A particular galvanic cell has a redox reaction in which a magnesium metal displaces nickel (II) ion from aqueous solution, as shows in the redox reaction below Mg (s) + Ni²*(ag) → Mg²*+ Ni(s) Determine the half-cell reaction for both the anode and cathode electrodes.

Use a table of Standard Reduction Potentials to predict if a reaction will occur between Fe metal and F2(g), when the two are brought in contact via standard 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 standard galvanic cell is constructed in which a Co2+ | Co 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.) The cathode reaction is Co2+ + 2e -> Co. Co is oxidized at the cathode. The anode compartment could be Fe³+|Fe²+. As the cell runs, anions will migrate from the Co²+ | Co compartment to the other compartment. In the external circuit, electrons flow from the Co²+ | Co compartment to the other compartment.

A certain half-reaction has a standard reduction potential Ed+0.57 V. An engineer proposes using this half-reaction at the anode of a galvanic cell that must provide at least 1.00 V of electrical power. The cell will operate under standard conditions. red Note for advanced students: assume the engineer requires this half-reaction to happen at the anode of the cell. Is there a minimum standard reduction potential that the half-reaction used at the cathode of this cell can have? 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. Is there a maximum standard reduction potential that the half-reaction used at the cathode of this cell can have? If so, check the "yes" box and calculate the maximum. Round your answer to 2 decimal places. If there is no upper Smit, check the "no" box. By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be used at…

A certain half-reaction has a standard reduction potential E = -0.23 V. An engineer proposes using this half-reaction at the anode of a red galvanic cell that must provide at least 0.60 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 anode of the cell. Is there a minimum standard reduction. potential that the half-reaction used at the cathode of this cell can have? 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. Is there a maximum standard reduction potential that the half-reaction used at the cathode of this cell can have? 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. By using the information in the ALEKS Data tab, write a balanced equation describing a half reaction that could be used…

A galvanic cell is powered by the following redox reaction: 2+ MnO₂ (s) + 4H* (aq) + 2 Br¯ (aq) → Mn²(aq) + 2 H₂O(1) + Br₂(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. Write a balanced equation for the half-reaction that takes place at the anode. Calculate the cell voltage under standard conditions. Round your answer to 2 decimal places. 0 = = Ov ローロ 0

Subject: chemistry

Q26 (A). Define an electrolytic cell. Describe with a neat diagram, an electrolytic cell for the decomposition of molten NaCl. Write the reactions at the anode and cathode

Use the standard reduction potentials given below to predict if a reaction will occur between Co(s) and Cl₂ (g), when the two are brought in contact via standard half-cells in a voltaic cell. Cl₂(g) + 2e → 2Cl(aq) = 1.360 V red = -0.280 V Co²+ (aq) + 2e → Co(s) E red 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. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) +

A non-standard state galvanic cell is constructed at 25.00°C as described here.  The Fe(s) anode is immersed in a 0.040 M Fe(NO3)2 solution.  The Cu(s) cathode is immersed in a 0.0060 M Cu(NO3)2.  The circuit is completed with a salt bridge containing 1.0 M KNO3.  The standard Fe/Fe2+ reduction potential is –0.44 V.  The standard Cu/Cu2+ reduction potential is +0.34 V.  Calculate the non-standard-state cell potential for this galvanic cell and determine if the reaction described is spontaneous under these conditions.