An electrochemical cell that uses the reaction

Ti^3+ + 2Cr^2+ -> Ti^1+ + 2Cr^3+

Has a standard cell potential of
E¢ªcell = +1.19V

a. Write the two half-cell reactions.
b. Labeling all parts and show the direction of flow of electrons. (Place the anode electrode on the left and the cathode on the right.)
c. Determine the E¢ªred(reduction).

a. The two half-cell reactions in the given electrochemical cell can be determined by splitting the overall reaction into two separate oxidation and reduction half-reactions.

Oxidation half-reaction:
Ti^3+ -> Ti^1+ + 2e^-

Reduction half-reaction:
2Cr^2+ + 2e^- -> 2Cr^3+

b. To label the parts and show the direction of electron flow, we need to understand the concepts of anode and cathode. In an electrochemical cell, the anode is where oxidation occurs, and the cathode is where reduction occurs. The electrons flow from the anode (oxidation) to the cathode (reduction).

So, in this case:
Anode (left side): Ti^3+ -> Ti^1+ + 2e^-
Cathode (right side): 2Cr^2+ + 2e^- -> 2Cr^3+

c. The standard reduction potential (E¢ªred) of a half-reaction can be calculated using the standard cell potential (E¢ªcell) and the standard oxidation potential (E¢ªox) of the other half-reaction. The relationship between these values is given by the Nernst equation:

E¢ªred = E¢ªcell - E¢ªox

Given E¢ªcell = +1.19V, we need to find the standard oxidation potential (E¢ªox) for the Ti^3+ -> Ti^1+ + 2e^- half-reaction.

You can find the standard oxidation potentials (E¢ªox) in a table of standard electrode potentials. Locate the half-reaction Ti^3+ -> Ti^1+ + 2e^- in the table and record the corresponding oxidation potential (E¢ªox).

Once you have the value of E¢ªox, substitute it into the Nernst equation to calculate the standard reduction potential (E¢ªred).