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1 | 705-708 | 1 Calculate the mass percentage of benzene (C6H6) and carbon
tetrachloride (CCl4) if 22 g of benzene is dissolved in 122 g of
carbon tetrachloride 1 2 Calculate the mole fraction of benzene in solution containing 30%
by mass in carbon tetrachloride 1 |
1 | 706-709 | 1 2 Calculate the mole fraction of benzene in solution containing 30%
by mass in carbon tetrachloride 1 3 Calculate the molarity of each of the following solutions: (a) 30 g of
Co(NO3)2 |
1 | 707-710 | 2 Calculate the mole fraction of benzene in solution containing 30%
by mass in carbon tetrachloride 1 3 Calculate the molarity of each of the following solutions: (a) 30 g of
Co(NO3)2 6H2O in 4 |
1 | 708-711 | 1 3 Calculate the molarity of each of the following solutions: (a) 30 g of
Co(NO3)2 6H2O in 4 3 L of solution (b) 30 mL of 0 |
1 | 709-712 | 3 Calculate the molarity of each of the following solutions: (a) 30 g of
Co(NO3)2 6H2O in 4 3 L of solution (b) 30 mL of 0 5 M H2SO4 diluted to
500 mL |
1 | 710-713 | 6H2O in 4 3 L of solution (b) 30 mL of 0 5 M H2SO4 diluted to
500 mL 1 |
1 | 711-714 | 3 L of solution (b) 30 mL of 0 5 M H2SO4 diluted to
500 mL 1 4 Calculate the mass of urea (NH2CONH2) required in making 2 |
1 | 712-715 | 5 M H2SO4 diluted to
500 mL 1 4 Calculate the mass of urea (NH2CONH2) required in making 2 5 kg of
0 |
1 | 713-716 | 1 4 Calculate the mass of urea (NH2CONH2) required in making 2 5 kg of
0 25 molal aqueous solution |
1 | 714-717 | 4 Calculate the mass of urea (NH2CONH2) required in making 2 5 kg of
0 25 molal aqueous solution 1 |
1 | 715-718 | 5 kg of
0 25 molal aqueous solution 1 5 Calculate (a) molality (b) molarity and (c) mole fraction of KI if the density
of 20% (mass/mass) aqueous KI is 1 |
1 | 716-719 | 25 molal aqueous solution 1 5 Calculate (a) molality (b) molarity and (c) mole fraction of KI if the density
of 20% (mass/mass) aqueous KI is 1 202 g mL-1 |
1 | 717-720 | 1 5 Calculate (a) molality (b) molarity and (c) mole fraction of KI if the density
of 20% (mass/mass) aqueous KI is 1 202 g mL-1 Rationalised 2023-24
6
Chemistry
Every solid does not dissolve in a given liquid |
1 | 718-721 | 5 Calculate (a) molality (b) molarity and (c) mole fraction of KI if the density
of 20% (mass/mass) aqueous KI is 1 202 g mL-1 Rationalised 2023-24
6
Chemistry
Every solid does not dissolve in a given liquid While sodium chloride
and sugar dissolve readily in water, naphthalene and anthracene do
not |
1 | 719-722 | 202 g mL-1 Rationalised 2023-24
6
Chemistry
Every solid does not dissolve in a given liquid While sodium chloride
and sugar dissolve readily in water, naphthalene and anthracene do
not On the other hand, naphthalene and anthracene dissolve readily in
benzene but sodium chloride and sugar do not |
1 | 720-723 | Rationalised 2023-24
6
Chemistry
Every solid does not dissolve in a given liquid While sodium chloride
and sugar dissolve readily in water, naphthalene and anthracene do
not On the other hand, naphthalene and anthracene dissolve readily in
benzene but sodium chloride and sugar do not It is observed that
polar solutes dissolve in polar solvents and non polar solutes in non-
polar solvents |
1 | 721-724 | While sodium chloride
and sugar dissolve readily in water, naphthalene and anthracene do
not On the other hand, naphthalene and anthracene dissolve readily in
benzene but sodium chloride and sugar do not It is observed that
polar solutes dissolve in polar solvents and non polar solutes in non-
polar solvents In general, a solute dissolves in a solvent if the
intermolecular interactions are similar in the two or we may say like
dissolves like |
1 | 722-725 | On the other hand, naphthalene and anthracene dissolve readily in
benzene but sodium chloride and sugar do not It is observed that
polar solutes dissolve in polar solvents and non polar solutes in non-
polar solvents In general, a solute dissolves in a solvent if the
intermolecular interactions are similar in the two or we may say like
dissolves like When a solid solute is added to the solvent, some solute dissolves
and its concentration increases in solution |
1 | 723-726 | It is observed that
polar solutes dissolve in polar solvents and non polar solutes in non-
polar solvents In general, a solute dissolves in a solvent if the
intermolecular interactions are similar in the two or we may say like
dissolves like When a solid solute is added to the solvent, some solute dissolves
and its concentration increases in solution This process is known as
dissolution |
1 | 724-727 | In general, a solute dissolves in a solvent if the
intermolecular interactions are similar in the two or we may say like
dissolves like When a solid solute is added to the solvent, some solute dissolves
and its concentration increases in solution This process is known as
dissolution Some solute particles in solution collide with the solid solute
particles and get separated out of solution |
1 | 725-728 | When a solid solute is added to the solvent, some solute dissolves
and its concentration increases in solution This process is known as
dissolution Some solute particles in solution collide with the solid solute
particles and get separated out of solution This process is known as
crystallisation |
1 | 726-729 | This process is known as
dissolution Some solute particles in solution collide with the solid solute
particles and get separated out of solution This process is known as
crystallisation A stage is reached when the two processes occur at the
same rate |
1 | 727-730 | Some solute particles in solution collide with the solid solute
particles and get separated out of solution This process is known as
crystallisation A stage is reached when the two processes occur at the
same rate Under such conditions, number of solute particles going
into solution will be equal to the solute particles separating out and
a state of dynamic equilibrium is reached |
1 | 728-731 | This process is known as
crystallisation A stage is reached when the two processes occur at the
same rate Under such conditions, number of solute particles going
into solution will be equal to the solute particles separating out and
a state of dynamic equilibrium is reached Solute + Solvent ⇌ Solution
(1 |
1 | 729-732 | A stage is reached when the two processes occur at the
same rate Under such conditions, number of solute particles going
into solution will be equal to the solute particles separating out and
a state of dynamic equilibrium is reached Solute + Solvent ⇌ Solution
(1 10)
At this stage the concentration of solute in solution will remain
constant under the given conditions, i |
1 | 730-733 | Under such conditions, number of solute particles going
into solution will be equal to the solute particles separating out and
a state of dynamic equilibrium is reached Solute + Solvent ⇌ Solution
(1 10)
At this stage the concentration of solute in solution will remain
constant under the given conditions, i e |
1 | 731-734 | Solute + Solvent ⇌ Solution
(1 10)
At this stage the concentration of solute in solution will remain
constant under the given conditions, i e , temperature and pressure |
1 | 732-735 | 10)
At this stage the concentration of solute in solution will remain
constant under the given conditions, i e , temperature and pressure Similar process is followed when gases are dissolved in liquid solvents |
1 | 733-736 | e , temperature and pressure Similar process is followed when gases are dissolved in liquid solvents Such a solution in which no more solute can be dissolved at the same
temperature and pressure is called a saturated solution |
1 | 734-737 | , temperature and pressure Similar process is followed when gases are dissolved in liquid solvents Such a solution in which no more solute can be dissolved at the same
temperature and pressure is called a saturated solution An
unsaturated solution is one in which more solute can be dissolved at
the same temperature |
1 | 735-738 | Similar process is followed when gases are dissolved in liquid solvents Such a solution in which no more solute can be dissolved at the same
temperature and pressure is called a saturated solution An
unsaturated solution is one in which more solute can be dissolved at
the same temperature The solution which is in dynamic equilibrium
with undissolved solute is the saturated solution and contains the
maximum amount of solute dissolved in a given amount of solvent |
1 | 736-739 | Such a solution in which no more solute can be dissolved at the same
temperature and pressure is called a saturated solution An
unsaturated solution is one in which more solute can be dissolved at
the same temperature The solution which is in dynamic equilibrium
with undissolved solute is the saturated solution and contains the
maximum amount of solute dissolved in a given amount of solvent Thus, the concentration of solute in such a solution is its solubility |
1 | 737-740 | An
unsaturated solution is one in which more solute can be dissolved at
the same temperature The solution which is in dynamic equilibrium
with undissolved solute is the saturated solution and contains the
maximum amount of solute dissolved in a given amount of solvent Thus, the concentration of solute in such a solution is its solubility Earlier we have observed that solubility of one substance into
another depends on the nature of the substances |
1 | 738-741 | The solution which is in dynamic equilibrium
with undissolved solute is the saturated solution and contains the
maximum amount of solute dissolved in a given amount of solvent Thus, the concentration of solute in such a solution is its solubility Earlier we have observed that solubility of one substance into
another depends on the nature of the substances In addition to these
variables, two other parameters, i |
1 | 739-742 | Thus, the concentration of solute in such a solution is its solubility Earlier we have observed that solubility of one substance into
another depends on the nature of the substances In addition to these
variables, two other parameters, i e |
1 | 740-743 | Earlier we have observed that solubility of one substance into
another depends on the nature of the substances In addition to these
variables, two other parameters, i e , temperature and pressure also
control this phenomenon |
1 | 741-744 | In addition to these
variables, two other parameters, i e , temperature and pressure also
control this phenomenon Effect of temperature
The solubility of a solid in a liquid is significantly affected by temperature
changes |
1 | 742-745 | e , temperature and pressure also
control this phenomenon Effect of temperature
The solubility of a solid in a liquid is significantly affected by temperature
changes Consider the equilibrium represented by equation 1 |
1 | 743-746 | , temperature and pressure also
control this phenomenon Effect of temperature
The solubility of a solid in a liquid is significantly affected by temperature
changes Consider the equilibrium represented by equation 1 10 |
1 | 744-747 | Effect of temperature
The solubility of a solid in a liquid is significantly affected by temperature
changes Consider the equilibrium represented by equation 1 10 This,
being dynamic equilibrium, must follow Le Chateliers Principle |
1 | 745-748 | Consider the equilibrium represented by equation 1 10 This,
being dynamic equilibrium, must follow Le Chateliers Principle In
general, if in a nearly saturated solution, the dissolution process is
endothermic (Dsol H > 0), the solubility should increase with rise in
temperature and if it is exothermic (Dsol H < 0) the solubility should
decrease |
1 | 746-749 | 10 This,
being dynamic equilibrium, must follow Le Chateliers Principle In
general, if in a nearly saturated solution, the dissolution process is
endothermic (Dsol H > 0), the solubility should increase with rise in
temperature and if it is exothermic (Dsol H < 0) the solubility should
decrease These trends are also observed experimentally |
1 | 747-750 | This,
being dynamic equilibrium, must follow Le Chateliers Principle In
general, if in a nearly saturated solution, the dissolution process is
endothermic (Dsol H > 0), the solubility should increase with rise in
temperature and if it is exothermic (Dsol H < 0) the solubility should
decrease These trends are also observed experimentally Effect of pressure
Pressure does not have any significant effect on solubility of solids in
liquids |
1 | 748-751 | In
general, if in a nearly saturated solution, the dissolution process is
endothermic (Dsol H > 0), the solubility should increase with rise in
temperature and if it is exothermic (Dsol H < 0) the solubility should
decrease These trends are also observed experimentally Effect of pressure
Pressure does not have any significant effect on solubility of solids in
liquids It is so because solids and liquids are highly incompressible
and practically remain unaffected by changes in pressure |
1 | 749-752 | These trends are also observed experimentally Effect of pressure
Pressure does not have any significant effect on solubility of solids in
liquids It is so because solids and liquids are highly incompressible
and practically remain unaffected by changes in pressure Many gases dissolve in water |
1 | 750-753 | Effect of pressure
Pressure does not have any significant effect on solubility of solids in
liquids It is so because solids and liquids are highly incompressible
and practically remain unaffected by changes in pressure Many gases dissolve in water Oxygen dissolves only to a small extent
in water |
1 | 751-754 | It is so because solids and liquids are highly incompressible
and practically remain unaffected by changes in pressure Many gases dissolve in water Oxygen dissolves only to a small extent
in water It is this dissolved oxygen which sustains all aquatic life |
1 | 752-755 | Many gases dissolve in water Oxygen dissolves only to a small extent
in water It is this dissolved oxygen which sustains all aquatic life On
the other hand, hydrogen chloride gas (HCl) is highly soluble in water |
1 | 753-756 | Oxygen dissolves only to a small extent
in water It is this dissolved oxygen which sustains all aquatic life On
the other hand, hydrogen chloride gas (HCl) is highly soluble in water Solubility of gases in liquids is greatly affected by pressure and
1 |
1 | 754-757 | It is this dissolved oxygen which sustains all aquatic life On
the other hand, hydrogen chloride gas (HCl) is highly soluble in water Solubility of gases in liquids is greatly affected by pressure and
1 3 |
1 | 755-758 | On
the other hand, hydrogen chloride gas (HCl) is highly soluble in water Solubility of gases in liquids is greatly affected by pressure and
1 3 1 Solubility of
a Solid in a
Liquid
1 |
1 | 756-759 | Solubility of gases in liquids is greatly affected by pressure and
1 3 1 Solubility of
a Solid in a
Liquid
1 3 |
1 | 757-760 | 3 1 Solubility of
a Solid in a
Liquid
1 3 2 Solubility of
a Gas in a
Liquid
Rationalised 2023-24
7
Solutions
temperature |
1 | 758-761 | 1 Solubility of
a Solid in a
Liquid
1 3 2 Solubility of
a Gas in a
Liquid
Rationalised 2023-24
7
Solutions
temperature The solubility of gases increase with increase of pressure |
1 | 759-762 | 3 2 Solubility of
a Gas in a
Liquid
Rationalised 2023-24
7
Solutions
temperature The solubility of gases increase with increase of pressure For solution of gases in a solvent, consider a system as shown in
Fig |
1 | 760-763 | 2 Solubility of
a Gas in a
Liquid
Rationalised 2023-24
7
Solutions
temperature The solubility of gases increase with increase of pressure For solution of gases in a solvent, consider a system as shown in
Fig 1 |
1 | 761-764 | The solubility of gases increase with increase of pressure For solution of gases in a solvent, consider a system as shown in
Fig 1 1 (a) |
1 | 762-765 | For solution of gases in a solvent, consider a system as shown in
Fig 1 1 (a) The lower part is solution and the upper part is gaseous
system at pressure p and temperature T |
1 | 763-766 | 1 1 (a) The lower part is solution and the upper part is gaseous
system at pressure p and temperature T Assume this system to be in
a state of dynamic equilibrium, i |
1 | 764-767 | 1 (a) The lower part is solution and the upper part is gaseous
system at pressure p and temperature T Assume this system to be in
a state of dynamic equilibrium, i e |
1 | 765-768 | The lower part is solution and the upper part is gaseous
system at pressure p and temperature T Assume this system to be in
a state of dynamic equilibrium, i e , under these conditions rate of
gaseous particles entering and leaving the solution phase is the same |
1 | 766-769 | Assume this system to be in
a state of dynamic equilibrium, i e , under these conditions rate of
gaseous particles entering and leaving the solution phase is the same Now increase the pressure over the solution phase by compressing the
gas to a smaller volume [Fig |
1 | 767-770 | e , under these conditions rate of
gaseous particles entering and leaving the solution phase is the same Now increase the pressure over the solution phase by compressing the
gas to a smaller volume [Fig 1 |
1 | 768-771 | , under these conditions rate of
gaseous particles entering and leaving the solution phase is the same Now increase the pressure over the solution phase by compressing the
gas to a smaller volume [Fig 1 1 (b)] |
1 | 769-772 | Now increase the pressure over the solution phase by compressing the
gas to a smaller volume [Fig 1 1 (b)] This will increase the number of
gaseous particles per unit volume over the solution and also the rate
at which the gaseous particles are striking the surface of solution to
enter it |
1 | 770-773 | 1 1 (b)] This will increase the number of
gaseous particles per unit volume over the solution and also the rate
at which the gaseous particles are striking the surface of solution to
enter it The solubility of the gas will increase until a new equilibrium
is reached resulting in an increase in the pressure of a gas above the
solution and thus its solubility increases |
1 | 771-774 | 1 (b)] This will increase the number of
gaseous particles per unit volume over the solution and also the rate
at which the gaseous particles are striking the surface of solution to
enter it The solubility of the gas will increase until a new equilibrium
is reached resulting in an increase in the pressure of a gas above the
solution and thus its solubility increases Henry was the first to give a
quantitative relation between
pressure and solubility of a gas in
a solvent which is known as
Henry’s law |
1 | 772-775 | This will increase the number of
gaseous particles per unit volume over the solution and also the rate
at which the gaseous particles are striking the surface of solution to
enter it The solubility of the gas will increase until a new equilibrium
is reached resulting in an increase in the pressure of a gas above the
solution and thus its solubility increases Henry was the first to give a
quantitative relation between
pressure and solubility of a gas in
a solvent which is known as
Henry’s law The law states that
at a constant temperature, the
solubility of a gas in a liquid is
directly proportional to the
partial pressure of the gas
present above the surface of
liquid or solution |
1 | 773-776 | The solubility of the gas will increase until a new equilibrium
is reached resulting in an increase in the pressure of a gas above the
solution and thus its solubility increases Henry was the first to give a
quantitative relation between
pressure and solubility of a gas in
a solvent which is known as
Henry’s law The law states that
at a constant temperature, the
solubility of a gas in a liquid is
directly proportional to the
partial pressure of the gas
present above the surface of
liquid or solution Dalton, a
contemporary of Henry, also
concluded independently that the
solubility of a gas in a liquid
solution is a function of partial
pressure of the gas |
1 | 774-777 | Henry was the first to give a
quantitative relation between
pressure and solubility of a gas in
a solvent which is known as
Henry’s law The law states that
at a constant temperature, the
solubility of a gas in a liquid is
directly proportional to the
partial pressure of the gas
present above the surface of
liquid or solution Dalton, a
contemporary of Henry, also
concluded independently that the
solubility of a gas in a liquid
solution is a function of partial
pressure of the gas If we use the mole fraction of a gas in
the solution as a measure of its solubility, then it can be
said that the mole fraction of gas in the solution is
proportional to the partial pressure of the gas over
the solution |
1 | 775-778 | The law states that
at a constant temperature, the
solubility of a gas in a liquid is
directly proportional to the
partial pressure of the gas
present above the surface of
liquid or solution Dalton, a
contemporary of Henry, also
concluded independently that the
solubility of a gas in a liquid
solution is a function of partial
pressure of the gas If we use the mole fraction of a gas in
the solution as a measure of its solubility, then it can be
said that the mole fraction of gas in the solution is
proportional to the partial pressure of the gas over
the solution The most commonly used form of Henry’s
law states that “the partial pressure of the gas in
vapour phase (p) is proportional to the mole fraction
of the gas (x) in the solution” and is expressed as:
p = KH x
(1 |
1 | 776-779 | Dalton, a
contemporary of Henry, also
concluded independently that the
solubility of a gas in a liquid
solution is a function of partial
pressure of the gas If we use the mole fraction of a gas in
the solution as a measure of its solubility, then it can be
said that the mole fraction of gas in the solution is
proportional to the partial pressure of the gas over
the solution The most commonly used form of Henry’s
law states that “the partial pressure of the gas in
vapour phase (p) is proportional to the mole fraction
of the gas (x) in the solution” and is expressed as:
p = KH x
(1 11)
Here KH is the Henry’s law constant |
1 | 777-780 | If we use the mole fraction of a gas in
the solution as a measure of its solubility, then it can be
said that the mole fraction of gas in the solution is
proportional to the partial pressure of the gas over
the solution The most commonly used form of Henry’s
law states that “the partial pressure of the gas in
vapour phase (p) is proportional to the mole fraction
of the gas (x) in the solution” and is expressed as:
p = KH x
(1 11)
Here KH is the Henry’s law constant If we draw a
graph between partial pressure of the gas versus mole
fraction of the gas in solution, then we should get a plot
of the type as shown in Fig |
1 | 778-781 | The most commonly used form of Henry’s
law states that “the partial pressure of the gas in
vapour phase (p) is proportional to the mole fraction
of the gas (x) in the solution” and is expressed as:
p = KH x
(1 11)
Here KH is the Henry’s law constant If we draw a
graph between partial pressure of the gas versus mole
fraction of the gas in solution, then we should get a plot
of the type as shown in Fig 1 |
1 | 779-782 | 11)
Here KH is the Henry’s law constant If we draw a
graph between partial pressure of the gas versus mole
fraction of the gas in solution, then we should get a plot
of the type as shown in Fig 1 2 |
1 | 780-783 | If we draw a
graph between partial pressure of the gas versus mole
fraction of the gas in solution, then we should get a plot
of the type as shown in Fig 1 2 Different gases have different KH values at the same
temperature (Table 1 |
1 | 781-784 | 1 2 Different gases have different KH values at the same
temperature (Table 1 2) |
1 | 782-785 | 2 Different gases have different KH values at the same
temperature (Table 1 2) This suggests that KH is a
function of the nature of the gas |
1 | 783-786 | Different gases have different KH values at the same
temperature (Table 1 2) This suggests that KH is a
function of the nature of the gas It is obvious from equation (1 |
1 | 784-787 | 2) This suggests that KH is a
function of the nature of the gas It is obvious from equation (1 11) that higher the
value of KH at a given pressure, the lower is the solubility
of the gas in the liquid |
1 | 785-788 | This suggests that KH is a
function of the nature of the gas It is obvious from equation (1 11) that higher the
value of KH at a given pressure, the lower is the solubility
of the gas in the liquid It can be seen from Table 1 |
1 | 786-789 | It is obvious from equation (1 11) that higher the
value of KH at a given pressure, the lower is the solubility
of the gas in the liquid It can be seen from Table 1 2
that KH values for both N2 and O2 increase with increase
of temperature indicating that the solubility of gases
Fig |
1 | 787-790 | 11) that higher the
value of KH at a given pressure, the lower is the solubility
of the gas in the liquid It can be seen from Table 1 2
that KH values for both N2 and O2 increase with increase
of temperature indicating that the solubility of gases
Fig 1 |
1 | 788-791 | It can be seen from Table 1 2
that KH values for both N2 and O2 increase with increase
of temperature indicating that the solubility of gases
Fig 1 1: Effect of pressure on the solubility of a gas |
1 | 789-792 | 2
that KH values for both N2 and O2 increase with increase
of temperature indicating that the solubility of gases
Fig 1 1: Effect of pressure on the solubility of a gas The
concentration of dissolved gas is proportional to the
pressure on the gas above the solution |
1 | 790-793 | 1 1: Effect of pressure on the solubility of a gas The
concentration of dissolved gas is proportional to the
pressure on the gas above the solution Fig |
1 | 791-794 | 1: Effect of pressure on the solubility of a gas The
concentration of dissolved gas is proportional to the
pressure on the gas above the solution Fig 1 |
1 | 792-795 | The
concentration of dissolved gas is proportional to the
pressure on the gas above the solution Fig 1 2: Experimental results for
the solubility of HCl gas in
cyclohexane at 293 K |
1 | 793-796 | Fig 1 2: Experimental results for
the solubility of HCl gas in
cyclohexane at 293 K The
slope of the line is the
Henry’s Law constant, KH |
1 | 794-797 | 1 2: Experimental results for
the solubility of HCl gas in
cyclohexane at 293 K The
slope of the line is the
Henry’s Law constant, KH Rationalised 2023-24
8
Chemistry
increases with decrease of temperature |
1 | 795-798 | 2: Experimental results for
the solubility of HCl gas in
cyclohexane at 293 K The
slope of the line is the
Henry’s Law constant, KH Rationalised 2023-24
8
Chemistry
increases with decrease of temperature It is due to this reason that
aquatic species are more comfortable in cold waters rather than in
warm waters |
1 | 796-799 | The
slope of the line is the
Henry’s Law constant, KH Rationalised 2023-24
8
Chemistry
increases with decrease of temperature It is due to this reason that
aquatic species are more comfortable in cold waters rather than in
warm waters Henry’s law finds several applications in industry and explains some
biological phenomena |
1 | 797-800 | Rationalised 2023-24
8
Chemistry
increases with decrease of temperature It is due to this reason that
aquatic species are more comfortable in cold waters rather than in
warm waters Henry’s law finds several applications in industry and explains some
biological phenomena Notable among these are:
· To increase the solubility of CO2 in soft drinks and soda water, the
bottle is sealed under high pressure |
1 | 798-801 | It is due to this reason that
aquatic species are more comfortable in cold waters rather than in
warm waters Henry’s law finds several applications in industry and explains some
biological phenomena Notable among these are:
· To increase the solubility of CO2 in soft drinks and soda water, the
bottle is sealed under high pressure · Scuba divers must cope with high concentrations of dissolved gases
while breathing air at high pressure underwater |
1 | 799-802 | Henry’s law finds several applications in industry and explains some
biological phenomena Notable among these are:
· To increase the solubility of CO2 in soft drinks and soda water, the
bottle is sealed under high pressure · Scuba divers must cope with high concentrations of dissolved gases
while breathing air at high pressure underwater Increased pressure
increases the solubility of atmospheric gases in blood |
1 | 800-803 | Notable among these are:
· To increase the solubility of CO2 in soft drinks and soda water, the
bottle is sealed under high pressure · Scuba divers must cope with high concentrations of dissolved gases
while breathing air at high pressure underwater Increased pressure
increases the solubility of atmospheric gases in blood When the
divers come towards surface, the pressure gradually decreases |
1 | 801-804 | · Scuba divers must cope with high concentrations of dissolved gases
while breathing air at high pressure underwater Increased pressure
increases the solubility of atmospheric gases in blood When the
divers come towards surface, the pressure gradually decreases This
releases the dissolved gases and leads to the formation of bubbles
of nitrogen in the blood |
1 | 802-805 | Increased pressure
increases the solubility of atmospheric gases in blood When the
divers come towards surface, the pressure gradually decreases This
releases the dissolved gases and leads to the formation of bubbles
of nitrogen in the blood This blocks capillaries and creates a medical
condition known as bends, which are painful and dangerous to life |
1 | 803-806 | When the
divers come towards surface, the pressure gradually decreases This
releases the dissolved gases and leads to the formation of bubbles
of nitrogen in the blood This blocks capillaries and creates a medical
condition known as bends, which are painful and dangerous to life If N2 gas is bubbled through water at 293 K, how many millimoles of N2
gas would dissolve in 1 litre of water |
1 | 804-807 | This
releases the dissolved gases and leads to the formation of bubbles
of nitrogen in the blood This blocks capillaries and creates a medical
condition known as bends, which are painful and dangerous to life If N2 gas is bubbled through water at 293 K, how many millimoles of N2
gas would dissolve in 1 litre of water Assume that N2 exerts a partial
pressure of 0 |
Subsets and Splits