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Physical Chemistry
Discuss the charecteristics of solids and their classification.
Physical Chemistry
5. Answer ALL parts a) — d).
The wavenumbers of the allowed rotational energy levels of a diatomic molecule are given by the equation
FJ = BJ(J+1)
a) State the factors that determine the rotational constant B for a molecule, and explain how changes in these factors would affect FJ .
b) Derive an equation for the difference in wavenumber ( ) between any two consecutive rotational energy levels.
The rotational constant for NO in the gas phase has a value of
1.705 cm 1. Calculate the wavenumber (in cm-1) of the first 4 rotational levels of NO and sketch them on an energy diagram.
d) State the specific selection rule for rotational energy level transitions for a linear molecule. Hence, draw a pure rotational spectrum for NO showing the wavenumbers of the first three transitions.
The wavenumbers of the allowed rotational energy levels of a diatomic molecule are given by the equation
FJ = BJ(J+1)
a) State the factors that determine the rotational constant B for a molecule, and explain how changes in these factors would affect FJ .
b) Derive an equation for the difference in wavenumber ( ) between any two consecutive rotational energy levels.
The rotational constant for NO in the gas phase has a value of
1.705 cm 1. Calculate the wavenumber (in cm-1) of the first 4 rotational levels of NO and sketch them on an energy diagram.
d) State the specific selection rule for rotational energy level transitions for a linear molecule. Hence, draw a pure rotational spectrum for NO showing the wavenumbers of the first three transitions.
Physical Chemistry
Element analysis reveals that a 270.469g sample, which corresponds to 15.01771 moles, contains 30.2763g of H, What is the correct molecular formula?
Physical Chemistry
In a reaction it was found that 3.0g of a metal *X* was oxidized by 25.0 cm³ of 0.10 mol dm-³ K2 Cr2 O2 under acidic conditions.
(i) Deduce the mole of ratio between *X* and Cr2 O7²- ion.
(ii) write a balanced equation of the redox reaction.
(iii) Give the oxidation numbers of chromium and *X* in both their reduced and oxidized forms.
[Molar mass of *X* = 200.6]
(i) Deduce the mole of ratio between *X* and Cr2 O7²- ion.
(ii) write a balanced equation of the redox reaction.
(iii) Give the oxidation numbers of chromium and *X* in both their reduced and oxidized forms.
[Molar mass of *X* = 200.6]
Physical Chemistry
How many atoms of copper are required to react with excess silver nitrate solution in a single replacement reaction if 16.3 grams of pure silver are formed? *
Physical Chemistry
0.3 gm of an organic compound was Kjeldahlised and the evolved NH3 required 30ml M/10 H2SO4 for complete neutralisation % of nitrogen is?
(1)28
(2)36
(3)21
(4)42
(1)28
(2)36
(3)21
(4)42
Physical Chemistry
if al3+ replaces na+ ions at the edge center of nacl lattice THEN CALCULATE THE VACANCIES IN 1 MOLE OF NACL
Physical Chemistry
what is the Emperical Formula of 0.44 gm of CO2 and 0.27 gm of H2O
Physical Chemistry
Hydrogen iodide undergoes decomposition according to the equation
2HI(g) ⇌ H2(g) + I2(g)
The equilibrium constant at 425 oC for this system is 0.018. If 1.0 mol of each of H2, I2, and HI were placed in a 1.0 L container at 425 oC, then
A) the concentration of HI would decrease.
B) the value of K would increase to 1.0.
C) because of reaction, the total number of molecules would decrease.
D) because of reaction, the total number of molecules would increase.
E) the concentration of H2 would decrease.
2HI(g) ⇌ H2(g) + I2(g)
The equilibrium constant at 425 oC for this system is 0.018. If 1.0 mol of each of H2, I2, and HI were placed in a 1.0 L container at 425 oC, then
A) the concentration of HI would decrease.
B) the value of K would increase to 1.0.
C) because of reaction, the total number of molecules would decrease.
D) because of reaction, the total number of molecules would increase.
E) the concentration of H2 would decrease.
Physical Chemistry
Which of the following can we predict from an equilibrium constant for a reaction?
1. the extent of a reaction
2. which direction a reaction will proceed by measuring the concentrations of reactants and products
3. whether a system is at equilibrium by measuring the concentrations of the reactants and products.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2 only
E) 1,2 and 3.
1. the extent of a reaction
2. which direction a reaction will proceed by measuring the concentrations of reactants and products
3. whether a system is at equilibrium by measuring the concentrations of the reactants and products.
A) 1 only
B) 2 only
C) 3 only
D) 1 and 2 only
E) 1,2 and 3.
