Chapter 5

a. Why is the following reaction called a combination reaction? $${\mathrm{H}}_2(g)+{\mathrm{Br}}_2(g)⟶2\mathrm{HBr}(g)$$ b. Why is the following reaction called a double replacement reaction? $${\mathrm{AgNO}}_3(aq)+\mathrm{NaCl}(aq)⟶\mathrm{AgCl}(s)+{\mathrm{NaNO}}_3(aq)$$

Classify each of the following reactions as a combination, decomposition, single replacement, double replacement, or combustion: a. $4\mathrm{Fe}(s)+3{\mathrm{O}}_2(g)⟶2{\mathrm{Fe}}_2{\mathrm{O}}_3(s)$ b. $\mathrm{Mg}(s)+2{\mathrm{AgNO}}_3(aq)⟶\mathrm{Mg}{\left({\mathrm{NO}}_3\right)}_2(aq)+2\mathrm{Ag}(s)$ c. ${\mathrm{CuCO}}_3(s)\stackrel{\mathrm{\Delta }}{⟶}\mathrm{CuO}(s)+{\mathrm{CO}}_2(g)$ d. $\mathrm{NaOH}(aq)+\mathrm{HCl}(aq)⟶\mathrm{NaCl}(aq)+{\mathrm{H}}_2\mathrm{O}(t)$ e. ${\mathrm{ZnCO}}_3(s)\stackrel{\mathrm{\Delta }}{⟶}{\mathrm{CO}}_2(g)+\mathrm{ZnO}(s)$ f. ${\mathrm{Al}}_2{\left({\mathrm{SO}}_4\right)}_3(aq)+6\mathrm{KOH}(aq)⟶$ $2\mathrm{Al}(\mathrm{OH}{)}_3(s)+3{\mathrm{K}}_2{\mathrm{SO}}_4(aq)$ $\mathrm{g}\cdot \mathrm{Pb}(s)+{\mathrm{O}}_2(g)⟶{\mathrm{PbO}}_2(s)$ h. ${\mathrm{C}}_4{\mathrm{H}}_8(g)+6{\mathrm{O}}_2(g)\stackrel{\mathrm{\Delta }}{⟶}4{\mathrm{CO}}_2(g)+4{\mathrm{H}}_2\mathrm{O}(g)$

Classify each of the following reactions as a combination, decomposition, single replacement, double replacement, or combustion: a. $\mathrm{CuO}(s)+2\mathrm{HCl}(aq)⟶{\mathrm{CuCl}}_2(aq)+{\mathrm{H}}_2\mathrm{O}(l)$ b. $2\mathrm{Al}(s)+3{\mathrm{Br}}_2(g)⟶2{\mathrm{AlBr}}_3(s)$ c. $\mathrm{Pb}{\left({\mathrm{NO}}_3\right)}_2(aq)+2\mathrm{NaCl}(aq)⟶{\mathrm{PbCl}}_2(s)+2{\mathrm{NaNO}}_3(aq)$ d. $2\mathrm{Mg}(s)+{\mathrm{O}}_2(g)\stackrel{\mathrm{\Delta }}{⟶}2\mathrm{MgO}(s)$ e. $2{\mathrm{C}}_2{\mathrm{H}}_2(g)+5{\mathrm{O}}_2(g)\stackrel{\mathrm{\Delta }}{⟶}4{\mathrm{CO}}_2(g)+2{\mathrm{H}}_2\mathrm{O}(g)$ f. ${\mathrm{Fe}}_2{\mathrm{O}}_3(s)+3\mathrm{C}(s)⟶2\mathrm{Fe}(s)+3\mathrm{CO}(g)$ g. ${\mathrm{C}}_6{\mathrm{H}}_{12}{\mathrm{O}}_6(aq)⟶2{\mathrm{C}}_2{\mathrm{H}}_6\mathrm{O}(aq)+2{\mathrm{CO}}_2(g)$ h. ${\mathrm{BaCl}}_2(aq)+{\mathrm{K}}_2{\mathrm{CO}}_3(aq)⟶{\mathrm{BaCO}}_3(s)+2\mathrm{KCl}(aq)$

Predict the products that would result from each of the following reactions and balance: a. combination: $\mathrm{Mg}(s)+{\mathrm{Cl}}_2(g)⟶$ b. decomposition: $\mathrm{HBr}(g)\stackrel{\mathrm{\Delta }}{⟶}$ c. single replacement: $\mathrm{Mg}(s)+\mathrm{Zn}{\left({\mathrm{NO}}_3\right)}_2(aq)⟶$ d. double replacement: ${\mathrm{K}}_2\mathrm{S}(aq)+\mathrm{Pb}{\left({\mathrm{NO}}_3\right)}_2(aq)⟶$ e. combustion: ${\mathrm{C}}_2{\mathrm{H}}_6(g)+{\mathrm{O}}_2(g)\stackrel{\mathrm{\Delta }}{⟶}$

Predict the products that would result from each of the following reactions and balance: a. combination: $\mathrm{Ca}(s)+{\mathrm{O}}_2(g)⟶$ b. combustion: ${\mathrm{C}}_6{\mathrm{H}}_6(g)+{\mathrm{O}}_2(g)\stackrel{\mathrm{\Delta }}{⟶}$ c. decomposition: ${\mathrm{PbO}}_2(s)\stackrel{\mathrm{\Delta }}{⟶}$ d. single replacement: $\mathrm{KI}(s)+{\mathrm{Cl}}_2(g)⟶$ e. double replacement: ${\mathrm{CuCl}}_2(aq)+{\mathrm{Na}}_2\mathrm{S}(aq)⟶$

Indicate each of the following as an oxidation or a reduction: a. ${\mathrm{Na}}^{+}(aq)+e^{-}⟶\mathrm{Na}(s)$ b. $\mathrm{Ni}(s)⟶{\mathrm{Ni}}^{2+}(aq)+2e^{-}$ c. ${\mathrm{Cr}}^{3+}(aq)+3e^{-}⟶\mathrm{Cr}(s)$ d. $2{\mathrm{H}}^{+}(aq)+2e^{-}⟶{\mathrm{H}}_2(g)$

Indicate each of the following as an oxidation or a reduction: a. ${\mathrm{O}}_2(g)+4e^{-}⟶2{\mathrm{O}}^{2-}(aq)$ b. $\mathrm{Al}(s)⟶{\mathrm{Al}}^{3+}(aq)+3e^{-}$ c. ${\mathrm{Fe}}^{3+}(aq)+e^{-}⟶{\mathrm{Fe}}^{2+}(aq)$ d. $2{\mathrm{Br}}^{-}(aq)⟶{\mathrm{Br}}_2(l)+2e^{-}$

In each of the following reactions, identify the reactant that is oxidized and the reactant that is reduced: a. $\mathrm{Zn}(s)+{\mathrm{Cl}}_2(g)⟶{\mathrm{ZnCl}}_2(s)$ b. ${\mathrm{Cl}}_2(g)+2\mathrm{NaBr}(aq)⟶2\mathrm{NaCl}(aq)+{\mathrm{Br}}_2(l)$ c. $2\mathrm{PbO}(s)⟶2\mathrm{Pb}(s)+{\mathrm{O}}_2(g)$ d. $2{\mathrm{Fe}}^{3+}(aq)+{\mathrm{Sn}}^{2+}(aq)⟶2{\mathrm{Fe}}^{2+}(aq)+{\mathrm{Sn}}^{4+}(aq)$

In each of the following reactions, identify the reactant that is oxidized and the reactant that is reduced: a. $2\mathrm{Li}(s)+{\mathrm{F}}_2(g)⟶2\mathrm{LiF}(s)$ b. ${\mathrm{Cl}}_2(g)+2\mathrm{KI}(aq)⟶2\mathrm{KCl}(aq)+{\mathrm{I}}_2(s)$ c. $2\mathrm{Al}(s)+3{\mathrm{Sn}}^{2+}(aq)⟶2{\mathrm{Al}}^{3+}(aq)+3\mathrm{Sn}(s)$ d. $\mathrm{Fe}(s)+{\mathrm{CuSO}}_4(aq)⟶{\mathrm{FeSO}}_4(aq)+\mathrm{Cu}(s)$

In the mitochondria of human cells, energy for the production of ATP is provided by the oxidation and reduction reactions of the iron ions in the cytochromes in electron transport. Identify each of the following reactions as an oxidation or reduction: a. ${\mathrm{Fe}}^{3+}+e^{-}⟶{\mathrm{Fe}}^{2+}$ b. ${\mathrm{Fe}}^{2+}⟶{\mathrm{Fe}}^{3+}+e^{-}$