Mercury(II) oxide (HgO) decomposes to form mercury (Hg) and oxygen (O2). The balanced chemical equation is shown below. 2HgO Rig

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Mercury(II) oxide (HgO) decomposes to form mercury (Hg) and oxygen (O2). The balanced chemical equation is shown below. 2HgO Rig

ht arrow. 2Hg O2 The molar mass of HgO is 216. 59 g/mol. 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 7. 813 15. 63 73. 87.

Chemistry

1 answer:

BigorU [14] · Answer 1 · 2022-09-27T00:12:11+03:00

Taking into account the reaction stoichiometry, the correct answer is the third option: 15.63 moles of HgO are needed to produce 250 g of O₂.

In first place, the balanced reaction is:

2 HgO → 2 Hg + O₂

By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

HgO: 2 moles
Hg: 2 moles
O₂: 1 moles

The molar mass of the compounds is:

HgO: 216.59 g/mole
Hg: 200.59 g/mole
O₂: 32 g/mole

Then, by reaction stoichiometry, the following mass quantities of each compound participate in the reaction:

HgO: 2 moles× 216.59 g/mole= 433.18 grams
Hg: 2 moles× 200.59 g/mole= 401.18 grams
O₂: 1 mole× 32 g/mole= 32 grams

Then the following rule of three can be applied: if by reaction stoichiometry 32 grams of O₂ are produced by 2 moles of HgO, 250 grams of O₂ are produced from how many moles of HgO?

$moles of HgO=\frac{250 grams of O_{2} x2 moles of HgO}{32grams of O_{2}}$

<u><em>moles of HgO= 15.625 moles≅ 15.63 moles</em></u>

Finally, the correct answer is the third option: 15.63 moles of HgO are needed to produce 250 g of O₂.

Learn more about reaction stoichiometry: