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Chapter 21: Q21.2P (page 972)

Why must an electrochemical process involve a redox reaction?

Short Answer

Expert verified

Because electrons require a source and recipient (in the form of reducing and oxidizing substances) for an electrochemical reaction to occur, redox reactions are used in electrochemical processes.

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 Why an electrochemical process involves a redox reaction

Because electrons are transported from one atom to another during redox reactions, electrochemical processes entail a redox reaction. For an electrochemical reaction to occur, electrons must have a source and a recipient (in the form of reducing and oxidizing substances).

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Most popular questions from this chapter

Compare and contrast a voltaic cell and an electrolytic cell with respect to each of the following:

(a) Sign of the free energy change

(b) Nature of the half-reaction at the anode

(c) Nature of the half-reaction at the cathode

(d) Charge on the electrode labelled 鈥渁node鈥�

(e) Electrode from which electrons leave the cell

When a piece of metal A is placed in a solution containing ions of metal , metal plates out on the piece of A.

(a) Which metal is being oxidized?

(b) Which metal is being displaced?

(c) Which metal would you use as the anode in a voltaic cell incorporating these two metals?

(d) If bubbles of H2form when is placed in acid, will they form if A is placed in acid? Explain

Electrodes used in electrocardiography are disposable, and many incorporate silvers. The metal is deposited in a thin layer on a small plastic 鈥渂utton,鈥� and then some is converted to AgCl:

Ag(s) + Cl-(aq)鈬�AgCl(s) +e-

(a) If the surface area of the button is2.0 cm2and the thickness of the silver layer is7.5脳10-6m, calculate the volume (incm3) ofused in one electrode.

(b) The density of silver metal is 10.5 g/cm3. How many grams of silver are used per electrode?

(c) Ifis plated on the button from an Ag+solution with a current of12.0 mA, how many minutes does the plating take?

(d) If bulk silver costs$ 13.00per troy ounce (31.10 g), what is the cost (in cents) of the silver in one disposable electrode?

In a concentration cell, is the more concentrated electrolyte in the cathode or the anode compartment? Explain.

Balance the following skeleton reactions and identify the oxidizing and reducing agents:

(a) SO32 -(aq) + Cl2(g)鈫�SO42 -(aq) + Cl-(aq) [basic](b) Fe(CN)63 -(aq) + Re(s)鈫�Fe(CN)64 -(aq) + ReO4-(aq) [basic]

(C) MnO4-(aq) + HCOOH(aq)鈫�Mn2 +(aq) + CO2(g)
See all solutions

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