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Chapter 8: Problem 82

Given \(\mathrm{A}^{+} / \mathrm{A} \longrightarrow+0.34 \mathrm{~V}\) \(\mathrm{B}^{+} / \mathrm{B} \longrightarrow-1.66 \mathrm{~V}\) \(\mathbf{C}^{+} ; \mathbf{C} \longrightarrow+0.76 \mathrm{~V}\) \(\mathrm{D}^{+} / \mathrm{D} \longrightarrow-0.28 \mathrm{~V}\) The most reactive metal which displaces other metals from their salt solution is (1) \(\mathrm{C}\) (2) D (3) \(\mathrm{B}\) (4) \(\Lambda\)

Short Answer

Expert verified
The most reactive metal is B.

Step by step solution

01

Understand Reactivity Series

Reactivity series is determined by the standard electrode potential (E鈦�) values. Metals with lower (more negative) E鈦� values are more reactive and can displace metals with higher (more positive) E鈦� values from their salt solutions.
02

List Electrode Potentials

Given the E鈦� values: \(\text{A}^{+}/\text{A} \rightarrow +0.34 \text{ V}\) \(\text{B}^{+}/\text{B} \rightarrow -1.66 \text{ V}\) \(\text{C}^{+}/\text{C} \rightarrow +0.76 \text{ V}\) \(\text{D}^{+}/\text{D} \rightarrow -0.28 \text{ V}\)
03

Identify Most Negative Potential

Compare the E鈦� values. The most reactive metal will have the most negative E鈦� value. Reviewing the values: +0.34 V (A), -1.66 V (B), +0.76 V (C), -0.28 V (D), it is clear that \(\text{B}^{+}/\text{B} \rightarrow -1.66 \text{ V}\) is the most negative.
04

Determine the Most Reactive Metal

Based on the comparison of electrode potentials, the metal with the most negative E鈦� value is B. Therefore, B is the most reactive metal and will displace other metals from their salt solutions.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Reactivity Series
The reactivity series is a critical concept in chemistry that ranks metals based on their ability to displace other metals from their compounds. It is determined by their standard electrode potentials (E鈦�). Metals with lower (more negative) E鈦� values are considered more reactive. These metals can displace metals with higher (more positive) E鈦� values from their salt solutions. This means, if you have a metal with a very negative E鈦� value, it will trump a metal with a less negative E鈦� value in reactivity. Understanding the reactivity series helps predict how metals will behave during chemical reactions.
Standard Electrode Potential
Standard electrode potential (E鈦�) is a measure of the tendency of a chemical species to be reduced, and it is measured under standard conditions (298 K, 1 M concentration, and 1 atm pressure). It is often represented in volts (V). Each metal has a unique E鈦� value that indicates how easily it can gain electrons compared to the standard hydrogen electrode, which is set at 0 V.
The more negative the E鈦� value, the higher the tendency to lose electrons (oxidize). Conversely, a less negative or more positive E鈦� value indicates a higher tendency to gain electrons (reduce). The given values in the exercise are:
  • A: +0.34 V
  • B: -1.66 V
  • C: +0.76 V
  • D: -0.28 V
From these values, you can infer the reactivity of each metal, with B having the most negative value indicating the highest reactivity.
Displacement Reactions
Displacement reactions are reactions where a more reactive metal displaces a less reactive metal from its compound. These reactions are common in aqueous solutions of metal salts. For example, if you add a piece of metal to a solution containing ions of a less reactive metal, the more reactive metal will displace the ions of the less reactive metal, forming a new compound and releasing the less reactive metal.
In the exercise, B (with an E鈦� of -1.66 V) is the most reactive. Thus, B can displace A, C, and D from their salt solutions due to its higher reactivity. This is because B has the highest tendency to lose electrons (most negative E鈦�), which drives it to react more readily and take over the spot of less reactive metals.

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Most popular questions from this chapter

Which of the following is not a simple displacement reaction? (1) \(\mathrm{Mg}+\mathrm{FeC} 1_{3} \longrightarrow \mathrm{MgCl}_{2}+\mathrm{Fe}\) (2) \(\mathrm{Al}+\mathrm{NiCl}_{2} \longrightarrow \mathrm{A} \mathrm{Cl}_{3}+\mathrm{Ni}\) (3) \(\mathrm{Zn}+\mathrm{H}_{2} \mathrm{SO}_{4} \longrightarrow \mathrm{ZnSO}_{4}+\mathrm{H}_{2}\) (4) \(\mathrm{NaCl}+\mathrm{AgNO}_{3} \longrightarrow \mathrm{AgCl}+\mathrm{NaNO}_{3}\)

When zinc is kept in \(\mathrm{CuSO}_{4}\) solution copper gets precipitated because (1) Standard reduction potential of zinc is more than copper (2) Standard reduction potential of zinc is less than copper (3) Atomic number of zinc is larger than copper (4) Atomic number of zinc is lower than copper

\(2 \mathrm{KClO}_{3}+\mathrm{I}_{2} \rightarrow 2 \mathrm{~K} 1 \mathrm{O}_{3}+\mathrm{Cl}_{2}\) Which of the following statements is correct regarding the above reaction? (1) It is a simple displaccment but not a redox reaction (2) Chlorine is reduced by iodine (3) Chlorinc is oxidiscd by iodine (4) It is a metathesis reaction

In which of the following pairs the difference in the positive oxidation numbers of the underlined elements is the greatest? (1) \(\mathrm{PCl}_{3}, \mathrm{PCl}_{5}\) (2) \(\mathrm{NO}_{2}, \mathrm{~N}_{2} \mathrm{O}_{4}\) (3) \(\mathrm{SO}_{2}, \mathrm{SO}_{3}\) (4) \(\mathrm{CO}_{2}, \mathrm{C}_{3} \mathrm{O}_{2}\)

A metal having negative reduction potential when dipped in the solution of its own jons has a tendency to (1) To pass into solution (2) To be deposited from the solution (3) To become clectrically positive (4) To remain neutral
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