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Ch.20 - Electrochemistry
Tro - Chemistry: A Molecular Approach 6th Edition
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Tutti i libri di testoTro 6th EditionCh.20 - ElectrochemistryProblema 61a
Capitolo 20, Problema 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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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.

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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.
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Identifying Redox Reactions

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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From Metal and Acid

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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Balancing Chemical Equations
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Domanda del libro di testo

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

Domanda del libro di testo

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. a. 2 Cu(s) + Mn2+(aq) → 2 Cu+(aq) + Mn(s)

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Domanda del libro di testo

Determine whether or not each metal dissolves in 1 M HNO3. For those metals that do dissolve, write a balanced redox equation for the reaction that occurs. a. Au