A galvanic cell is set up by making 1 M solutions of FeSO4 and ZnSO4, with an iron (Fe) electrode in the FeSO4 solution and a zinc (Zn) electrode in the ZnSO4 solution.   The half reactions that drive the galvanic cell are:    Fe2+ + 2e- → Fe      (at the cathode)               Zn  →  Zn2+ + 2e-    (at the anode) What happens to the cell voltage, ε0, while the cell runs?

A voltaic cell operating under standard conditions (1.0 M ion concentrations) utilizes the following reaction: What is the effect on the cell emf of each of the following changes? (a) Water is added to the anode compartment, diluting the solution. O The positive cell emf rises, becoming more positive. O The positive cell emf drops closer to zero. O The negative cell emf rises closer to zero. O The negative cell emf drops, becoming more negative. No change in cell emf occurs. (b) The size of the chromium electrode is increased. The positive cell emf rises, becoming more positive. O The positive cell emf drops closer to zero. O The negative cell emf rises closer to zero. O The negative cell emf drops, becoming more negative. O No change in cell emf occurs. x (c) A solution of 1.0 M CrCl3 is added to the anode compartment. The positive cell emf rises, becoming more positive. O The positive cell emf drops closer to zero. O The negative cell emf rises closer to zero. O The negative cell emf…

For the galvanic (voltaic) cell 2+ - Fe(s) + Mn²+ (aq) → Fe²+ (aq) + Mn(s) (E° = 0.77 V at 25 °C), what is [Fe²+] if [Mn²+] = 0.090 M and E = 0.78 V? Assume T is 298 K 1 4 7 +/- 2 LO 5 8 0.196 M 3 6 9 O X C x 100

Many electronic calculators use rechargeable nickel-cadmium batteries. The overall equation for the spontaneous reaction in these cells is: Cd(s) +NiO2(s) + H₂O(l) → Cd(OH)2(s) + Ni(OH)2(s) What is the reducing agent, oxidizing agent (correspondently)? O Cd(s); NiO₂(s) O NiO2(s), H₂O(l) O NiO2(s), Cd(s) ONIO₂(s), Cd(OH)2(s)

A voltaic cell is constructed with two silver electrodes, each of which is based on the following half reaction: AgCl (s)  + e- -> Ag (s) + Cl- (aq) The two half cells have [Cl-] = 0.0150 M and [Cl-] = 2.55 M, respectively. Determine the overall reaction that takes place in the cell.

A voltaic cell employs the following redox reaction: 2 Fe3+ Calculate the cell potential at 25 °C under each of the following conditions. (ag) + 3 Mg (s) → 2 Fe (s) + 3 Mg²+ (aq) Part C [Fe+] = 3.10 M ; [Mg²+] = 1.2x10-3 M Ecell Submit Previous Answers Request Answer X Incorrect; Try Again; 5 attempts remaining

a) Balance the following redox reaction in basic solution: H2O2(aq) + ClO2(aq) → ClO2-(aq) + O2(g) b) Sketch the voltaic cell for the redox reaction, labeling the direction for electron flow, the anode and cathode , and the species present in each half-cell. Show all the work please!

Consider a voltaic cell in which the following reaction takes place. 2Fe 2+ (aq) + H₂O2 (aq) + 2 H+ (aq) --→2Fe ³+ (aq) +2H₂O (1) calculate Eº Calculate E and Gibbs free energy when [Fe²+] = 0.00813 M, [H₂O₂] = 0.914 M, [Fe ³+] = 0.199 M, [H] = 1.32 x 10³ M

A voltaic cell is constructed with two silver–silver chloride electrodes, each of which is based on the following half-reaction: AgCl1s2 + e- ¡ Ag1s2 + Cl -1aq2 The two half-cells have 3Cl -4 = 0.0150 M and 3Cl -4= 2.55 M, respectively. What is the standard emf of the cell?

Calculate Ecell (volts) for the galvanic cell containing the reaction shown below where the concentration of the ion at the anode is 0.400 M and the concentration of the ion at the cathode is 1.86 M.