A certain half-reaction has a standard reduction potential Ed=+1.34 V. An engineer proposes using this half-reaction at the cathode 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 requires this half-reaction to happen at the cathode of the celI. Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? Ov yes, there is a minimum. red 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. no minimum Is there a maximum standard reduction potential that the half-reaction used at the anode of this cell can have? yes, there is a maximum. red dh Data If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper limit, check the "no" box. no maximum E° (V) Half-Reaction F2 (g) + 2e → 2F¯ (aq) 2.866 Co3+ (aq) + e -→ Co2+ (aq) 1.92 By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be used at the anode of this cell. H2O2 (aq) + 2H+ (aq) + 2e 2H2O (I) 1.776 Au+ (aq) + e Au (s) 1.692 Mn2+ (aq) + 4H2O (I) MnO4 (aq) + 8H+ (aq) + 5e- 1.507 Note: write the half reaction as it would actually occur at the anode. Au3+ (aq) + 3e Au (s) 1.498 2C1 (aq) Cl2 (g) + 2e- 1.35827 O2 (g) + 4H+ (aq) + 4e → 2H20 (I) 1.229 Mn2+ (aq) + 2H2O (I) MnO2 (s) + 4H+ (aq) + 2e¯ → 1.224 2103 (aq) + 12H+ (aq) + 10e I2 (s) + 6H2O (I) 1.195 Br2 (1) + 2e- → 2Br (aq) 1.066 Vo2+ (aq) + 2H+ (aq) + e-→ vO2+ (aq) + H20 (1) 0.991 Explanation Check NO (g) + H20 (I) HNO2 (aq) + H+ (aq) + e 0.983 dard reduction ction used at Ov yes, there is a minimum. %3D red have? ala nh Data and calculate - answer to 2 no lower 2H+ (aq) + 2e- H2 (g) 0.000 no minimum Fe3+ (aq) + 3e Fe (s) -0.037 Pb2+ (aq) + 2e Pb (s) -0.1262 CrO42- (aq) + 4H,0 (1) + 3e → Cr(OH)3 (s) + 50H (aq) -0.13 dard reduction ction used at have? yes, there is a Sn2+ (aq) + 2e Sn (s) -0.1375 Ni2+ (aq) + 2e→ Ni (s) -0.257 and calculate r answer to 2 no upper Co2+ (aq) + 2e Co (s) -0.28 no maximum PBSO4 (s) + H+ (aq) + 2e Pb (s) + HSO4 (aq) -0.3588 Cr+ (aq) + e Cr2+ (aq) -0.407 Fe2+ (aq) + 2e Fe (s) -0.447 n the ALEKS equation chat could be cell. Cr3+ (aq) + 3e Cr (s) -0.744 Zn2+ (aq) + 2e Zn (s) -0.7618 on as it would e. 2H20 (1) + 2e→ H2 (g) + 2OH- (aq) -0.8277 Cr2+ (aq) + 2e Cr (s) =0.913 N2 (g) + 4H2O (I) + 4e → 40H- (aq) + N2H4 (aq) -1.16 Mn2+ (aq) + 2e Mn (s) -1.185 Al3+ (aq) + 3e- Al (s) -1.676 Sc3+ (aq) + 3e Sc (s) -2.077 Mg2+ (aq) + 2e Mg (s) -2.372 Na+ (aq) + e Na (s) -2.71 Check Ca2+ (aq) + 2e Ca (s) -2.868 Ba2+ (ag) + 2e Ba (s) -2.912

To work better as a sacrificial anode, an alloy can potentially be created to have a more (positive/negative/neutral) reduction potential than the original metal.

Enter electrons as e-. Use smallest possible integer coefficients. If a box is not needed, leave it blank. Use the table 'Standard Reduction Potentials' located in the 'Tables', to predict if a reaction will occur between Mg metal and F2(g), when the two are brought in contact via half-cells in a voltaic cell.If a reaction will occur, write a balanced net ionic equation for the reaction, assuming that the product ions are in aqueous solution. If no reaction will occur, leave all boxes blank.     +              +

A certain half-reaction has a standard reduction potential Eed = +0.01 V. An engineer proposes using this half-reaction at the cathode of a galvanic cell that must provide at least 1.00 V of electrical power. The cell will operate under standard conditions. Note for advanced students: assume the engineer requires this half-reaction to happen at the cathode of the cell. olo ローロ Is there a minimum standard reduction potential that the half-reaction used at the anode of this cell can have? O yes, there is a minimum. = Uv red 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

Determine the minimum voltage required to produce Br2 (1) in an AIBR3 (aq) cell with inert electrodes. Your answer should follow the format: a) Write the half reaction that occurs at the cathode b) Write the half reaction that occurs at the anode c) Write the overall net cell reaction d) Voltage Required

please place it in  the correct order and write down if its a aq,l,g or s

Use the Standard Reduction Table to answer the following questions. Write a balanced net redox equation and determine both the standard cell potential and the number of electrons transferred for the spontaneous redox process that occurs when the following couples are connected. Use the lowest possib matter under the given conditions in your answer. For the reaction arrow, please use an extensive arrow to the right (-->). d) Fe2+/Fe + Zn²+/Zn chemPad XX→← Zn (s) + Fe2+ (aq) → Zn²+ (aq) + Fe ( Zn (s) + Fe^2+ (aq) --> Zn^2+ (aq) + Fe (s) Correct. E° = .31 Reduction half-reactions Li¹+ (aq) + e¹- K¹+ (aq)+ e¹- Ba²+ (aq) + 2 e¹- Ca²+ (aq) + 2 e¹- Na¹ + (aq) + e¹- Mg²+ (aq) + 2 e¹- Al³+ (aq) + 3 e¹- U³+ (aq) + 3 e¹- Ti²+ (aq) + 2 e¹- Mn²+ (aq) + 2 e¹- 2 H₂O +2 e¹- Zn²+ (aq) + 2 e¹- Cr³+ (aq) + 3 e¹- HCHO(aq) + 2 H₂O +2e¹- Fe²+ (aq) + 2 e¹- 2 H₂O +2 e¹- X V Cd²+ (aq) + 2 e¹- PbSO4(s) + 2 e¹- In³+ (aq) + 3 e¹- Co²+ (aq) + 2 e¹- → Help Greek n (moles of e") = 2 E°(V) -3.04 -2.92 -2.92 -2.84…

A standard galvanic cell is constructed in which a Cd2+ | Cd half cell acts as the cathode. Which of the following statements are correct? Hint: Refer to a table of standard reduction potentials. (Choose all that apply.) A)   As the cell runs, anions will migrate from the Cd2+|Cd compartment to the other compartment. B)    The anode compartment could be F2|F-. C)    The anode reaction could be Cr2+ -> Cr3+ + e- D)    The cathode reaction is Cd -> Cd2+ + 2e- E)    Cd2+ is reduced at the cathode.