A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge. 2Cr *(aq) + 3Zn(s) → 2Cr(s) + 3Zn²*(aq) The anode reaction is: The cathode reaction is: |the Cr|Cr³* electrode| In the external circuit, electrons migrate | Zn|Zn2* electrode. | the |the Zn|Zn²* compartment | In the salt bridge, anions migrate| Cr|Cr* compartment. v the

Consider the following voltaic cellat 25°C: Al(s) | Al3*(0.20 M, aq) || Al3+(0.75 M, aq) | Al(s) If the standard reduction potential for the Al3+(aq) /Al(s) redox couple is -1.66 V, what is the overall cell reaction and the cell potential of the voltaic cell shown above? (Reference the cell as written above.) The overall cell reaction is Al3+(0.75 M, aq) AIS*(0.20 M, ag) and E°cell = +0.0113 V. There is no overall cell reaction and E°cell = 0.00 V. The overall cell reaction is Al3+(0.20 M, aq) Als*(0.75 M, aq) and E°cell = +0.0113 V. The overall cell reaction is Al3+(0.20 M, aq) →A13+(0.75 M, ag) and E°cell| = -0.0113 V. The overall cell reaction is Al3*(0.75 M, aq) →AI3*(0.20 M, aq) and E°cell = -0.0113 V. None of these

Consider the following half-reactions and their standard reduction potentials then give the standard line (cell) notation for a voltaic cell built on these half reactions. Mn2*(aq) + 2 e Mn(s) E° = -1.18 V Fe(aq) +3 e Fe(s) E° = -0.036 V A. Fe(s) | Fe3t(aq, 1.0 M) || Mn (s) | Mn 2*(aq. 1.0 M) B. Mn (s) | Mn 2*(aq, 1.0 M) | | Fe(s) | Fe(aq. 1.0 M) C. Fe(s) | Fe3t(aq. 1.0 M) || Mn2*(aq, 1.0 M) | Mn(s) D. Mn (s) | Mn 2*(aq. 1.0 M) || Fe(aq, 1.0 M) | Fe(s)

A voltaic cell is constructed in which the anode is a Sn|Sn²+ half cell and the cathode is a Cu+| Cu²+ half cell. The half-cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) I The anode reaction is: + The cathode reaction is: + The net cell reaction is: + In the external circuit, electrons migrate electrode the Cu+I Cu²+ electrode. In the salt bridge, anions migrate the Sn|Sn²+ compartment. + + + the Sn|Sn²+ the Cu+I Cu2+ compartment

Consider the voltaic cellZn(s) | Zn2+(aq, 0.100 mol L−1) || Cu2+(aq, 1.200 mol L−1) | Cu(s)with the concentrations in the compartments as indicated. The circuit is closed and the battery is discharged until the concentration of Cu2+(aq) is 0.850 mol L−1. What is the electromotive force of the cell at that stage in the discharge?A) 1.048 VB) 0.508 VC) 0.434 VD) 1.132 VE) 1.108 V

A voltaic cell is constructed in which the following cell reaction occurs. The half-cell compartments are connected by a salt bridge. Pb2+(aq) + Mn(s) Pb(s) + Mn2+(aq) The anode reaction is: The cathode reaction is: + + In the external circuit, electrons migrate e the Mn|Mn2+ electrode e the Pb|Pb2+ electrode. In the salt bridge, anions migrate e the Pb|Pb²+ compartment e the Mn|Mn2+ compartment. +

The cell potential of the following cell at 25°C is 0.475 V: Zn|Zn?t (1.0 M) || H* (test solution) H2 (1.0 atm)|Pt What is the pH of the test solution? The standard reduction potential for Zn+ is –0.76 V. (Enter your answer to two significant figures.) pH =

Enter electrons as e A voltaic cell is constructed in which the anode is a Fe2+|Fe3+ half cell and the cathode is a F|F, half cell. The half-cell compartments are connected by a salt bridge. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) The anode reaction is: The cathode reaction is: The net cell reaction is: +. In the external circuit, electrons migrate the Fe2+|Fe3+ electrode the F|F, electrode. from to In the salt bridge, anions migrate the F|F, compartment 3- the Fe2+|Fe+ compartment. +. +. 1

Balance the REDOX reaction associated with the cell shown below, in acidic medium: 2+ Fe(s) | Fe² || MnO (aq) Mn²) | Pt(s) Μη '(aq) 4(aq)' Enter the number for the coefficient of H₂O in the balanced equation:

3) Draw a picture of the galvanic cell represented by the line notation below and then write the reduction half-reactions for each electrode. Also identify the anode and cathode for each half cell. Pt (s) | Fe3+ (aq), Fe2+ (aq) || Cr2O72-(aq), Cr3+ (aq), HA (aq) | Pt (s)