At STP,
p = 1 atm
T = 273 K
R = 0.0821 L.atm/K.mol
V = 0.750 L
n = ?
Ideal gas equation,
p V = n R T
1 X 0.750 = n X 0.0821 X 273
0.750 = n X 22.4
n = 0.750 / 22.4
n = 0.0335 mol
The given balanced equation is,
2 HgO (s) --------------> 2 Hg (l) + O2 (g)
From the balanced equation,
1 mol of O2 is produced from 2 mol of HgO
Then,
0.0335 mol of O2 is produced from 2 X 0.0335 = 0.0670 mol of HgO
Moles of HgO required = 0.0670 mol
Molar mass of HgO = 216.59 g/mol
Mass of HgO = Moles X molar mass
= 0.0670 X 216.59
= 14.5 g.
Therefore,
Mass of mercuric oxide decomposed = 14.5 g.
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