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Chapter 4: Q4.88P (page 181)

Balance each of the following redox reactions and classify it as a combination, decomposition, or displacement reaction:
$(a) H I (g) 鈫� H_{2} (g) + I_{2} (g)$
$(b) Z n (s) + A g N O_{3} (a q) 鈫� Z n {(N O_{3})}_{2} (a q) + A g (s)$
$(c) N O (g) + O_{2} (g) 鈫� N_{2} O_{4} (l)$

Short Answer

Expert verified

The classifications of the given reactions are:

(a) Decomposition reaction

(b) Displacement reaction

(c) Combination reaction

Step by step solution

01

Write balanced reaction of equation (a)

The given reaction is:

$H I (g) 鈫� H_{2} (g) + I_{2} (g)$

The balanced reaction is:

$2 H I (g) 鈫� H_{2} (g) + I_{2} (g)$

The given redox reaction is a decomposition reaction.

In this reaction, HI decomposes and forms $H_{2}$ and $I_{2} .$

02

Write balanced reaction of equation (b)

The given reaction is:

$Z n (s) + A g N O_{3} (a q) 鈫� Z n {(N O_{3})}_{2} (a q) + A g (s)$

The balanced reaction is:

$Z n (s) + 2 A g N O_{3} (a q) 鈫� Z n {(N O_{3})}_{2} (a q) + 2 A g (s)$

The given redox reaction is a displacement reaction.

The zinc atom replaces silver atom from $A g N O_{3}$ and forms $Z n {(N O_{3})}_{2} .$

03

Write balanced reaction of equation (c)

The given reaction is:

$N O (g) + O_{2} (g) 鈫� N_{2} O_{4} (l)$

The balanced reaction is:

$2 N O (g) + O_{2} (g) 鈫� N_{2} O_{4} (l)$

The given redox reaction is a combination reaction.

In this reaction, NO andO₂combines and formsN₂O_4.

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Most popular questions from this chapter

If 25.98 mL of a standard 0.1180 M KOH solution reacts with 52.50 mL of solution, what is the molarity of the acid solution?

A chemical engineer determines the mass percent of iron in an ore sample by converting the Fe to Fe²⁺ in acid and then titrating the Fe²⁺ with MnO₄^-. A 1.1081-g sample was dissolved in acid and then titrated with 39.32mL of 0.03190M KMnO₄. The balanced equation is

$8 H^{+} (aq) + 5 {Fe}^{2 +} (aq) + {MnO}_{4}^{鈭�} (aq) 鈫� 5 {Fe}^{3 +} (aq) + {Mn}^{2 +} (aq) + 4 H_{2} O (l)$

Calculate the mass percent of iron in the ore.

The brewing industry uses yeast microorganisms to convert glucose to ethanol for wine and beer. The baking industry uses the carbon dioxide produced to make bread rise:

$C_{6} H_{12} O_{6} (s) \overset{yeast}{鈫�} 2 C_{2} H_{5} OH (l) + 2 {CO}_{2} (g)$

How many grams of ethanol can be produced from 100g of glucose? What volume of CO₂ is produced? (Assume 1 mol of gas occupies 22.4 L at the conditions used.)

Thyroxine (C₁₅H₁₁I₄NO₄) is a hormone synthesized by the thyroid gland and used to control many metabolic functions in the body. A physiologist determines the mass percent of thyroxine in a thyroid extract by igniting 0.4332 g of extract with sodium carbonate, which converts the iodine to iodide. The iodide is dissolved in water, and bromine and hydrochloric acid are added, which convert the iodide to iodate.

(a) How many moles of iodate form per mole of thyroxine?

(b) Excess bromine is boiled off and more iodide is added, which reacts as shown in the following unbalancedequation:

${IO}_{3}^{-} (aq) + H^{+} (aq) + I^{-} (aq) 鈫� I_{2} (aq) + H_{2} O (I)$

How many moles of iodine are produced per mole of thyroxine?

(Hint:Be sure to balance the charges as well as the atoms.) What are the oxidizing and reducing agents in the reaction?

(c) The iodine reacts completely with 17.23 mL of 0.1000 Mthiosulfate as shown in the following unbalancedequation:

$I_{2} (aq) + S_{2} O_{3}^{2 -} (aq) 鈫� I^{-} (aq) + S_{4} O_{6}^{2 -} (aq)$

What is the mass percent of thyroxine in the thyroid extract?

Question: State a general equation for a neutralization reaction.

See all solutions

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