/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 77 At which electrode (anode/cathod... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 17: Problem 77

At which electrode (anode/cathode) do species gain electrons in a galvanic cell?

Short Answer

Expert verified
Species gain electrons at the cathode in a galvanic cell, as it is where the reduction process occurs.

Step by step solution

01

Understanding a Galvanic Cell

A galvanic cell is an electrochemical device that transforms the chemical energy of a spontaneous redox reaction into electrical energy. It consists of two different metal electrodes (anode and cathode) connected by a wire and an electrolyte solution. The two electrodes are also connected via a salt bridge, which allows the movement of ions to maintain electrical neutrality in each half-cell.
02

Redox Reactions and Electron Transfer

In a galvanic cell, a redox (reduction-oxidation) reaction occurs. During a redox reaction, one species loses electrons (oxidation) while another species gains electrons (reduction). The species that lose electrons are said to be oxidized, and the species that gain electrons are said to be reduced.
03

Role of Anode and Cathode in a Galvanic Cell

In a galvanic cell, each electrode serves a specific purpose related to the redox reaction. The anode is the electrode where the oxidation process occurs, meaning the species loses electrons and goes from a reduced form to an oxidized form. The cathode, on the other hand, is the electrode where the reduction process takes place, meaning the species gains electrons and goes from an oxidized form to a reduced form.
04

Answering the Given Question

According to the role of the electrodes in a galvanic cell, species gain electrons at the cathode as it is where the reduction process occurs.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91影视!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Elemental bromine can be prepared by treatment of seawater with chlorine gas. \(\mathrm{Cl}_{2}(g)+2 \mathrm{NaBr}(a q) \rightarrow \mathrm{Br}_{2}(a q)+2 \mathrm{NaCl}(a q)\) Identify the atoms that are oxidized and reduced, and specify the oxidizing and reducing agents.

Assign oxidation states to all of the atoms in each of the following: a. \(\mathrm{NaHSO}_{4}\) b. \(\mathrm{CaCO}_{3}\) c. \(\mathrm{KMnO}_{4}\) d. \(\mathrm{MnO}_{2}\)

What must be the sum of the oxidation states of all the atoms in a polyatomic ion?

In each of the following reactions, identify which element is oxidized and which is reduced. a. \(\mathrm{Zn}(s)+2 \mathrm{HCl}(a q) \rightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{H}_{2}(g)\) b. \(2 \operatorname{CuI}(s) \rightarrow \operatorname{CuI}_{2}(s)+\operatorname{Cu}(s)\) c. \(6 \mathrm{Fe}^{2+}(a q)+\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q)+14 \mathrm{H}^{+}(a q) \rightarrow\) \(6 \mathrm{Fe}^{3+}(a q)+2 \mathrm{Cr}^{3+}(a q)+7 \mathrm{H}_{2} \mathrm{O}(l)\)

What is a half-reaction? What does each of the two half-reactions that make up an overall process represent?
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Kinetics

Read Explanation

Ionic and Molecular Compounds

Read Explanation

The Earths Atmosphere

Read Explanation

Nuclear Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.