(Solved): Aluminum reacts with aqueous sodium hydroxide to produce hydrogen gas according to the followin ...

Aluminum reacts with aqueous sodium hydroxide to produce hydrogen gas according to the following equation: $2\mathrm{Al}(s)+2\mathrm{NaOH}(aq)+6{\mathrm{H}}_2\mathrm{O}(l)?2\mathrm{NaAl}(\mathrm{OH}{)}_4(aq)+3{\mathrm{H}}_2(g)$ The product gas, ${\mathrm{H}}_2$, is collected over water at a temperature of $25^{?}\mathrm{C}$ and a pressure of $749.0\mathrm{mm}\mathrm{Hg}$. If the wet ${\mathrm{H}}_2$ gas formed occupies a volume of $8.27\mathrm{L}$, the number of grams of ${\mathrm{H}}_2$ formed is ${}^{?}\mathrm{C}$. g. The vapor pressure of water is $23.8\mathrm{mm}\mathrm{Hg}$ at 25 9 mere group attempts remaining A mixture of oxygen and neon gases, at a total pressure of $806\mathrm{mm}\mathrm{Hg}$, contains 5.71 grams of oxygen and 2.53 grams of neon. What is the partial pressure of each gas in the mixture? $\begin{array}{ll}{P}_{{\mathrm{O}}_2}=& \mathrm{mm}\mathrm{Hg}\\ P_{\mathrm{Ne}}=& \mathrm{mm}\mathrm{Hg}\end{array}$ A mixture of helium and oxygen gases contains helium at a partial pressure of $270\mathrm{mm}\mathrm{Hg}$ and oxygen at a partial pressure of $423\mathrm{mm}\mathrm{Hg}$. What is the mole fraction of each gas in the mixture? $\begin{array}{l}{x}_{{\mathrm{He}}_e}=\\ x_{{\mathrm{O}}_2}=\end{array}$ Caicium carbide reacts with water to produce acetylene gas according to the following equation: ${\mathrm{CaC}}_2(s)+2{\mathrm{H}}_2\mathrm{O}(l)?{\mathrm{C}}_2{\mathrm{H}}_2(g)+\mathrm{Ca}(\mathrm{OH}{)}_2(aq)$ The product gas, ${\mathrm{C}}_2{\mathrm{H}}_2$, is collected over water at a temperature of $20^{?}\mathrm{C}$ and a pressure of $752.0\mathrm{mm}\mathrm{Hg}$. If the wet ${\mathrm{C}}_2{\mathrm{H}}_2\mathrm{gas}$ formed occupies a volume of $6.12\mathrm{L}$, the number of grams of ${\mathrm{C}}_2{\mathrm{H}}_2$ formed is $\mathrm{Hg}$ at $20^{?}\mathrm{C}$. g. The vapor pressure of water is $17.5\mathrm{mm}$