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Physical Chemistry
Calculate the frequency, energy and wavelength of the radiation corresponding to the spectral line of lowest frequency in Lyman's series in the spectra of hydrogen atom. Also calculate the energy for the corresponding line in the spectra of Li2+.(Rh=1.09678 x 10^7, c= 3 x 10^8)
Physical Chemistry
Calculate the frequency, energy and wavelength of the radiation corresponding to the spectral line of lowest frequency in Lyman's series in the spectra of hydrogen atom. Also calculate the energy for the corresponding line in the spectra of Li2+.(Rh=1.09678 x 10^7, c= 3 x 10^8)
Physical Chemistry
given swimming pool water with following initial quality just after addition of bleach and hcl to lower the ph to desired range
ca2+ 1E-3 M [hco3]=2E-3M na+ 2.05E-3M cl-2.00E-3 M ocl- 5E-5 M Ph=7.3
a. find the ph after watet comes to equilibrium with the atmospheric concentration of 350 ppm co2 (g) asumming the free chlorine doesnot dissipate by conversion to CL-
b. find the PH after the water comes to equilibrium with an atmospheric concentration of 350 ppm co2(g) assuming the free chlorine does dissipate by catalytic reduction (by UV radiation in sunlight ) to CL- assuming the other half reaction is the oxidation of water to oxygen .
ca2+ 1E-3 M [hco3]=2E-3M na+ 2.05E-3M cl-2.00E-3 M ocl- 5E-5 M Ph=7.3
a. find the ph after watet comes to equilibrium with the atmospheric concentration of 350 ppm co2 (g) asumming the free chlorine doesnot dissipate by conversion to CL-
b. find the PH after the water comes to equilibrium with an atmospheric concentration of 350 ppm co2(g) assuming the free chlorine does dissipate by catalytic reduction (by UV radiation in sunlight ) to CL- assuming the other half reaction is the oxidation of water to oxygen .
Physical Chemistry
(a) Deduce the SI units for the gas constant, R. (3) (b) Define the following terms: (1×2) (i) Catalyst (ii) Adsorption
Physical Chemistry
Copper crystallizes in a fcc lattice with a unit cell length of 362pm what thatha radius of the copper atom in pm..
1)157
2)181
3)108
4)128
1)157
2)181
3)108
4)128
Physical Chemistry
In gaseous solutions, the solvent is _______________.
liquid
solid
gas
none of the above
19 The temperature at which a pair of partially miscible liquid becomes completely miscible is called _________.
Miscible temperature
Boiling temperature
Critical solution temperature
Melting temperature
20 Which of the following is a pure substance made up of one type of atom?
A mixture
An element
A compound
A solution
liquid
solid
gas
none of the above
19 The temperature at which a pair of partially miscible liquid becomes completely miscible is called _________.
Miscible temperature
Boiling temperature
Critical solution temperature
Melting temperature
20 Which of the following is a pure substance made up of one type of atom?
A mixture
An element
A compound
A solution
Physical Chemistry
In gaseous solutions, the solvent is _______________.
liquid
solid
gas
none of the above
19 The temperature at which a pair of partially miscible liquid becomes completely miscible is called _________.
Miscible temperature
Boiling temperature
Critical solution temperature
Melting temperature
20 Which of the following is a pure substance made up of one type of atom?
A mixture
An element
A compound
A solution
liquid
solid
gas
none of the above
19 The temperature at which a pair of partially miscible liquid becomes completely miscible is called _________.
Miscible temperature
Boiling temperature
Critical solution temperature
Melting temperature
20 Which of the following is a pure substance made up of one type of atom?
A mixture
An element
A compound
A solution
Physical Chemistry
The gaseous mixture is a ___________ phase system.
two
double
triple
one
14 A mixture of graphite and diamond constitutes __________ phases.
two
four
six
twelve
15 Which of these is not a colligative property?
Elevation of boiling point
Osmotic pressure
Relative lowering of vapor pressure
Depression of boiling point
16 Which of these assumes the shape of the container it is placed?
Solid
Liquid
Gas
All of the above
17 Which statement is true?
As temperature goes up, the solubility of solids goes up.
As temperature goes up, the solubility of gases goes up
As temperature goes down, the solubility of solids goes up
More than one of these is true
two
double
triple
one
14 A mixture of graphite and diamond constitutes __________ phases.
two
four
six
twelve
15 Which of these is not a colligative property?
Elevation of boiling point
Osmotic pressure
Relative lowering of vapor pressure
Depression of boiling point
16 Which of these assumes the shape of the container it is placed?
Solid
Liquid
Gas
All of the above
17 Which statement is true?
As temperature goes up, the solubility of solids goes up.
As temperature goes up, the solubility of gases goes up
As temperature goes down, the solubility of solids goes up
More than one of these is true
Physical Chemistry
Which of these mixtures is not a nearly ideal liquid mixture?
n-hexane and n-heptane
benzene and toluene
water and ethanol
carbon tetrachloride and silicon tetrachloride
9 The mole fraction of He in a gaseous solution prepared from 4.0 g of He, 6.5 g of Ar, and 10.0 g of Ne is __________.
0.6
1.5
0.2
0.11
10 Molality is defined as the __________.
moles solute / moles solvent
moles solute / Liters solution
moles solute / kg solution
moles solute / kg solvent
11 Which of the following is a pure substance made up of one type of atoms?
A mixture
An element
A compound
A solution
12 Ethanol dissolved in water would be an example of ___
a solution between two miscible liquids
a solution between a solid and liquid
a suspension between two liquids
ethanol and water do not form a solution
n-hexane and n-heptane
benzene and toluene
water and ethanol
carbon tetrachloride and silicon tetrachloride
9 The mole fraction of He in a gaseous solution prepared from 4.0 g of He, 6.5 g of Ar, and 10.0 g of Ne is __________.
0.6
1.5
0.2
0.11
10 Molality is defined as the __________.
moles solute / moles solvent
moles solute / Liters solution
moles solute / kg solution
moles solute / kg solvent
11 Which of the following is a pure substance made up of one type of atoms?
A mixture
An element
A compound
A solution
12 Ethanol dissolved in water would be an example of ___
a solution between two miscible liquids
a solution between a solid and liquid
a suspension between two liquids
ethanol and water do not form a solution
Physical Chemistry
Which of the following statements is true about compounds and mixtures?
Both mixtures and compounds always contain a fixed proportion of elements by mass.
Unlike compounds, very little or no exchange of energy occurs during the formation of mixtures.
A mixture cannot be easily separated into its constituents while constituents of a compound can be easily separated.
Compounds and mixtures can be separated into its constituents by chemical methods.
5 __________ is the ratio of molar enthalpy of a liquid to its boiling point.
Raoult's law
Enthalpy rule
Trouton’s rule
Entropy rule
6 The temperature at which the vapor pressure of a liquid equals the external pressure is called its _____________.
Boiling point
freezing point
Melting point
Condensation point
7 What law states that the vapor pressure of a solution containing a non-volatile solute is equal to the vapor pressure of pure solvent times the mole fraction of the solvent?
Gay-Lussac’s Law
Raoult's law
Henry's law
Dalton's law
Both mixtures and compounds always contain a fixed proportion of elements by mass.
Unlike compounds, very little or no exchange of energy occurs during the formation of mixtures.
A mixture cannot be easily separated into its constituents while constituents of a compound can be easily separated.
Compounds and mixtures can be separated into its constituents by chemical methods.
5 __________ is the ratio of molar enthalpy of a liquid to its boiling point.
Raoult's law
Enthalpy rule
Trouton’s rule
Entropy rule
6 The temperature at which the vapor pressure of a liquid equals the external pressure is called its _____________.
Boiling point
freezing point
Melting point
Condensation point
7 What law states that the vapor pressure of a solution containing a non-volatile solute is equal to the vapor pressure of pure solvent times the mole fraction of the solvent?
Gay-Lussac’s Law
Raoult's law
Henry's law
Dalton's law
