The document contains a chemistry exam with multiple choice questions about reaction rates and stoichiometry. Question 1 asks about the relationship between the rates of disappearance of H2 and appearance of HF in the reaction H2 + F2 → 2HF. Question 2 asks about the relationship between the average rate of appearance of product B and disappearance of reactant A in the reaction 3A → 2B. Question 3 asks about the order of reactants and overall order of the reaction for the hydrolysis of t-butyliodide.

1. KEY
GENERAL CHEMISTRY-II (1412)
S.I. # 16
1. For the gas-phase reaction H2 (g) + F2 (g)  2HF (g), how is the rate of
disappearance of H2 related to the rate of appearance of HF? _____C______
a. ∆[H2] / ∆t = 2 ∆[HF] / ∆t
b. ∆[H2] / ∆t = - 2 ∆[HF] / ∆t
c. ∆[H2] / ∆t = - ∆[HF] / 2∆t
d. ∆[H2] / ∆t = ∆[HF] / ∆t
e. ∆[H2] / ∆t = ∆[HF] / 2∆t
2. Consider the reaction 3A  2B.
The average rate of appearance of B is given by [B] /t. How is the average rate of
appearance of B related to the rate of disappearance of A?
-2[A]
3t
3. The hydrolysis of t-butyliodide is (CH3)3Cl + H2O  (CH3)3COH + HI
and the equation governing the rate of this reaction is rate = k[(CH3)3Cl]1
. What is
the order of each reactant and the over all order of the reaction?
t-butyliodide r.o. = 1
water r.o. = 0
overall rxn order = 1
4. If 2N2O5  4 NO2 + O2 and the rate law is 1st
order in N2O5, writ the rate law for
the reaction.
Rate = k [N2O5]
5. The reaction 2 NO + 2H2  N2 + 2H2O is 1st
order in H2 and 2nd
order in NO.
Write the rate law for the reaction.
Rate = k [NO]2
[H2]
6. If the reaction 2 A + 3 D  products is 1st
order in A and 2nd
order in D, the rate
law will have the form rate equal to:
rate = k [A][D]2
7. For 1st
order reactions, the rate constant, k, has the unit(s): ________E________

2. KEY
a. time b. time mol L-1
c. L mol-1
d. (mol/L)-1
time-1
e. time-1
8. The rate equation for the decomposition of H2O2 in the presence of I-
is the rate =
k [H2O2][I-
]. What are the unit(s) of k?
mol L-1
tim-1
or mol/L s
9. In the reaction A  products, the initial concentration of A is 1.56 M and the
initial rate is 0.0190 M/sec. What is the value of the rate constant k in sec-1
?
k = rate / [A]  0.0190 / 1.56 = 1.22x10-2
s-1
10. Write the equilibrium constant fo the heterogeneous reaction
2NaHCO3 (s)  Na2CO3(s) + CO2(g) + H2O (g)
Keq = [CO2][H2O]
NOMENCLATURE!!!
1. Butyl Chloride C4H9Cl
2. Butyl Alcohol C4H9OH
3. O3 Ozone
4. NH4 Ammonium
5. Nitrite NO2
6. NO Nitric Oxide
7. (CH3)2O Dimethyl ether
8. Methyl isonitrile CH3NC
9. Acetonitrile CH3CN
10. CH3Br Methyl bromide
11. H2O2 Hydrogen peroxide
12. Ethylene C2H4
13. Ethane C2H6
14. Al2O3 Alumina
15. HCOOH Formic Acid
16. C2H5Br Ethyl bromide
17. Peroxydisulfate S2O8
18. Sucrose C12H22O11
19. Silica SiO2
20. H2SHydrogen sulfide
21. CHCl3 Chloroform
22. OCl-
Hypochlorate
23. HgCl2 Mercury (II) chloride
24. C2O4
2-
Oxylate ion
25. Urea NH2CONH2
26. Cyclopentadiene C5H6
27. Dicyclopentadiene C10H12
28. C2H5OH Ethanol
29. CoCl2 Colbalt (II) chloride
30. CCl4 carbon tetra chloride
31. NaOCl sodium hypochlorite
32. AgCl silver chloride
33. FeCl3 6H2O Iron(III)chloride
hexahydrate
34. Sodium Sulfate Na2SO4
35. Sodium Acetate NaC2H3O2
36. Ammonia NH3
37. Hydrogen sulfide H2S
38. Ammonium Nitrate NH4NO3