Calculate the standard potential of Chlorine given the standard EMF of a Zinc-Chloride battery and the…

Question

Calculate the standard potential of Chlorine given the standard EMF of a Zinc-Chloride battery and the standard reduction potential of Zinc.

ScanSolve AI Tutor · Accepted Answer

Here's how to calculate the standard potential of Chlorine:

Identify the given values.
The standard EMF of the Zinc-Chloride battery ( $E^\circ_{cell}$ ) is $2.1234\,V$ .
The standard reduction potential of Zinc ( $E^\circ_{red}(Zn^{2+}/Zn)$ ) is $-0.7634\,V$ .
Determine the roles of Zinc and Chlorine in the battery.
In a Zinc-Chloride battery, Zinc acts as the anode (where oxidation occurs), and Chlorine acts as the cathode (where reduction occurs).
The half-reactions are:
Anode (oxidation): $Zn(s) \longrightarrow Zn^{2+}(aq) + 2e^-$
Cathode (reduction): $Cl_2(g) + 2e^- \longrightarrow 2Cl^-(aq)$
Use the formula for standard cell potential.
The standard cell potential is given by the formula:
$E^\circ_{cell} = E^\circ_{red}(cathode) - E^\circ_{red}(anode)$
In this case, the cathode is Chlorine and the anode is Zinc.
$E^\circ_{cell} = E^\circ_{red}(Cl_2/Cl^-) - E^\circ_{red}(Zn^{2+}/Zn)$
Substitute the known values and solve for the standard reduction potential of Chlorine.
$2.1234\,V = E^\circ_{red}(Cl_2/Cl^-) - (-0.7634\,V)$ $2.1234\,V = E^\circ_{red}(Cl_2/Cl^-) + 0.7634\,V$
Now, isolate $E^\circ_{red}(Cl_2/Cl^-)$ :
$E^\circ_{red}(Cl_2/Cl^-) = 2.1234\,V - 0.7634\,V$ $E^\circ_{red}(Cl_2/Cl^-) = +1.3600\,V$
The standard potential of Chlorine is $\boxed{+1.3600\,V}$ .

Calculate the standard potential of Chlorine given the standard EMF of a Zinc-Chloride battery and the standard reduction potential of Zinc.