Question

I need help on balancing the equations and on what type of reaction it is.

Answer 1

Explanations:

Given the balanced chemical reaction expressed as:

`2Au_2O_3\rightarrow4Au+3O_2`

A Redox reaction is a reaction that involves the transfer of electrons and changes in the oxidation state between the elements.

The given chemical equation is therefore an oxidation-reduction reaction since it involves a change in the oxidation state of the elements.

Determine the moles of Au₂O₃

`\begin{gathered} \text{Mole = }\frac{Mass}{Molar\text{ mass}} \\ \text{Mole of Au}_2O_3=\frac{10g}{441.93g\text{/mol}} \\ \text{Mole of Au}_2O_3=0.02263\text{moles} \end{gathered}`

According to stochiometry, you can see that 2 moles of Gold(III)oxide produce 4 moles of Gold. Hence the moles of Gold produced will be:

`\begin{gathered} \text{moles of Gold=}(0.02263*4)/(2) \\ \text{moles of Gold=}0.02263*2 \\ \text{moles of Gold=}0.0453\text{moles} \end{gathered}`

Determine the mass of Gold.

`\begin{gathered} \text{Mass of Gold=moles}* molar\text{ mass} \\ \text{Mass of Gold=}0.0453*196.97 \\ \text{Mass of Gold}=8.91\text{grams} \end{gathered}`

Next is determining the mole of Oxygen

According to stochiometry, you can see that 2 moles of Gold(III)oxide produce 3 moles of Oxygen. Hence the moles of Oxygen produced will be:

`\begin{gathered} \text{moles of Oxygen=}(0.02263*3)/(2) \\ \text{moles of Oxygen}=0.033945\text{moles} \end{gathered}`

Determine the mass of oxygen produced

`\begin{gathered} \text{Mass of O}_2=moles*\text{Molar mass} \\ \text{Mass of O}_2=0.033945*16 \\ \text{Mass of O}_2=0.543\text{grams} \end{gathered}`

Hence the mass of oxygen produced is 0.543 grams