Give the answer to $3$ significant figures. $4.80 {\mathrm{dm}}^3$ of chlorine gas was reacted with sodium hydroxide solution. The reaction taking place was as follows:

${\mathrm{Cl}}_2\left(\mathrm{g}\right)+2\mathrm{NaOH}\left(\mathrm{aq}\right)\to \mathrm{NaCl}\left(\mathrm{aq}\right)+\mathrm{NaOCl}\left(\mathrm{aq}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$.

(${\mathrm{A}}_{\mathrm{r}}$ values: $\mathrm{Na}=23.0; \mathrm{Cl}=35.5; \mathrm{O}=16.0$)

Calculate the number of moles of ${\mathrm{Cl}}_2$ reacted.

Give the answer to $3$ significant figures. $4.80 {\mathrm{dm}}^3$ of chlorine gas was reacted with sodium hydroxide solution. The reaction taking place was as follows:

${\mathrm{Cl}}_2\left(\mathrm{g}\right)+2\mathrm{NaOH}\left(\mathrm{aq}\right)\to \mathrm{NaCl}\left(\mathrm{aq}\right)+\mathrm{NaOCl}\left(\mathrm{aq}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$.

(${\mathrm{A}}_{\mathrm{r}}$ values: $\mathrm{Na}=23.0; \mathrm{Cl}=35.5; \mathrm{O}=16.0$)

Calculate the mass of $\mathrm{NaOCl}$ formed.

Give the answer to $3$ significant figures. $4.80 {\mathrm{dm}}^3$ of chlorine gas was reacted with sodium hydroxide solution. The reaction taking place was as follows:

${\mathrm{Cl}}_2\left(\mathrm{g}\right)+2\mathrm{NaOH}\left(\mathrm{aq}\right)\to \mathrm{NaCl}\left(\mathrm{aq}\right)+\mathrm{NaOCl}\left(\mathrm{aq}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$.

(${\mathrm{A}}_{\mathrm{r}}$ values: $\mathrm{Na}=23.0; \mathrm{Cl}=35.5; \mathrm{O}=16.0$)

The concentration of the $\mathrm{NaOH}$ was $2.00 \mathrm{mol} {\mathrm{dm}}^{-3}$. Calculate the volume of sodium hydroxide solution required.

Give the answer to $3$ significant figures. $4.80 {\mathrm{dm}}^3$ of chlorine gas was reacted with sodium hydroxide solution. The reaction taking place was as follows:

${\mathrm{Cl}}_2\left(\mathrm{g}\right)+2\mathrm{NaOH}\left(\mathrm{aq}\right)\to \mathrm{NaCl}\left(\mathrm{aq}\right)+\mathrm{NaOCl}\left(\mathrm{aq}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$.

(${\mathrm{A}}_{\mathrm{r}}$ values: $\mathrm{Na}=23.0; \mathrm{Cl}=35.5; \mathrm{O}=16.0$)

Write an ionic equation for this reaction.

Calcium oxide reacts with hydrochloric acid according to the equation:

$\mathrm{CaO}+2\mathrm{HCl}\to {\mathrm{CaCl}}_2+{\mathrm{H}}_2\mathrm{O}$.

${\mathrm{A}}_{\mathrm{r}}$ values: $\mathrm{H}=1.0; \mathrm{O}=16.0; \mathrm{Cl}=35.5; \mathrm{Ca}=40.1$

Calculate the mass of calcium chloride formed when $28.05 \mathrm{g}$ of calcium oxide reacts with excess hydrochloric acid.

Calcium oxide reacts with hydrochloric acid according to the equation:

$\mathrm{CaO}+2\mathrm{HCl}\to {\mathrm{CaCl}}_2+{\mathrm{H}}_2\mathrm{O}$.

${\mathrm{A}}_{\mathrm{r}}$ values: $\mathrm{H}=1.0; \mathrm{O}=16.0; \mathrm{Cl}=35.5; \mathrm{Ca}=40.1$

Calculate the mass of hydrochloric acid that reacts with $28.05 \mathrm{g}$ of calcium oxide.

Calcium oxide reacts with hydrochloric acid according to the equation:

$\mathrm{CaO}+2\mathrm{HCl}\to {\mathrm{CaCl}}_2+{\mathrm{H}}_2\mathrm{O}$.

${\mathrm{A}}_{\mathrm{r}}$ values: $\mathrm{H}=1.0; \mathrm{O}=16.0; \mathrm{Cl}=35.5; \mathrm{Ca}=40.1$

Calculate the mass of water produced when $28.05 \mathrm{g}$ calcium oxide reacts with excess of hydrochloric acid.

When ammonia gas and hydrogen chloride gas mix together, they react to form a solid called ammonium chloride.

${\mathrm{A}}_{\mathrm{r}}$ values: $\mathrm{H}=1.0; \mathrm{N}=14.0; \mathrm{Cl}=35.5$

Write a balanced equation for this reaction, including state symbols.

When ammonia gas and hydrogen chloride gas mix together, they react to form a solid called ammonium chloride.

${\mathrm{A}}_{\mathrm{r}}$ values: $\mathrm{H}=1.0; \mathrm{N}=14.0; \mathrm{Cl}=35.5$

Calculate the molar masses of ammonia, hydrogen chloride and ammonium chloride.