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Chapter 8: Problem 95

Classify each reaction as combination, decomposition, single-replacement, or double-replacement: (a) \(2 \mathrm{NaCl} \rightarrow 2 \mathrm{Na}+\mathrm{Cl}_{2}\) (b) \(\mathrm{Ba}_{3} \mathrm{~N}_{2} \rightarrow 3 \mathrm{Ba}+\mathrm{N}_{2}\) (c) \(\mathrm{Cl}_{2}+2 \mathrm{NaI} \rightarrow 2 \mathrm{NaCl}+\mathrm{I}_{2}\) (d) \(\mathrm{KNO}_{3}+\mathrm{AgBr} \rightarrow \mathrm{AgNO}_{3}+\mathrm{KBr}\)

Short Answer

Expert verified
(a) Decomposition (b) Decomposition (c) Single-replacement (d) Double-replacement

Step by step solution

01

Definition of Combination Reaction

A combination reaction is a reaction in which two or more reactants combine to form a single product.
02

Definition of Decomposition Reaction

A decomposition reaction is a reaction in which a single reactant breaks down into two or more simpler products.
03

Definition of Single-Replacement Reaction

A single-replacement reaction is a reaction in which a more reactive element in a reactant compound is replaced by a less reactive element.
04

Definition of Double-Replacement Reaction

A double-replacement reaction is a reaction in which the ions of two compounds exchange places, resulting in the formation of two new compounds. Now, let's analyze and classify each reaction:
05

Reaction (a) Classification

Given: \(2 \mathrm{NaCl} \rightarrow 2 \mathrm{Na} + \mathrm{Cl}_{2}\) In this reaction, we have one reactant (\(NaCl\)), which breaks down into its constituent elements, sodium (\(Na\)) and chlorine (\(Cl_2\)), as the products. This is an example of a decomposition reaction.
06

Reaction (b) Classification

Given: \(\mathrm{Ba}_{3} \mathrm{~N}_{2} \rightarrow 3 \mathrm{Ba} + \mathrm{N}_{2}\) In this reaction, we have one reactant (\(Ba_3N_2\)), which breaks down into its constituent elements, barium (\(Ba\)) and nitrogen (\(N_2\)), as the products. This is another example of a decomposition reaction.
07

Reaction (c) Classification

Given: \(\mathrm{Cl}_{2} + 2 \mathrm{NaI} \rightarrow 2 \mathrm{NaCl} + \mathrm{I}_{2}\) In this reaction, we have two reactants (\(Cl_2\) and \(NaI\)). The more reactive element, chlorine (\(Cl_2\)), replaces the less reactive element, iodine (\(I\)), in the compound \(NaI\), resulting in the formation of \(2 NaCl\) and iodine (\(I_2\)). This is an example of a single-replacement reaction.
08

Reaction (d) Classification

Given: \(\mathrm{KNO}_{3} + \mathrm{AgBr} \rightarrow \mathrm{AgNO}_{3} + \mathrm{KBr}\) In this reaction, we have two reactants (\(KNO_3\) and \(AgBr\)). The ions of the two compounds (\(K^+\) and \(NO_3^-\) in \(\mathrm{KNO}_{3}\), \(Ag^+\) and \(Br^-\) in \(\mathrm{AgBr}\)) exchange places, resulting in the formation of two new compounds (\(AgNO_3\) and \(KBr\)). This is an example of a double-replacement reaction.

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Most popular questions from this chapter

Balance this chemical equation and assign it a reaction type: \(\mathrm{Fe}\left(\mathrm{NO}_{3}\right)_{3}(a q)+\mathrm{Na}_{2} \mathrm{~S}(a q) \rightarrow \mathrm{Fe}_{2} \mathrm{~S}_{3}(s)+\mathrm{NaNO}_{3}(a q)\)

What is the number of molecules of \(\mathrm{NaOH}\) required to neutralize one molecule of: (a) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (b) HI (c) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) (d) \(\mathrm{HNO}_{3}\) (e) \(\mathrm{CH}_{3} \mathrm{COOH}\)

You need nickel(II) hydroxide, but there is none in the lab. However, there are lots of other ionic compounds on the shelves. Propose a synthesis for nickel(II) hydroxide.

Sulfur dioxide and water are formed when hydrogen sulfide, \(\mathrm{H}_{2} \mathrm{~S}\), reacts with oxygen gas. Write the balanced equation for the reaction.

Is the reaction \(\mathrm{LiOH}+\mathrm{HCN} \rightarrow \mathrm{H}_{2} \mathrm{O}+\mathrm{LiCN}\) a combination, decomposition, single-replacement, or double-replacement?
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