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WorksheetsAdv. Chemistry-Semester 2 Review
Total questions: 25
Worksheet time: 6hrs 15mins
What are the atomic orbitals that participate in forming the sigma bond between the C and H atoms in C2H4?
sp2
sp3
sp3d
sp
sp2d
According to molecular orbital theory, which of the following is NOT predicted to exist?
H2
F2
O2
Ar2
What is the bond order of O2, N2, F2
1,2, 3
3,2,1
2,3,1
1, 3/2, 1/2
In O2, what are the HOMO and LUMO levels?
HOMO: σ* 2px, 2py
LUMO: π*2pz
HOMO: σ*2pz
LUMO: π*2px, 2py
HOMO: σ2pz
LUMO: π2px, 2py
HOMO: π2px, 2py
LUMO: σ2pz
What would be the significant type of intermolecular forces in liquid ozone? O3
hydrogen bonding
dipole-dipole
Ion-Ion
Dispersion
Identify the kinds of intermolecular forces that might arise between molecules of ethanol: CH3CH2OH. Select all that apply
Dispersion Forces
Hydrogen Bonding
Dipole-Dipole forces
Ion-Ion Interaction
Which of the following molecules are likely to form hydrogen bonds?
CH4
NH3
HF
PH3
A system had 120 kJ of work done on it and its internal energy decreased by 80 kJ. How much energy did the system gain or lose as heat?
Lost 200 kJ
Gained 200 kJ
Lost 40 kJ
Gained 40 kJ
The temperature of 2.00 mol of Ne (g) is increased from 25oC to 200oC at constant pressure. Assume the heat capacity of Ne is 20.8 J/(K⋅mol). Calculate the change in the entropy of neon. Assume ideal behavior.
19.2 J/K
86.5 J/K
9.61 J/K
0.924 J/K
Calculate the enthalpy change for the reaction:
2SO2 (g) + O2 → 2SO3 (g)
ΔHf° for SO2 (g) = -16.9 kJ/mol
ΔHf° for SO3 (g) = -21.9 kJ/mol
-10.0 kJ/mol
-388.8 kJ/mol
11.0 kJ/mol
-77.6 kJ/mol
What is the standard free energy change for the formation reaction of NO2 (g) at 298 K if:
ΔHf° (kJ/mol)
NO2 (g) 33.18
N2 (g) 0
O2 (g) 0
ΔSrxn° = -60.885 JK-1mol-1
51.32 kJ/mol
181,000 kJ/mol
214.6 kJ/mol
15.00 kJ/mol
Which of these statements is correct?
A reaction stops when the equilibrium is reached.
A reaction at equilibrium in unaffected by increasing the concentrations of products.
If one starts with higher concentrations of reactants, the equilibrium constant will be larger.
In an equilibrium reaction the reverse reaction will begin as soon as any products are formed.
If we make a reaction go faster, we can increase the amount of product at equilibrium.
For gases initially contained in a 1.0 L vessel and the reaction
2NO2(g)↔ N2O4(g)
ΔH° = -37.7 kJ/mol,
which of the following would NOT cause the equilibrium to shift to the left and convert some N2O4 to NO2?
addition of 1 mol He (g) to the vessel
isothermally decreasing the volume of the container to 0.425 L
addition of 1 mol of N2O4 (g)
increasing the temperature
After the reaction
CH3COOH(aq) + H2O (l)↔ H3O+(aq) + CH3COO-(aq)
has come to equilibrium, additional water is added to the mixture without changing the temperature. Which of the following would happen?
The number of moles of molecular acetic acid would decrease.
The molar concentration of H3O+ would increase.
The reaction would shift to the left.
The equilibrium constant would increase.
The equilibrium constant would decrease.
The equilibrium constant (dimensionless) for
A↔B
is 2.0. If the initial concentrations of A and B are each 1.0 M, what are the final concentrations of A and B respectively?
[A] = 0.67 M; [B] = 0.33 M
[A] = 0.50 M; [B] = 1.0 M
[A] = 1.0 M; [B] = 1.3 M
[A] = 0.67 M; [B] = 1.3 M
The equilibrium constant for the reaction
4NH3 (g) + 5O2 (g) ↔ 4NO (g) + 6H2O (g)
is K. Calculate the equilibrium constant for the reaction
2NO (g) + 3H2O (g) ↔ 2NH3 + O2 (g).
-K/2
1/K
1/√K
-K
-2K
Consider the reaction
A + 2B ↔ C + 2D
which has an equilibrium constant of 3.7 x 10-1. Consider a reaction mixture with
[A] = 2.0 x 10-2M
[B] = 1.7 x 10-4M
[C] = 2.4 x 10-6 M
[D] = 3.5 x 10-3M
Which of the following statements is definitely true?
Heat will be evolved.
The forward reaction can occur to a
greater extent than the reverse reaction until equilibrium is established.
The system is at equilibrium.
The reverse reaction can occur to a
greater extent than the forward reaction until
equilibrium is established.
No conclusions about the system can be made without additional information.
Most common acids are
electron pair acceptors and proton donors.
electron pair donors and proton donors.
electron pair acceptors and proton acceptors.
electron pair donors and proton acceptors.
Given that the dissociation of a weak acid is endothermic, as the temperature is raised for a weak acid solution one would expect the pH to
be unaffected
increase
decrease
there is no way to know since Kw is also temperature dependent
Which of the following is true about a 0.10 M solution of a weak acid HX?
[HX] > [H+]
Two of the answers are correct
pH = 1
[H+] = 0.10 M
[X-] = 0.10 M
Under what condition is the H3O+ concentration in water expected to be ZERO?
in a solution of a very strong base
Never
in a solution of a very weak base
in a solution of a very strong acid
in a solution of a very weak acid
What is the pH of 500 mL of solution containing 0.0124 g of Ca(OH)2 (74.1 g/mol)?
3.17
10.83
9.68
11.04
10.52
The specific heat capacity of liquid water is 4.18 J/gK. How many joules of heat are needed to raise the temperature of 5.00 g of water from 25.1oC to 65.3oC?
48.1
8.40 x 102
1.89 x 103
2.08 x 10-2
54.4
Given the data in the table below, ΔHorxn for the reaction is _________.
PCl3 + 3HCl → 3Cl2 + PH3
Compound ΔHfo (kJ/mol)
PCl3 -288.07
HCl -92.30
PH3 5.40
-385.77 kJ
-570.37 kJ
570.37 kJ
385.77 kJ
The value of ΔSo for the oxidation of solid elemental sulfur to gaseous sulfur trioxide.
2S (s, rhombic) + 3O2 (g) ↔ 2SO3 (g)
S (s, rhombic): ΔHfo = 0 kJ/mol; ΔGfo = 0 kJ/mol; S = 31.88 J/kmol
O2: ΔHfo = 0 kJ/mol; ΔGfo = 0 kJ/mol; S = 205.0 J/kmol
SO3: ΔHfo = -395.2 kJ/mol; ΔGfo = -370.4 kJ/mol; S = 256.2 J/kmol
+19.3 J/Kmol
-19.3 J/Kmol
493.1 J/Kmol
-166.4 J/Kmol
-493 J/Kmol
