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.
Look up the reduction potential for Zn^2+ + 2e ==> Zn(s) in your text. Reverse the sign.
Add that to the reduction potential for
Ag^+ + e ==> Ag(s)
That potential will be for the reaction of
Zn(s) + 2Ag^+(aq) ==> 2Ag(s) + Zn^2+(aq)
reduction potential for the Zn is -.76 for Ag it is .80
so i take the Zn change the sign so it it .76 then i go
.76+.80=1.56 does this sound right?
yes
Well, if I were to calculate that, I'd probably end up with a short circuit! Electrocchemistry is not my strong suit, and I'm more of a joker than a scientist. However, I can tell you that the standard cell potential can be calculated by subtracting the standard electrode potential of the zinc electrode from the standard electrode potential of the silver electrode. So, you might want to grab that textbook and use the values given to calculate the standard cell potential. Good luck, and if you need a good laugh along the way, feel free to ask!
To calculate the standard cell potential for a cell with a zinc electrode and a silver electrode, we need to use the values from a table of standard electrode potentials. Here's how you can do it:
1. Start by finding the standard reduction potential for the zinc half-reaction. Look for the entry in the table that corresponds to the reduction of Zn2+ to Zn. The standard reduction potential for this reaction is -0.76 V.
2. Next, find the standard reduction potential for the silver half-reaction. Look for the entry in the table that corresponds to the reduction of Ag+ to Ag. The standard reduction potential for this reaction is +0.80 V.
3. The standard cell potential is calculated by taking the difference between the reduction potentials of the two half-reactions. In this case, it would be:
Standard cell potential = Reduction potential of Ag+ - Reduction potential of Zn2+
= (+0.80 V) - (-0.76 V)
= +1.56 V
So, the standard cell potential for this cell is +1.56 V.
Keep in mind that the standard cell potential is a measure of the driving force behind a redox reaction. It indicates the tendency of a reaction to occur spontaneously. Positive values indicate spontaneous reactions, while negative values indicate non-spontaneous reactions.