Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 20: Problem 27

Indicate whether each statement is true or false: (a) The cathode is the electrode at which oxidation takes place. (b) A galvanic cell is another name for a voltaic cell. (c) Electrons flow spontaneously from anode to cathode in a voltaic cell.

Short Answer

Expert verified
(a) False, as cathode is the electrode where reduction occurs, not oxidation. (b) True, since galvanic cells and voltaic cells are the same and the terms can be used interchangeably. (c) True, as electrons flow spontaneously from the anode to the cathode in a voltaic cell due to the redox reaction.

Step by step solution

01

Understanding Cathode and Oxidation

In electrochemical cells, cathode is the electrode where reduction takes place, and anode is the electrode where oxidation occurs. Oxidation involves the loss of electrons, while reduction involves the gain of electrons. Now let's analyze the statement: (a) The cathode is the electrode at which oxidation takes place.
02

Verifying Statement (a)

Since we know that the cathode is where reduction occurs and not oxidation, the statement is false. #Statement b#
03

Understanding Galvanic Cells and Voltaic Cells

Galvanic cells and voltaic cells are names for the same type of electrochemical cell. These cells convert chemical energy into electrical energy through spontaneous redox reactions. The terms are used interchangeably. Now let's analyze the statement: (b) A galvanic cell is another name for a voltaic cell.
04

Verifying Statement (b)

Since galvanic cells and voltaic cells are the same and can be used interchangeably, the statement is true. #Statement c#
05

Understanding Electron Flow in Voltaic Cells

In a voltaic cell, the anode is where oxidation occurs, and the cathode is where reduction occurs. During the redox reaction, electrons are released at the anode (oxidation) and flow to the cathode (reduction) through an external circuit, generating an electric current. Now let's analyze the statement: (c) Electrons flow spontaneously from anode to cathode in a voltaic cell.
06

Verifying Statement (c)

Since electrons do flow spontaneously from the anode to the cathode in a voltaic cell due to the redox reaction, the statement is true.

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.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

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 voltaic cell utilizes the following reaction: $$ 4 \mathrm{Fe}^{2+}(a q)+\mathrm{O}_{2}(g)+4 \mathrm{H}^{+}(a q) \longrightarrow 4 \mathrm{Fe}^{3+}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l) $$ (a) What is the emf of this cell under standard conditions? (b) What is the emf of this cell when \(\left[\mathrm{Fe}^{2+}\right]=1.3 \mathrm{M},\left[\mathrm{Fe}^{3+}\right]=\) \(0.010 \mathrm{M}, P_{\mathrm{O}_{2}}=0.50 \mathrm{atm}\) , and the \(\mathrm{pH}\) of the solution in the cathode half-cell is 3.50\(?\)

Mercuric oxide dry-cell batteries are often used where a flat discharge voltage and long life are required, such as in watches and cameras. The two half-cell reactions that occur in the battery are $$ \begin{array}{l}{\mathrm{HgO}(s)+\mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{e}^{-} \longrightarrow \mathrm{Hg}(l)+2 \mathrm{OH}^{-}(a q)} \\ {\mathrm{Zn}(s)+2 \mathrm{OH}^{-}(a q) \longrightarrow \mathrm{znO}(s)+\mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{e}^{-}}\end{array} $$ (a) Write the overall cell reaction. (b) The value of \(E_{\text { red }}^{\circ}\) for the cathode reaction is \(+0.098 \mathrm{V}\) . The overall cell potential is \(+1.35 \mathrm{V}\) . Assuming that both half-cells operate under standard conditions, what is the standard reduction potential for the anode reaction? (c) Why is the potential of the anode reaction different than would be expected if the reaction occurred in an acidic medium?

A voltaic cell is constructed with two silver-silver chloride electrodes, each of which is based on the following half-reaction: $$ \operatorname{AgCl}(s)+\mathrm{e}^{-} \longrightarrow \mathrm{Ag}(s)+\mathrm{Cl}^{-}(a q) $$ The two half-cells have \(\left[\mathrm{Cl}^{-}\right]=0.0150 \mathrm{M}\) and \(\left[\mathrm{Cl}^{-}\right]=\) \(2.55 \mathrm{M},\) respectively. (a) Which electrode is the cathode of the cell? (b) What is the standard emf of the cell? (c) What is the cell emf for the concentrations given? (d) For each electrode, predict whether \(\left[\mathrm{Cl}^{-}\right]\) will increase, decrease, or stay the same as the cell operates.

Indicate whether each of the following statements is true or false: (a) If something is reduced, it is formally losing electrons. (b) A reducing agent gets oxidized as it reacts. (c) An oxidizing agent is needed to convert CO into \(\mathrm{CO}_{2}\) .

(a) What is the definition of the volt? (b) Do all voltaic cells produce a positive cell potential?
See all solutions

Recommended explanations on Chemistry Textbooks

The Earths Atmosphere

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Physical Chemistry

Read Explanation

Kinetics

Read Explanation

Chemical Reactions

Read Explanation

Chemical Analysis

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.

Sign-up for free