Chemistry CP Final Exam Review #2
Chapter 10: Energy
Define the following terms: energy, potential energy, kinetic energy, radiant energy, Law of
conservation of energy, state function, temperature, heat, exothermic reaction, endothermic
reaction, calorie, specific heat, enthalpy, calorimeter, Hess’s Law, fossil fuels, petroleum,
natural gas, coal, greenhouse effect, entropy
Problems:
Use the specific heat equation to compete the following problems.
Q = m x C x T
(Remember: C = 4.184 J/g*C for water)
1. The temperature of a metal bar with a mass of 87 grams is raised from 31oC to 132oC. In
the process, 790.0 Joules of heat were absorbed. Find the specific heat of the metal.
2. How much heat is required to raise the temperature of an 18.7 gram sample of platinum
by 2.3oC if the specific heat of platinum is 1.3 J/g.oC?
3. A 23.6 g sample of metal, originally at 88.0oC, was places in 62 grams of water originally
at 17.0oC. After some time, the system reached equilibrium and the final temperature of
the system was 21.5oC. Find the specific heat of the metal.
Use Hess’s Law to complete the following problems.
4. Calculate the Enthalpy change for the reaction, N2 (g) + 2 O2 (g)  2 NO2 (g) , given the
information below.
N2 (g) + O2 (g)  2 NO(g)
2NO(g) + O2 (g)  2 NO2 (g)
H = 180 kJ
H = -112 KJ
5. Find the H for the reaction: 2 Cu(s) + O2 (g)  2 CuO(s)
4 CuO(s)  2 Cu2O(s) + O2 (g)
Cu2O(s)  Cu(s) + CuO(s)
H = 288 kJ
H = 11 kJ
Complete the following heat and stoichiometry problems:
6. Nitrogen reacts with hydrogen to produce ammonia (NH3). Ho = -46.2 kJ. How many kJ of
heat is absorbed when 97 grams of NH3 is produced? (Hint: write the reaction first.)
7. How much heat is transferred when 9.22 grams of glucose (C6H12O6) in your body reacts
with O2 to produce CO2 and H2O? (Ho = -2500 kJ) (Hint: write the reaction first.)
Chapter 11: Modern Atomic Theory
Define the following terms: electromagnetic radiation, wavelength, frequency, photons,
quantized, line spectrum, continuous spectrum, orbital, principal energy levels, sublevels,
electron configuration, orbital diagram, valence electrons, core electrons, representative
elements, metals, nonmetals, metalloids, atomic size, ionization energy
1. Describe the Rutherford model of the atom
2. Describe the Bohr model of the atom.
3. Describe the Wave-mechanical model of the atom
4. Draw orbital diagrams for the following elements and determine the number of unpaired
electrons.
a. Magnesium
b. Oxygen
c. Aluminum
d. Argon
e. Scandium
5. Write electron configurations for:
a. Lead
b. Nickel
6. Describe the trends on the periodic table for atomic size and explain why elements follow
these trends.
7. Describe the trends on the periodic table for ionization energy and explain why elements
follow these trends.