Question

Mercury(ii) oxide (hgo) decomposes to form mercury (hg) and oxygen (o2). the balanced chemical equation is shown below. 2hgo right arrow. 2hg o2 the molar mass of o2 is 32.00 g/mol. how many moles of hgo are needed to produce 250.0 g of o2? 3.906 moles 7.813 moles 15.63 moles 73.87 moles

Answer 1

Decomposition reaction results in the formation of the products by splitting the reactants. Moles of mercury(ii) oxide needed are 15.63 moles.

What are moles?

Moles are the ratio of mass and the molar mass of the compound or the molecule.

Moles of oxygen are calculated as:

$\begin{aligned}\rm n &= \rm \dfrac {mass}{molar\; mass}\\\\&= \dfrac{250}{32}\\\\&= 7.8125 \;\rm moles\end{aligned}$

The balanced chemical reaction can be shown as,

$\rm 2HgO \rightarrow 2Hg + O_{2}$

From the reaction, it can be said that 1 mole of oxygen requires 2 moles of mercury oxide.

Moles of mercury oxide are calculated as:

$\begin{aligned} \rm n HgO& = (7.8125 \;\rm moles \; O_{2}) \times (\dfrac{2 \;\rm moles\; HgO}{1 \;\rm mole \; O_{2}})\\\\\rm n HgO &= 15.625 \;\rm moles \end{aligned}$

Therefore, option C. 15.63 moles of mercury (II) oxide is needed.

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