Exam3_Eqns - 1 T 2 1 T 1 G cell = -(n)( ) E cell Q = It K w...

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MIT OpenCourseWare http://ocw.mit.edu 5.111 Principles of Chemical Science Fall 2008 For information about citing these materials or our Terms of Use, visit: http://ocw.mit.edu/terms .
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Page 9 of 10 pages Equations and constants for Exam 3 x = b ± b 2 4ac 2a pK a = -log [K a ] R = 8.315 J K -1 mol -1 pOH = -log [OH - ] (Faraday's constant) = 96,485 C mol -1 pH = -log [H 3 O + ] 1V = 1 J/C 1A = 1C/s pH pK a - log [HA] [A - ] K w = 1.00 x 10 -14 at 25°C Δ E ° (cell) = E ° (cathode) - E ° (anode) 14.00 = pH + pOH at 25 °C RT/ = 0.025693 V at 25.00 ° C /RT = 38.921 V -1 at 25.00 °C Δ G ° = - RT ln K Δ E cell = E ° cell (RT/ n) lnQ Δ G = Δ G ° + RT ln Q ln K = (n /RT) Δ E ° Δ G ° = Δ H ° - T Δ S ° E 3 ° = [n 1 E 1 ° (reduction) – n 2 E 2 ° (oxidation)]/n 3 ln K 2 K 1 = - Δ H ° R
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Unformatted text preview: 1 T 2 1 T 1 G cell = -(n)( ) E cell Q = It K w = K a K b Standard Reduction Potentials at 25C Half-Reactions E (volts) Au + ( aq )+ e- Au (s) 1.69 MnO 4-(aq) + 8H + (aq) + 5e- Mn 2+ (aq) + 4H 2 O (l) 1.51 Ag + (aq) + 1e- Ag (s) 0.80 Cu 2+ ( aq ) + 2e- Cu( s ) 0.34 AgCl (s) + 1e- Ag (s) + Cl-(aq) 0.22 Sn 4+ (aq) + 2e- Sn 2+ (aq) 0.15 2H + ( aq ) + 2e- H 2 0 Pb 2+ ( aq ) + 2 e- Pb (s) -0.13 Sn 2+ ( aq ) + 2 e- Sn (s) -0.14 Ni 2+ ( aq ) + 2 e- Ni (s) -0.23 Fe 2+ ( aq ) + 2e- Fe ( s ) -0.44 Cr 3+ ( aq ) + 3e- Cr ( s ) -0.74 Zn 2+ ( aq ) + 2e- Zn (s) -0.76 Image by MIT OpenCourseWare...
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This note was uploaded on 11/27/2011 for the course CHEMICAL E 20.410j taught by Professor Rogerd.kamm during the Spring '03 term at MIT.

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Exam3_Eqns - 1 T 2 1 T 1 G cell = -(n)( ) E cell Q = It K w...

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