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Chapter 6: Problem 141

Which of the following is/are not redox reaction? a. \(\mathrm{Zn}+2 \mathrm{AgCN} \rightarrow 2 \mathrm{Ag}+\mathrm{Zn}(\mathrm{CN})_{2}\) b. \(\mathrm{Mg}(\mathrm{OH})_{2}+2 \mathrm{NH}_{4} \mathrm{Cl} \rightarrow\) \(\mathrm{MgCl}_{2}+2 \mathrm{NH}_{4} \mathrm{OH}\) c. \(\mathrm{NaCl}+\mathrm{KNO}_{3} \rightarrow \mathrm{NaNO}_{3}+\mathrm{KCl}\) d. \(\mathrm{CaC}_{2} \mathrm{O}_{4}+2 \mathrm{HCl} \rightarrow \mathrm{CaCl}_{2}+\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\)

Short Answer

Expert verified
Reactions (b), (c), and (d) are not redox reactions.

Step by step solution

01

Understanding Redox Reactions

A redox reaction involves the transfer of electrons between two species, resulting in a change in the oxidation states of the involved elements. To identify a redox reaction, we need to look for changes in the oxidation states of the elements.
02

Analyze Reaction (a)

For reaction (a) \( \mathrm{Zn} + 2 \mathrm{AgCN} \rightarrow 2 \mathrm{Ag} + \mathrm{Zn(CN)_2} \), check the oxidation states: Zn goes from 0 to +2, and Ag goes from +1 to 0. Since there's a change in oxidation states, this is a redox reaction.
03

Analyze Reaction (b)

For reaction (b) \( \mathrm{Mg(OH)}_2 + 2 \mathrm{NH}_4\mathrm{Cl} \rightarrow \mathrm{MgCl}_2 + 2 \mathrm{NH}_4\mathrm{OH} \), all involved elements retain their oxidation states throughout the reaction. Due to no change in oxidation states, this is not a redox reaction.
04

Analyze Reaction (c)

For reaction (c) \( \mathrm{NaCl} + \mathrm{KNO}_3 \rightarrow \mathrm{NaNO}_3 + \mathrm{KCl} \), the oxidation states of the elements remain unchanged, implying this is not a redox reaction, but rather a double displacement reaction.
05

Analyze Reaction (d)

For reaction (d) \( \mathrm{CaC}_2\mathrm{O}_4 + 2 \mathrm{HCl} \rightarrow \mathrm{CaCl}_2 + \mathrm{H}_2\mathrm{C}_2\mathrm{O}_4 \), there is no change in the oxidation states of the elements involved. Therefore, this is not a redox reaction.

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Key Concepts

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

Oxidation states
Oxidation states, often called oxidation numbers, are crucial in understanding redox reactions. They help us determine the electron flow in chemical reactions. An oxidation state indicates the degree of oxidation for an atom in a compound. By assigning these states, one can identify which element loses electrons and which one gains them.
In redox reactions, an increase in oxidation state means oxidation, implying loss of electrons. Conversely, a decrease indicates reduction, implying a gain of electrons. For instance, if an atom goes from an oxidation state of 0 to +2, as in the conversion of Zn to Zn in reaction (a), it has lost electrons and is oxidized.
  • To assign oxidation states, follow these general rules:
  • Elements in their elemental form, like O2 or Zn, have an oxidation state of 0.
  • For hydrogen, it's +1; for oxygen, it's -2 in most compounds.
  • The sum of oxidation states in a neutral compound is zero, whereas it's equal to the charge in ions.
By identifying changes in oxidation states, we can classify reactions as redox or not, such as discerning reaction (a) as a redox process and reaction (b) as not.
Electron transfer
Electron transfer is the hallmark of redox reactions, setting them apart from other types of chemical reactions. The term 'redox' itself is derived from reduction-oxidation processes, where electrons are shifted from one reactant to another. During this transfer, one substance gets oxidized, losing electrons, while another gets reduced, gaining those electrons.
Let's focus on reaction (a):
  • Zn loses electrons, going from an oxidation state of 0 to +2, indicating oxidation.
  • Ag+ reduces, as it gains electrons, transitioning from +1 to 0.
The electron movement results not only in changes in oxidation states but also provides the energy driving the reaction. The key takeaway is identifying which species donates electrons and which accepts them. Understanding this dynamic is critical for analyzing and balancing redox reactions, and it's this electron flow that distinguishes a redox reaction from others.
Double displacement reactions
Double displacement reactions, or metathesis reactions, differ fundamentally from redox reactions as they involve the exchange of ions between two reactants, forming new compounds but without any electron transfer. These reactions are typically characterized by swapping ions in aqueous solutions.
Consider reaction (c):
  • NaCl and KNO3 have their cation (positive ion) and anion (negative ion) parts switched, resulting in NaNO3 and KCl.
  • Throughout the process, the oxidation states remain unchanged, indicating no redox activity.
These reactions are essential in various processes, such as the precipitation of salts, neutralization reactions, and gas formation reactions. The stable nature of ion exchange in double displacement reactions means they don't involve changes in oxidation numbers, unlike in redox reactions where electron movement is a pivotal aspect.

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Most popular questions from this chapter

The standard reduction potentials of \(\mathrm{Zn}\) and Ag in water are \(\mathrm{Zn}^{2+}+2 \mathrm{e}^{-} \leftrightarrow \mathrm{Zn}\); \(\left(\mathrm{E}^{\circ}=-0.76 \mathrm{~V}\right)\) and \(\mathrm{Ag}^{+}+\mathrm{e}^{-} \leftrightarrow \mathrm{Ag}\) \(\left(\mathrm{E}^{\circ}=+0.80 \mathrm{~V}\right)\) at \(298 \mathrm{~K}\). Which of the following reaction is/are not feasible? a. \(\mathrm{Zn}^{2+}(\mathrm{aq})+\mathrm{Ag}^{+}(\mathrm{aq}) \rightarrow \mathrm{Zn}(\mathrm{s})+\mathrm{Ag}(\mathrm{s})\) b. \(\mathrm{Zn}^{2+}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s}) \rightarrow 2 \mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{Zn}(\mathrm{s})\) c. \(\mathrm{Zn}(\mathrm{s})+\mathrm{Ag}(\mathrm{s}) \rightarrow \mathrm{Zn}^{2+}(\mathrm{aq})+\mathrm{Ag}^{+}(\mathrm{aq})\) d. \(\mathrm{Zn}(\mathrm{s})+2 \mathrm{Ag}^{+}(\mathrm{aq}) \rightarrow \mathrm{Zn}^{2+}(\mathrm{aq})+2 \mathrm{Ag}\) (s)

The equilibrium constant of the reaction: \(\mathrm{Cu}(\mathrm{s})+2 \mathrm{Ag}^{+}(\mathrm{aq}) \rightarrow \mathrm{Cu}^{2+}(\mathrm{aq})+2 \mathrm{Ag}(\mathrm{s})\) \(\mathrm{E}^{\circ}=0.46 \mathrm{~V}\) at \(298 \mathrm{~K}\) is a. \(2.4 \times 10^{10}\) b. \(2.0 \times 10^{10}\) c. \(4.0 \times 10^{10}\) d. \(4.0 \times 10^{15}\)

Sodium fusion extract, obtained from aniline, on treatment with iron (II) sulphate and \(\mathrm{H}_{2} \mathrm{SO}_{4}\) in presence of air gives a Prussian blue precipitate. The blue colour is due to the formation of a. \(\mathrm{Fe}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]_{3}\) b. \(\mathrm{Fe}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]_{2}\) c. \(\mathrm{Fe}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]_{2}\) d. \(\mathrm{Fe}_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]_{3}\)

For the reduction of \(\mathrm{NO}_{3}^{-}\)ion in an aqueous solution, \(\mathrm{E}^{\circ}\) is \(+0.96 \mathrm{~V}\). Values of \(\mathrm{E}^{\circ}\) for some metal ions are given below. \(\mathrm{V}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightarrow \mathrm{V}\) \(\mathrm{E}^{\circ}=-1.19 \mathrm{~V}\) \(\mathrm{Fe}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \rightarrow \mathrm{Fe} \quad \mathrm{E}^{\circ}=-0.04 \mathrm{~V}\) \(\mathrm{Au}^{3+}(\mathrm{aq})+3 \mathrm{e}^{-} \rightarrow \mathrm{Au} \quad \mathrm{E}^{\circ}=+1.40 \mathrm{~V}\) \(\mathrm{Hg}^{2+}(\mathrm{aq})+2 \mathrm{e}^{-} \rightarrow \mathrm{Hg} \quad \mathrm{E}^{o}=+0.86 \mathrm{~V}\) The pair of metals that is/are oxidized by \(\mathrm{NO}_{3}^{-}\)in aqueous solution is/are a. \(\mathrm{V}\) and \(\mathrm{Hg}\) b. \(\mathrm{Hg}\) and \(\mathrm{Fe}\) c. \(\mathrm{Fe}\) and \(\mathrm{Au}\) d. Fe and \(\mathrm{V}\)

Consider the following standard oxidation potentials (at \(25^{\circ} \mathrm{C}\) ). \(\mathrm{Ag}\left|\mathrm{Ag}^{+}:-0.799 \mathrm{~V} ; \mathrm{Hg}\right| \mathrm{Hg}^{2+}:-0.789 \mathrm{~V} ; \mathrm{Mg} \mid \mathrm{Mg}^{2+}\) \(+2.37 \mathrm{~V} ; \mathrm{Mn} \mid \mathrm{Mn}^{2+}:+1.18 \mathrm{~V}\) \(\mathrm{Sn} \mid \mathrm{Sn}^{2+}: 0.136 \mathrm{~V}\) Which of the following statements is/are incorrect under standard conditions? (i) Sn can displace \(\mathrm{Mg}\) and \(\mathrm{Ag}\) from their solutions. (ii) Ag can displace \(\mathrm{Hg}\) and \(\mathrm{Mg}\) from their solutions. iii) Mn can displace \(\mathrm{Sn}, \mathrm{Hg}\) and \(\mathrm{Ag}\) from their solutions. iv) Mn can displace \(\mathrm{Sn}, \mathrm{Mg}\) and \(\mathrm{Hg}\) from their solutions. a. (i), (ii),(iii) b. (ii), (iii), (iv) c. (i), (ii), (iv) d. (i), (ii), (iii), (iv)
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