What is the empirical formula and empirical formu…
What is the empirical formula and empirical formula mass for each of the following compounds?
$\begin{array}{ll}{\text { (a) } \mathrm{C}_{4} \mathrm{H}_{8}} & {\text { (b) } \mathrm{C}_{3} \mathrm{H}_{6} \mathrm{O}_{3}} & {\text { (c) } \mathrm{P}_{4} \mathrm{O}_{10}}\end{array}$
(d) $\mathrm{Ga}_{2}\left(\mathrm{SO}_{4}\right)_{3} \quad$ (e) $\mathrm{Al}_{2} \mathrm{Br}_{6}$
Ethanol $\left(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\right),$ the intoxicant in alcoholic beverages, is also used to make other organic compounds. In concentrated sulfuric acid, ethanol forms diethyl ether and water:
2 \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}(l) \longrightarrow \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OCH}_{2} \mathrm{CH}_{3}(l)+\mathrm{H}_{2} \mathrm{O}(g)
In a side reaction, some ethanol forms ethylene and water:
\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}(l) \longrightarrow \mathrm{CH}_{2} \mathrm{CH}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g)
(a) If 50.0 g of ethanol yields 35.9 g of diethyl ether, what is the percent yield of diethyl ether? (b) If 45.0$\%$ of the ethanol that did not produce the ether reacts by the side reaction, what mass (g) of
ethylene is produced?
Give the name, empirical formula, and molar mass of the compound depicted in Figure P3.38.
What is the molecular formula of each compound?
(a) Empirical formula $\mathrm{CH}_{2}(M=42.08 \mathrm{g} / \mathrm{mol})$
(b) Empirical formula $\mathrm{NH}_{2}(\mathscr{M}=32.05 \mathrm{g} / \mathrm{mol})$
(c) Empirical formula $\mathrm{NO}_{2}(\mathscr{M}=92.02 \mathrm{g} / \mathrm{mol})$
(d) Empirical formula CHN $(M=135.14 \mathrm{g} / \mathrm{mol})$
Md M.
Auburn University Main Campus
$\begin{array}{ll}{\text { (a) } \mathrm{C}_{2} \mathrm{H}_{4}} & {\text { (b) } \mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O}_{2}} & {\text { (c) } \mathrm{N}_{2} \mathrm{O}_{5}} \\ {\text { (d) } \mathrm{Ba}_{3}\left(\mathrm{PO}_{4}\right)_{2}} & {\text { (e) } \mathrm{Te}_{4} \mathrm{I}_{16}}\end{array}$
What is the molecular formula of each of the following compounds?
\begin{array}{l}{\text { (a) empirical formula } \mathrm{HCO}_{2} \text { , molar mass }=90.0 \mathrm{g} / \mathrm{mol}} \\ {\text { (b) empirical formula } \mathrm{C}_{2} \mathrm{H}_{4} \mathrm{O}, \text { molar mass }=88.0 \mathrm{g} / \mathrm{mol}}\end{array}