Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 17: Q1P (page 427)

The figure shows the behavior of Ptand Ag cathodes at whichreduction ofH3O+toH2(g)occurs. Explain why the two curves arenot superimposed.

Current versus voltage forPtand Agelectrodes in O2 -free, aqueous H2SO4

Adjusted topH3.2.

Short Answer

Expert verified

The voltage of Ag(0.4751V) required to overcome the activation energy for a reaction at an electrode is higher than of Pt(0.0154V) electrode.

Step by step solution

01

Define Electrochemical cell:

  • Since oxidation always occurs at the cathode in an electrochemical cell, reduction occurs there.
02

To discern the graph:

  • According to the graph, and table 17-1, we can see that for reduction of H3O+ to H2 Ag electrode needs 0.5V more negative potential than the Pt electrode.

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

From the two standard additions of 50 pm Fe(III) in the figure, find the concentration of Fe(III) in the seawater. Estimate where the baseline should be drawn for each trace and measure the peak height from the baseline. Consider the volume to be constant for all three solutions.

(a) which voltage,V1orV2in the diagram is constant in controlled-potential electrolysis? Which are the working, auxiliary, and reference electrodes in the diagram?

(b) Explain how the Luggin capillary in Figure 17-4 measures the electric potential at the opening of the capillary.

17-17. The experiment in Figure 17 - 9 required 5.32mA for 864s for complete reaction of a5.00 - mLaliquot of unknown cyclohexene solution.

(a) How many moles of electrons passed through the cell?

(b) How many moles of cyclohexene reacted?

(c) What was the molarity of cyclohexene in the unknown?

A solution of Sn2+is to be electrolyzed to reduce the Sn2+to Sn(s). Calculate the cathode potential (versus S.H.E.) needed to reduce[Sn2+]to1.0×10-8Mif no concentration polarization occurs. What would be the potential versus S.C.E. instead of S.H.E? Would the potential be more positive or more negative if concentration polarization occurred?

Ions that react with Ag+can be determined electrogravimetrically by deposition on a silver working anode:

Ag(s)+X-→AgX(s)+e-

(a) What will be the final mass of a silver anode used to electrolyze 75.00 mL of 0.02380 M KSCN if the initial mass of the anode is 12.4638 g?

(b) At what electrolysis voltage (versus S.C.E.) will AgBr(s) be deposited from 0.10M Br? (Consider negligible current flow, so that there is no ohmic potential, concentration polarization, or overpotential.)

(c) Is it theoretically possible to separate 99.99% of0.10M Klfrom0.10MKBr by controlled-potential electrolysis?
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

Chemistry Branches

Read Explanation

Making Measurements

Read Explanation

Chemical Reactions

Read Explanation

Inorganic Chemistry

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.

Sign-up for free