A sample of mercury(II) oxide is placed in a 5.00 L evacuated container and heat

Question

A sample of mercury(II) oxide is placed in a 5.00 L evacuated container and heated until it decomposes entirely to mercury metal and oxygen gas. The container is then cooled to 25 A sample of mercury(II) oxide is placed in a 5.00 L evacuated container and heated until it decomposes entirely to mercury metal and oxygen gas. The container is then cooled to 25 A sample of mercury(II) oxide is placed in a 5.00 L evacuated container and heated until it decomposes entirely to mercury metal and oxygen gas. The container is then cooled to 25

Explanation / Answer

PV = nRT

P = gas pressure in atm = 1.73
V = volume of container in L = 5.00
n = moles of O2 = ?
R = gas constant = 0.0821 L atm / K mole
T = Kelvin temperature = 25 C + 273 = 298 K

n = PV / RT = (1.73)(5.00) / (0.0821)(298) = 0.354 moles O2

The equation for the decomposition of HgO is

2HgO ==> 2Hg + O2

1 mole of HgO produces 1 mole of O2.

0.354 moles O2 x (1 mole HgO / 1 mole O2) = 0.354 moles HgO

0.354 moles HgO x (216.6 g HgO / 1 mole HgO) = 76.7 g HgO

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