91Ó°ÊÓ

Balance each of the following chemical equations:

$\text{a.}\mathrm{Mg}\left(s\right)+{\mathrm{AgNO}}_3\left(aq\right)âŸ\P \mathrm{Mg}{\left({\mathrm{NO}}_3\right)}_2\left(aq\right)+\mathrm{Ag}\left(s\right)$

$\text{b.}\mathrm{Al}\left(s\right)+{\mathrm{CuSO}}_4\left(aq\right)âŸ\P {\mathrm{Al}}_2{\left({\mathrm{SO}}_4\right)}_3\left(aq\right)+\mathrm{Cu}\left(s\right)$
$\text{c.}\mathrm{Pb}{\left({\mathrm{NO}}_3\right)}_2\left(aq\right)+\mathrm{NaCl}\left(aq\right)âŸ\P {\mathrm{PbCl}}_2\left(s\right)+{\mathrm{NaNO}}_3(aq$

$\text{d.}\mathrm{Al}\left(s\right)+\mathrm{HCl}\left(aq\right)âŸ\P {\mathrm{H}}_2\left(g\right)+{\mathrm{AlCl}}_3\left(aq\right)$

Calculate each of the following:

1. number of $\mathrm{Li}$atoms in $4.5$moles of $\mathrm{Li}$
2. number of ${\mathrm{CO}}_2$molecules in $0.0180$mole of ${\mathrm{CO}}_2$
3. moles of $\mathrm{Cu}$in $7.8×{10}^{21}$atoms of Cu
4. moles of ${\mathrm{C}}_2{\mathrm{H}}_6$in $3.75×{10}^{23}$molecules of ${\mathrm{C}}_2{\mathrm{H}}_6$
   

Balance each of the following chemical equations:

$$\begin{gathered} \text{a.}\mathrm{Zn}\left(s\right)+{\mathrm{HNO}}_3\left(aq\right)âŸ\P {\mathrm{H}}_2\left(g\right)+\mathrm{Zn}{\left({\mathrm{NO}}_3\right)}_2\left(aq\right) \\ \text{b.}\mathrm{Al}\left(s\right)+{\mathrm{H}}_2{\mathrm{SO}}_4\left(aq\right)âŸ\P {\mathrm{H}}_2\left(g\right)+{\mathrm{Al}}_2{\left({\mathrm{SO}}_4\right)}_3\left(aq\right) \\ \text{c.}{\mathrm{K}}_2{\mathrm{SO}}_4\left(aq\right)+{\mathrm{BaCl}}_2\left(aq\right)âŸ\P {\mathrm{BaSO}}_4\left(s\right)+\mathrm{KCl}\left(aq\right) \\ \text{d.}{\mathrm{CaCO}}_3\left(s\right)âŸ\P \mathrm{CaO}\left(s\right)+{\mathrm{CO}}_2\left(g\right) \end{gathered}$$

Classify each of the following as a combination, decomposition, single replacement, double replacement, or combustion reaction:

a. $2{\mathrm{Al}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)\stackrel{∆}{→}4\mathrm{Al}\left(\mathrm{s}\right)+3{\mathrm{O}}_2\left(\mathrm{g}\right)$

b. ${\mathrm{Br}}_2\left(\mathrm{l}\right)+{\mathrm{BaI}}_2\left(\mathrm{s}\right)→{\mathrm{BaBr}}_2\left(\mathrm{s}\right)+{\mathrm{I}}_2\left(\mathrm{s}\right)$

c. $2{\mathrm{C}}_2{\mathrm{H}}_2\left(\mathrm{g}\right)+5{\mathrm{O}}_2\left(\mathrm{g}\right)\stackrel{∆}{→}4{\mathrm{CO}}_2\left(\mathrm{g}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$

d. ${\mathrm{BaCl}}_2\left(\mathrm{aq}\right)+{\mathrm{K}}_2{\mathrm{CO}}_3\left(\mathrm{aq}\right)→{\mathrm{BaCO}}_3\left(\mathrm{s}\right)+\mathrm{KCl}\left(\mathrm{aq}\right)$

e.$\mathrm{Pb}\left(\mathrm{s}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)→{\mathrm{PbO}}_2\left(\mathrm{s}\right)$

Classify each of the following as a combination, decomposition, single replacement, double replacement, or combustion reaction:

a.$H_{\mathit{2}}\left(g\right)+B{r}_{\mathit{2}}\left(l\right)→2HBr\left(\mathrm{g}\right)$

b. ${\mathrm{AgNO}}_3\left(\mathrm{aq}\right)+\mathrm{NaCl}\left(\mathrm{aq}\right)→\mathrm{AgCl}\left(\mathrm{s}\right)+{\mathrm{NaNO}}_3\left(\mathrm{aq}\right)$

c.$2{\mathrm{H}}_2{\mathrm{O}}_2\left(\mathrm{aq}\right)→2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)$

d. $\mathrm{Zn}\left(\mathrm{s}\right)+{\mathrm{CuCl}}_2\left(\mathrm{aq}\right)→\mathrm{Cu}\left(\mathrm{s}\right)+{\mathrm{ZnCl}}_2\left(\mathrm{aq}\right)$

e.${\mathrm{C}}_5{\mathrm{H}}_8\left(\mathrm{g}\right)+{70}_2\left(\mathrm{g}\right)→5{\mathrm{CO}}_2\left(\mathrm{g}\right)+4{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$

Classify each of the following as a combination, decomposition, single replacement, double replacement, or combustion reaction:

a.$4\mathrm{Fe}\left(\mathrm{s}\right)+3{\mathrm{O}}_2\left(\mathrm{g}\right)→2{\mathrm{Fe}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)$

b.$\mathrm{Mg}\left(\mathrm{s}\right)+2{\mathrm{AgNO}}_3\left(\mathrm{aq}\right)→2\mathrm{Ag}\left(\mathrm{s}\right)+\mathrm{Mg}{\left({\mathrm{NO}}_3\right)}_2\left(\mathrm{aq}\right)$

c.${\mathrm{CuCO}}_3\left(\mathrm{s}\right)→\mathrm{CuO}\left(\mathrm{s}\right)+{\mathrm{CO}}_2\left(\mathrm{g}\right)$

d. ${\mathrm{Al}}_2{\left({\mathrm{SO}}_4\right)}_3\left(\mathrm{aq}\right)+6\mathrm{KOH}\left(\mathrm{aq}\right)→2\mathrm{Al}{\left(\mathrm{OH}\right)}_3\left(\mathrm{s}\right)+3{\mathrm{K}}_2{\mathrm{SO}}_4\left(\mathrm{aq}\right)$

e.${\mathrm{C}}_4{\mathrm{H}}_8\left(\mathrm{g}\right)+6{\mathrm{O}}_2\left(\mathrm{g}\right)→4{\mathrm{CO}}_2\left(\mathrm{g}\right)+4{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$

Classify each of the following as a combination, decomposition, single replacement, double replacement, or combustion reaction:

a.$\mathrm{CuO}\left(\mathrm{s}\right)+2\mathrm{HCl}\left(\mathrm{aq}\right)→{\mathrm{CuCl}}_2\left(\mathrm{aq}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

b.$2\mathrm{Al}\left(\mathrm{s}\right)+3{\mathrm{Br}}_2\left(\mathrm{l}\right)→2{\mathrm{AlBr}}_3\left(\mathrm{s}\right)$

c.$2{\mathrm{C}}_2{\mathrm{H}}_2\left(\mathrm{g}\right)+5{\mathrm{O}}_2\left(\mathrm{g}\right)→4{\mathrm{CO}}_2\left(\mathrm{g}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{g}\right)$

d.${\mathrm{Fe}}_2{\mathrm{O}}_3\left(\mathrm{s}\right)+3\mathrm{C}\left(\mathrm{s}\right)→2\mathrm{Fe}\left(\mathrm{s}\right)+3\mathrm{CO}\left(\mathrm{g}\right)$

e.${\mathrm{C}}_6{\mathrm{H}}_{12}{\mathrm{O}}_6\left(\mathrm{aq}\right)→2{\mathrm{C}}_2{\mathrm{H}}_6\mathrm{O}\left(\mathrm{aq}\right)+2{\mathrm{CO}}_2\left(\mathrm{g}\right)$

Identify each of the following as an oxidation or a reduction:

a.${\mathrm{Na}}^{+}\left(\mathrm{aq}\right)+{\mathrm{e}}^{-}→2\mathrm{Na}\left(\mathrm{s}\right)$

b.$\mathrm{Ni}\left(\mathrm{s}\right)→{\mathrm{Ni}}^{2+}\left(\mathrm{aq}\right)+2{\mathrm{e}}^{-}$

c.${\mathrm{Cr}}^{3+}\left(\mathrm{aq}\right)+3{\mathrm{e}}^{-}→\mathrm{Cr}\left(\mathrm{s}\right)$

d.$2{\mathrm{H}}^{+}\left(\mathrm{aq}\right)+2{\mathrm{e}}^{-}→{\mathrm{H}}_2\left(\mathrm{g}\right)$

Identify each of the following as an oxidation or a reduction:

a. ${\mathrm{O}}_2\left(\mathrm{g}\right)+4{\mathrm{e}}^{-}→2{\mathrm{O}}^{2-}\left(\mathrm{aq}\right)$

b. $\mathrm{Ag}\left(\mathrm{s}\right)→{\mathrm{Ag}}^{+}\left(\mathrm{aq}\right)+{\mathrm{e}}^{-}$

c.${\mathrm{Fe}}^{3+}\left(\mathrm{aq}\right)+{\mathrm{e}}^{-}→{\mathrm{Fe}}^{2+}\left(\mathrm{aq}\right)$

d.$2\mathrm{Br}{}^{-}\left(\mathrm{aq}\right)→\mathrm{Br}2\left(\mathrm{l}\right)+2{\mathrm{e}}^{-}$

In each of the following, identify the reactant that is oxidized and the reactant that is reduced:

a. $Zn\left(s\right)+C{l}_2\left(g\right)→ZnC{l}_2\left(s\right)$

b.${\mathrm{CI}}_2\left(\mathrm{g}\right)+2\mathrm{NaBr}\left(\mathrm{aq}\right)→2\mathrm{NaCl}\left(\mathrm{aq}\right)+{\mathrm{Br}}_2\left(\mathrm{l}\right)$

c.$2\mathrm{PbO}\left(\mathrm{s}\right)→2\mathrm{Pb}\left(\mathrm{s}\right)+{\mathrm{O}}_2\left(\mathrm{g}\right)$

d.$2\mathrm{Fe}\left(\mathrm{aq}\right)+{\mathrm{Sn}}^{2+}\left(\mathrm{aq}\right)→2{\mathrm{Fe}}^{2+}\left(\mathrm{aq}\right)+{\mathrm{Sn}}^{4+}\left(\mathrm{aq}\right)$