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Chapter 7: Problem 62

By now, you are familiar with enough chemical compounds to begin to write your own chemical reaction equations. Write two examples each of what we mean by a synthesis reaction and by a decomposition reaction.

Short Answer

Expert verified
Examples of Synthesis Reactions: 1. \(2H_2 + O_2 \rightarrow 2H_2O\) (Hydrogen gas and oxygen gas react to form water) 2. \(2Na + Cl_2 \rightarrow 2NaCl\) (Sodium and chlorine gas react to form sodium chloride) Examples of Decomposition Reactions: 1. \(CaCO_3 \rightarrow CaO + CO_2\) (Calcium carbonate decomposes into calcium oxide and carbon dioxide when heated) 2. \(2H_2O_2 \rightarrow 2H_2O + O_2\) (Hydrogen peroxide decomposes into water and oxygen gas)

Step by step solution

01

Choose Simple Compounds

Select two simple compounds that can combine to form a more complex compound. In this case, let's choose hydrogen gas (H2) and oxygen gas (O2).
02

Combine the Compounds

Next, combine the selected compounds to form a new, more complex compound. By this, we mean that hydrogen gas and oxygen gas will react to form water (H2O). The balanced chemical equation for this reaction is: \(2H_2 + O_2 \rightarrow 2H_2O\) Example 2: Synthesis Reaction
03

Choose Simple Compounds

Select two simple compounds that can combine to form a more complex compound. In this case, let's choose sodium (Na) and chlorine gas (Cl2).
04

Combine the Compounds

Next, combine the selected compounds to form a new, more complex compound. By this, we mean that sodium and chlorine gas will react to form sodium chloride (NaCl). The balanced chemical equation for this reaction is: \(2Na + Cl_2 \rightarrow 2NaCl\) Example 1: Decomposition Reaction
05

Choose a Complex Compound

Select a complex compound that can be broken down into simpler compounds. In this case, let's choose calcium carbonate (CaCO3).
06

Decompose the Compound

Next, write the balanced chemical equation for the decomposition of the chosen compound. Calcium carbonate will decompose into calcium oxide (CaO) and carbon dioxide (CO2) when heated. The balanced chemical equation for this reaction is: \(CaCO_3 \rightarrow CaO + CO_2\) Example 2: Decomposition Reaction
07

Choose a Complex Compound

Select a complex compound that can be broken down into simpler compounds. In this case, let's choose hydrogen peroxide (H2O2).
08

Decompose the Compound

Next, write the balanced chemical equation for the decomposition of the chosen compound. Hydrogen peroxide will decompose into water (H2O) and oxygen gas (O2). The balanced chemical equation for this reaction is: \(2H_2O_2 \rightarrow 2H_2O + O_2\)

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Most popular questions from this chapter

For each of the following metals, how many electrons will the metal atoms lose when the metal reacts with a nonmetal? a. sodium b. potassium c. magnesium d. barium e. aluminum

What do we mean by a precipitation reaction?

Identify each of the following unbalanced reaction equations as belonging to one or more of the following categories: precipitation, acid-base, or oxidation-reduction. a. \(\mathrm{H}_{2} \mathrm{O}_{2}(a q) \rightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{O}_{2}(g)\) b. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Cu}(s) \rightarrow \mathrm{CuSO}_{4}(a q)+\mathrm{H}_{2}(g)\) c. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{NaOH}(a q) \rightarrow \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) d. \(\mathrm{H}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Ba}(\mathrm{OH})_{2}(a q) \rightarrow \mathrm{BaSO}_{4}(s)+\mathrm{H}_{2} \mathrm{O}(l)\) e. \(\mathrm{AgNO}_{3}(a q)+\mathrm{CuCl}_{2}(a q) \rightarrow \mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\) \(\mathrm{AgCl}(s)\) f. \(\mathrm{KOH}(a q)+\mathrm{CuSO}_{4}(a q) \rightarrow \mathrm{Cu}(\mathrm{OH})_{2}(s)+\mathrm{K}_{2} \mathrm{SO}_{4}(a q)\) g. \(\mathrm{Cl}_{2}(g)+\mathrm{F}_{2}(g) \rightarrow \operatorname{ClF}(g)\) h. \(\mathrm{NO}(g)+\mathrm{O}_{2}(g) \rightarrow \mathrm{NO}_{2}(g)\) i. \(\mathrm{Ca}(\mathrm{OH})_{2}(s)+\mathrm{HNO}_{3}(a q) \rightarrow \mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\)

What salt would form when each of the following strong acid/strong base reactions takes place? a. \(\mathrm{HCl}(a q)+\mathrm{KOH}(a q) \rightarrow\) b. \(\operatorname{RbOH}(a q)+\mathrm{HNO}_{3}(a q) \rightarrow\) c. \(\mathrm{HClO}_{4}(a q)+\mathrm{NaOH}(a q) \rightarrow\) d. \(\mathrm{HBr}(a q)+\mathrm{CaOH}(a q) \rightarrow\)

Sulfuric acid, \(\mathrm{H}_{2} \mathrm{SO}_{4}\), oxidizes many metallic elements. One of the effects of acid rain is that it produces sulfuric acid in the atmosphere, which then reacts with metals used in construction. Write balanced oxidation-reduction equations for the reaction of sulfuric acid with Fe, \(\mathrm{Zn}, \mathrm{Mg}, \mathrm{Co},\) and \(\mathrm{Ni}\).
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