/*! 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} Q40E Explain what happens to battery ... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 17: Q40E (page 961)

Explain what happens to battery voltage as a battery is used, in terms of the Nernst equation.

Short Answer

Expert verified

According to the Nernst equation That is, when we switch on the battery, a chemical process begins and continues indefinitely until it finds equilibrium - the battery dies.

Step by step solution

01

Nernst equation:

  • The Nernst equation specifies the link between cell potential and standard potential, as well as the electrically active (electroactive) species' activities.
  • It connects the effective concentrations (activities) of cell reaction components to the standard cell potential.
02

Determine the voltage of a battery when it is in use:

  • In order to explain this, we need to remind ourselves of the Nernst equation

\(E({\rm{ cell }}) = E({\rm{ cell }},{\rm{ standard }}) - \frac{{0.0592V}}{n} \cdot \log Q\)

  • When the battery runs out, it means that its voltage becomes\(\;0\).
  • From the Nernst equation, we can conclude that this happens when

\(E({\rm{ cell }},{\rm{ standard }}) = \frac{{0.0592V}}{n} \cdot \log Q\)

  • If we know that

\(E({\rm{ cell }},{\rm{ standard }}) = \frac{{0.0592V}}{n} \cdot \log K\)

  • We can see that the cell voltage will become zero when the chemical reaction occurring in the battery reaches equilibrium.
  • That means that when we turn the battery on, a chemical reaction starts happening and it goes on, like any chemical reaction, until it reaches equilibrium.
  • And when it reaches equilibrium, we see from the Nernst equation that the \(E(cell)\) becomes zero, which means that the battery dies when the chemical reaction occurring inside reaches equilibrium.

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

The mass of three different metal electrodes, each from a different galvanic cell, were determined before andafter the current generated by the oxidation-reduction reaction in each cell was allowed to flow for a few minutes.The first metal electrode, given the label A, was found to have increased in mass; the second metal electrode, giventhe label B, did not change in mass; and the third metal electrode, given the label C, was found to have lost mass.

Make an educated guess as to which electrodes were active and which were inert electrodes, and which wereanode(s) and which were the cathode(s)

Identify the species that undergoes oxidation, the species that undergoes reduction, the oxidizing agent, and thereducing agent in each of the reactions of the previous problem.

\(\begin{array}{l}{\bf{(a) H_2O_2 + S}}{{\bf{n}}^{{\bf{2 + }}}} \to {\bf{H_2O + S}}{{\bf{n}}^{{\bf{4 + }}}}\\{\bf{(b) PbO_2 + Hg}} \to {\bf{Hg}}{{\bf{2}}^{{\bf{2 + }}}}{\bf{ + P}}{{\bf{b}}^{{\bf{2 + }}}}\\{\bf{(c) Al + Cr_2O}}{{\bf{7}}^{{\bf{2 - }}}} \to {\bf{A}}{{\bf{l}}^{{\bf{3 + }}}}{\bf{ + C}}{{\bf{r}}^{{\bf{3 + }}}}\end{array}\)

Determine the overall reaction and its standard cell potential at 25 掳C for the reaction involving the galvanic cell in which cadmium metal is oxidized to 1 M cadmium(II) ion and a half-cell consisting of an aluminum electrode

in 1 M aluminum nitrate solution. Is the reaction spontaneous at standard conditions?

If a sample of iron and a sample of zinc come into contact, the zinc corrodes but the iron does not. If a sample of iron comes into contact with a sample of copper, the iron corrodes but the copper does not. Explain this phenomenon.

For each reaction listed, determine its standard cell potential at 25oC and whether the reaction is spontaneous at standard conditions.

(a) \({\rm{Mg}}(s) + {\rm{N}}{{\rm{i}}^{2 + }}(aq) \to {\rm{M}}{{\rm{g}}^{2 + }}(aq) + {\rm{Ni}}(s)\)

(b) \(2{\rm{A}}{{\rm{g}}^ + }(aq) + {\rm{Cu}}(s) \to {\rm{C}}{{\rm{u}}^{2 + }}(aq) + 2{\rm{Ag}}(s)\)

(c) \({\rm{Mn}}(s) + {\rm{Sn}}{\left( {{\rm{N}}{{\rm{O}}_3}} \right)_2}(aq) \to {\mathop{\rm Mn}\nolimits} {\left( {{\rm{N}}{{\rm{O}}_3}} \right)_2}(aq) + {\mathop{\rm Sn}\nolimits} (s)\)

(d) \(3{\rm{Fe}}{\left( {{\rm{N}}{{\rm{O}}_3}} \right)_2}(aq) + {\rm{Au}}{\left( {{\rm{N}}{{\rm{O}}_3}} \right)_3}(aq) \to 3{\rm{Fe}}{\left( {{\rm{N}}{{\rm{O}}_3}} \right)_3}(aq) + {\rm{Au}}(s)\)
See all solutions

Recommended explanations on Chemistry Textbooks

Chemical Analysis

Read Explanation

Inorganic Chemistry

Read Explanation

Organic Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Chemical Reactions

Read Explanation

Making Measurements

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.