A sample of mercury (II) oxide is placed in a 10.00 L evacuated container and he

Question

A sample of mercury (II) oxide is placed in a 10.00 L evacuated container and heated until it decomposes entirely to mercury metal and oxygen gas. The container is then cooled to 22.5 degress celcius. One now finds that the gas pressure inside the container is 0.871 atm. What is the mass of the mercury (II) oxide that was originally placed into the container?

Explanation / Answer

2Hgo -> 2Hg + O2 . P=0.871 atm, T= 22.5 deg=295.65 K, V = 10 L . therefore for O2 n = PV/(RT)= 0.871x10/(0.0821x295.65)=0.3588 moles, therefore moles of Hg=2 x moles of O2=0.7177. Therefore moles of HgO= 0.7177, therefore mass= moles x Molar mass=0.7177x(200.59+16)=155.44 gm.

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