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+?

Verified step by step guidance

insert step 1> Identify the reduction half-reaction for C^{2+} and note its standard electrode potential, E^\(\circ\).

insert step 2> Understand that a substance can oxidize C^{2+} if it has a higher standard electrode potential than the C^{2+}/C half-reaction.

insert step 3> Review the table of standard electrode potentials provided in the problem.

insert step 4> Compare the E^\(\circ\) values of other substances with the E^\(\circ\) value of the C^{2+}/C half-reaction.

insert step 5> Identify the substances with higher E^\(\circ\) values than C^{2+}/C, as these can oxidize C^{2+}.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above.

Video duration:

Was this helpful?

Key Concepts

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

Standard Electrode Potential

Standard electrode potential (E°) is a measure of the tendency of a chemical species to be reduced, expressed in volts. It indicates how easily a species can gain electrons in a half-reaction. A higher E° value means a greater ability to be reduced, while a lower E° indicates a stronger tendency to oxidize. Understanding these values is crucial for predicting the direction of redox reactions.

Oxidizing and Reducing Agents

In redox reactions, an oxidizing agent is a substance that gains electrons and is reduced, while a reducing agent loses electrons and is oxidized. To determine which substances can oxidize C2+, one must identify those with higher standard electrode potentials than C2+. This relationship is essential for predicting which species can facilitate the oxidation of another.

Half-Reaction Method

The half-reaction method involves separating oxidation and reduction processes to analyze redox reactions. Each half-reaction can be assigned a standard electrode potential, allowing for the comparison of different species. By using this method, one can determine the feasibility of reactions and identify which substances can act as oxidizers or reducers based on their respective potentials.

Recommended video:

Guided course

01:49

Method 1 of Radioactive Half-Life

Related Practice

Textbook Question

The electrodes in a silver oxide battery are silver oxide 1Ag2O2 and zinc (b) Which battery do you think has an energy density most similar to the silver oxide battery: a Li-ion battery, a nickel– cadmium battery, or a lead–acid battery? [Section 20.7]

431

views

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?

660

views