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Chapter 4: Problem 83

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. \(\mathrm{HCl}(g)+\mathrm{NH}_{3}(\mathrm{~g}) \rightarrow \mathrm{NH}_{4} \mathrm{Cl}(s)\) c. \(\mathrm{SiCl}_{4}(l)+2 \mathrm{H}_{2} \mathrm{O}(l) \rightarrow 4 \mathrm{HCl}(a q)+\mathrm{SiO}_{2}(s)\) d. \(\mathrm{SiCl}_{4}(l)+2 \mathrm{Mg}(s) \rightarrow 2 \mathrm{MgCl}_{2}(s)+\operatorname{Si}(s)\) e. \(\mathrm{Al}(\mathrm{OH})_{4}^{-}(a q) \rightarrow \mathrm{AlO}_{2}^{-}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l)\)

Short Answer

Expert verified
The redox reactions are: a. \(Cu(s)+2Ag^+(aq) \rightarrow 2Ag(s)+Cu^{2+}(aq)\): Oxidizing agent: \(Ag^+\), Reducing agent: \(Cu\), Substance being oxidized: \(Cu\), Substance being reduced: \(Ag^+\) d. \(SiCl_4(l)+2Mg(s) \rightarrow 2MgCl_2(s)+Si(s)\): Oxidizing agent: \(SiCl_4\), Reducing agent: \(Mg\), Substance being oxidized: \(Mg\), Substance being reduced: \(SiCl_4\)

Step by step solution

01

Oxidation numbers for reaction a

\(Cu(0), Ag^+(+1)\) for the reactants and \(Ag(0), Cu^{2+}(+2)\) for the products. #b.
02

Oxidation numbers for reaction b

\(H(+1), Cl(-1), N(-3), H(+1)\) for the reactants and \(N(-3), H(+1), Cl(-1)\) for the product. #c.
03

Oxidation numbers for reaction c

\(Si(+4), Cl(-1), H(+1), O(-2)\) for the reactants and \(H(+1), Cl(-1), Si(+4), O(-2)\) for the products. #d.
04

Oxidation numbers for reaction d

\(Si(+4), Cl(-1), Mg(0)\) for the reactants and \(Mg(+2), Cl(-1), Si(0)\) for the products. #e.
05

Oxidation numbers for reaction e

\(Al(+3), O(-2), H(+1)\) for the reactant and \(Al(+3), O(-2), H(+1)\) for the products. Step 2: Compare the oxidation states of reactants and products for each reaction Check if there is any change in the oxidation states between reactants and products in each reaction. #a.
06

Comparing oxidation states for reaction a

Cu goes from 0 to +2, and Ag goes from +1 to 0, indicating a redox reaction. #b.
07

Comparing oxidation states for reaction b

No change in oxidation states, thus it's not a redox reaction. #c.
08

Comparing oxidation states for reaction c

No change in oxidation states, thus it's not a redox reaction. #d.
09

Comparing oxidation states for reaction d

Si goes from +4 to 0, and Mg goes from 0 to +2, indicating a redox reaction. #e.
10

Comparing oxidation states for reaction e

No change in oxidation states, thus it's not a redox reaction. Step 3: Identify the redox agents and the substances being oxidized/reduced in each redox reaction #a.
11

Redox agents and substances for reaction a

Oxidizing agent: \(Ag^+\), Reducing agent: \(Cu\), Substance being oxidized: \(Cu\), Substance being reduced: \(Ag^+\) #d.
12

Redox agents and substances for reaction d

Oxidizing agent: \(SiCl_4\), Reducing agent: \(Mg\), Substance being oxidized: \(Mg\), Substance being reduced: \(SiCl_4\)

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Most popular questions from this chapter

A solution is prepared by dissolving \(10.8 \mathrm{~g}\) ammonium sulfate in enough water to make \(100.0 \mathrm{~mL}\) of stock solution. A \(10.00\) mL sample of this stock solution is added to \(50.00 \mathrm{~mL}\) of water. Calculate the concentration of ammonium ions and sulfate ions in the final solution.

The concentration of a certain sodium hydroxide solution was determined by using the solution to titrate a sample of potassium hydrogen phthalate (abbreviated as KHP). KHP is an acid with one acidic hydrogen and a molar mass of \(204.22 \mathrm{~g} / \mathrm{mol}\). In the titration, \(34.67 \mathrm{~mL}\) of the sodium hydroxide solution was required to react with \(0.1082\) g KHP. Calculate the molarity of the sodium hydroxide.

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A 230.-mL sample of a \(0.275 \mathrm{M} \mathrm{CaCl}_{2}\) solution is left on a hot plate overnight; the following morning, the solution is \(1.10 \mathrm{M}\). What volume of water evaporated from the \(0.275 \mathrm{M} \mathrm{CaCl}_{2}\) solution?

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