Question

Mercury(II) oxide (HgO) decomposes to form mercury (Hg) and oxygen (O2). The balanced chemical equation is shown below.2HgO Right arrow. 2Hg + O2The 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?

Answer 1

C-15.63

Step-by-step explanation:

Correct on EDGE

Answer 2

Answer: 15.62 moles of
`HgO` are needed to produce 250.0 g of
`O_2`

Step-by-step explanation:

To calculate the moles :

`\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}`

`\text{Moles of} O_2=(250.0g)/(32g/mol)=7.812moles`

`2HgO\rightarrow 2Hg+O_2`

According to stoichiometry :

1 mole of
`O_2` is produced from decomposition of = 2 moles of
`HgO`

Thus 7.812 moles of
`O_2` will be produced from decomposition of =
`(2)/(1)* 7.812=15.62moles` of
`HgO`

Thus 15.62 moles of
`HgO` are needed to produce 250.0 g of
`O_2`