Given the following half-cell reactions: Cr+3  +  3e-  ->  Cr           E° = -0.74 V Zn+2  +  2e-  ->  Zn          E° = -0.83 V Determine the electrochemical cell reaction.

7-A fuel cell uses the following reduction half-reactions. O2(g) + 2H20(1) + 4e- 40H- (ag) E° = 0.401 V CO3-(aq) + 7H2O(1) + 8e– → CH«(g) + 100H-(ag) E° = 0.110 V Ja) What is the maximum cell voltage that can be generated (b) What is the overall cell reaction that occurs?

A certain half-reaction has a standard reduction potential E=+1.34 V. An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 1.20 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer reguires this half-reaction to happen at the anode of the cell. nh Data Half-Reaction E° (V) 0.7996 Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? = Ov Ag+ (aq) + e- -→ Ag (s) O yes, there is a minimum. E %3D red Al3+ (aq) + 3e- → Al (s) -1.676 1.692 Au+ (aq) + e → Au (s) If so, check the "yes" box and calculate the minimum. Round your answer to 2 decimal places. If there is no lower limit, check the "no" box. O no minimum Au3+ (aq) + 3e- → Au (s) 1.498 Ba2+ (ag) + 2e- - Ba (s) -2.912 Brz (1) + 2e 2Br (aq) 1.066 - Ca2+ (ag) + 2e Ca (s) -2.868 Is there a maximum standard reduction potential that the half-reaction used at the…

Calculate the cell potential of a voltaic cell given the following standard potentials: X -> X2+ + 2 e-         Eo = -1.69 V Y3+ -> + 3 e- -> Y        Eo = 0.94 V    Note: Answer in 2 decimal places.

Predict reaction and calculate E°cell from standard reduction potentials. A voltaic cell is constructed from a standard AI3+|Al half cell (E°red = -1.660V) and a standard F2|F° half cell (E°red = 2.870V). What is the spontaneous reaction that takes place, and what is the standard cell potential? Spontaneous cell reaction:Write a balanced equation using the smallest integer coefficients possible. + Standard cell potential: V.

Given the electrochemical reaction, Mg/ Mg 2(aq) // Zn2(aq) / Zn, E+1.61 V. If the standard reduction potential of Zn²-Zn is -0.76V. What is the standard reduction potential of Mg2+ = Mg? -2.37 V (В 0.85 V -0.85 V 2.37 V

A voltaic cell is constructed with two silver electrodes, where the half-reaction isAg2+(aq) + 2e- → Ag (s)   E° = -0.322 VDetermine the cell emf at 25 °C when the concentrations of chloride ion in the two compartments are 4.0 Mand 0.050 M, respectively.

Given the following standard reduction half reactions calculate the standard cell potential (E°cell) to 2 decimal places. O2(g) + 4H+ + 4e" 1 4H* (aq) 2H20L) ; E°red. = 1.23 V A13+ (aq) + Зе Al(s) ; E°red. = -1.66 V

A voltaic cell using Pb²⁺/Pb and Ni²⁺/Ni half-cells is set up at standard conditions, and each compartment has a volume of 355 mL. What is the cell potential, in V, after it has delivered 0.150 A for 51.0 hours at 25.0 °C? (E° for Pb²⁺/Pb = -0.130 V and E° for Ni²⁺/Ni = -0.250 V.)

A lithium battery is being developed. Its voltaic cell is constructed based on Li metal electrode and PbsO4 solid electrode. Their standard reduction potentials at 25 °C are given below. E°(Li* (aq) → Li (s)) = -3.040 Volt E°(PbSO4 (S) > Pb (s) + SO42 (aq) = - 0.356 Volt. Which of the following statements is true about this working (spontaneous) voltaic cell? a. The anode is PbsO4 (s) electrode. The standard cell potential of this voltaic cell is E°(cell) = 2.328 Volt O. PBSO4 (s) is a weaker oxidizing agent than Lit. To make a commercial product, the voltaic cell is adjusted to have [Lit] = 2.1 M and [SO42] = 3.5 M. The cell d. potential E under this condition should be less than the standard cell potential E°(cell). e. None of the above