Gary Horner Solutions for Chapter: Function, Exercise 16: Exercise 16

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.

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:

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

What mass of magnesium oxide is produced?

What mass of barium sulfate would be produced when $10 \mathrm{g}$ of barium chloride is completely consumed in the following reaction?

${\mathrm{BaCl}}_2 \left(\mathrm{aq}\right) + {\mathrm{H}}_2{\mathrm{SO}}_4 \left(\mathrm{aq}\right) \to {\mathrm{BaSO}}_4 \left(\mathrm{aq}\right) + 2\mathrm{HCl}\left(\mathrm{aq}\right)$

Copper sulfate reacts with sodium hydroxide to produce a precipitate of copper hydroxide.

${\mathrm{CuSO}}_4 \left(\mathrm{aq}\right) + 2\mathrm{NaOH}\left(\mathrm{aq}\right) \to \mathrm{Cu}{\left(\mathrm{OH}\right)}_2 \left(\mathrm{s}\right) + {\mathrm{Na}}_2{\mathrm{SO}}_4 \left(\mathrm{aq}\right)$

Calculate the mass of sodium hydroxide needed to convert $15.95 \mathrm{g}$ of copper sulfate into copper hydroxide.

Copper sulfate reacts with sodium hydroxide to produce a precipitate of copper hydroxide.

${\mathrm{CuSO}}_4 \left(\mathrm{aq}\right) + 2\mathrm{NaOH}\left(\mathrm{aq}\right) \to \mathrm{Cu}{\left(\mathrm{OH}\right)}_2 \left(\mathrm{s}\right) + {\mathrm{Na}}_2{\mathrm{SO}}_4 \left(\mathrm{aq}\right)$

Calculate the mass of copper hydroxide produced from $15.95 \mathrm{g}$ of copper sulfate.