What is the equilibrium constant (K) and standard Gibbs energy (ΔG°) at 25°C for the following cell reaction? Fe (s) + Co2+ (aq) → Fe2+ (aq) + Co (s) Note: this is the original reaction posted for the question was wrong. Someone suggested that this equation might be correct. Option choices are given below. If the answer found is not in the given answer choices, the reaction is wrong. The reaction given for the original problem was Fe(s) +Ni2+→Ni2+ + Co(s) Equilibrium constant: A. 1.39x1018 B. 6.0 C. 4.7 D. 9.7 E. 5.7x106   Gibbs Energy: A. 4.4 B. 39 C. -3.85 D. -4.4 E. 39

Silver metal can be dissolved in acidic solutions via a redox reaction with generation of hydrogen gas. Which of the following is the correct cell notation for the reaction that will occur?

Calculate the K and AG for the following reaction at 25 °C: Zn(s) + CuSO₂(aq) → ZnSO₂(aq) + Cu (s) Note: Reference the Standard reduction potentials at 25 °C and Fundamental constants tables for additional information. Part 1 of 2 Round your answer to 3 significant digits. Bo = Part 2 of 2 AGⓇ ☐x10 = Round your answer to 4 significant digits. X kJ mol 0x10 3 X Ś

Consider this cell diagram for an electrochemical cell: Pt(s) | H2(g) | H*(aq) || Cu*(aq) | Cu(s) What is the overall balanced reaction for this redox reaction? O 2H (aq) + 2Cu(s) H2(g) + 2Cu (aq). O H2(g) + 2Cu'(aq) → 2H*(aq) + 2Cu(s) O H2(g) + 2Cu(s)H'(aq) + 2Cu'(aq) O H2(g) + Cu (aq) H'(aq) + Cu(s)

Balance the following reaction. Calculate the cell potential and Gibbs free energy of this reaction at standard conditions. Write the line representations for the Galvanic Cells, indicating the anode and cathode.   MnO4-  +     H+    +      Ce3+     ->         Ce4+     +     Mn2+    +      H2O

. Consider the oxidation-reduction reaction Mg (s) + Cu2+ (aq) → Mg2+ (aq) + Cu (s)           Sketch a galvanic cell that uses this reaction. Which metal ion is reduced? Which metal is oxidized? What half-reaction takes place at the anode in the cell? What half-reaction takes place at the cathode?

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Consider the following reaction at 298K. Hg²+ (aq) + Ni(s)→→→→→→ Hg({) + Ni²+ (aq) The standard Gibbs free energy change for this reaction is -213.27 kJ. Use the Gibbs free energy change to calculate the standard cell potential for this reaction. Eºcell =

A student made measurements on some electrochemical cells and calculated three quantities: • The standard reaction free energy AGº. • 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 aG K E -21 1.42 x 10 A 1 119. kJ/mol O 1.23 V -- В - 51. kJ/mol 1.16 X 10 -0.53 V -11 2.06 X 10 1 -61. kJ/mol 0.63 V

Balance the following reactions. Calculate the cell potential and the Gibbs free energy of these reactions at standard conditions. Identify the reactions with K > 1 among the following redox reactions. Write the line representations for the Galvanic cells, indicating the anode and 1. cathode. a. Cl2 + Br → Ct + Br2 b. Mnoa + H* + Ce → Cet + Mn2 + H20