/*! 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 86 (a) What is an electrolytic cell... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 20: Problem 86

(a) What is an electrolytic cell? (b) The negative terminal of a voltage source is connected to an electrode of an electrolytic cell. Is the electrode the anode or the cathode of the cell? Explain. (c) The electrolysis of water is often done with a small amount of sulfuric acid added to the water. What is the role of the sulfuric acid?

Short Answer

Expert verified
(a) An electrolytic cell is a device that uses an electric current to drive chemical reactions, typically reduction-oxidation, at the electrodes through a process known as electrolysis. (b) The electrode connected to the negative terminal of a voltage source is the cathode of the electrolytic cell, where reduction occurs due to the gain of electrons. (c) Sulfuric acid, when added to water during electrolysis, serves as an electrolyte, enhancing the electrical conductivity of the solution and facilitating the flow of electric current for a more efficient process.

Step by step solution

01

(a) Definition of Electrolytic Cell

An electrolytic cell is a device in which an electric current is passed through a solution containing ions, causing a chemical reaction (typically reduction-oxidation) to occur at the electrodes. This process, known as electrolysis, can result in the deposition of a substance, the production of gases, or the dissociation of a solution.
02

(b) Identification of the Anode or Cathode

Since the negative terminal of a voltage source is connected to the electrode, this electrode is the cathode of the electrolytic cell. In an electrolytic cell, the cathode is where reduction occurs, meaning a gain of electrons. Electrons flow from the negative terminal of the voltage source to the cathode, allowing for the reduction reaction to take place at this electrode.
03

(c) Role of Sulfuric Acid in Water Electrolysis

The role of sulfuric acid in the electrolysis of water is to act as an electrolyte, or a substance that increases the electrical conductivity of the solution. This helps to facilitate the flow of electric current through the solution, making the electrolysis process more efficient. Since pure water has very low electrical conductivity, the addition of a small amount of sulfuric acid (H鈧係O鈧�) significantly improves the rate of electrolysis by providing a greater number of ions to carry the electric current.

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

A student designs an ammeter (a device that measures electrical current) that is based on the electrolysis of water into hydrogen and oxygen gases. When electrical current of unknown magnitude is run through the device for \(2.00 \mathrm{~min}, 12.3 \mathrm{~mL}\) of water-saturated \(\mathrm{H}_{2}(\mathrm{~g})\) is collected. The temperature of the system is \(25.5^{\circ} \mathrm{C}\), and the atmospheric pressure is 768 torr. What is the magnitude of the current in amperes?

Indicate whether each of the following statements is true or false: (a) If something is oxidized, it is formally losing electrons. (b) For the reaction \(\mathrm{Fe}^{3+}(a q)+\mathrm{Co}^{2+}(a q)-\cdots\) \(\mathrm{Fe}^{2+}(a q)+\mathrm{Co}^{3+}(a q), \mathrm{Fe}^{3+}(a q)\) is the reducing agent and \(\mathrm{Co}^{2+}(a q)\) is the oxidizing agent. (c) If there are no changes in the oxidation state of the reactants or products of a particular reaction, that reaction is not a redox reaction.

A \(1 M\) solution of \(\mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}\) is placed in a beaker with a strip of Cu metal. A \(1 M\) solution of \(\mathrm{SnSO}_{4}\) is placed in a second beaker with a strip of Sn metal. A salt bridge connects the two beakers, and wires to a voltmeter link the two metal electrodes. (a) Which electrode serves as the anode, and which as the cathode? (b) Which electrode gains mass and which loses mass as the cell reaction proceeds? (c) Write the equation for the overall cell reaction. (d) What is the emf generated by the cell under standard conditions?

During a period of discharge of a lead-acid battery, \(402 \mathrm{~g}\) of \(\mathrm{Pb}\) from the anode is converted into \(\mathrm{PbSO}_{4}(s) .\) What mass of \(\mathrm{PbO}_{2}(s)\) is reduced at the cathode during this same period?

Derive an equation that directly relates the standard emf of a redox reaction to its equilibrium constant.
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Making Measurements

Read Explanation

The Earths Atmosphere

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Reactions

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.