key_q3 - 2 10] = 3.6 x 10 6 G = G 0 + RT ln Q = 457.14...

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1. a) The oxidation state decreases for oxidizing agent and increases for reducing agent during a redox reaction. b) The anode is where oxidation half-reaction occurs . Electrons are lost by the substance being oxidized and leave the cell at the anode. The cathode is where reduction half-reaction occurs . Electrons are gained by the substance being reduced and enter the cell at the cathode. c) A salt bridge allows ions to flow through both compartments and completes the circuit . 2. a) I I 2 + 2e (1) Fe 3+ + e Fe 2+ (2) (1)+2 × (2): 2Fe 3+ + 2I 2Fe 2+ + I 2 b) MnO 4 + 8H + + 5e → Mn 2+ + 4H 2 O (1) SO 3 2 + H 2 O SO 4 2 + 2H + +2e (2) (1) × 2 + (2) × 5: 2MnO 4 + 5SO 3 2 + 6H + 2Mn 2+ + 5SO 4 2 + 3H 2 O 3. Q = (6 × 10 4 ) 2 /[(0.1)
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Unformatted text preview: 2 10] = 3.6 x 10 6 G = G 0 + RT ln Q = 457.14 kJ/mol + 8.314 J/(mol K) 298 K ln (3.6 10 6 ) = 488.2 kJ/mol (or 4.882 10 5 J/mol) 4. G = RT ln K = 8.314 J/(mol K) 298 K ln 6.74 = 4.73 kJ/mol 5. H = ( 393.5 4 + 0) [110.5 4 + ( 1118.4)] kJ/mol = 897.6 kJ/mol S = (213.7 4 + 27.3 3) (146.4 4 + 197.7) J/(mol K) = 153.4 J/(mol K) G 0 = H T S 0 = 897.6 kJ/mol 300 K 153.4 J/(mol K) 1 kJ/1000 J = 943.6 kJ/mol 6. a) non-spontaneous; spontaneous. b) T transition = H / S = 100 kJ/mol / [100 J/(mol K) 1 kJ/1000 J] = 1000 K...
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This note was uploaded on 12/10/2011 for the course ENU 4612c taught by Professor Ghita during the Fall '11 term at University of Florida.

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