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1 | 1005-1008 | 21)
It means that no heat is absorbed or evolved when the components
are mixed Also, the volume of solution would be equal to the sum of
volumes of the two components At molecular level, ideal behaviour of
the solutions can be explained by considering two components A and
B In pure components, the intermolecular attractive interactions will
be of types A-A and B-B, whereas in the binary solutions in addition
to these two interactions, A-B type of interactions will also be present |
1 | 1006-1009 | Also, the volume of solution would be equal to the sum of
volumes of the two components At molecular level, ideal behaviour of
the solutions can be explained by considering two components A and
B In pure components, the intermolecular attractive interactions will
be of types A-A and B-B, whereas in the binary solutions in addition
to these two interactions, A-B type of interactions will also be present If the intermolecular attractive forces between the A-A and B-B are
nearly equal to those between A-B, this leads to the formation of ideal
solution |
1 | 1007-1010 | At molecular level, ideal behaviour of
the solutions can be explained by considering two components A and
B In pure components, the intermolecular attractive interactions will
be of types A-A and B-B, whereas in the binary solutions in addition
to these two interactions, A-B type of interactions will also be present If the intermolecular attractive forces between the A-A and B-B are
nearly equal to those between A-B, this leads to the formation of ideal
solution A perfectly ideal solution is rare but some solutions are nearly
ideal in behaviour |
1 | 1008-1011 | In pure components, the intermolecular attractive interactions will
be of types A-A and B-B, whereas in the binary solutions in addition
to these two interactions, A-B type of interactions will also be present If the intermolecular attractive forces between the A-A and B-B are
nearly equal to those between A-B, this leads to the formation of ideal
solution A perfectly ideal solution is rare but some solutions are nearly
ideal in behaviour Solution of n-hexane and n-heptane, bromoethane
and chloroethane, benzene and toluene, etc |
1 | 1009-1012 | If the intermolecular attractive forces between the A-A and B-B are
nearly equal to those between A-B, this leads to the formation of ideal
solution A perfectly ideal solution is rare but some solutions are nearly
ideal in behaviour Solution of n-hexane and n-heptane, bromoethane
and chloroethane, benzene and toluene, etc fall into this category |
1 | 1010-1013 | A perfectly ideal solution is rare but some solutions are nearly
ideal in behaviour Solution of n-hexane and n-heptane, bromoethane
and chloroethane, benzene and toluene, etc fall into this category When a solution does not obey Raoult’s law over the entire range of
concentration, then it is called non-ideal solution |
1 | 1011-1014 | Solution of n-hexane and n-heptane, bromoethane
and chloroethane, benzene and toluene, etc fall into this category When a solution does not obey Raoult’s law over the entire range of
concentration, then it is called non-ideal solution The vapour pressure
of such a solution is either higher or lower than that predicted by
Raoult’s law (equation 1 |
1 | 1012-1015 | fall into this category When a solution does not obey Raoult’s law over the entire range of
concentration, then it is called non-ideal solution The vapour pressure
of such a solution is either higher or lower than that predicted by
Raoult’s law (equation 1 16) |
1 | 1013-1016 | When a solution does not obey Raoult’s law over the entire range of
concentration, then it is called non-ideal solution The vapour pressure
of such a solution is either higher or lower than that predicted by
Raoult’s law (equation 1 16) If it is higher, the solution exhibits positive
deviation and if it is lower, it exhibits negative deviation from Raoult’s
law |
1 | 1014-1017 | The vapour pressure
of such a solution is either higher or lower than that predicted by
Raoult’s law (equation 1 16) If it is higher, the solution exhibits positive
deviation and if it is lower, it exhibits negative deviation from Raoult’s
law The plots of vapour pressure as a function of mole fractions
for such solutions are shown in Fig |
1 | 1015-1018 | 16) If it is higher, the solution exhibits positive
deviation and if it is lower, it exhibits negative deviation from Raoult’s
law The plots of vapour pressure as a function of mole fractions
for such solutions are shown in Fig 1 |
1 | 1016-1019 | If it is higher, the solution exhibits positive
deviation and if it is lower, it exhibits negative deviation from Raoult’s
law The plots of vapour pressure as a function of mole fractions
for such solutions are shown in Fig 1 6 |
1 | 1017-1020 | The plots of vapour pressure as a function of mole fractions
for such solutions are shown in Fig 1 6 The cause for these deviations lie in the nature of interactions at the
molecular level |
1 | 1018-1021 | 1 6 The cause for these deviations lie in the nature of interactions at the
molecular level In case of positive deviation from Raoult’s law, A-B
interactions are weaker than those between A-A or B-B, i |
1 | 1019-1022 | 6 The cause for these deviations lie in the nature of interactions at the
molecular level In case of positive deviation from Raoult’s law, A-B
interactions are weaker than those between A-A or B-B, i e |
1 | 1020-1023 | The cause for these deviations lie in the nature of interactions at the
molecular level In case of positive deviation from Raoult’s law, A-B
interactions are weaker than those between A-A or B-B, i e , in this case
the intermolecular attractive forces between the solute-solvent molecules
are weaker than those between the solute-solute and solvent-solvent
molecules |
1 | 1021-1024 | In case of positive deviation from Raoult’s law, A-B
interactions are weaker than those between A-A or B-B, i e , in this case
the intermolecular attractive forces between the solute-solvent molecules
are weaker than those between the solute-solute and solvent-solvent
molecules This means that in such solutions, molecules of A (or B) will
find it easier to escape than in pure state |
1 | 1022-1025 | e , in this case
the intermolecular attractive forces between the solute-solvent molecules
are weaker than those between the solute-solute and solvent-solvent
molecules This means that in such solutions, molecules of A (or B) will
find it easier to escape than in pure state This will increase the vapour
Fig |
1 | 1023-1026 | , in this case
the intermolecular attractive forces between the solute-solvent molecules
are weaker than those between the solute-solute and solvent-solvent
molecules This means that in such solutions, molecules of A (or B) will
find it easier to escape than in pure state This will increase the vapour
Fig 1 |
1 | 1024-1027 | This means that in such solutions, molecules of A (or B) will
find it easier to escape than in pure state This will increase the vapour
Fig 1 5
If a solution obeys
Raoult's law for all
concentrations, its
vapour pressure
would vary linearly
from zero to the
vapour pressure of
the pure solvent |
1 | 1025-1028 | This will increase the vapour
Fig 1 5
If a solution obeys
Raoult's law for all
concentrations, its
vapour pressure
would vary linearly
from zero to the
vapour pressure of
the pure solvent 1 |
1 | 1026-1029 | 1 5
If a solution obeys
Raoult's law for all
concentrations, its
vapour pressure
would vary linearly
from zero to the
vapour pressure of
the pure solvent 1 5
1 |
1 | 1027-1030 | 5
If a solution obeys
Raoult's law for all
concentrations, its
vapour pressure
would vary linearly
from zero to the
vapour pressure of
the pure solvent 1 5
1 5
1 |
1 | 1028-1031 | 1 5
1 5
1 5
1 |
1 | 1029-1032 | 5
1 5
1 5
1 5
1 |
1 | 1030-1033 | 5
1 5
1 5
1 5 Ideal and Non-
Ideal and Non-
Ideal and Non-
Ideal and Non-
Ideal and Non-
ideal Solutions
ideal Solutions
ideal Solutions
ideal Solutions
ideal Solutions
1 |
1 | 1031-1034 | 5
1 5
1 5 Ideal and Non-
Ideal and Non-
Ideal and Non-
Ideal and Non-
Ideal and Non-
ideal Solutions
ideal Solutions
ideal Solutions
ideal Solutions
ideal Solutions
1 5 |
1 | 1032-1035 | 5
1 5 Ideal and Non-
Ideal and Non-
Ideal and Non-
Ideal and Non-
Ideal and Non-
ideal Solutions
ideal Solutions
ideal Solutions
ideal Solutions
ideal Solutions
1 5 1 Ideal
Solutions
1 |
1 | 1033-1036 | 5 Ideal and Non-
Ideal and Non-
Ideal and Non-
Ideal and Non-
Ideal and Non-
ideal Solutions
ideal Solutions
ideal Solutions
ideal Solutions
ideal Solutions
1 5 1 Ideal
Solutions
1 5 |
1 | 1034-1037 | 5 1 Ideal
Solutions
1 5 2 Non-ideal
Solutions
Rationalised 2023-24
14
Chemistry
pressure and result in positive deviation |
1 | 1035-1038 | 1 Ideal
Solutions
1 5 2 Non-ideal
Solutions
Rationalised 2023-24
14
Chemistry
pressure and result in positive deviation Mixtures of ethanol and acetone
behave in this manner |
1 | 1036-1039 | 5 2 Non-ideal
Solutions
Rationalised 2023-24
14
Chemistry
pressure and result in positive deviation Mixtures of ethanol and acetone
behave in this manner In pure ethanol, molecules are hydrogen bonded |
1 | 1037-1040 | 2 Non-ideal
Solutions
Rationalised 2023-24
14
Chemistry
pressure and result in positive deviation Mixtures of ethanol and acetone
behave in this manner In pure ethanol, molecules are hydrogen bonded On adding acetone, its molecules get in between the host molecules and
break some of the hydrogen bonds between them |
1 | 1038-1041 | Mixtures of ethanol and acetone
behave in this manner In pure ethanol, molecules are hydrogen bonded On adding acetone, its molecules get in between the host molecules and
break some of the hydrogen bonds between them Due to weakening of
interactions, the solution shows positive deviation from Raoult’s law
[Fig |
1 | 1039-1042 | In pure ethanol, molecules are hydrogen bonded On adding acetone, its molecules get in between the host molecules and
break some of the hydrogen bonds between them Due to weakening of
interactions, the solution shows positive deviation from Raoult’s law
[Fig 1 |
1 | 1040-1043 | On adding acetone, its molecules get in between the host molecules and
break some of the hydrogen bonds between them Due to weakening of
interactions, the solution shows positive deviation from Raoult’s law
[Fig 1 6 (a)] |
1 | 1041-1044 | Due to weakening of
interactions, the solution shows positive deviation from Raoult’s law
[Fig 1 6 (a)] In a solution formed by adding carbon disulphide to
acetone, the dipolar interactions between solute-solvent molecules are
weaker than the respective interactions among the solute-solute and
solvent-solvent molecules |
1 | 1042-1045 | 1 6 (a)] In a solution formed by adding carbon disulphide to
acetone, the dipolar interactions between solute-solvent molecules are
weaker than the respective interactions among the solute-solute and
solvent-solvent molecules This solution also shows positive deviation |
1 | 1043-1046 | 6 (a)] In a solution formed by adding carbon disulphide to
acetone, the dipolar interactions between solute-solvent molecules are
weaker than the respective interactions among the solute-solute and
solvent-solvent molecules This solution also shows positive deviation In case of negative deviations from Raoult’s law, the intermolecular
attractive forces between A-A and B-B are weaker than those between
A-B and leads to decrease in vapour pressure resulting in negative
deviations |
1 | 1044-1047 | In a solution formed by adding carbon disulphide to
acetone, the dipolar interactions between solute-solvent molecules are
weaker than the respective interactions among the solute-solute and
solvent-solvent molecules This solution also shows positive deviation In case of negative deviations from Raoult’s law, the intermolecular
attractive forces between A-A and B-B are weaker than those between
A-B and leads to decrease in vapour pressure resulting in negative
deviations An example of this type is a mixture of phenol and aniline |
1 | 1045-1048 | This solution also shows positive deviation In case of negative deviations from Raoult’s law, the intermolecular
attractive forces between A-A and B-B are weaker than those between
A-B and leads to decrease in vapour pressure resulting in negative
deviations An example of this type is a mixture of phenol and aniline In this case the intermolecular hydrogen bonding between phenolic
proton and lone pair on nitrogen atom of aniline is stronger than the
respective intermolecular hydrogen bonding between similar
molecules |
1 | 1046-1049 | In case of negative deviations from Raoult’s law, the intermolecular
attractive forces between A-A and B-B are weaker than those between
A-B and leads to decrease in vapour pressure resulting in negative
deviations An example of this type is a mixture of phenol and aniline In this case the intermolecular hydrogen bonding between phenolic
proton and lone pair on nitrogen atom of aniline is stronger than the
respective intermolecular hydrogen bonding between similar
molecules Similarly, a mixture of chloroform and acetone
forms a solution with negative deviation from Raoult’s law |
1 | 1047-1050 | An example of this type is a mixture of phenol and aniline In this case the intermolecular hydrogen bonding between phenolic
proton and lone pair on nitrogen atom of aniline is stronger than the
respective intermolecular hydrogen bonding between similar
molecules Similarly, a mixture of chloroform and acetone
forms a solution with negative deviation from Raoult’s law This is because chloroform molecule is able to form hydrogen
bond with acetone molecule as shown |
1 | 1048-1051 | In this case the intermolecular hydrogen bonding between phenolic
proton and lone pair on nitrogen atom of aniline is stronger than the
respective intermolecular hydrogen bonding between similar
molecules Similarly, a mixture of chloroform and acetone
forms a solution with negative deviation from Raoult’s law This is because chloroform molecule is able to form hydrogen
bond with acetone molecule as shown This decreases the escaping tendency of molecules for each
component and consequently the vapour pressure decreases resulting
in negative deviation from Raoult’s law [Fig |
1 | 1049-1052 | Similarly, a mixture of chloroform and acetone
forms a solution with negative deviation from Raoult’s law This is because chloroform molecule is able to form hydrogen
bond with acetone molecule as shown This decreases the escaping tendency of molecules for each
component and consequently the vapour pressure decreases resulting
in negative deviation from Raoult’s law [Fig 1 |
1 | 1050-1053 | This is because chloroform molecule is able to form hydrogen
bond with acetone molecule as shown This decreases the escaping tendency of molecules for each
component and consequently the vapour pressure decreases resulting
in negative deviation from Raoult’s law [Fig 1 6 |
1 | 1051-1054 | This decreases the escaping tendency of molecules for each
component and consequently the vapour pressure decreases resulting
in negative deviation from Raoult’s law [Fig 1 6 (b)] |
1 | 1052-1055 | 1 6 (b)] Some liquids on mixing, form azeotropes which are binary mixtures
having the same composition in liquid and vapour phase and boil at
a constant temperature |
1 | 1053-1056 | 6 (b)] Some liquids on mixing, form azeotropes which are binary mixtures
having the same composition in liquid and vapour phase and boil at
a constant temperature In such cases, it is not possible to separate the
components by fractional distillation |
1 | 1054-1057 | (b)] Some liquids on mixing, form azeotropes which are binary mixtures
having the same composition in liquid and vapour phase and boil at
a constant temperature In such cases, it is not possible to separate the
components by fractional distillation There are two types of azeotropes
called minimum boiling azeotrope and maximum boiling
azeotrope |
1 | 1055-1058 | Some liquids on mixing, form azeotropes which are binary mixtures
having the same composition in liquid and vapour phase and boil at
a constant temperature In such cases, it is not possible to separate the
components by fractional distillation There are two types of azeotropes
called minimum boiling azeotrope and maximum boiling
azeotrope The solutions which show a large positive deviation from
Raoult’s law form minimum boiling azeotrope at a specific composition |
1 | 1056-1059 | In such cases, it is not possible to separate the
components by fractional distillation There are two types of azeotropes
called minimum boiling azeotrope and maximum boiling
azeotrope The solutions which show a large positive deviation from
Raoult’s law form minimum boiling azeotrope at a specific composition Fig |
1 | 1057-1060 | There are two types of azeotropes
called minimum boiling azeotrope and maximum boiling
azeotrope The solutions which show a large positive deviation from
Raoult’s law form minimum boiling azeotrope at a specific composition Fig 1 |
1 | 1058-1061 | The solutions which show a large positive deviation from
Raoult’s law form minimum boiling azeotrope at a specific composition Fig 1 6
The vapour
pressures of two
component systems
as a function of
composition (a) a
solution that shows
positive deviation
from Raoult's law
and (b) a solution
that shows negative
deviation from
Raoult's law |
1 | 1059-1062 | Fig 1 6
The vapour
pressures of two
component systems
as a function of
composition (a) a
solution that shows
positive deviation
from Raoult's law
and (b) a solution
that shows negative
deviation from
Raoult's law Rationalised 2023-24
15
Solutions
For example, ethanol-water mixture (obtained by fermentation of sugars)
on fractional distillation gives a solution containing approximately 95%
by volume of ethanol |
1 | 1060-1063 | 1 6
The vapour
pressures of two
component systems
as a function of
composition (a) a
solution that shows
positive deviation
from Raoult's law
and (b) a solution
that shows negative
deviation from
Raoult's law Rationalised 2023-24
15
Solutions
For example, ethanol-water mixture (obtained by fermentation of sugars)
on fractional distillation gives a solution containing approximately 95%
by volume of ethanol Once this composition, known as azeotrope
composition, has been achieved, the liquid and vapour have the same
composition, and no further separation occurs |
1 | 1061-1064 | 6
The vapour
pressures of two
component systems
as a function of
composition (a) a
solution that shows
positive deviation
from Raoult's law
and (b) a solution
that shows negative
deviation from
Raoult's law Rationalised 2023-24
15
Solutions
For example, ethanol-water mixture (obtained by fermentation of sugars)
on fractional distillation gives a solution containing approximately 95%
by volume of ethanol Once this composition, known as azeotrope
composition, has been achieved, the liquid and vapour have the same
composition, and no further separation occurs The solutions that show large negative deviation from Raoult’s law
form maximum boiling azeotrope at a specific composition |
1 | 1062-1065 | Rationalised 2023-24
15
Solutions
For example, ethanol-water mixture (obtained by fermentation of sugars)
on fractional distillation gives a solution containing approximately 95%
by volume of ethanol Once this composition, known as azeotrope
composition, has been achieved, the liquid and vapour have the same
composition, and no further separation occurs The solutions that show large negative deviation from Raoult’s law
form maximum boiling azeotrope at a specific composition Nitric acid
and water is an example of this class of azeotrope |
1 | 1063-1066 | Once this composition, known as azeotrope
composition, has been achieved, the liquid and vapour have the same
composition, and no further separation occurs The solutions that show large negative deviation from Raoult’s law
form maximum boiling azeotrope at a specific composition Nitric acid
and water is an example of this class of azeotrope This azeotrope has
the approximate composition, 68% nitric acid and 32% water by mass,
with a boiling point of 393 |
1 | 1064-1067 | The solutions that show large negative deviation from Raoult’s law
form maximum boiling azeotrope at a specific composition Nitric acid
and water is an example of this class of azeotrope This azeotrope has
the approximate composition, 68% nitric acid and 32% water by mass,
with a boiling point of 393 5 K |
1 | 1065-1068 | Nitric acid
and water is an example of this class of azeotrope This azeotrope has
the approximate composition, 68% nitric acid and 32% water by mass,
with a boiling point of 393 5 K 1 |
1 | 1066-1069 | This azeotrope has
the approximate composition, 68% nitric acid and 32% water by mass,
with a boiling point of 393 5 K 1 6
1 |
1 | 1067-1070 | 5 K 1 6
1 6
1 |
1 | 1068-1071 | 1 6
1 6
1 6
1 |
1 | 1069-1072 | 6
1 6
1 6
1 6
1 |
1 | 1070-1073 | 6
1 6
1 6
1 6 Colligative
Colligative
Colligative
Colligative
Colligative
Properties and
Properties and
Properties and
Properties and
Properties and
Determination
Determination
Determination
Determination
Determination
of Molar Mass
of Molar Mass
of Molar Mass
of Molar Mass
of Molar Mass
We have learnt in Section 1 |
1 | 1071-1074 | 6
1 6
1 6 Colligative
Colligative
Colligative
Colligative
Colligative
Properties and
Properties and
Properties and
Properties and
Properties and
Determination
Determination
Determination
Determination
Determination
of Molar Mass
of Molar Mass
of Molar Mass
of Molar Mass
of Molar Mass
We have learnt in Section 1 4 |
1 | 1072-1075 | 6
1 6 Colligative
Colligative
Colligative
Colligative
Colligative
Properties and
Properties and
Properties and
Properties and
Properties and
Determination
Determination
Determination
Determination
Determination
of Molar Mass
of Molar Mass
of Molar Mass
of Molar Mass
of Molar Mass
We have learnt in Section 1 4 3 that the vapour pressure of solution
decreases when a non-volatile solute is added to a volatile solvent |
1 | 1073-1076 | 6 Colligative
Colligative
Colligative
Colligative
Colligative
Properties and
Properties and
Properties and
Properties and
Properties and
Determination
Determination
Determination
Determination
Determination
of Molar Mass
of Molar Mass
of Molar Mass
of Molar Mass
of Molar Mass
We have learnt in Section 1 4 3 that the vapour pressure of solution
decreases when a non-volatile solute is added to a volatile solvent There are many properties of solutions which are connected with this
decrease of vapour pressure |
1 | 1074-1077 | 4 3 that the vapour pressure of solution
decreases when a non-volatile solute is added to a volatile solvent There are many properties of solutions which are connected with this
decrease of vapour pressure These are: (1) relative lowering of vapour
pressure of the solvent (2) depression of freezing point of the solvent
(3) elevation of boiling point of the solvent and (4) osmotic pressure of
the solution |
1 | 1075-1078 | 3 that the vapour pressure of solution
decreases when a non-volatile solute is added to a volatile solvent There are many properties of solutions which are connected with this
decrease of vapour pressure These are: (1) relative lowering of vapour
pressure of the solvent (2) depression of freezing point of the solvent
(3) elevation of boiling point of the solvent and (4) osmotic pressure of
the solution All these properties depend on the number of solute
particles irrespective of their nature relative to the total number
of particles present in the solution |
1 | 1076-1079 | There are many properties of solutions which are connected with this
decrease of vapour pressure These are: (1) relative lowering of vapour
pressure of the solvent (2) depression of freezing point of the solvent
(3) elevation of boiling point of the solvent and (4) osmotic pressure of
the solution All these properties depend on the number of solute
particles irrespective of their nature relative to the total number
of particles present in the solution Such properties are called
colligative properties (colligative: from Latin: co means together, ligare
means to bind) |
1 | 1077-1080 | These are: (1) relative lowering of vapour
pressure of the solvent (2) depression of freezing point of the solvent
(3) elevation of boiling point of the solvent and (4) osmotic pressure of
the solution All these properties depend on the number of solute
particles irrespective of their nature relative to the total number
of particles present in the solution Such properties are called
colligative properties (colligative: from Latin: co means together, ligare
means to bind) In the following Sections we will discuss these
properties one by one |
1 | 1078-1081 | All these properties depend on the number of solute
particles irrespective of their nature relative to the total number
of particles present in the solution Such properties are called
colligative properties (colligative: from Latin: co means together, ligare
means to bind) In the following Sections we will discuss these
properties one by one We have learnt in Section 1 |
1 | 1079-1082 | Such properties are called
colligative properties (colligative: from Latin: co means together, ligare
means to bind) In the following Sections we will discuss these
properties one by one We have learnt in Section 1 4 |
1 | 1080-1083 | In the following Sections we will discuss these
properties one by one We have learnt in Section 1 4 3 that the vapour pressure of a solvent in
solution is less than that of the pure solvent |
1 | 1081-1084 | We have learnt in Section 1 4 3 that the vapour pressure of a solvent in
solution is less than that of the pure solvent Raoult established that the
lowering of vapour pressure depends only on the concentration of the
solute particles and it is independent of their identity |
1 | 1082-1085 | 4 3 that the vapour pressure of a solvent in
solution is less than that of the pure solvent Raoult established that the
lowering of vapour pressure depends only on the concentration of the
solute particles and it is independent of their identity The equation (1 |
1 | 1083-1086 | 3 that the vapour pressure of a solvent in
solution is less than that of the pure solvent Raoult established that the
lowering of vapour pressure depends only on the concentration of the
solute particles and it is independent of their identity The equation (1 20)
given in Section 1 |
1 | 1084-1087 | Raoult established that the
lowering of vapour pressure depends only on the concentration of the
solute particles and it is independent of their identity The equation (1 20)
given in Section 1 4 |
1 | 1085-1088 | The equation (1 20)
given in Section 1 4 3 establishes a relation between vapour pressure of
the solution, mole fraction and vapour pressure of the solvent, i |
1 | 1086-1089 | 20)
given in Section 1 4 3 establishes a relation between vapour pressure of
the solution, mole fraction and vapour pressure of the solvent, i e |
1 | 1087-1090 | 4 3 establishes a relation between vapour pressure of
the solution, mole fraction and vapour pressure of the solvent, i e ,
p1
= x1 p1
0
(1 |
1 | 1088-1091 | 3 establishes a relation between vapour pressure of
the solution, mole fraction and vapour pressure of the solvent, i e ,
p1
= x1 p1
0
(1 22)
The reduction in the vapour pressure of solvent (Dp1) is given as:
Dp1 = p1
0 – p1 = p1
0 – p1
0 x1
= p1
0 (1 – x1)
(1 |
1 | 1089-1092 | e ,
p1
= x1 p1
0
(1 22)
The reduction in the vapour pressure of solvent (Dp1) is given as:
Dp1 = p1
0 – p1 = p1
0 – p1
0 x1
= p1
0 (1 – x1)
(1 23)
Knowing that x2 = 1 – x1, equation (1 |
1 | 1090-1093 | ,
p1
= x1 p1
0
(1 22)
The reduction in the vapour pressure of solvent (Dp1) is given as:
Dp1 = p1
0 – p1 = p1
0 – p1
0 x1
= p1
0 (1 – x1)
(1 23)
Knowing that x2 = 1 – x1, equation (1 23) reduces to
Dp1 = x2 p1
0
(1 |
1 | 1091-1094 | 22)
The reduction in the vapour pressure of solvent (Dp1) is given as:
Dp1 = p1
0 – p1 = p1
0 – p1
0 x1
= p1
0 (1 – x1)
(1 23)
Knowing that x2 = 1 – x1, equation (1 23) reduces to
Dp1 = x2 p1
0
(1 24)
In a solution containing several non-volatile solutes, the lowering of the
vapour pressure depends on the sum of the mole fraction of different solutes |
1 | 1092-1095 | 23)
Knowing that x2 = 1 – x1, equation (1 23) reduces to
Dp1 = x2 p1
0
(1 24)
In a solution containing several non-volatile solutes, the lowering of the
vapour pressure depends on the sum of the mole fraction of different solutes Equation (1 |
1 | 1093-1096 | 23) reduces to
Dp1 = x2 p1
0
(1 24)
In a solution containing several non-volatile solutes, the lowering of the
vapour pressure depends on the sum of the mole fraction of different solutes Equation (1 24) can be written as
01
1
p
p
=
10
1
0
1
p
p
p
= x2
(1 |
1 | 1094-1097 | 24)
In a solution containing several non-volatile solutes, the lowering of the
vapour pressure depends on the sum of the mole fraction of different solutes Equation (1 24) can be written as
01
1
p
p
=
10
1
0
1
p
p
p
= x2
(1 25)
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Intext Question
Intext Question
1 |
1 | 1095-1098 | Equation (1 24) can be written as
01
1
p
p
=
10
1
0
1
p
p
p
= x2
(1 25)
Intext Question
Intext Question
Intext Question
Intext Question
Intext Question
1 8 The vapour pressure of pure liquids A and B are 450 and 700 mm Hg
respectively, at 350 K |
1 | 1096-1099 | 24) can be written as
01
1
p
p
=
10
1
0
1
p
p
p
= x2
(1 25)
Intext Question
Intext Question
Intext Question
Intext Question
Intext Question
1 8 The vapour pressure of pure liquids A and B are 450 and 700 mm Hg
respectively, at 350 K Find out the composition of the liquid mixture if total
vapour pressure is 600 mm Hg |
1 | 1097-1100 | 25)
Intext Question
Intext Question
Intext Question
Intext Question
Intext Question
1 8 The vapour pressure of pure liquids A and B are 450 and 700 mm Hg
respectively, at 350 K Find out the composition of the liquid mixture if total
vapour pressure is 600 mm Hg Also find the composition of the vapour phase |
1 | 1098-1101 | 8 The vapour pressure of pure liquids A and B are 450 and 700 mm Hg
respectively, at 350 K Find out the composition of the liquid mixture if total
vapour pressure is 600 mm Hg Also find the composition of the vapour phase 1 |
1 | 1099-1102 | Find out the composition of the liquid mixture if total
vapour pressure is 600 mm Hg Also find the composition of the vapour phase 1 6 |
1 | 1100-1103 | Also find the composition of the vapour phase 1 6 1 Relative
Lowering of
Vapour
Pressure
Rationalised 2023-24
16
Chemistry
The expression on the left hand side of the equation as mentioned
earlier is called relative lowering of vapour pressure and is equal to
the mole fraction of the solute |
1 | 1101-1104 | 1 6 1 Relative
Lowering of
Vapour
Pressure
Rationalised 2023-24
16
Chemistry
The expression on the left hand side of the equation as mentioned
earlier is called relative lowering of vapour pressure and is equal to
the mole fraction of the solute The above equation can be written as:
10
01
1
p – p
p
=
2
1
2
n
n
n
2
2
1
2
since
n
x
n
n
(1 |
1 | 1102-1105 | 6 1 Relative
Lowering of
Vapour
Pressure
Rationalised 2023-24
16
Chemistry
The expression on the left hand side of the equation as mentioned
earlier is called relative lowering of vapour pressure and is equal to
the mole fraction of the solute The above equation can be written as:
10
01
1
p – p
p
=
2
1
2
n
n
n
2
2
1
2
since
n
x
n
n
(1 26)
Here n1 and n2 are the number of moles of solvent and solute
respectively present in the solution |
1 | 1103-1106 | 1 Relative
Lowering of
Vapour
Pressure
Rationalised 2023-24
16
Chemistry
The expression on the left hand side of the equation as mentioned
earlier is called relative lowering of vapour pressure and is equal to
the mole fraction of the solute The above equation can be written as:
10
01
1
p – p
p
=
2
1
2
n
n
n
2
2
1
2
since
n
x
n
n
(1 26)
Here n1 and n2 are the number of moles of solvent and solute
respectively present in the solution For dilute solutions n2 < < n1,
hence neglecting n2 in the denominator we have
10
1
0
1
p
p
p
=
2
1
n
n
(1 |
1 | 1104-1107 | The above equation can be written as:
10
01
1
p – p
p
=
2
1
2
n
n
n
2
2
1
2
since
n
x
n
n
(1 26)
Here n1 and n2 are the number of moles of solvent and solute
respectively present in the solution For dilute solutions n2 < < n1,
hence neglecting n2 in the denominator we have
10
1
0
1
p
p
p
=
2
1
n
n
(1 27)
or
10
1
0
1
-
p
p
p
=
2
1
2
1
w ×
× w
M
M
(1 |
Subsets and Splits