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WorksheetsChem 113 / Exam 1 Review
Total questions: 14
Worksheet time: 42mins
You add excess Sodium Acetate (NaCH3COOH), Sodium Chloride (NaCl), and Sodium Iodide (NaI) to an aqueous solution of Silver Nitrate (AgNO3). Which salt would you expect to form a precipitate?
Sodium Nitrate (NaNO3)
Silver Chloride (AgCl)
Silver Iodide (AgI)
Silver Acetate (AgCH3COOH)
Mg(OH)2 is an insoluble alkali metal hydroxide salt with Ksp = 7 x 10–12. How will the molar solubility of Mg(OH)2 change if the pH of its aqueous mixture is lowered from pH = 7 (neutral) to pH = 5?
No change/not dependent on pH
The solubility will increase by a factor of 2
The solubility will increase by a factor of 100
The solubility will increase by a factor of 10,000
Copper (II) forms an insoluble salt with sulfide (CuS, Ksp = 8 x 10–37) and a soluble complex with ammonia (Kf = 1.1 x 1012). Which of the following equilibrium constants accurately describes the solubility of CuCl in an aqueous solution of ammonia?
K = Ksp * Kf
K = Ksp / Kf
K = Ksp + Kf
K = Ksp – Kf
The balanced solubility equilibrium of CuS in aqueous ammonia is CuS(s) + 4 NH3 (aq) ⇌ [Cu(NH3)4]2+(aq) + S2–(aq). If the molar solubility of CuS is represented by S, what would the equilibrium expression be for the solubility in a 1 M solution of ammonia?
K = S4 / (1 - 4S)
K = S4 / (1 - S)
K = S2 / (1 - 4S)
K = S2 / (1 - S)
Balance the redox reaction:
a MnO4– + b H+ + c Ce3+ → d Ce4+ + e Mn2+ + f H2O
a = 1, b = 8, c = 1, d = 1, e = 1, f = 4
a = 1, b = 4, c = 1, d = 1, e = 1, f = 1
a = 1, b = 8, c = 3, d = 3, e = 1, f = 4
a = 1, b = 8, c = 5, d = 5, e = 1, f = 4
A galvanic cell is made from an Mg/Mg(2+) (ΔE°red = -2.375 V) and Ni/Ni(2+) (ΔE°red = -0.23 V) half cells. Which is the anode and cathode of the cell?
Mg anode, Ni cathode
Mg and Ni both anodes
Mg cathode, Ni anode
Mg and Ni both cathodes
The galvanic cell has the redox reaction:
Ni2+ + Mg → Ni + Mg2+
If a current of 1 A passes through the wire for 10 s, how many atoms of Ni are deposited on the corresponding electrode?
(Qelectron = 1.60 x 10–19 C)
(1) (10) (1.60 x 1019) (2)
(1) (10) (1.60 x 1019) (2) (6.02 x 1023)
(1) (10) (1.60 x 1019)-1 (2)-1
(1) (10) (1.60 x 1019)-1 (2)-1 (6.02 x 1023)
A galvanic cell carries out the reaction:
2 Ag (s) + Cl2 (g) → 2 Ag+ (aq) + 2 Cl– (aq).
Which is the correct Nernst equation expression for the reaction?
ΔE° = ΔE°cell - 0.0592 log ([Ag+]2 [Cl–]2 / PCl2)
ΔE° = ΔE°cell - 0.0592 log ([Ag+]2 [Cl–]2)
ΔE° = ΔE°cell - 0.0296 log ([Ag+]2 [Cl–]2 / PCl2)
ΔE° = ΔE°cell - 0.0592 log ([Ag+] [Cl–] / PCl2)
For a reaction, the activation energy is 8.314 kJ/mol and the rate constant is k = 10 s-1 at 100 K. What is the rate constant at 300 K, given the combined Arrhenius equation at two temperatures:
ln(k2/k1) = - Ea / R (1/T2 - 1/T1). (R = 8.314 J /mol K)
k = 0.013 s-1
k = 10. s-1
k = 78 s-1
k = 7800 s-1
For a given reaction (2A + 2B → C), it was determined that doubling the concentration of reactant A caused the reaction rate to increase by a factor of four. Conversely, the concentration of reactant B had no impact on the rate. Provide a rate law for this reaction:
rate = k [A] [B]
rate = k [A]2 [B]2
rate = k [A]2
rate = k [B]2
Describe the following decay process:
15570 Yb → 15168 Er + 42 He
Alpha emission
Beta emission
Gamma emission
Fission
The rate law for a reaction is rate = k [A] [B]2 where k = 10 M-2 s-1. Provide the initial rate of reaction when 2.0 mol A and 1.0 mol B occupy a container with volume 2.0 L
rate = 2.5 M s-1
rate = 5.0 M s-1
rate = 10. M s-1
rate = 20. M s-1
64 mCi of fluorine-18 (t1/2 ~ 110 min) is produced at 1:00 p.m.. How much activity is expected to remain at 6:30 p.m. (5.5 hours later)?
2.0 mCi
8.0 mCi
11.6 mCi
32 mCi
A sample of a radioactive isotope has an initial activity of 9.0 MBq. How many radioactive nuclei were present in the sample if the isotope has a decay constant of k = 3.0 x 10-3 s-1. (1 Becquerel = 1 decay event per second)
2.7 x 105 nuclei
3.0 x 106 nuclei
3.0 x 109 nuclei
2.7 x 1012 nuclei
