a. Choose the balanced equation for the following half-reaction:2+Fe(s) → Fe²+ (aq)OFe(s) → Fe²+ (aq) — 2e¯© Fe(s) → Fe²+ (aq) + 3e¯OFe(s) → Fe²+ (aq) + 2e¯OFe(s) → Fe²+ (aq) + le¯b. Choose the balanced equation for the following half-reaction:2+Co3+(aq) → Co®+ (aq)2+)e– Co3+ (aq) → Co+ (aq)e +Co3+ (aq) → Co+(aq)3e +Co®+ (aq) → Co+(aq)2e +Co®+(aq) →Co+ (aq)3+2+c. Choose the balanced equation for the following half-reaction:Se² (aq) → Se(s)Se² (aq) → 2Se(s) + 2e¯2Se²- (aq) → Se(s) + 2e¯Se²- (aq) → Se(s) + e¯O Se- (aq) → Se(s) + 2e¯d. Choose the balanced equation for the following half-reaction:2+Fe²+ (aq) → Fe(s)2+De¯ — Fe²+ (aq) → Fe(s)2+3e¯ + Fe²+ (aq) → Fe(s)e¯¯ + Fe²+ (aq) → Fe(s)2e¯ + Fe²+ (aq) → Fe(s)

Answered: a. Choose the balanced equation for the…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Concept explainers

Question

a. Choose the balanced equation for the following half-reaction:
2+
Fe(s) → Fe²+ (aq)
OFe(s) → Fe²+ (aq) — 2e¯
© Fe(s) → Fe²+ (aq) + 3e¯
OFe(s) → Fe²+ (aq) + 2e¯
OFe(s) → Fe²+ (aq) + le¯
b. Choose the balanced equation for the following half-reaction:
2+
Co3+(aq) → Co®+ (aq)
2+
)e
– Co3+ (aq) → Co+ (aq)
e +Co3+ (aq) → Co+(aq)
3e +Co®+ (aq) → Co+(aq)
2e +Co®+(aq) →Co+ (aq)
3+
2+
c. Choose the balanced equation for the following half-reaction:
Se² (aq) → Se(s)
Se² (aq) → 2Se(s) + 2e¯
2Se²- (aq) → Se(s) + 2e¯
Se²- (aq) → Se(s) + e¯
O Se- (aq) → Se(s) + 2e¯
d. Choose the balanced equation for the following half-reaction:
2+
Fe²+ (aq) → Fe(s)
2+
De¯ — Fe²+ (aq) → Fe(s)
2+
3e¯ + Fe²+ (aq) → Fe(s)
e¯¯ + Fe²+ (aq) → Fe(s)
2e¯ + Fe²+ (aq) → Fe(s)

Expert Solution

Step 1

Oxidation reduction reaction (Redox reaction)

It can be defined as the chemical reaction in which simultaneously oxidation and reduction take place.

In this reaction one species is oxidized and another is reduced.

Oxidation : loss of electrons (oxidation number increases)

Reduction: gain of electrons (oxidation number decreases)

Oxidizing agent: oxidizing agent can be define as the substance which can cause the oxidation of another substance. It acts as an electron acceptor as a result it's oxidation state decreases.

Reducing agent: reducing agent can be define as the substances which can cause reduction of another substances. It acts as an electron donor as a result it's oxidation state increases.

When the reactant donates electrons during redox reaction it get Oxidised (oxidation number increased). But when the reactant accept electrons during redox reaction it get reduced (oxidation number decreased).

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions