For the cell reaction, Zn(s) | Zn2*(aq, 1 M) || Cu2*(aq, 1 M) | Cu(s), the electrode potential of cathode and anode are 0.34 V and -0.76 V respectively, what is the cell potential? O 1.10 V O -0.42 V -1.10 V O 0.42 V

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential 2+ Cu (aq)+e E. + - Cu' (aq) ʼred =+0.153 V 2+ MnO,(s)+4H"(aq)+2e - Mn (aq)+2H2O(1) =+1.23 V ʼred Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode. Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written. lo

A chemist designs a galvanic cell that uses these two half-reactions: half-reaction standard reduction potential Br,(1)+2e 2 Br (aq) E=+1.065 V || 'red 2+ MnO2(s)+4H (aq)+2e - Mn"(aq)+2 H,O(1) = +1.23 V red Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. Write a balanced equation for the half-reaction that happens at the anode, Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is

= 2.26 A voltaio cell employs the following redox reaction: 2 Fe (aq) +3 Mg (s) 2 Fe (s) +3 Mg (aq) Calculate the cell potential at 25 °C under each of the following conditions. In this solution, Ecel 1). Therefore, the reaction will proceed to the left. Part C [Fe"] = 2.85 M ; [Mg?+] = 2.1x10-3 M Express your answer in units of volts. Ecell= V

If the E cell of the following cell is 0.895 V, what is the pH in the anode compartment? Pt(s) | H2 (1.00 atm) | H"(aq) || Ag*(0.100 M) | Ag(s)

5. The following voltaic cell is made: Sn(s) | Snt2(aq) |I Fe*2(aq) | Fe(s) The tin electrode is placed in 1.00 L of 0.22 M SNSO4 solution and the iron electrode is placed in 1.00 L of 0.07 M FeSO4 solution. It's standard cell potential (E°cell) is 0.91 V. If this voltaic cell is run at 65°C, a non- standard condition, what is the cell potential of this voltaic cell?

An electrochemical cell is made by placing an iron electrode in 1.00 L of 0.19 M FeSO4 solution and a copper electrode in 1.00 L of 8.80 × 10-² M CuSO4 solution. Standard Electrode (Reduction) Potentials in Aqueous Solution at 25°C Cathode (Reduction) Half-Reaction ¯(aq) + 2e¯ ⇒ Fe(s) Cu²+ (aq) + 2e¯¯ ≈ Cu(s) Fe²+ Standard Potential, E° (V) -0.41 = 0.34 a. What is the initial voltage of this cell when it is properly constructed? Initial voltage 2+ b. Calculate the final concentration of Cu²+ in this cell if it is allowed to produce an average current of 1.78 amp for 241 s. Final concentration of Cu²+ M

For the cell shown, the measured cell potential, E cell, is -0.3643 V at 25 °C. Pt(s) | H₂(g,0.895 atm) | H* (aq, ? M) || Cd² +(aq, 1.00 M) | Cd(s) The balanced reduction half-reactions for the cell, and their respective standard reduction potential values, Eº, are → H₂ (g) 2 H+ (aq) + 2 e [H+] Cd²+(aq) + 2e Calculate the H+ concentration. = 0.141 → Cd(s) Incorrect E° = 0.00 V Eº = -0.403 V M

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31)Calculate the cell potential for the following reaction that takes place in an electrochemical cell at 25°C, given the standard reduction potentials for the half- reactions. Sn(s) | Sn2+(ag, 0.022 M) || Ag*(aq, 2.7 M) | Ag(s) Sn2+(ag) + 2 e → Sn(s) E° = -0.14 V Ag*(aq) + e¯ → Ag(s) E° = +0.80 V a. +1.01 V b. -0.83 V c. +1.31 V d. +0.01 V e. -0.66 V