Calculate the number of particles present in $9.80 \mathrm{g}$ of phosphoric acid, ${\mathrm{H}}_3{\mathrm{PO}}_4$.

Calculate the number of particles present in $60.77 \mathrm{g}$ of iron(II) sulfate, ${\mathrm{FeSO}}_4$.

Calculate the number of particles present in $12.10 \mathrm{g}$ of ethanoic acid, ${\mathrm{C}}_2{\mathrm{H}}_4{\mathrm{O}}_2$.

Calculate the number of particles present in $6.40 \mathrm{g}$ of sulfur dioxide, ${\mathrm{SO}}_2$.

Calculate the volume of each of the following samples of gases at STP $7.6 \mathrm{g}$ of argon, $\mathrm{Ar}$ (Give the value rounded-off to one decimal place)

Calculate the volume (in ${\mathrm{dm}}^3$) of the following sample of gas at STP, $100 \mathrm{g}$ of ethene, ${\mathrm{C}}_2{\mathrm{H}}_4$. (Give the value rounded-off to one decimal place)

Magnesium burns in the presence of oxygen to form the metal oxide, magnesium oxide. This oxidation reaction is commonly performed in a school laboratory. A student weighs out $18.0 \mathrm{g}$ of magnesium for the reaction. The equation for the reaction is as follows:

$\mathrm{Mg}\left(\mathrm{s}\right) +{\mathrm{O}}_2\left(\mathrm{g}\right) \to \mathrm{MgO}\left(\mathrm{s}\right)$

Balance the chemical equation.

Magnesium burns in the presence of oxygen to form the metal oxide, magnesium oxide. This oxidation reaction is commonly performed in a school laboratory. A student weighs out $18.0 \mathrm{g}$ of magnesium for the reaction. The equation for the reaction is as follows:

$\mathrm{Mg}\left(\mathrm{s}\right) +{\mathrm{O}}_2\left(\mathrm{g}\right) \to \mathrm{MgO}\left(\mathrm{s}\right)$

Calculate the number of moles of the reactant, magnesium. (Give the value rounded-off to two decimal places)

Magnesium burns in the presence of oxygen to form the metal oxide, magnesium oxide. This oxidation reaction is commonly performed in a school laboratory. A student weighs out $18.0 \mathrm{g}$ of magnesium for the reaction. The equation for the reaction is as follows:

$\mathrm{Mg}\left(\mathrm{s}\right) +{\mathrm{O}}_2\left(\mathrm{g}\right) \to \mathrm{MgO}\left(\mathrm{s}\right)$

If oxygen is in excess and all the magnesium is used up, calculate the number of moles of magnesium oxide formed.