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Ch.20 - Electrochemistry
Tro - Chemistry: A Molecular Approach 6th Edition
Tro6th EditionChemistry: A Molecular ApproachISBN: 9780137832217Not the one you use?Change textbook
All textbooksTro 6th EditionCh.20 - ElectrochemistryProblem 61a
Chapter 20, Problem 61a

Determine whether or not each metal dissolves in 1 M HCl. For those metals that do dissolve, write a balanced redox reaction showing what happens when the metal dissolves. a. Cu

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1
Identify the reactivity of copper (Cu) with hydrochloric acid (HCl). Copper is less reactive than hydrogen and does not dissolve in HCl.
Understand that for a metal to dissolve in HCl, it must be able to displace hydrogen from the acid, forming hydrogen gas and a metal chloride.
Consult the activity series of metals, which ranks metals by their ability to displace hydrogen from acids. Copper is below hydrogen in the activity series.
Since copper is below hydrogen in the activity series, it does not react with 1 M HCl to produce hydrogen gas.
Conclude that copper does not dissolve in 1 M HCl, and therefore, no redox reaction occurs.

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Redox Reactions

Redox reactions involve the transfer of electrons between two species, leading to changes in oxidation states. In these reactions, one species is oxidized (loses electrons) while another is reduced (gains electrons). Understanding redox processes is crucial for predicting how metals will react with acids, such as HCl, and determining the products formed.

Metal Reactivity with Acids

The reactivity of metals with acids is determined by their position in the reactivity series. More reactive metals, like zinc and magnesium, readily dissolve in acids, displacing hydrogen ions and forming metal ions. In contrast, less reactive metals, such as copper, do not react significantly with dilute acids, which is essential for predicting whether a metal will dissolve in HCl.
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Balanced Chemical Equations

A balanced chemical equation represents a chemical reaction with equal numbers of each type of atom on both sides of the equation. Balancing is essential for accurately depicting the stoichiometry of the reaction, including the reactants and products. In the context of metal dissolution in HCl, writing a balanced equation helps illustrate the transformation of the metal and the generation of hydrogen gas.
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Related Practice
Textbook Question

Determine whether or not each metal dissolves in 1 M HNO3. For those metals that do dissolve, write a balanced redox reaction showing what happens when the metal dissolves. a. Ag

Textbook Question

Determine whether or not each redox reaction occurs spontaneously in the forward direction.

a. Ca2+(aq) + Zn(s) → Ca(s) + Zn2+(aq)

b. 2 Ag+(aq) + Ni(s) → 2 Ag(s) + Ni2+(aq)

c. Fe(s) + Mn2+(aq) → Fe2+(aq) + Mn(s)

d. 2 Al(s) + 3 Pb2+(aq) → 2 Al3+(aq) + 3 Pb(s)

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Which metal could you use to reduce Zn2+ ions but not Al3+ ions?

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Which metal can be oxidized with an Mn2+ solution but not with an Mg2+ solution?

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Calculate E°cell for each balanced redox reaction and determine if the reaction is spontaneous as written. b. MnO2(aq) + 4 H+(aq) + Zn(s) → Mn2+(aq) + 2H2O(l) + Zn2+(aq) c. Cl2(g) + 2 F–(aq) → F2(g) + 2 Cl–(aq)

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Textbook Question

Calculate E°cell for each balanced redox reaction and determine if the reaction is spontaneous as written. a. 2 Cu(s) + Mn2+(aq) → 2 Cu+(aq) + Mn(s)

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