1. Ozone (O3) in the atmosphere can react with nitric oxide (NO): O3(g) + NO(g) ( NO2(g) + O2(g), with (H( = -199 kJ/mol, (S( = -4.1 J/K·mol. Calculate the (G( for this reaction at 25(C.
A. 1020 kJ/mol
B. -1.22 ( 103 kJ/mol
C. 2.00 ( 103 kJ/mol
D. -1.42 ( 103 kJ/mol
E. -198 kJ/mol
2. For the reaction H2(g) + S(s) ( H2S(g), (H( = -20.2 kJ/mol and (S( = +43.1 J/K·mol. Which of these statements is true?
A. The reaction is only spontaneous at low temperatures.
B. The reaction is spontaneous at all temperatures.
C. (G( becomes less favorable as temperature increases.
D. The reaction is spontaneous only at high temperatures.
E. The reaction is at equilibrium at 25(C under standard conditions.
3. Calculate (G( for the combustion of ethanol vapor, C2H5OH(g), at 750(C in oxygen to form carbon dioxide and water vapor.
A. -1407 kJ/mol
B. -2151 kJ/mol
C. -1307 kJ/mol
D. -4486 kJ/mol
E. -1377 kJ/mol
4. Hydrogen peroxide (H2O2) decomposes according to the equation: H2O2(l) ( H2O(l) + (1/2)O2(g). Calculate Kp for this reaction at 25(C. ((H( = -98.2 kJ/mol, (S( = 70.1 J/K·mol)
A. 1.3 ( 10-21
C. 3.46 ( 1017
D. 7.5 ( 1020
E. 8.6 ( 104
5. The equilibrium constant for the reaction AgBr(s) ℜ Ag+(aq) + Br- (aq) is 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/mol, nonspontaneous
B. (G = -69.1 kJ/mol, spontaneous
C. (G = 97.5 kJ/mol, spontaneous
D. (G = 40.6 kJ/mol, nonspontaneous
E. (G = -97.5 kJ/mol, nonspontaneous
6. The element oxygen was prepared by Joseph Priestley in 1774 by heating mercury(II) oxide:
HgO(s) ( Hg(l) + ½ O2(g)
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