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Chapter 10: Problem 104

The spontaneous redox reaction \(\mathrm{Mn}+\mathrm{Cd}^{2+} \rightarrow \mathrm{Mn}^{2+}+\mathrm{Cd}\) takes place in a battery. (a) What is the oxidizing agent? (b) What is the reducing agent? (c) Which metal is the cathode? (d) Which metal is the anode?

Short Answer

Expert verified
(a) The oxidizing agent is Cd^2+. (b) The reducing agent is Mn. (c) Cd is the cathode. (d) Mn is the anode.

Step by step solution

01

Identify the oxidation states of the elements in the reaction

To determine the oxidation states of the elements in the reaction, we can use the following rule: The sum of the oxidation states of all the elements in a neutral compound is zero. In the given reaction: Mn + Cd^2+ → Mn^2+ + Cd Oxidation state of Mn in Mn = 0 (since it is in its elemental form) Oxidation state of Cd^2+ = +2 (as given) Oxidation state of Mn^2+ = +2 (as given) Oxidation state of Cd in Cd = 0 (since it is in its elemental form) Now that we have the oxidation states of all the elements involved, we can move on to the next step.
02

Identify the oxidizing and reducing agents

An oxidizing agent is a substance that accepts electrons from another substance, causing that other substance to be oxidized. Conversely, a reducing agent is a substance that donates electrons to another substance, causing that other substance to be reduced. In our reaction, Mn is going from an oxidation state of 0 to +2, indicating it is losing 2 electrons and is being oxidized. On the other hand, Cd^2+ is going from an oxidation state of +2 to 0, indicating it is gaining 2 electrons and is being reduced. (a) The oxidizing agent in this reaction is Cd^2+. (b) The reducing agent in this reaction is Mn.
03

Identify the cathode and anode

In a redox reaction, the cathode is the electrode where reduction occurs, and the anode is the electrode where oxidation occurs. Since Cd^2+ is reduced, it will gain electrons at the cathode. Therefore, (c) Cd is the cathode. Since Mn is oxidized, it will lose electrons at the anode. Therefore, (d) Mn is the anode.

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Most popular questions from this chapter

Under what circumstances does fluorine not have an oxidation state of \(-1 ?\)

Hydrogen peroxide \(\left(\mathrm{H}_{2} \mathrm{O}_{2}\right)\) can be made to decompose into water and oxygen as shown below. (The hydrogen peroxide in the beaker is decomposing to give a cloud of water vapor. Oxygen gas is also being produced.) Is this a redox reaction? If so, prove it.

What happens when you place an active metal in a solution of ions of a less active metal?

Indicate whether each reaction is a redox reaction. If it is, which atom gets oxidized and which atom gets reduced? Consult the shortcut rules. \(\mathrm{Ca}+2 \mathrm{H}^{+} \rightarrow \mathrm{Ca}^{2+}+\mathrm{H}_{2}\)

Suppose the shortcut rules can determine the oxidation state of every atom in a compound except one. How can you find the oxidation state of the remaining atom?
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