a. Given the following standard cell notation, draw and label the electrochemical cell. Be sure to label: anode, cathode, salt bridge, flow of electrons, flow of all ions. b. Write the half reactions for each half cell, and the net cell reaction. c. Calculate the cell potential. Mg(s) | Mg(NO3)2(aq) ||AgNO3(aq) [Ag(s)

An electrochemical cell contains sodium chloride as a salt bridge and has the following line notation: X(s) | X* (aq) || Ag (aq) | Ag (s) (Note that X is a chemical that you will need to identify with oxidation state. +n) E° cell = 1.329 V a. Write the half-reaction that occurs at the anode and determine the E° anode. (Use the symbol X for now if this is the reaction at the anode). Write the half-reaction that occurs at the cathode and determine the E° cathode. (Use the symbol X for now if this is the reaction at the cathode). b. Identify the X(s)Xn* (ag) half-reaction and determine the Eo for this half-reaction.

6. Sketch a voltaic cell for the following overall redox reaction. 3 Cl2(g) + 2 Fe(s) — 6 CІ (аq) + 2 Fe3+(aq) а. Label the anode and cathode b. Indicate the half-reaction occurring at each electrode c. Indicate the species present in each solution.

If a voltaic cell is created between a Sr2+/Sr electrode and a In3+/In electrode

Consider a voltaic cell that can be described like so. It is set up at standard conditions. A gold electrode is in contact with Au(NO3)3 (aq) and a lead electrode in contact with Pb(NO3)2 (aq) at 25 degrees C. Write true or false next to each of the following statements regarding the voltaic cell. I. Adding H20 to the lead half-cell will increase the measured cell potential. II. A salt-bridge is used to prevent charge buildup in the half-cells. III. This will result in the production of Pb2+ ions.

Consider the cell diagram: Pb(s)|Pb(NO3)2(aq)||FeCl3(aq)|Fe(s). Write the balanced net-ionic equations for the half-reactions that occur at the two electrodes. a. Anode= b. Cathode=

What statement about a galvanic cell constructed with Cut/Cu and Fe2+/Fe is correct? Standard Reduction Potentials E°red / V Cu* + e→ Cu +0.52 Fe2* + 2e-→ Fe -0.44 а. Fe(s) will reduce Cu*(aq). b. Fe(s) is a stronger oxidizing agent than Cu(s). С. The standard cell potential (E°cell) is +1.40 V. d. Fe<+(aq) is reduced at the cathode.

A student constructed a voltaic cell by combining Sn/Sn2+ and Zn/Zn2+ two half cells and measured a cell potential of 0.620 V. He then constructed a voltaic cell by combining Sn/Sn2+ and Ni/Ni2+ two half cells and measured a cell potential of 0.140 V. It is seen that the tin metal precipitated out of the solution in each above cell. Except for the reduction potential of Zn which is known as -0.763V, the reduction potentials of all the other two electrodes are unknown.  a. Calculate the reduction potential of Sn2+ (aq)+ 2e- ---> Sn(s).  b. Calculate the reduction potential of Ni2+(aq)+2e- ----> Ni(s) c. Write the cell reaction for the cell of Sn/Sn2+ and Zn/Zn2+