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1 | 1705-1708 | 33
19 5 g of CH2FCOOH is dissolved in 500 g of water The depression in the freezing
point of water observed is 1 00 C |
1 | 1706-1709 | 5 g of CH2FCOOH is dissolved in 500 g of water The depression in the freezing
point of water observed is 1 00 C Calculate the van’t Hoff factor and dissociation
constant of fluoroacetic acid |
1 | 1707-1710 | The depression in the freezing
point of water observed is 1 00 C Calculate the van’t Hoff factor and dissociation
constant of fluoroacetic acid 1 |
1 | 1708-1711 | 00 C Calculate the van’t Hoff factor and dissociation
constant of fluoroacetic acid 1 34
Vapour pressure of water at 293 K is 17 |
1 | 1709-1712 | Calculate the van’t Hoff factor and dissociation
constant of fluoroacetic acid 1 34
Vapour pressure of water at 293 K is 17 535 mm Hg |
1 | 1710-1713 | 1 34
Vapour pressure of water at 293 K is 17 535 mm Hg Calculate the vapour
pressure of water at 293 K when 25 g of glucose is dissolved in 450 g of water |
1 | 1711-1714 | 34
Vapour pressure of water at 293 K is 17 535 mm Hg Calculate the vapour
pressure of water at 293 K when 25 g of glucose is dissolved in 450 g of water 1 |
1 | 1712-1715 | 535 mm Hg Calculate the vapour
pressure of water at 293 K when 25 g of glucose is dissolved in 450 g of water 1 35
Henry’s law constant for the molality of methane in benzene at 298 K is
4 |
1 | 1713-1716 | Calculate the vapour
pressure of water at 293 K when 25 g of glucose is dissolved in 450 g of water 1 35
Henry’s law constant for the molality of methane in benzene at 298 K is
4 27 × 105 mm Hg |
1 | 1714-1717 | 1 35
Henry’s law constant for the molality of methane in benzene at 298 K is
4 27 × 105 mm Hg Calculate the solubility of methane in benzene at 298 K
under 760 mm Hg |
1 | 1715-1718 | 35
Henry’s law constant for the molality of methane in benzene at 298 K is
4 27 × 105 mm Hg Calculate the solubility of methane in benzene at 298 K
under 760 mm Hg 1 |
1 | 1716-1719 | 27 × 105 mm Hg Calculate the solubility of methane in benzene at 298 K
under 760 mm Hg 1 36
100 g of liquid A (molar mass 140 g mol–1) was dissolved in 1000 g of liquid B
(molar mass 180 g mol–1) |
1 | 1717-1720 | Calculate the solubility of methane in benzene at 298 K
under 760 mm Hg 1 36
100 g of liquid A (molar mass 140 g mol–1) was dissolved in 1000 g of liquid B
(molar mass 180 g mol–1) The vapour pressure of pure liquid B was found to be
500 torr |
1 | 1718-1721 | 1 36
100 g of liquid A (molar mass 140 g mol–1) was dissolved in 1000 g of liquid B
(molar mass 180 g mol–1) The vapour pressure of pure liquid B was found to be
500 torr Calculate the vapour pressure of pure liquid A and its vapour pressure
in the solution if the total vapour pressure of the solution is 475 Torr |
1 | 1719-1722 | 36
100 g of liquid A (molar mass 140 g mol–1) was dissolved in 1000 g of liquid B
(molar mass 180 g mol–1) The vapour pressure of pure liquid B was found to be
500 torr Calculate the vapour pressure of pure liquid A and its vapour pressure
in the solution if the total vapour pressure of the solution is 475 Torr Rationalised 2023-24
30
Chemistry
1 |
1 | 1720-1723 | The vapour pressure of pure liquid B was found to be
500 torr Calculate the vapour pressure of pure liquid A and its vapour pressure
in the solution if the total vapour pressure of the solution is 475 Torr Rationalised 2023-24
30
Chemistry
1 37
Vapour pressures of pure acetone and chloroform at 328 K are 741 |
1 | 1721-1724 | Calculate the vapour pressure of pure liquid A and its vapour pressure
in the solution if the total vapour pressure of the solution is 475 Torr Rationalised 2023-24
30
Chemistry
1 37
Vapour pressures of pure acetone and chloroform at 328 K are 741 8 mm
Hg and 632 |
1 | 1722-1725 | Rationalised 2023-24
30
Chemistry
1 37
Vapour pressures of pure acetone and chloroform at 328 K are 741 8 mm
Hg and 632 8 mm Hg respectively |
1 | 1723-1726 | 37
Vapour pressures of pure acetone and chloroform at 328 K are 741 8 mm
Hg and 632 8 mm Hg respectively Assuming that they form ideal solution
over the entire range of composition, plot ptotal, pchloroform, and pacetone as a
function of xacetone |
1 | 1724-1727 | 8 mm
Hg and 632 8 mm Hg respectively Assuming that they form ideal solution
over the entire range of composition, plot ptotal, pchloroform, and pacetone as a
function of xacetone The experimental data observed for different compositions
of mixture is:
100 x xacetone
0
11 |
1 | 1725-1728 | 8 mm Hg respectively Assuming that they form ideal solution
over the entire range of composition, plot ptotal, pchloroform, and pacetone as a
function of xacetone The experimental data observed for different compositions
of mixture is:
100 x xacetone
0
11 8
23 |
1 | 1726-1729 | Assuming that they form ideal solution
over the entire range of composition, plot ptotal, pchloroform, and pacetone as a
function of xacetone The experimental data observed for different compositions
of mixture is:
100 x xacetone
0
11 8
23 4
36 |
1 | 1727-1730 | The experimental data observed for different compositions
of mixture is:
100 x xacetone
0
11 8
23 4
36 0
50 |
1 | 1728-1731 | 8
23 4
36 0
50 8
58 |
1 | 1729-1732 | 4
36 0
50 8
58 2
64 |
1 | 1730-1733 | 0
50 8
58 2
64 5
72 |
1 | 1731-1734 | 8
58 2
64 5
72 1
pacetone /mm Hg
0
54 |
1 | 1732-1735 | 2
64 5
72 1
pacetone /mm Hg
0
54 9 110 |
1 | 1733-1736 | 5
72 1
pacetone /mm Hg
0
54 9 110 1 202 |
1 | 1734-1737 | 1
pacetone /mm Hg
0
54 9 110 1 202 4 322 |
1 | 1735-1738 | 9 110 1 202 4 322 7 405 |
1 | 1736-1739 | 1 202 4 322 7 405 9 454 |
1 | 1737-1740 | 4 322 7 405 9 454 1 521 |
1 | 1738-1741 | 7 405 9 454 1 521 1
pchloroform /mm Hg
632 |
1 | 1739-1742 | 9 454 1 521 1
pchloroform /mm Hg
632 8 548 |
1 | 1740-1743 | 1 521 1
pchloroform /mm Hg
632 8 548 1 469 |
1 | 1741-1744 | 1
pchloroform /mm Hg
632 8 548 1 469 4 359 |
1 | 1742-1745 | 8 548 1 469 4 359 7 257 |
1 | 1743-1746 | 1 469 4 359 7 257 7 193 |
1 | 1744-1747 | 4 359 7 257 7 193 6 161 |
1 | 1745-1748 | 7 257 7 193 6 161 2 120 |
1 | 1746-1749 | 7 193 6 161 2 120 7
Plot this data also on the same graph paper |
1 | 1747-1750 | 6 161 2 120 7
Plot this data also on the same graph paper Indicate whether it has positive
deviation or negative deviation from the ideal solution |
1 | 1748-1751 | 2 120 7
Plot this data also on the same graph paper Indicate whether it has positive
deviation or negative deviation from the ideal solution 1 |
1 | 1749-1752 | 7
Plot this data also on the same graph paper Indicate whether it has positive
deviation or negative deviation from the ideal solution 1 38
Benzene and toluene form ideal solution over the entire range of composition |
1 | 1750-1753 | Indicate whether it has positive
deviation or negative deviation from the ideal solution 1 38
Benzene and toluene form ideal solution over the entire range of composition The vapour pressure of pure benzene and toluene at 300 K are 50 |
1 | 1751-1754 | 1 38
Benzene and toluene form ideal solution over the entire range of composition The vapour pressure of pure benzene and toluene at 300 K are 50 71 mm Hg
and 32 |
1 | 1752-1755 | 38
Benzene and toluene form ideal solution over the entire range of composition The vapour pressure of pure benzene and toluene at 300 K are 50 71 mm Hg
and 32 06 mm Hg respectively |
1 | 1753-1756 | The vapour pressure of pure benzene and toluene at 300 K are 50 71 mm Hg
and 32 06 mm Hg respectively Calculate the mole fraction of benzene in vapour
phase if 80 g of benzene is mixed with 100 g of toluene |
1 | 1754-1757 | 71 mm Hg
and 32 06 mm Hg respectively Calculate the mole fraction of benzene in vapour
phase if 80 g of benzene is mixed with 100 g of toluene 1 |
1 | 1755-1758 | 06 mm Hg respectively Calculate the mole fraction of benzene in vapour
phase if 80 g of benzene is mixed with 100 g of toluene 1 39
The air is a mixture of a number of gases |
1 | 1756-1759 | Calculate the mole fraction of benzene in vapour
phase if 80 g of benzene is mixed with 100 g of toluene 1 39
The air is a mixture of a number of gases The major components are oxygen
and nitrogen with approximate proportion of 20% is to 79% by volume at 298
K |
1 | 1757-1760 | 1 39
The air is a mixture of a number of gases The major components are oxygen
and nitrogen with approximate proportion of 20% is to 79% by volume at 298
K The water is in equilibrium with air at a pressure of 10 atm |
1 | 1758-1761 | 39
The air is a mixture of a number of gases The major components are oxygen
and nitrogen with approximate proportion of 20% is to 79% by volume at 298
K The water is in equilibrium with air at a pressure of 10 atm At 298 K if the
Henry’s law constants for oxygen and nitrogen at 298 K are 3 |
1 | 1759-1762 | The major components are oxygen
and nitrogen with approximate proportion of 20% is to 79% by volume at 298
K The water is in equilibrium with air at a pressure of 10 atm At 298 K if the
Henry’s law constants for oxygen and nitrogen at 298 K are 3 30 × 107 mm and
6 |
1 | 1760-1763 | The water is in equilibrium with air at a pressure of 10 atm At 298 K if the
Henry’s law constants for oxygen and nitrogen at 298 K are 3 30 × 107 mm and
6 51 × 107 mm respectively, calculate the composition of these gases in water |
1 | 1761-1764 | At 298 K if the
Henry’s law constants for oxygen and nitrogen at 298 K are 3 30 × 107 mm and
6 51 × 107 mm respectively, calculate the composition of these gases in water 1 |
1 | 1762-1765 | 30 × 107 mm and
6 51 × 107 mm respectively, calculate the composition of these gases in water 1 40
Determine the amount of CaCl2 (i = 2 |
1 | 1763-1766 | 51 × 107 mm respectively, calculate the composition of these gases in water 1 40
Determine the amount of CaCl2 (i = 2 47) dissolved in 2 |
1 | 1764-1767 | 1 40
Determine the amount of CaCl2 (i = 2 47) dissolved in 2 5 litre of water such
that its osmotic pressure is 0 |
1 | 1765-1768 | 40
Determine the amount of CaCl2 (i = 2 47) dissolved in 2 5 litre of water such
that its osmotic pressure is 0 75 atm at 27° C |
1 | 1766-1769 | 47) dissolved in 2 5 litre of water such
that its osmotic pressure is 0 75 atm at 27° C 1 |
1 | 1767-1770 | 5 litre of water such
that its osmotic pressure is 0 75 atm at 27° C 1 41
Determine the osmotic pressure of a solution prepared by dissolving 25 mg of
K2SO4 in 2 litre of water at 25° C, assuming that it is completely dissociated |
1 | 1768-1771 | 75 atm at 27° C 1 41
Determine the osmotic pressure of a solution prepared by dissolving 25 mg of
K2SO4 in 2 litre of water at 25° C, assuming that it is completely dissociated Answers to Some Intext Questions
1 |
1 | 1769-1772 | 1 41
Determine the osmotic pressure of a solution prepared by dissolving 25 mg of
K2SO4 in 2 litre of water at 25° C, assuming that it is completely dissociated Answers to Some Intext Questions
1 1
C6H6 = 15 |
1 | 1770-1773 | 41
Determine the osmotic pressure of a solution prepared by dissolving 25 mg of
K2SO4 in 2 litre of water at 25° C, assuming that it is completely dissociated Answers to Some Intext Questions
1 1
C6H6 = 15 28%, CCl4 = 84 |
1 | 1771-1774 | Answers to Some Intext Questions
1 1
C6H6 = 15 28%, CCl4 = 84 72%
1 |
1 | 1772-1775 | 1
C6H6 = 15 28%, CCl4 = 84 72%
1 2
0 |
1 | 1773-1776 | 28%, CCl4 = 84 72%
1 2
0 459, 0 |
1 | 1774-1777 | 72%
1 2
0 459, 0 541
1 |
1 | 1775-1778 | 2
0 459, 0 541
1 3
0 |
1 | 1776-1779 | 459, 0 541
1 3
0 024 M, 0 |
1 | 1777-1780 | 541
1 3
0 024 M, 0 03 M
1 |
1 | 1778-1781 | 3
0 024 M, 0 03 M
1 4
36 |
1 | 1779-1782 | 024 M, 0 03 M
1 4
36 946 g
1 |
1 | 1780-1783 | 03 M
1 4
36 946 g
1 5
1 |
1 | 1781-1784 | 4
36 946 g
1 5
1 5 mol kg–1 , 1 |
1 | 1782-1785 | 946 g
1 5
1 5 mol kg–1 , 1 45 mol L–1 0 |
1 | 1783-1786 | 5
1 5 mol kg–1 , 1 45 mol L–1 0 0263
1 |
1 | 1784-1787 | 5 mol kg–1 , 1 45 mol L–1 0 0263
1 9
23 |
1 | 1785-1788 | 45 mol L–1 0 0263
1 9
23 4 mm Hg
1 |
1 | 1786-1789 | 0263
1 9
23 4 mm Hg
1 10 121 |
1 | 1787-1790 | 9
23 4 mm Hg
1 10 121 67 g
1 |
1 | 1788-1791 | 4 mm Hg
1 10 121 67 g
1 11 5 |
1 | 1789-1792 | 10 121 67 g
1 11 5 077 g
1 |
1 | 1790-1793 | 67 g
1 11 5 077 g
1 12 30 |
1 | 1791-1794 | 11 5 077 g
1 12 30 96 Pa
Rationalised 2023-24
Electrochemistry is the study of production of
electricity from energy released during spontaneous
chemical reactions and the use of electrical energy
to bring about non-spontaneous chemical
transformations |
1 | 1792-1795 | 077 g
1 12 30 96 Pa
Rationalised 2023-24
Electrochemistry is the study of production of
electricity from energy released during spontaneous
chemical reactions and the use of electrical energy
to bring about non-spontaneous chemical
transformations The subject is of importance both
for theoretical and practical considerations |
1 | 1793-1796 | 12 30 96 Pa
Rationalised 2023-24
Electrochemistry is the study of production of
electricity from energy released during spontaneous
chemical reactions and the use of electrical energy
to bring about non-spontaneous chemical
transformations The subject is of importance both
for theoretical and practical considerations A large
number of metals, sodium hydroxide, chlorine,
fluorine and many other chemicals are produced by
electrochemical methods |
1 | 1794-1797 | 96 Pa
Rationalised 2023-24
Electrochemistry is the study of production of
electricity from energy released during spontaneous
chemical reactions and the use of electrical energy
to bring about non-spontaneous chemical
transformations The subject is of importance both
for theoretical and practical considerations A large
number of metals, sodium hydroxide, chlorine,
fluorine and many other chemicals are produced by
electrochemical methods Batteries and fuel cells
convert chemical energy into electrical energy and are
used on a large scale in various instruments and
devices |
1 | 1795-1798 | The subject is of importance both
for theoretical and practical considerations A large
number of metals, sodium hydroxide, chlorine,
fluorine and many other chemicals are produced by
electrochemical methods Batteries and fuel cells
convert chemical energy into electrical energy and are
used on a large scale in various instruments and
devices The reactions carried out electrochemically
can be energy efficient and less polluting |
1 | 1796-1799 | A large
number of metals, sodium hydroxide, chlorine,
fluorine and many other chemicals are produced by
electrochemical methods Batteries and fuel cells
convert chemical energy into electrical energy and are
used on a large scale in various instruments and
devices The reactions carried out electrochemically
can be energy efficient and less polluting Therefore,
study of electrochemistry is important for creating new
technologies that are ecofriendly |
1 | 1797-1800 | Batteries and fuel cells
convert chemical energy into electrical energy and are
used on a large scale in various instruments and
devices The reactions carried out electrochemically
can be energy efficient and less polluting Therefore,
study of electrochemistry is important for creating new
technologies that are ecofriendly The transmission of
sensory signals through cells to brain and vice versa
and communication between the cells are known to
have electrochemical origin |
1 | 1798-1801 | The reactions carried out electrochemically
can be energy efficient and less polluting Therefore,
study of electrochemistry is important for creating new
technologies that are ecofriendly The transmission of
sensory signals through cells to brain and vice versa
and communication between the cells are known to
have electrochemical origin Electrochemistry, is
therefore, a very vast and interdisciplinary subject |
1 | 1799-1802 | Therefore,
study of electrochemistry is important for creating new
technologies that are ecofriendly The transmission of
sensory signals through cells to brain and vice versa
and communication between the cells are known to
have electrochemical origin Electrochemistry, is
therefore, a very vast and interdisciplinary subject In
this Unit, we will cover only some of its important
elementary aspects |
1 | 1800-1803 | The transmission of
sensory signals through cells to brain and vice versa
and communication between the cells are known to
have electrochemical origin Electrochemistry, is
therefore, a very vast and interdisciplinary subject In
this Unit, we will cover only some of its important
elementary aspects After studying this Unit, you will be
·able to
describe an electrochemical cell
and differentiate between galvanic
and electrolytic cells;
·
apply
Nernst
equation
for
calculating the emf of galvanic cell
and define standard potential of
the cell;
·
derive relation between standard
potential of the cell, Gibbs energy
of cell reaction and its equilibrium
constant;
·
define resistivity (r), conductivity
(k) and molar conductivity (✆m) of
ionic solutions;
·
differentiate
between
ionic
(electrolytic)
and
electronic
conductivity;
·
describe
the
method
for
measurement of conductivity of
electrolytic
solutions
and
calculation
of
their
molar
conductivity;
·
justify
the
variation
of
conductivity
and
molar
conductivity of solutions with
change in their concentration and
define
m
(molar conductivity at
zero concentration or infinite
dilution);
·
enunciate Kohlrausch law and
learn its applications;
·
understand quantitative aspects
of electrolysis;
·
describe the construction of some
primary and secondary batteries
and fuel cells;
·
explain
corrosion
as
an
electrochemical process |
1 | 1801-1804 | Electrochemistry, is
therefore, a very vast and interdisciplinary subject In
this Unit, we will cover only some of its important
elementary aspects After studying this Unit, you will be
·able to
describe an electrochemical cell
and differentiate between galvanic
and electrolytic cells;
·
apply
Nernst
equation
for
calculating the emf of galvanic cell
and define standard potential of
the cell;
·
derive relation between standard
potential of the cell, Gibbs energy
of cell reaction and its equilibrium
constant;
·
define resistivity (r), conductivity
(k) and molar conductivity (✆m) of
ionic solutions;
·
differentiate
between
ionic
(electrolytic)
and
electronic
conductivity;
·
describe
the
method
for
measurement of conductivity of
electrolytic
solutions
and
calculation
of
their
molar
conductivity;
·
justify
the
variation
of
conductivity
and
molar
conductivity of solutions with
change in their concentration and
define
m
(molar conductivity at
zero concentration or infinite
dilution);
·
enunciate Kohlrausch law and
learn its applications;
·
understand quantitative aspects
of electrolysis;
·
describe the construction of some
primary and secondary batteries
and fuel cells;
·
explain
corrosion
as
an
electrochemical process Objectives
Chemical reactions can be used to produce electrical energy,
conversely, electrical energy can be used to carry out chemical
reactions that do not proceed spontaneously |
1 | 1802-1805 | In
this Unit, we will cover only some of its important
elementary aspects After studying this Unit, you will be
·able to
describe an electrochemical cell
and differentiate between galvanic
and electrolytic cells;
·
apply
Nernst
equation
for
calculating the emf of galvanic cell
and define standard potential of
the cell;
·
derive relation between standard
potential of the cell, Gibbs energy
of cell reaction and its equilibrium
constant;
·
define resistivity (r), conductivity
(k) and molar conductivity (✆m) of
ionic solutions;
·
differentiate
between
ionic
(electrolytic)
and
electronic
conductivity;
·
describe
the
method
for
measurement of conductivity of
electrolytic
solutions
and
calculation
of
their
molar
conductivity;
·
justify
the
variation
of
conductivity
and
molar
conductivity of solutions with
change in their concentration and
define
m
(molar conductivity at
zero concentration or infinite
dilution);
·
enunciate Kohlrausch law and
learn its applications;
·
understand quantitative aspects
of electrolysis;
·
describe the construction of some
primary and secondary batteries
and fuel cells;
·
explain
corrosion
as
an
electrochemical process Objectives
Chemical reactions can be used to produce electrical energy,
conversely, electrical energy can be used to carry out chemical
reactions that do not proceed spontaneously 2
Electrochemistry
Unit
Unit
Unit
Unit2Unit
Electrochemistry
Rationalised 2023-24
32
Chemistry
Cu
Eext >1 |
1 | 1803-1806 | After studying this Unit, you will be
·able to
describe an electrochemical cell
and differentiate between galvanic
and electrolytic cells;
·
apply
Nernst
equation
for
calculating the emf of galvanic cell
and define standard potential of
the cell;
·
derive relation between standard
potential of the cell, Gibbs energy
of cell reaction and its equilibrium
constant;
·
define resistivity (r), conductivity
(k) and molar conductivity (✆m) of
ionic solutions;
·
differentiate
between
ionic
(electrolytic)
and
electronic
conductivity;
·
describe
the
method
for
measurement of conductivity of
electrolytic
solutions
and
calculation
of
their
molar
conductivity;
·
justify
the
variation
of
conductivity
and
molar
conductivity of solutions with
change in their concentration and
define
m
(molar conductivity at
zero concentration or infinite
dilution);
·
enunciate Kohlrausch law and
learn its applications;
·
understand quantitative aspects
of electrolysis;
·
describe the construction of some
primary and secondary batteries
and fuel cells;
·
explain
corrosion
as
an
electrochemical process Objectives
Chemical reactions can be used to produce electrical energy,
conversely, electrical energy can be used to carry out chemical
reactions that do not proceed spontaneously 2
Electrochemistry
Unit
Unit
Unit
Unit2Unit
Electrochemistry
Rationalised 2023-24
32
Chemistry
Cu
Eext >1 1
e
–
Current
Cathode
+ve
Anode
–ve
Zn
Fig |
1 | 1804-1807 | Objectives
Chemical reactions can be used to produce electrical energy,
conversely, electrical energy can be used to carry out chemical
reactions that do not proceed spontaneously 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 |
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