Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 7: Problem 40

Identify the false statement among the following: (a) Oxidation takes place at positive electrode in electrolytic cell, whereas reduction at negative electrode in voltaic cell. (b) Deposition of metals takes place in both electrolytic and galvanic cells. (c) Direction of flow of current is from cathode to anode in electrolytic cell. (d) Both (a) and (b)

Short Answer

Expert verified
a) Oxidation occurs at the anode, and reduction occurs at the cathode. b) Deposition of metals can occur on the electrodes. c) Direction of flow of current is from cathode to anode. d) Both (a) and (b) are false. Answer: c) Direction of flow of current is from cathode to anode.

Step by step solution

01

Statement (a) Analysis

Oxidation occurs when a substance loses electrons, and reduction occurs when a substance gains electrons. In an electrolytic cell, the positive electrode (anode) is where oxidation takes place, and the negative electrode (cathode) is where reduction takes place. In a voltaic (galvanic) cell, the reverse is true: oxidation takes place at the negative electrode (anode), and reduction takes place at the positive electrode (cathode). Thus, statement (a) is true.
02

Statement (b) Analysis

In both electrolytic and galvanic cells, deposition of metals can occur. In an electrolytic cell, deposition of metals occurs during the reduction process at the cathode. In a voltaic cell, the deposition can occur at the cathode as well during the reduction process. Therefore, statement (b) is also true.
03

Statement (c) Analysis

The direction of flow of current is defined as the direction in which positive charge moves. In an electrolytic cell, positive ions move towards the cathode (negative electrode) to be reduced, and negative ions move towards the anode (positive electrode) to be oxidized. Therefore, the direction of flow of current is from the positive electrode (anode) to the negative electrode (cathode). Hence, statement (c) is false.
04

Statement (d) Analysis

Statement (d) claims that both (a) and (b) are false. We have already explained that statement (a) is true and statement (b) is true, so statement (d) is also false.
05

Conclusion

Among the given statements, the false statement is (c) Direction of flow of current is from cathode to anode in the electrolytic cell.

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

Which of the following electrolytes exhibits maximum conductivity? (a) \(1 \mathrm{M} \mathrm{NaCl}\) (b) \(1 \mathrm{M} \mathrm{KCl}\) (c) \(1 \mathrm{M} \mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) (d) \(1 \mathrm{M} \mathrm{Al}_{2}\left(\mathrm{SO}_{4}\right)_{3}\)

Fill in the blanks. In cell representation, oxidation half-cell is represented on the ___ .

Negative sign in the standard electrode potential indicates (a) greater ease of oxidation compared to that of hydrogen (b) greater ease of reduction compared to that of hydrogen (c) lesser ease of oxidation compared to that of hydrogen (d) none of the above

Identify the set of metals which require same amount of charge for the deposition of one mole of metals: (a) \(\mathrm{Na}, \mathrm{Ag}, \mathrm{Al}\) (b) \(\mathrm{Zn}, \mathrm{Cu}, \mathrm{Ag}\) (c) \(\mathrm{Al}, \mathrm{Cu}, \mathrm{Zn}\) (d) \(\mathrm{Mg}, \mathrm{Zn}, \mathrm{Cd}\)

Pairs of electrodes and their corresponding standard electrode potentials are given. Arrange the cells constructed by these electrodes in increasing order of emf values. (1) Electrode \(\rightarrow \mathrm{A}, \mathrm{E}^{\circ}=-2.92 \mathrm{~V}\) and Electrode \(\rightarrow\) \(\mathrm{B}, \mathrm{E}^{\circ}=-2.71 \mathrm{~V}\) (2) Electrode \(\rightarrow \mathrm{C}, \mathrm{E}^{\circ}=-0.760 \mathrm{~V}\) and Electrode \(\rightarrow\) \(\mathrm{D}, \mathrm{E}^{\circ}=-0.44 \mathrm{~V}\) (3) Electrode \(\rightarrow \mathrm{B}, \mathrm{E}^{\circ}=-2.71 \mathrm{~V}\) and Electrode \(\rightarrow\) \(\mathrm{D}, \mathrm{E}^{\circ}=-0.44 \mathrm{~V}\) (4) Electrode \(\rightarrow \mathrm{A}, \mathrm{E}^{\circ}=-2.92 \mathrm{~V}\) and Electrode \(\rightarrow\) \(\mathrm{C}, \mathrm{E}^{\circ}=-0.76 \mathrm{~V}\) (a) 2143 (b) 1243 (c) 2413 (d) 2431
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Read Explanation

Physical Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Making Measurements

Read Explanation

The Earths Atmosphere

Read Explanation

Organic 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.

Sign-up for free