Question

What mass of oxygen would be released by the thermal decomposition of 918.7 grams of Mercury (II) Oxide?

HgO --> Hg + O2

Answer 1

Step-by-step explanation:

`(918.7 g)/(1) *(1)/(216.59m ) = 4.241 mol` To start off the mol of HgO must be found.

After that the molar ratio between HgO and O must be found but in this case its 1:1

`4.241 mol HgO*(1 molO)/(1molHgO) = 4.241 mol O` the mols of HgO is put on the bottom to cancel out with the other one leaving just mols of oxygen. Finally to find g of oxygen it must be multiplied by its molar mass.

`(4.241 molO)/(1) * (15.999 g)/(mol) = 67.85 g` Oxygen