Specify which of the following are oxidation-reduction reactions, and identify the oxidizing agent, the reducing agent, the substance being oxidized, and the substance being reduced. a. \(\mathrm{Cu}(s)+2 \mathrm{Ag}^{+}(a q) \rightarrow 2 \mathrm{Ag}(s)+\mathrm{Cu}^{2+}(a q)\) b. \(\mathrm{HCl}(g)+\mathrm{NH}_{3}(g) \rightarrow \mathrm{NH}_{4} \mathrm{Cl}(s)\) c. \(\mathrm{SiCl}_{4}(l)+2 \mathrm{H}_{2} \mathrm{O}(l) \rightarrow 4 \mathrm{HCl}(a q)+\mathrm{SiO}_{2}(s)\) d. \(\mathrm{SiCl}_{4}(l)+2 \mathrm{Mg}(s) \rightarrow 2 \mathrm{MgCl}_{2}(s)+\mathrm{Si}(s)\) e. \(\mathrm{Al}(\mathrm{OH})_{4}^{-}(a q) \rightarrow \mathrm{AlO}_{2}^{-}(a q)+2 \mathrm{H}_{2} \mathrm{O}(i)\)

Step by step solution

01

Identify reaction type and changes in oxidation numbers

To see if the reaction is redox, we will calculate the oxidation numbers of elements before and after the reaction: Cu: 0 -> +2 Ag: +1 -> 0 Cu has increased in oxidation number (lost electrons) and thus, undergoes oxidation, turning to Cu²⁺(aq). Ag¹⁺(aq) has decreased in oxidation number (gained electrons) and thus undergoes reduction, turning to Ag(s).

02

Identify the oxidizing and reducing agents

The oxidizing agent is Ag¹⁺(aq), and the reducing agent is Cu(s). The substance being oxidized is Cu(s), and the substance being reduced is Ag¹⁺(aq). b.

03

Identify reaction type and changes in oxidation numbers

Checking the oxidation numbers for each element: Cl: -1 -> -1 H: +1 -> +1 N: -3 -> -3 No change in oxidation numbers, hence, this is not an oxidation-reduction reaction. c.

04

Identify reaction type and changes in oxidation numbers

Checking the oxidation numbers for each element: Si: +4 -> +4 Cl: -1 -> -1 O: -2 -> -2 H: +1 -> +1 No change in oxidation numbers, hence, this is not an oxidation-reduction reaction. d.

05

Identify reaction type and changes in oxidation numbers

Checking the oxidation numbers for each element: Si: +4 -> 0 Mg: 0 -> +2 Cl: -1 -> -1 Si has decreased in oxidation number (gained electrons) and thus undergoes reduction, turning to Si(s). Mg undergoes oxidation, losing electrons, and having its oxidation number increase to form Mg²⁺(aq).

06

Identify the oxidizing and reducing agents

The oxidizing agent is SiCl₄(l), and the reducing agent is Mg(s). The substance being oxidized is Mg(s), and the substance being reduced is SiCl₄(l). e.

07

Identify reaction type and changes in oxidation numbers

Checking the oxidation numbers for each element: Al: +3 -> +3 O: -2 -> -2 H: +1 -> +1 No change in oxidation numbers, hence, this is not an oxidation-reduction reaction. In conclusion, a and d are oxidation-reduction reactions, with the oxidizing agents being Ag¹⁺(aq) and SiCl₄(l), the reducing agents are Cu(s) and Mg(s), the substance being oxidized being Cu(s) and Mg(s), and the substance being reduced is Ag¹⁺(aq) and SiCl₄(l), respectively.

Unlock Step-by-Step Solutions & Ace Your Exams!

• Full Textbook Solutions

  Get detailed explanations and key concepts

• Unlimited Al creation

  Al flashcards, explanations, exams and more...

• Ads-free access

  To over 500 millions flashcards

• Money-back guarantee

  We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!