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Chapter 21: Q21.3P (page 972)

Can one half-reaction in a redox process take place independently of the other? Explain

Short Answer

Expert verified

No, in a redox process, one half-reaction cannot occur on its own.

Step by step solution

01

Definition of redox reaction

Electrons are transferred from one chemical material to another in many chemical processes. The oxidation-reduction or Redox reaction is the name given to these electron transport reactions.

02

determining the half-reaction in a redox process

Half responses are incompatible with one another.

If one half of the reaction includes oxidation or electron loss, the other half must involve the reduction or electron gain.

The redox reaction is made up of both of these processes.

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Most popular questions from this chapter

A Voltaic cell consists of a metal $A / A^{+}$ electrode and a metal $B / B^{+}$ electrode, with the $A / A^{+}$ electrode negative. The initial $[A^{+}] / [B^{+}]$ is such thatrole="math" localid="1659592400010" $E_{cell}$ >role="math" localid="1659592428249" $E_{cell}^{o}$

(a) How dorole="math" localid="1659592855546" $[A^{+}]$ and $[B^{+}]$ change as the cell operates?

(b) How doesrole="math" localid="1659592922361" $E_{cell}$ change as the cell operates?

(c) What is role="math" localid="1659592941387" $[A^{+}] / [B^{+}]$ when $E_{cell}$ =role="math" localid="1659592990948" $E_{cell}^{o}$ ? Explain.

(d) Is it possible forrole="math" localid="1659593025964" $E_{cell}^{}$ to be less than $E_{cell}^{o}$ ? Explain

Consider the following general voltaic cell:

Identify the (a) anode, (b) cathode, (c) salt bridge, (d) electrode at which leave the cell, (e) electrode with a positive charge, and electrode that gains mass as the cell operates (assuming that a metal plates out).

A voltaic cell is constructed with a ${Cu/Cu}^{2 +}$ half-cell and an ${Ni/Ni}^{2 +}$ half-cell. The nickel electrode is negative.

(a) Write balanced half-reactions and the overall reaction.

(b) Diagram the cell, labeling electrodes with their charges and showing the directions of electron flow in the circuit and of cation and anion flow in the salt bridge

The overall cell reaction occurring in an alkaline battery is

${Zn(s) + MnO}_{2} {(s) +H}_{2} O(l) \to {ZnO(s) + Mn(OH)}_{2} (s)$

(a) How many moles of electrons flow per mole of reaction?

(b) If $4.50 g$ of zinc is oxidized, how many grams of manganese dioxide and of water are consumed?

(c) What is the total mass of reactants consumed in part (b)?

(d) How many coulombs are produced in part (b)?

(e) In practice, voltaic cells of a given capacity (coulombs) are heavier than the calculation in part (c) indicates. Explain.

Magnesium bars are connected electrically to underground iron pipes to serve as sacrificial anodes.

(a) Do electrons flow from the bar to the pipe or the reverse?

(b) A $12kgMg$ bar is attached to an iron pipe, and it takes $8.5 yr$ for the Mgto be consumed. What is the average current flowing between the Mgand the Feduring this period?

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