Name ____________________________________________
Regents Review #4
Kinetics, Redox, and Organic Chemistry
Base your answers to questions 1 through 3 on the information below.
At room temperature, a reaction occurs when KIO3 (aq) is mixed with NaHSO3 (aq) that
contains a small amount of starch. The colorless reaction mixture turns dark blue after a
period of time that depends on the concentration of the reactants.
In a laboratory, 12 drops of a 0.02 M NaHSO3 (aq) solution containing starch were placed
in each of six test tubes. A different number of drops of 0.02 M KIO 3 (aq) and enough water
to maintain a constant volume were added to each test tube and the time for the dark-blue
color to appear was measured. The data were recorded in the table below.
1. On the grid on your answer sheet: [2]
 Mark an appropriate scale on the axis labeled “Time (s).”
 Plot the data from the data table. Circle and connect the points.
2. State how increasing the number of drops of 0.02 M KIO3 (aq) used in the reaction
affects the rate of reaction.
3. Identify one factor, other than the concentration of the reactants, that would affect the
rate of this reaction.
Base your answer to question 4 on the information below.
The balanced equation below represents the decomposition of potassium chlorate.
4. State why the entropy of the reactant is less than the entropy of the products.
Base your answers to questions 5 and 6 on the information below.
At 550˚C, 1 mole of CO2 (g) and 1 mole of H2 (g) are placed in a 1 liter reaction vessel. The
substances react to form CO (g) and H2O (g). Changes in the concentrations of the reactants
and the concentrations of the products are shown in the graph below.
5. Determine the change in the concentration of CO2 (g) between time t0 and time t1.
6. What can be concluded from the graph about the concentrations of the reactants and the
concentrations of the products between time t1 and time t2?
Base your answers to questions 7 through 9 on the information below.
At standard pressure, hydrogen peroxide, H2O2, melts at -0.4˚C, boils at 151˚C, and is very
soluble in water. A bottle of aqueous hydrogen peroxide, H2O2 (aq), purchased from a
pharmacy has a pressure-releasing cap. Aqueous hydrogen peroxide decomposes at room
temperature, as represented by the balanced equation below.
7. State, in terms of both melting point and boiling point, why H2O2 is a liquid at room
temperature.
8. State evidence that indicates the decomposition of H2O2 (aq) is exothermic.
9. Explain why a hydrogen peroxide bottle needs a pressure-releasing cap.
Base your answers to questions 10 through 12 on the information below.
A student performed a laboratory activity to observe the reaction between aluminum foil
and an aqueous copper (II) chloride solution. The reaction is represented by the balanced
equation below.
The procedures and corresponding observations for the activities are given below.
10. State one observation that indicates Cu2+ ions became Cu atoms.
11. Describe one change in the procedure that would cause the reaction to occur faster.
12. State one safety procedure that the student should perform after completing the
laboratory activity.
Base your answers to questions 13 and 14 on the information below.
Two sources of copper are cuprite, which has the IUPAC name copper (I) oxide, and
malachite, which has the formula Cu2CO3(OH)2. Copper is used in home wiring and
electric motors because it has good electrical conductivity. Other uses of copper not related
to its electrical conductivity include coins, plumbing, roofing, and cooking pans.
Aluminum is also used for cooking pans.
At room temperature, the electrical conductivity of a copper wire is 1.6 times greater than
an aluminum wire with the same length and cross-sectional area. At room temperature, the
heat conductivity of copper is 1.8 times greater than the heat conductivity of aluminum. At
STP, the density of copper is 3.3 times greater than the density of aluminum.
13. Write the chemical formula of cuprite.
14. Determine the oxidation number of oxygen in the carbonate ion found in malachite.
Base your answer to question 15 on the equation below.
15. Determine the oxidation number of chlorine in the reactant in the equation.
Base your answers to questions 16 through 19 on the information below.
A student constructs an electrochemical cell during a laboratory investigation. When the
switch is closed, electrons flow through the external circuit. The diagram and equation
below represent this cell and the reaction that occurs.
16. State the direction of electron flow through the wire when the switch is closed.
17. Write a balanced half-reaction equation for the oxidation that occurs when the switch is
closed.
18. Determine the number of moles of Al (s) needed to completely react with 9.0 moles of
Ni2+ (aq) ions.
19. State, in terms of energy, why this cell is a voltaic cell.
Base your answers to questions 20 and 21 on the information below.
Glycine, NH2CH2COOH, is an organic compound found in proteins. Acetamide,
CH3CONH2, is an organic compound that is an excellent solvent. Both glycine and
acetamide consist of the same four elements, but the compounds have different functional
groups.
20. Identify one functional group in a glycine molecule.
21. Draw a structural formula for acetamide.
Base your answers to questions 22 and 23 on the information below.
A reaction between bromine and a hydrocarbon is represented by the balanced equation
below.
22. Identify the type of organic reaction.
23. Write the name of the homologous series to which the hydrocarbon belongs.
Base your answers to questions 24 and 25 on the information below.
One type of soap is produced when ethyl stearate and sodium hydroxide react. The soap
produced by this reaction is called sodium stearate. The other product of the reaction is
ethanol. The reaction is represented by the balanced equation below.
24. Identify the type of organic reaction used to make soap.
25. To which class of organic compounds does ethyl stearate belong?