Consider the following reaction at 298K. Fe3+ (aq) + Cu+ (aq)  Fe2+ (aq) + Cu2+ (aq) Which of the following statements are correct? Choose all that apply. 1. n = 5 mol electrons 2. The reaction is reactant-favored. 3. delta Go > 0 4. Eocell > 0 5. K > 1

If the equilibrium constant for a one-electron redox reaction at 298 KK is 8.3×1048.3×104, calculate the corresponding ΔG∘ΔG∘ and E∘cellEcell∘. You may want to reference (Pages 868 - 871) Section 20.5 while completing this problem.     Part A Express your answer using two significant figures.         ΔG∘ΔG∘ = nothing kJkJ   SubmitRequest Answer Part B Express your answer using two significant figures.         E∘cellEcell∘ = nothing V

11. Consider the following reaction and its AG-AGo at 25.00 °C 2Ag(aq)+Cu(s) 2Ag(s)+Cu (aq) AG =-88660 J/mol a. Calculate the standard cell potential, E, for the reaction. b. Calculate the equilibrium constant, K, for the reaction.

A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AG. • The equilibrium constant K at 25.0 °C. • The cell potential under standard conditions E°. His results are listed below. Unfortunately, the student may have made some mistakes. Examine his results carefully and tick the box next to the incorrect quantity in each row, if any. Note: If there is a mistake in a row, only one of the three quantities listed is wrong. Also, you may assume the number of significant digits in each quantity is correct. Also note: for each cell, the number n of electrons transferred per redox reaction is 1. calculated quantities (Check the box next to any that are wrong.) cell n AGº K A 1 -19. kJ/mol 4.69 × 10 0 E 0.20 V 13 B 1 77. kJ/mol 3.09 × 10 0.80 V -14 C 1 75. kJ/mol 7.25 X 10 0.78 V