How many moles of carbon dioxide are produced when $0.2 \mathrm{mol}$ of sodium carbonate reacts with excess hydrochloric acid? 

Solid sodium carbonate reacts with aqueous hydrochloric acid to form aqueous sodium chloride, carbon dioxide and water.

${\mathrm{Na}}_2{\mathrm{CO}}_3+2\mathrm{HCl}\to 2\mathrm{NaCl}+{\mathrm{CO}}_2+{\mathrm{H}}_2\mathrm{O}$

Calculate the volume of this number of moles of carbon dioxide at r.t.p. ($1 \mathrm{mol}$ of gas occupies $24 {\mathrm{dm}}^3$ at r.t.p.).

Hydrocarbons are compounds of carbon and hydrogen only. Hydrocarbon $\mathrm{Z}$ is composed of $80\%$ carbon and $20\%$ hydrogen.

a. Calculate the empirical formula of hydrocarbon $\mathrm{Z}$. (${\mathrm{A}}_{\mathrm{r}}$ values: $\mathrm{C}=12.0, \mathrm{H}=1.0$).

b. The molar mass of hydrocarbon $\mathrm{Z}$ is $30.0 \mathrm{g} {\mathrm{mol}}^{-1}$. Deduce the molecular formula of this hydrocarbon.

When $50 {\mathrm{cm}}^3$ of hydrocarbon $\mathrm{Y}$ is burnt, it reacts with exactly $300 {\mathrm{cm}}^3$ of oxygen to form $200 {\mathrm{cm}}^3$ of carbon dioxide. Water is also formed in the reaction. Construct the equation for this reaction. Explain your reasoning.

Propane has the molecular formula ${\mathrm{C}}_3{\mathrm{H}}_8$. Calculate the mass of $600 {\mathrm{cm}}^3$ of propane at r.t.p. ($1 \mathrm{mol}$ of gas occupies $24 {\mathrm{dm}}^3$ at r.t.p.).

(${\mathrm{A}}_{\mathrm{r}}$ values: $\mathrm{C}=12.0, \mathrm{H}=1.0$).

When sodium reacts with titanium chloride $\left({\mathrm{TiCl}}_4\right)$, sodium chloride $\left(\mathrm{NaCl}\right)$ and titanium $\left(\mathrm{Ti}\right)$ are produced. Calculate the mass of titanium produced from $380 \mathrm{g}$ of titanium chloride. Give your answer to $3$ significant figures. (${\mathrm{A}}_{\mathrm{r}}$ values: $\mathrm{Ti}=47.9, \mathrm{Cl}=35.5$).

When sodium reacts with titanium chloride $\left({\mathrm{TiCl}}_4\right)$, sodium chloride $\left(\mathrm{NaCl}\right)$ and titanium $\left(\mathrm{Ti}\right)$ are produced. Calculate the mass of titanium produced using $46.0 \mathrm{g}$ of sodium. Give your answer to $3$ significant figures. (${\mathrm{A}}_{\mathrm{r}}$ value: $\mathrm{Na}=23.0$).

Give all answers to $3$ significant figures. Ammonium nitrate decomposes on heating to give nitrogen(II) oxide and water as follows:

${\mathrm{NH}}_4{\mathrm{NO}}_3\left(\mathrm{s}\right)\to {\mathrm{N}}_2\mathrm{O}\left(\mathrm{g}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

(${\mathrm{A}}_{\mathrm{r}}$ values: $\mathrm{N}=14.0, \mathrm{H}=1.0, \mathrm{O}=16.0$).

Deduce the formula mass of ammonium nitrate.

Give all answers to $3$ significant figures. Ammonium nitrate decomposes on heating to give nitrogen(II) oxide and water as follows:

${\mathrm{NH}}_4{\mathrm{NO}}_3\left(\mathrm{s}\right)\to {\mathrm{N}}_2\mathrm{O}\left(\mathrm{g}\right)+2{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

(${\mathrm{A}}_{\mathrm{r}}$ values: $\mathrm{N}=14.0, \mathrm{H}=1.0, \mathrm{O}=16.0$).

How many moles of ammonium nitrate are present in $0.800 \mathrm{g}$ of the solid?