1) Using a table of standard electrode potentials (such as the one in your textbook), calculate the
standard cell potential for a cell made by placing a zinc electrode in a Zn2+(aq) solution which is
connected by an electrolyte to a Ag+(aq) solution containing a silver electrode. Show your work.
Same 'ol same 'ol. See your other posts.
To calculate the standard cell potential for the given cell, we can use the standard electrode potentials from a table. Here's how you can do it:
Step 1: Identify the half-reactions
In this cell, we have two half-reactions:
- Oxidation half-reaction: Zn(s) → Zn2+(aq) + 2e-
- Reduction half-reaction: Ag+(aq) + e- → Ag(s)
Step 2: Look up the standard electrode potentials
Refer to the table of standard electrode potentials in your textbook or any reliable source. Find the standard electrode potentials for both the oxidation and reduction half-reactions.
From the table, you may find the following values:
- Standard electrode potential for Zn2+(aq) + 2e- → Zn(s): E°(Zn2+/Zn) = -0.76 V
- Standard electrode potential for Ag+(aq) + e- → Ag(s): E°(Ag+/Ag) = +0.80 V
Step 3: Determine the overall cell potential
The overall cell potential (Ecell) can be calculated using the equation:
Ecell = E°(reduction) - E°(oxidation)
Substituting the values we found:
Ecell = E°(Ag+/Ag) - E°(Zn2+/Zn)
= (+0.80 V) - (-0.76 V)
= +0.80 V + 0.76 V
= +1.56 V
Therefore, the standard cell potential for the given cell is +1.56 V.