-cell cannot be measured We can
measure only the difference between the two half-cell potentials that
gives the emf of the cell If we arbitrarily choose the potential of one
electrode (half-cell) then that of the other can be determined with respect
to this According to convention, a half-cell
called standard hydrogen electrode (Fig |
1 | 1897-1900 | We can
measure only the difference between the two half-cell potentials that
gives the emf of the cell If we arbitrarily choose the potential of one
electrode (half-cell) then that of the other can be determined with respect
to this According to convention, a half-cell
called standard hydrogen electrode (Fig 3 |
1 | 1898-1901 | If we arbitrarily choose the potential of one
electrode (half-cell) then that of the other can be determined with respect
to this According to convention, a half-cell
called standard hydrogen electrode (Fig 3 3)
represented by Pt(s)ú H2(g)ú H+(aq), is assigned
a zero potential at all temperatures
corresponding to the reaction
H+ (aq) + e– ® 1
2 H2(g)
The standard hydrogen electrode consists
of a platinum electrode coated with platinum
black |
1 | 1899-1902 | According to convention, a half-cell
called standard hydrogen electrode (Fig 3 3)
represented by Pt(s)ú H2(g)ú H+(aq), is assigned
a zero potential at all temperatures
corresponding to the reaction
H+ (aq) + e– ® 1
2 H2(g)
The standard hydrogen electrode consists
of a platinum electrode coated with platinum
black The electrode is dipped in an acidic
solution and pure hydrogen gas is bubbled
through it |
1 | 1900-1903 | 3 3)
represented by Pt(s)ú H2(g)ú H+(aq), is assigned
a zero potential at all temperatures
corresponding to the reaction
H+ (aq) + e– ® 1
2 H2(g)
The standard hydrogen electrode consists
of a platinum electrode coated with platinum
black The electrode is dipped in an acidic
solution and pure hydrogen gas is bubbled
through it The concentration of both the
reduced and oxidised forms of hydrogen is
maintained at unity (Fig |
1 | 1901-1904 | 3)
represented by Pt(s)ú H2(g)ú H+(aq), is assigned
a zero potential at all temperatures
corresponding to the reaction
H+ (aq) + e– ® 1
2 H2(g)
The standard hydrogen electrode consists
of a platinum electrode coated with platinum
black The electrode is dipped in an acidic
solution and pure hydrogen gas is bubbled
through it The concentration of both the
reduced and oxidised forms of hydrogen is
maintained at unity (Fig 2 |
1 | 1902-1905 | The electrode is dipped in an acidic
solution and pure hydrogen gas is bubbled
through it The concentration of both the
reduced and oxidised forms of hydrogen is
maintained at unity (Fig 2 3) |
1 | 1903-1906 | The concentration of both the
reduced and oxidised forms of hydrogen is
maintained at unity (Fig 2 3) This implies
that the pressure of hydrogen gas is one bar
and the concentration of hydrogen ion in the
solution is one molar |
1 | 1904-1907 | 2 3) This implies
that the pressure of hydrogen gas is one bar
and the concentration of hydrogen ion in the
solution is one molar 2 |
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