EPSA/CSU’s Chemistry Aid Centre + FSG: CHMA10 Final Exam Review Session
1. Use the data given below to construct a Born-Haber cycle to determine the second ionization
energy of Sr. (Chapter 6)
ΔH° (kJ mol-1)
Sr(s) → Sr(g)
164
+
Sr(g) → Sr (g) + e
549
2Cl(g) → Cl2(g)
-243
Cl(g) + e- → Cl-349
2+
Sr (g) + 2Cl (g) → SrCl2(s)
-2150
Sr(s) + Cl2(g) → SrCl2 (s)
-828
2. Calculate the amount of heat (in kJ) required to raise the temperature of a 86.0 g sample of
ethanol from 298.0 K to 390.0 K. The specific heat capacity of ethanol is 2.42 J g-1 °C-1. (Chapter
6 and 11)
3. What element is being oxidized in the following (unbalanced) redox reaction? (Chapter 4)
Zn2+ (aq) + NH4+ (aq) → Zn (s) + NO3- (aq)
a) Zn
b) N
c) H
d) O
*Extra practice: write the balanced redox reaction in acidic medium
4. Predict whether each compound is soluble or insoluble: (Chapter 4)
a. Li2CO3
b. Mg3(PO4)2
c. NiS
d. NH4Cl
5. Write a balanced chemical equation for each reaction: (Chapter 4)
a. The reaction between lithium metal and liquid water
b. The reaction between gaseous hydrogen and liquid bromine
c. The reaction between aluminum metal and chlorine gas
6. Which transition will result in emitted light with the shortest wavelength? (Chapter 7)
a. n=5 → n=4
b. n= 4 → n= 3
c. n= 3 → n= 2
7. A student is doing experiments with CO2 (g). Originally, a sample of the gas is in a rigid container
at 299 K and 0.70 atm. The student increases the temperature of the CO2 (g) in the container to
425 K. (Chapter 5)
a. Describe the effect of raising the temperature on the motion of the CO2 (g) molecules.
b. Calculate the pressure of the CO2 (g) in the container at 425 K
c. In terms of kinetic molecular theory, briefly explain why the pressure of the CO2 (g) in
the container changes as it is heated to 425 K.
d. The student measures the actual pressure of the CO2 (g) in the container at 425 K and
observes that it is less than the pressure predicted by the ideal gas law. Explain this
observation.
8. Answer the following about Monochloramine and Nitrosyl Chloride. (Chapters 9 and 10)
a. Draw the Lewis diagram of Monochloramine (NH2Cl) and Nitrosyl Chloride (NOCl)
given their molecular formulas.
b. What are Monochloramine and Nitrosyl chloride’s molecular geometries? What about
each of their nitrogen atom's hybridization?
c. Calculate the number of moles of Monochloramine present in 1.0 L of a solution in which
the concentration of Monochloramine is 0.0016 g/L.
d. Monochloramine is highly soluble in water, whereas Nitrosyl Chloride is almost
insoluble. Explain this observation in terms of the types and relative strengths of the
intermolecular forces between each of the solutes and water.
9. Determine the vapor pressure in mm Hg of a substance at 45°C if its normal boiling point is 115°C and
its enthalpy of vaporization is 57.9 kJ/mol (Gas constant = 8.314 J K-1 mol-1). (Chapter 11)