For a spontaneous reaction A1aq2 + B1aq2 → A-1aq2 + B+1aq2, answer the following questions: (a) If you made a voltaic cell out of this reaction, what half-reaction would be occurring at the cathode, and what half-reaction would be occurring at the anode?

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Identify the oxidation and reduction processes in the given reaction. Oxidation involves the loss of electrons, while reduction involves the gain of electrons.

Write the half-reaction for the oxidation process. In this reaction, A1aq2 is oxidized to A-1aq2, meaning it loses electrons.

Write the half-reaction for the reduction process. In this reaction, B1aq2 is reduced to B+1aq2, meaning it gains electrons.

Determine which half-reaction occurs at the cathode. In a voltaic cell, the cathode is where reduction takes place.

Determine which half-reaction occurs at the anode. In a voltaic cell, the anode is where oxidation takes place.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Voltaic Cell

A voltaic cell, also known as a galvanic cell, is an electrochemical cell that converts chemical energy from spontaneous redox reactions into electrical energy. It consists of two half-cells, each containing an electrode and an electrolyte. The flow of electrons from the anode to the cathode generates an electric current, making it essential to understand the roles of oxidation and reduction in this process.

Oxidation and Reduction

Oxidation and reduction are complementary processes in redox reactions. Oxidation involves the loss of electrons, while reduction involves the gain of electrons. In a voltaic cell, the anode is where oxidation occurs (loss of electrons), and the cathode is where reduction takes place (gain of electrons). Identifying which species is oxidized and which is reduced is crucial for determining the half-reactions at each electrode.

Half-Reactions

Half-reactions are the individual reactions that occur at the anode and cathode in an electrochemical cell. They represent the oxidation and reduction processes separately, allowing for a clearer understanding of electron transfer. In the context of the given reaction, identifying the correct half-reactions involves determining which species is oxidized and which is reduced, thus providing insight into the overall cell reaction.

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Redox Half Reactions Example

Related Practice

Textbook Question

The diagram that follows represents a molecular view of a process occurring at an electrode in a voltaic cell.

Textbook Question

Assume that you want to construct a voltaic cell that uses the following half-reactions: A2+1aq2 + 2 e- ¡ A1s2 Ered ° = -0.10 V B2+1aq2 + 2 e- ¡ B1s2 E°red = -1.10 V You begin with the incomplete cell pictured here in which the electrodes are immersed in water.

(a) What additions must you make to the cell for it to generate a standard emf?

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Textbook Question

Consider the following table of standard electrode potentials for a series of hypothetical reactions in an aqueous solution: reduction half-reaction E °(V) (c) Which substance(s) can oxidize C2+?

Textbook Question

Consider the following voltaic cell:

(c) What is the change in the cell voltage when the ion concentrations in the cathode half-cell are increased by a factor of 10?