1. in an Aqueous Solution of Sodium Chloride, What Is the Solute?

1. In an aqueous solution of sodium chloride, what is the solute?

a) water b) NaCl

3. The concentration of a 525 mL solution containing 10.0 g of NaCl is:

a) 0.326 M b) 3.26 x 10–4M c) 19.0 M d) 1.90 x 10–2M

6. When the following reaction occurs, C(s) + O2(g) → CO2(g), 394 kJ/mol of energy are released. The reaction:

a) is exothermic

b) has a negative ΔE

c) is a redox reaction

d) all of the above are correct

7. The addition of a catalyst increases the energy released by exothermic reactions.

a) True b) False c) It depends upon the specific reaction

9. The rate law of the reaction A → products is found to be: rate = k [A]2. When the concentration of A is doubled, the rate:

a) remains the same b) doubles c) triples d) quadruples

10. Give the oxidation number of the atoms in each of the following species.

SO42- S: ______O: ______

F2 F: ______

N2O4 N: ______O: ______

13. How many mL of a 3.00 M solution of NaCl do you need to take to prepare 400.0 mL of a 2.00 M solution?

16. Consider the following balanced equation.

2 Fe(NO3)3(aq) + 3 Ba(OH)2(aq) → 2 Fe(OH)3(s) + 3 Ba(NO3)2(aq)

a) How many milliliters of a 0.250 M solution of iron (III) nitrate are necessary to completely

react with 25.5 mL of a 0.655 M solution of barium hydroxide?

b) What is the theoretical yield in grams of Fe(OH)3 when 10.0 mL of a 0.250 M solution of

Ba(OH)2 are reacted with the stoichiometric amount of Fe(NO3)3? Molar mass of Fe(OH)3: 106.83 g/mol.

17. Consider the energy diagram below. On the diagram indicate:

a) reactants

b) products

c) the activation energy, Ea.

d) the reaction ΔE.

The reaction is: endothermic or exothermic?

19. Experimental evidence suggests that the reaction between nitrogen dioxide and carbon monoxide has the following mechanism consisting of two elementary steps:

Step 1: NO2(g) + NO2(g) → NO(g) + NO3(g)

Step 2: NO3(g) + CO(g) → NO2(g) + CO2(g)

a) Write the overall balanced reaction.

c) What is NO3? Circle the correct answer:

a) transition state b) reaction intermediate c) catalyst d) reaction product

4. For a given solute in water, the energy changes are ∆Esolute separation = 845 kJ, ∆Esolvent separation = 95 kJ, and ∆Esolvation = -835 kJ. Will this solute dissolve in water? Circle your choice.

Yes No

Briefly but legibly explain your answer in terms of the three-step model of a solute’s dissolving

in solvent.

5. Use average bond energies (or bond enthalpies) to estimate ∆E for the following decomposition reaction of hydrogen peroxide to form water and oxygen gas.

11. It was experimentally observed that the reaction,

2 ClO2(aq) + 2 OH-(aq) -- ClO3-(aq) + ClO2-(aq) + H2O(l), is second order in [ClO2] and first order in [OH-]. The reaction rate was found to be 0.02484 M/s when [ClO2] = 0.060 M and [OH-] = 0.030 M. Calculate the value of rate constant, k. Express your answer in correct number of sig figs and in proper unit for full credit.

7. Calculate the molar concentration of a solution prepared by diluting 43.7 mL of 1.005 M aqueous K2Cr2O7 to 500.0 ml.

12. Consider the neutralization reaction:

2 H3PO4(aq) + 3 Ba(OH)2(aq) -- 6 H2O(l) + 2 Ba3(PO4)3(s)

What volume (mL) of 0.26 M phosphoric acid H3PO4 can be neutralized by 78.0 mL of 0.49 M barium hydroxide Ba(OH)2?

20. Kinetics data was collected for the reaction:

H2O2(aq) + 3 I–(aq) + 2 H+(aq) -- I3–(aq) + 2 H2O(l)

Which rate expression is correct?

a) Rate = k [H2O2] [I–] [H+]

b) Rate = k [H2O2]2[I–] [H+]

c) Rate = k [H2O2]2[I–]2

d) Rate = k [H2O2] [I–]

e) Rate = k [H2O2] [I–]3[H+]2

1. True or False. In a Galvanic or voltaic cell, oxidation occurs at the anode.

4. True or False. The following reaction will happen spontaneously:

2 Ag + Cu2 + → 2 Ag+ + Cu

13. True or False. As the pressure of a gas is increased, the solubility of the gas decreases.

15. Consider the balanced equation 3 Ca(OH)2 (aq) + 2 H3PO4 (aq) → Ca3(PO4)2 (s) + 6 H2O (l).

a) What is the maximum mass of Ca3(PO4)2, in grams, that can be formed from 100.0 mL of 0.350 M Ca(OH)2? The molar mass of Ca3(PO4)2 is 310.2 g/mol.

b) What is the maximum mass of Ca3(PO4)2, in grams, that can be formed from 150.0 mL of 0.650 M H3PO4?

c) What is the limiting reagent if 100.0 mL of 0.350 M Ca(OH)2 is reacted with 150.0 mL of 0.650 M H3PO4?