In the following reaction, what mass of mercury(II) oxide, HgO,
would be required to produce 199 L of oxygen, O2, measured at
STP?
2HgO(s) --> 2Hg(s)+O2(g)
AT STP, 1 mol of any gas occupy 22.4 L
So,
moles of O2 produced = volume of O2 / molar volume
= 199 / 22.4
= 8.884 mol
From reaction,
moles of HgO = 2*moles of O2
= 2*8.884 mol
= 17.768 mol
Molar mass of HgO = 1*MM(Hg) + 1*MM(O)
= 1*200.6 + 1*16.0
= 216.6 g/mol
we have below equation to be used:
mass of HgO,
m = number of mol * molar mass
= 17.768 mol * 216.6 g/mol
= 3.85*10^3 g
Answer: 3.85*10^3 g
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