Given the standard oxidation potentials: and . What is the standard electromotive force () in Volts — Electrochemistry Chemistry Question
Question
Given the standard oxidation potentials: $E^\circ_{Zn/Zn^{2+}} = +0.76\text{ V}$ and $E^\circ_{Fe/Fe^{2+}} = +0.41\text{ V}$. What is the standard electromotive force ($E^\circ_{cell}$) in Volts for the standard galvanic cell represented by $Zn(s) \| Zn^{2+}(aq) \|\| Fe^{2+}(aq) \| Fe(s)$?
Answer: 0.35
💡 Solution & Explanation
The standard reduction potentials (SRP) are the negative of the standard oxidation potentials (SOP). $E^\circ_{Zn^{2+}/Zn} = -0.76\text{ V}$ and $E^\circ_{Fe^{2+}/Fe} = -0.41\text{ V}$. In the cell representation $Zn \| Zn^{2+} \|\| Fe^{2+} \| Fe$, Zinc is the anode (oxidation) and Iron is the cathode (reduction). $E^\circ_{cell} = E^\circ_{cathode(SRP)} - E^\circ_{anode(SRP)} = -0.41 - (-0.76) = +0.35\text{ V}$.
💬Ask on WhatsApp →
Still have doubts about this question?
Send it to our AI chemistry tutor on WhatsApp — gets answered in minutes