Sketch the galvanic cells based on the following overall...

Sketch the galvanic cells based on the following overall reactions. Show the direction of electron flow, the direction of ion migration through the salt bridge, and identify the cathode and anode. Give the overall balanced equation. Assume that all concentrations are $1.0 M$ and that all partial pressures are $1.0 \mathrm{~atm}$. a. $\mathrm{IO}_{3}^{-}(a q)+\mathrm{Fe}^{2+}(a q) \rightleftharpoons \mathrm{Fe}^{3+}(a q)+\mathrm{I}_{2}(a q)$ b. $\mathrm{Zn}(s)+\mathrm{Ag}^{+}(a q) \rightleftharpoons \mathrm{Zn}^{2+}(a q)+\mathrm{Ag}(s)$

Sketch the galvanic cells based on the following overall reactions. Show the direction of electron flow, the direction of ion migration through the salt bridge, and identify the cathode and anode. Give the overall balanced equation. Assume that all concentrations are $1.0 M$ and that all partial pressures are $1.0 \mathrm{~atm}$.
a. $\mathrm{IO}_{3}^{-}(a q)+\mathrm{Fe}^{2+}(a q) \rightleftharpoons \mathrm{Fe}^{3+}(a q)+\mathrm{I}_{2}(a q)$
b. $\mathrm{Zn}(s)+\mathrm{Ag}^{+}(a q) \rightleftharpoons \mathrm{Zn}^{2+}(a q)+\mathrm{Ag}(s)$

Key Concepts

Overall Balanced Redox Equation

Combining the oxidation and reduction half-reactions, after ensuring that the electron transfer is balanced, results in the overall balanced redox equation. This equation represents the net chemical change occurring in the galvanic cell, providing insight into the stoichiometry and the flow of charge that underlies cell operation.

Galvanic Cell

A galvanic cell is an electrochemical cell that harnesses the energy released from a spontaneous redox reaction to generate electrical energy. It consists of two separate half-cells connected by an external circuit and a salt bridge or porous membrane that maintains charge neutrality. The overall operation of the cell is predicated on the conversion of chemical energy to electrical energy through redox reactions at the electrodes.

Oxidation and Reduction Half-Reactions

In every redox reaction, oxidation refers to the loss of electrons while reduction refers to the gain of electrons. These processes occur separately in two half-cells: the electrode where oxidation occurs is called the anode, and the electrode where reduction occurs is called the cathode. Writing the half-reactions helps in the systematic balancing of the overall reaction by ensuring that the electrons lost are equal to the electrons gained.

Electron Flow in Electrochemical Cells

In a galvanic cell, electrons move from the anode, where oxidation takes place, to the cathode, where reduction occurs. This directional electron flow through the external circuit is the primary mechanism by which the cell produces an electric current. Understanding electron flow is essential for proper cell design and for predicting cell behavior under various conditions.

Salt Bridge and Ion Migration

The salt bridge is a critical component in a galvanic cell that allows the migration of ions between the two half-cells, thereby maintaining electrical neutrality as the redox reaction proceeds. Positive ions typically migrate toward the cathode compartment while negative ions move toward the anode compartment, balancing the buildup of charge that occurs due to the transfer of electrons.

Electrode Identification (Anode and Cathode)

The identification of the anode and cathode is based on the redox behavior of the constituents in the half-cells. The anode is where oxidation occurs and electrons are produced, while the cathode is where reduction takes place and electrons are consumed. Recognizing which electrode serves as the anode or the cathode is essential for correctly sketching the cell diagram and predicting the direction of electron flow.

Transcript

00:01 First, we need to draw the generic electrochemical cell, so we can then identify the direction of which electrons flow.

00:11 The two half -reactions that comprise the overall reaction are fe3 -plus, going to fe2 -plus, and then if we look closely, we will find this half -reaction for the iodate and the iodine.

00:25 If we look at the reduction potentials, and we see that the greatest reduction potential is the iodate going to the iodine.

00:32 Dine, so that reduction will occur, and that will comprise the cathode compartment.

00:37 The other half reaction will be forced to be flipped and serve as the anode.

00:41 It will occur in the opposite direction, and that will then be the anode compartment.

00:46 We need to have platinum in both cases to carry the electrons, and the electrons will travel from the anode to the cathode.

00:54 This question also asks us to identify the movement of the ions in the salt bridge.

01:00 If we have electrons leaving this anode compartment, then the anode compartment is going to become more and more positively charged.

01:08 So to neutralize that positive charge, we need to have the anions in the salt bridge travel towards the anode.

01:14 And as the electrons reach the cathode, the cathode compartment will become negatively charged.

01:20 So we need to have the cations go towards the cathode compartment in order to neutralize that charge.

01:26 The cell potential then is simply going to be the cathode compartment...

Please give Ace some feedback