In acidic solution, Oz and Mn²+ ions react spontaneously: 03(g) + Mn²*(aq) + H,O(1) → 0,(8) + MnO,(s) + 2H*(aq) E cell 0.84 V Write the balanced half-reactions and calculate E when given E = 2.07 V. manganese ozone Include states of matter in your answers. Reduction half-reaction: 0,+2H +2e =H,0+02 2+ Oxidation half-reaction: Mn +2H,0=MnO,+2e +4H E -1.23 V manganese

Electrolysis of molten  NaClNaCl is done in a Downs cell operating at 7.0 volts (V) and 5.0×104 AA . How much  Na(s)Na(s) and Cl2Cl2 can be produced in eight hours in such a cell? Enter the mass of  NaNa and mass of  Cl2Cl2 in grams, separated by a comma.

Alkaline Batteries (AA/AAA) Cathode: 2 Mno2 (s) + H2O (I) + 2 e→ Mn,O3 (s) + 2 OH: (aq) +3 · Anode: Zn (s) + 2 OH (aq) → ZnO (s) + H2O (I) + 2 e- · Anode: Zn; Cathode: MnO2 (s) What is the overall balanced equation for the redox reaction occurring in an alkaline (AA/AAA) battery?

Galvanic cell has 2 half reactions O2(g) + 4H+(aq) + 4e- → 2H2O(l)    E0red = +1.23 V            Cr3+(aq) + 3e- → Cr(s)         E0red = -0.74 V Write a balanced equation that describes the cell, ensuring that E0cell > 0 V and Calculate E0cell

Consider the standard reduction potentials and redox couples used in a galvanic cell. Unbalanced Half-Reaction E°(V) MnO4 (aq) + 3e MnO2(s) (at basic pH) 0.59 Fe3+(aq) + e- Fe2*(aq) 0.77 What is the balanced reaction taking place in the cell (in basic solution)? 2 H20(1) + Mn04 (aq) + 3 Fe3+(aq) → 3 Fe2*(aq) + MnO2(s) + 4 OH- MnO2(s) + 4 OH¯ + 3 Fe3+(aq) 3 Fe2+(aq) + 2 H20(1) + MnO4¯(aq) MO 3 Fe2*(aq) + 2 H2O(1) + MnO4¯(aq) MnO2(s) + 4 OH¯ + 3 Fe3+(aq) M 3 Fe2+(aq) + MnO2(s) + 4 OH → 2 H20(1) + MnO4 (aq) + 3 Fe3+(aq)

Consider the galvanic cell based on the following half-reactions. Ag+ + e Ni²+ + 2e →→ Ni (a) Determine the overall cell reaction and calculate Omit states-of-matter from your answer.) chemPad XX→ (c) 8 cell → Ag 8⁰ = +0.80 V 8° -0.23 V Calculate 8 Help Greek º (b) Calculate AGº (in kJ) and K for the cell reaction at 25°C. AGO kJ K (in V). (Use the lowest possible whole number coefficients. cell (in V) at 25°C when [Ag+] = 1.0x10-4 M and [Ni²+] = 1.0×10-² M. cell V

G ロ・ロ A galvanic cell at a temperature of 25.0 °C is powered by the following redox reaction: 2+ 3+ MnO2 (s) + 4H* (aq) +2Cr²* (aq) → Mn²* (aq) + 2H2O (1) +2Cr³+ (aq) Suppose the cell is prepared with 0.190 M H* and 6.41 M Cr²+ in one half-cell and 0.205 M Mn2+ and 1.94 M Cr3+ in the other. Calculate the cell voltage under these conditions. Round your answer to 3 significant digits. ☐ ☐ x10 μ

A galvanic cell is powered by the following redox reaction: 2 Br,(1) + N,H,(aq) + 4OH (aq) 4 Br (aq) + N,(g) + 4 H,O(1) Answer the following questions about this cell. If you need any electrochemical data, be sure you get it from the ALEKS Data tab. Write a balanced equation for the half-reaction that takes place at the cathode. ローロ e Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. E - Round your answer to 2 decimal places. の

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!

What is the voltage of the following cell? Use the Reduction Potential Table found in Chapter 17 notes. Cr(s)|Cr³*(0.25 M) || |2(s)|1-(0.20 M)|Pt(s)