This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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Here's how to calculate the standard potential of Chlorine: Step 1: Identify the given values. The standard EMF of the Zinc-Chloride battery (E^_cell) is 2.1234\,V. The standard reduction potential of Zinc (E^_red(Zn^2+/Zn)) is -0.7634\,V. Step 2: 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) Zn^2+(aq) + 2e^- Cathode (reduction): Cl_2(g) + 2e^- 2Cl^-(aq) Step 3: Use the formula for standard cell potential. The standard cell potential is given by the formula: E^_cell = E^_red(cathode) - E^_red(anode) In this case, the cathode is Chlorine and the anode is Zinc. E^_cell = E^_red(Cl_2/Cl^-) - E^_red(Zn^2+/Zn) Step 4: Substitute the known values and solve for the standard reduction potential of Chlorine. 2.1234\,V = E^_red(Cl_2/Cl^-) - (-0.7634\,V) 2.1234\,V = E^_red(Cl_2/Cl^-) + 0.7634\,V Now, isolate E^_red(Cl_2/Cl^-): E^_red(Cl_2/Cl^-) = 2.1234\,V - 0.7634\,V E^_red(Cl_2/Cl^-) = +1.3600\,V The standard potential of Chlorine is +1.3600\,V. 3 done, 2 left today. You're making progress.