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Chapter 18: Problem 15

Define oxidation and reduction in terms of both change in oxidation number and electron loss or gain.

Short Answer

Expert verified
Oxidation and reduction can be defined in two ways: (1) Change in oxidation number: oxidation involves an increase in oxidation number, while reduction involves a decrease in oxidation number. (2) Electron loss or gain: oxidation is the loss of electrons, and reduction is the gain of electrons.

Step by step solution

01

Definition 1: Change in Oxidation Number

Oxidation and reduction reactions are chemical transformations that involve changes in the oxidation numbers of atoms. An oxidation reaction results in the increase of the oxidation number for an atom, while a reduction reaction leads to the decrease of the oxidation number.
02

Definition 2: Electron Loss or Gain

Oxidation and reduction reactions can also be described in terms of electron loss or gain. In electrochemistry, oxidation is a process in which an atom loses one or more electrons, and reduction is a process where an atom gains one or more electrons. Oxidation: Loss of electrons Reduction: Gain of electrons To summarize: Oxidation: 1. Increase in oxidation number 2. Loss of electrons Reduction: 1. Decrease in oxidation number 2. Gain of electrons

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Most popular questions from this chapter

A solution containing \(\mathrm{Pt}^{4+}\) is electrolyzed with a current of \(4.00 \mathrm{~A}\). How long will it take to plate out \(99 \%\) of the platinum in \(0.50 \mathrm{~L}\) of a \(0.010-M\) solution of \(\mathrm{Pt}^{4+}\) ?

Calculate \(\mathscr{E}^{\circ}\) values for the following cells. Which reactions are spontaneous as written (under standard conditions)? Balance the equations that are not already balanced. Standard reduction potentials are found in Table \(18.1 .\) a. \(\mathrm{H}_{2}(g) \longrightarrow \mathrm{H}^{+}(a q)+\mathrm{H}^{-}(a q)\) b. \(\mathrm{Au}^{3+}(a q)+\mathrm{Ag}(s) \longrightarrow \mathrm{Ag}^{+}(a q)+\mathrm{Au}(s)\)

Direct methanol fuel cells (DMFCs) have shown some promise as a viable option for providing "green" energy to small electrical devices. Calculate \(\mathscr{E}^{\circ}\) for the reaction that takes place in DMFCs: $$ \mathrm{CH}_{3} \mathrm{OH}(l)+3 / 2 \mathrm{O}_{2}(g) \longrightarrow \mathrm{CO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l) $$ Use values of \(\Delta G_{\mathrm{f}}^{\circ}\) from Appendix \(4 .\)

Balance the following oxidation-reduction reactions that occur in basic solution. a. \(\mathrm{Al}(s)+\mathrm{MnO}_{4}^{-}(a q) \rightarrow \mathrm{MnO}_{2}(s)+\mathrm{Al}(\mathrm{OH})_{4}^{-}(a q)\) b. \(\mathrm{Cl}_{2}(g) \rightarrow \mathrm{Cl}^{-}(a q)+\mathrm{OCl}^{-}(a q)\) c. \(\mathrm{NO}_{2}^{-}(a q)+\mathrm{Al}(s) \rightarrow \mathrm{NH}_{3}(g)+\mathrm{AlO}_{2}^{-}(a q)\)

The measurement of \(\mathrm{pH}\) using a glass electrode obeys the Nernst equation. The typical response of a pH meter at \(25.00^{\circ} \mathrm{C}\) is given by the equation $$ \mathscr{E}_{\text {meas }}=\mathscr{E}_{\text {ref }}+0.05916 \mathrm{pH} $$ where \(\mathscr{E}_{\text {ref }}\) contains the potential of the reference electrode and all other potentials that arise in the cell that are not related to the hydrogen ion concentration. Assume that \(\mathscr{E}_{\mathrm{ref}}=0.250 \mathrm{~V}\) and that \(\mathscr{B}_{\text {meas }}=0.480 \mathrm{~V}\). a. What is the uncertainty in the values of \(\mathrm{pH}\) and \(\left[\mathrm{H}^{+}\right]\) if the uncertainty in the measured potential is \(\pm 1 \mathrm{mV}\) \((\pm 0.001 \mathrm{~V}) ?\) b. To what precision must the potential be measured for the uncertainty in \(\mathrm{pH}\) to be \(\pm 0.02 \mathrm{pH}\) unit?
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