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Material Type: Exam; Professor: Autrey; Class: General Chemistry II; Subject: Chemistry; University: Fayetteville State University; Term: Spring 2006;
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Practice Final Exam (150 points)
Name _________________________ May 8, 2006
General Instructions
1 amu = 1.66054 × 10 -27^ kg 1 atm = 760 Torr = 760 mm Hg Boltzmann constant (k) = 1.38065 × 10 -23^ J K- Gas constant (R) = 0.08205 L atm mole-1^ K- = 8.31447 J mole-1^ K- Avogadro’s number (Na) = 6.02214 × 1023 mole- Ion Product of Water (Kw) = 1.000 × 10 -14^ at 25.0 °C Faraday constant (F) = 96,485 C mole- RT/F = 0.0257 V at 25°C
F-, fluoride S 2 O 3 2-, thiosulfate Cl-, chloride C 2 O 4 2-, oxalate Br-, bromide CN-, cyanide I-, iodide SCN-, thiocyanate NO 3 - , nitrate ClO 4 - , perchlorate NO 2 - , nitrite SO 3 2-, sulfite SO 4 2-, sulfate edta4-, ethylenediaminetetraacetate
MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.
A. CH 4 B. Cl 2 C. Kr D. CH 3 Cl E. N 2
B. CH 2 Cl (^2) C. C 2 H 5 OH D. CH 3 Br E. HOCH 2 CH 2 OH
A. a high heat of vaporization B. a high critical temperature C. a high vapor pressure D. a high boiling point E. None of the above.
40.7 kJ/mol. How many kilojoules (kJ) of heat must be provided to convert one gram of liquid water at 67°C into one gram of steam at 100°C?
o ∆ Hvap
A. 22.6 kJ B. 40.8 kJ C. 2.2 kJ D. 2,400 J E. 40.8 J
A. melting of a solid B. vaporization C. raising the temperature of a gas D. condensation of water vapor E. sublimation of dry ice
( ∆ Hvapo ) is 39.3 kJ/mol. What is the vapor pressure of ethanol, in mmHg ,at 34.9°C?
A. 1,510 mmHg B. 100 mmHg C. 200 mmHg D. 0.0099 mmHg E. 4.61 mmHg
A + 2B → products
was found to follow the rate law: rate = k[A] 2 [B]. Predict by what factor the rate of reaction will increase when the concentration of A is doubled and the concentration of B is tripled, and the temperature remains constant.
E. None of the above.
1 0.021 0.065 1.46 M/min 2 0.021 0.260 1.46 M/min 3 0.042 0.065 5.84 M/min
A. rate = k[NO] B. rate = k[NO] 2 C. rate = k[NO][H 2 ] D. rate = k[NO] 2 [H 2 ] E. rate = k[NO] 2 [H 2 ]^2
A. 21 min B. 42 min C. 84 min D. 101 min E. 120 min
A. 95.8 s B. 201 s C. 231 s D. 462 s E. 41.7 s
By what factor (how many times) will the rate constant increase when the temperature is raised from 10°C to 28°C?
2 3 4+
2 +
Calculate Kp for this reaction if Kc = 0.083 at 900°C.
has an equilibrium constant Kc = 4.3 × 106 , and the following concentrations are present:
Is the mixture at equilibrium? If not at equilibrium, in which direction,
left to right, or right to left, will reaction occur to reach equilibrium?
A. yes, the mixture is at equilibrium. B. no, left to right C. no, right to left D. There is not enough information to tell.
a system is prepared with:
[PCl 3 ] = 0.10 M [Cl 2 ] = 0.15 M [PCl 5 ] = 0.60 M.
Which response is correct? The reaction
A. is at equilibrium. B. will form more PCl 5 until equilibrium is reached. C. will form PCl 3 and Cl 2 until equilibrium is reached. D. None of the above.
if we increase the reaction temperature, the equilibrium will
O
A. shift to the right. B. shift to the left. C. stay the same. D. The question cannot be answered because Keq is not given.
A. tastes bitter B. increases [OH-] when placed in H 2 O C. acts as a proton donor D. acts as an electron pair donor E. acts as a proton acceptor
A. increases [H+] when placed in H 2 O B. tastes sour F. acts as an electron pair acceptor G. acts as an electron pair donor H. acts as a proton donor
C. 0.10 MNaCl D. 0.10 MH 2 CO 3 E. 0.10 MNaOH
A. NaCl B. KNO 2 C. NaCN D. NH 4 NO 3 E. FeCl (^3)
A. NaCl B. KCN C. NaNO 3 D. NH 4 NO 3 E. FeCl (^3)
A. LiBr B. NaF C. KOH D. FeCl 3 E. NaCN
A. 0.40 M HCN and 0.10 KCN B. 0.20 M CH 3 COOH C. 1.0 M HNO 3 and 1.0 MNaNO 3 D. 0.10 M KCN E. 0.50 M HCl and 0.10 NaCl
A. 0.10 M CH 3 COOH and 0.10 M CH 3 COONa B. 0.10 M CH 3 COOH C. 0.10 M HNO 2 D. 0.10 M HNO 2 and 0.10 M NaNO 2 E. 0.10 M CH 3 COONa
0.15 M sodium benzoate (C 6 H 5 COONa). Given Ka = 6.5 × 10 –5^ for benzoic acid.
A. OH–^ + HOCl → H 2 O + OCl – B. OH–^ + OCl –^ → HOCl + O2– C. Na +^ + HOCl → NaCl + OH– D. H+^ + HOCl → H 2 + OCl – E. NaOH + HOCl → H 2 O + NaCl
.
A. 0.023 M B. 0.032 M C. 7.7 × 10–8^ M D. 2.9 × 10 –9^ M E. 6.9 × 10 –10^ M
A. 0.10 M AgNO 3 B. distilled water C. 0.10 M NaCl D. 0.10 M HCl E. 0.10 M aqueous NH 3
A. CH 3 OH(l) B. CO(g) C. MgCO 3 (s) D. H 2 O(l) E. Ni(s)
Given the following absolute entropies;
S°(J/K• mol) SO 3 256. H 2 O 69. H 2 SO 4 156.
A. always negative. B. always positive. C. sometimes is positive and sometimes is negative. D. usually zero.
A. the reaction is exothermic. B. the reaction is endothermic. C. the reaction is fast. D. the reaction is spontaneous. E. ∆S must be > 0.
2 2 2 2
From the following data calculate Kp for this reaction at 25°C.
∆H° = –98.2 kJ ∆S° = 70.1 J/K
is the solubility product constant, Ksp = 7.7 × 10–13^ at 25°C. Calculate ∆G for the reaction when [Ag+^ ] = 1.0 × 10–2^ M and [Br–] = 1.0 × 10–3^ M. Is the reaction spontaneous or nonspontaneous at these concentrations?
A. ∆G = 69.1 kJ, nonspontaneous B. ∆G = -69.1 kJ, spontaneous C. ∆G = 97.5 kJ, spontaneous D. ∆G = 40.6 kJ, nonspontaneous E. ∆G = -97.5 kJ, nonspontaneous
Which is the half-reaction occurring at the anode?
2+
−
2+
−
2+ 2+
3+
2+
A. Cr 3+^ B. Cr C. Mn2+^ D. Co E. MnO 4 –