Trying to finish, but I am stuck on the electrochemical portions:
4) Determine the concentration of the magnesium ion when a cell voltage of 2.68V is obtained using 0.405 M copper (ll) nitrate.
5) Determine the free energy for the cell
6) Consider a galvanic cell consisting of the following redox couples:
Electrochemsitry and Redox Reactions
(20 points) Using a suitable reference table, write the corresponding half-reactions for the following electrochemical cell and determine the standard cell potential. Identify which cell represents the anode and which represents the cathode 3. Mg (s) | Mg (aq) I Cu2 (aq) | Cu (s) anede cothode 4. (20 points) For the cell in problem 3, determine the concentration of the magnesium ion when a cell voltage of 2.68 V is obtained using a 0.405 M copper) nitrate solution. 5. (10 points) Determine the free energy for the cell in Problem 4 6. (20 points) Consider a galvanic cell consisting of the following two redox couples: Ag, (aq, 0.010 M) + e' â Ag (s) CrD+ (aq, 0.010 M) + 3e. â Cr(s) Write the equation for the half-reaction at the cathode E"= +0.80 V Eo=-0.74 V a. b. Write the equation for the half-reaction at the anode c.Write a shorthand cell notation version of this battery d. Calculate the standard cell potential for this battery
Here, Zn undergoes oxidation by losing 2eâ, and the Cu2+ ions accept 2eâ to form metallic Cu, which is deposited at the copper electrode. At the zinc electrode, oxidation occurs, and hence it is known as the anode. Reduction occurs at the copper electrode, and hence it is called the cathode.
The electrochemical cell notation for this cell is Zn(s)|Zn2+(aq)||Cu2+(aq)|Cu(s).
Construction of a voltaic cell
Consider a chromium-silver voltaic cell that is constructed such that one half-cell consists of the chromium, Cr, electrode immersed in a Cr(NO3)3 solution, and the other half-cell consists of the silver, Ag, electrode immersed in a AgNO3 solution. The two electrodes are connected by a copper wire. The Cr electrode acts as the anode, and the Ag electrode acts as the cathode. To maintain electric neutrality, you add a KNO3 salt bridge separating the two half-cells. Use this information to solve Parts B, C, and D.
Part B
The half-cell is a chamber in the voltaic cell where one half-cell is the site of the oxidation reaction and the other half-cell is the site of the reduction reaction.
Type the half-cell reaction that takes place at the anode for the chromium-silver voltaic cell. Indicate the physical states using the abbreviation (s), (l), or (g) for solid, liquid, or gas, respectively. Use (aq) for an aqueous solution. Do not forget to add electrons in your reaction.
Express your answer as a chemical equation.
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Part C
The half-cell is a chamber in the voltaic cell where one half-cell is the site of an oxidation reaction and the other half-cell is the site of a reduction reaction.
Type the half-cell reaction that takes place at the cathode for the chromium-silver voltaic cell. Indicate physical states using the abbreviation (s), (l), or (g) for solid, liquid, or gas, respectively. Use (aq) for an aqueous solution. Do not forget to add electrons in your reaction.
