Lecture_Notes_102309b

# Lecture_Notes_102309b - Practice Problem Calculate Ksp for...

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Practice Problem y Calculate K sp for iron(II) sulfide given the following data: { FeS (s) + 2 e - Fe (s) + S 2- (aq) ε o = -1.01 V { Fe 2+ (aq) + 2 e - Fe (s) ε o = -0.44 V

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How many electrons are transferred in the following balanced redox reaction? 2 Fe 3+ (aq) + 2 Cr 3+ (aq) + 7 H 2 O (l) 2 Fe (s) + Cr 2 O 7 2- (aq) + 14 H + (aq) none 2 4 6 20% 49% 17% 14% 1. none 2. 2 3. 4 4. 6
If ε o cell = 0.45 V for a reaction where 2 electrons are transferred, what is the value of the equilibrium constant at 25 o C? 0.45 1.67 x 1015 4.08 x 107 cannot be determined... 5% 1% 12% 81% 1. 0.45 2. 1.67 x 10 15 3. 4.08 x 10 7 4. cannot be determined from the information given

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Nernst Equation y A voltaic cell employs the following redox reaction: { 2 Fe 3+ (aq) + 3 Mg (s) 2 Fe (s) + 3 Mg 2+ (aq) ε o = 2.33 V y Calculate the cell potential under each of the following conditions. y [Fe 3+ ] = 1.00 x 10 -3 M; [Mg 2+ ] = 2.50 M y [Fe 3+ ] = 2.00 M; [Mg 2+ ] = 1.50 x 10 -3 M
Nernst Equation y A voltaic cell consists of a Zn/Zn 2+ half-cell and a Ni/Ni 2+ half-cell at 25 o C. The initial concentrations of Ni 2+ and Zn 2+ are 1.50 M and 0.100 M respectively.

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