| H+ | + | HSO4- | + | OH- |  |
H20 | + | SO42- | |
| Before rxn | 0.5 mol | 0.5 mol | 0.75 mol | - | 0 | ||||
| after rxn | 0 |
|
0 | - |
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| Chem 110, Dr. Paselk |
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Name |
| Fall 2002 |
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Lab |
This examination is scheduled for fifty (50) minutes. At the end of this fifty minute period you will have five (5) minutes to place your examination at the front of the examination room.
1. (15 @ 3 ea) True/False. Indicate whether the following statements are True (T) or False (F).
A state function depends mostly on the initial and final conditions of a process, with only a slight contribution by the temperature. _______F________
Oxidation half-reactions occur at the anode. _______T________
The Nernst Equation is used to calculate the free energy of a galvanic cell. _______F________
Ammonia is a strong base. _______F________
For covalent molecules the electronic geometry is the same as the molecular shape _______F________
2. (20 @ 4 ea) Answer the following in the spaces provided: Significant Figures Count!
What is the solubility of BaCO3 if it’s Ksp=1.6 x 10-9? __4.0 x 10-5___
Which of the following materials is best to prepare a buffer with a pH of 5.5? _______c________
(a) H2S / NaSH Ka= 1.0 x 10-7
(b) HOCl / NaOCl Ka= 3.5 x 10-8
(c) HC3H5O2 / Na C3H5O2 Ka= 1.3 x 10-5
For which of the following reactions is D So expected to be negative? _______a & c________
(a) H2O(g) ´ H2O(l)
(b) Br2(g) + Cl2(g) ´ 2 BrCl(g)
(c) 2H2(g) + O2(g) ´ 2 H2O(l)
A particular chemical reaction has value of D H= -2.0 J and D S= -73 J/K @ 25°C. Is it spontaneous? _No, non-spontaneous__
What is the shape of IF4-1? _Square planar__
3. (10 @ 5 ea) Solve the following stoichiometry problems, stating answers to the proper number of significant figures. SHOW WORK FOR CREDIT!
a. What is the concentration of hydrogen ions in a solution created by adding 500.0 mL of 1.5 M NaOH to 500.0 mL of 1.0 M H2SO4 (Ka2= 1.2 x 10-2)
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b. What is the concentration of ammonium ions in a solution created by adding 500.0 mL of 0.50 M HCl to 500.0 mL of 0.50 M ammonia?
4. ( 10) For the reaction
SF6(g)
the value for D G° is —374 J/K· mole. Find the value of D G°f for SF4(g) given that: for F2(g) S° = 203 J/mol, while for SF6(g) S° = 292 J/mol and D H°f = -1209 kJ/mol. SHOW WORK FOR CREDIT!
5. (10) Calculate the pH of a solution of 0.95 M acetic acid and 1.25 M potassium acetate. The Ka of acetic acid (HC2H3O2) is 1.8 x 10-5. SHOW WORK FOR CREDIT!
6. (10) Calculate the [Cu2+] in a solution prepared by dissolving 0.10 mol of copper(II) nitrate in 1.00 L of 1.00 M ammonia (assume no volume change). For the copper ammonia complex ion Kdiss = 1.0 x 10-12; Kb = 1.8 x 10-5 for ammonia. SHOW WORK FOR CREDIT!
Cu2+ + 4 NH3
7. (6) Write the NET ionic equation for the reaction which occurs when the following are mixed. (If there is no reaction, indicate by "NR." )
a. Copper(II) nitrate is mixed with excess ammonia.
Cu2+ + 4 NH3 Cu(NH3)42+
b. Sodium sulfide is mixed with excess hydrochloric acid.
S- + 2 H+ c. Tin(IV) sulfide is mixed with 6 M hydrochloric acid.
SnCl62- + 2 H2S
8. (19) Consider the galvanic cell diagramed below:
where E° for Sn2+/Sn = - 0.133V and E° for Ag+/Ag = +0.799V
a. Write out the balanced net ionic equation for the cell. SHOW WORK!
Sn2+ + 2 e- E° = - 0.133 V Ag+ + e- E° = + 0.799 V Reversing the tin reaction and adding: Sn E° = + 0.133 V
- 2(Ag+ + e-
- E° = + 0.799 V
2Ag+ + Sn E° = + 0.932 V b. Calculate the cell potential, E, for this cell. SHOW WORK FOR CREDIT!
E = E° - (RT/nF)lnQ; Q = [Sn2+]/[Ag+]2 E = 0.932 V - {(8.314 J/K*mol)(298 K)/2(96,485 C/mol)}ln(0.10)/(020)2 E = 0.932 V - (+1.176 x 10-2 V) = 0.920 V (V = J/C) c. How much free energy is available from this cell? SHOW WORK FOR CREDIT!
DG = -nFE = - 2 mol(96,485 C/mol)(0.920 V) = - 1.77 x 10-2
| Syllabus/Schedule |
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© R A Paselk
Last modified 13 June 2006
