1. Sodium can be extracted by heating naturally occurring salt until it is molten. An electrochemical process is then used to extract the sodium. Cl2 is produced at the anode, and Na is collected at the cathode. A standard reduction potential graph for the reaction is shown below.

(A and B are negative with A being closer to 0.)

a. Write the half-reactions that occur at the anode and the cathode. Identify each as either oxidation or reduction. (4 points)

b. Based on these half-reactions, determine the standard electrode potential levels that should be placed at points A and B on the graph. (2 points)

c. Use the graph to determine Eºcell . (2 points)

d. Based on the graph, is the process shown in the figure an example of a galvanic reaction or an electrolytic reaction? Explain. (2 points)

a. The half-reaction at the anode is 2Cl⁻ → Cl₂ + 2e⁻, which is an oxidation reaction. The half-reaction at the cathode is Na⁺ + e⁻ → Na, which is a reduction reaction.

b. Point A on the graph represents the half-reaction at the anode, which is the oxidation reaction. Since A is closer to 0, it has a higher standard electrode potential. Point B on the graph represents the half-reaction at the cathode, which is the reduction reaction. B is negative, indicating a lower standard electrode potential.

c. To determine Eºcell, subtract the value at B (reduction) from the value at A (oxidation). Eºcell = Eº(B) - Eº(A).

d. Based on the graph, the process shown is an electrolytic reaction. This is because the standard reduction potential values at the anode and cathode are different, indicating the need for an external power source to drive the reaction.

a. The half-reaction that occurs at the anode is the oxidation of chloride ions (Cl-) to chlorine gas (Cl2):

2Cl- -> Cl2 + 2e-

This is an oxidation reaction.

The half-reaction that occurs at the cathode is the reduction of sodium ions (Na+) to sodium metal (Na):

2Na+ + 2e- -> 2Na

This is a reduction reaction.

b. Point A on the graph should represent the standard electrode potential for the half-reaction at the anode, which is the oxidation of chloride ions to chlorine gas. Since A is closer to 0, it has a lower standard electrode potential.

Point B on the graph should represent the standard electrode potential for the half-reaction at the cathode, which is the reduction of sodium ions to sodium metal. Since B is negative and further from 0, it has a higher standard electrode potential.

c. To determine Eºcell , we need to find the difference between the standard electrode potentials at points A and B on the graph.

Since A is closer to 0, its standard electrode potential is lower. Let's assume it is -0.5 V.

Since B is further from 0, its standard electrode potential is higher. Let's assume it is -1.0 V.

Eºcell = Eºcathode - Eºanode = (-1.0 V) - (-0.5 V) = -0.5 V

Therefore, Eºcell is -0.5 V.

d. The process shown in the figure is an example of an electrolytic reaction. This is because a voltage source is required to drive the electrochemical process. In this case, the electrochemical process involves the electrolysis of molten salt to extract sodium.

a. The half-reaction that occurs at the anode is the oxidation reaction, where Cl- ions lose electrons and are converted into Cl2 gas. The half-reaction can be written as:

2Cl- -> Cl2 + 2e-

The half-reaction that occurs at the cathode is the reduction reaction, where Na+ ions gain electrons and are converted into metallic sodium. The half-reaction can be written as:

2Na+ + 2e- -> 2Na

b. To determine the standard electrode potential levels at points A and B on the graph, we need to identify the half-reaction with the higher reduction potential (more positive value) and assign it to point B. The half-reaction with the lower reduction potential (less positive value) will be assigned to point A.

In this case, the reduction reaction of sodium (Na+) has a more positive reduction potential, so it should be assigned to point B. The oxidation reaction of chloride (Cl-) has a less positive reduction potential, so it should be assigned to point A.

c. To determine Eºcell from the graph, we need to find the difference in the reduction potentials between points A and B. The difference in potential is given by the vertical distance between the two points.

d. The process shown in the figure is an example of an electrolytic reaction. In an electrolytic reaction, an external potential difference is applied to drive the reaction and produce the desired products, in this case, sodium (Na) and chlorine gas (Cl2). This is different from a galvanic reaction, where the redox reaction occurs spontaneously without the need for an external power source.

I can do a but not b,c,d. No diagram.