There are 2 binary comp of Hg and O. Heating either of them results in the decompostion of the cmpd, with O gas escaping into the atmosphere while leaving a residue of pure Hg. Heating .6498 g of one of the cmpd leaves a residue of .6018 g. Heating .4172 g of the other cmpd results in a mass loss of .016. Determine the empirical formula of each cmpd.
Please show the work.
2007-08-21 16:23:54 · 3 answers · asked by Krazym0nkey 2 in Science & Mathematics ➔ Chemistry
For the first compound, the weight of the contained mercury is 0.6018g (the weight of the residue).
The weight of contained oxygen is: 0.6498-0.6018 = 0.048g
To get molar ratios we need to divide by the respective masses of the elements:
0.6018g/200.6g/mol = 0.003mol mercury
0.048g/16g/mol = 0.003mol oxygen
The molar ratio is 1 to 1 or the formula HgO
For the second one the weight of the mercury is: 0.4172g- 0.016g = 0.4012
The weight of the oxygen is 0.016g
So, we do the same thing as before to get molar ratio.
0.4012g/200.6g/mol = 0.002mol mercury
0.016g/16g/mol = 0.001mol oxygen
The molar ratio is 2 to 1, the formula is Hg2O
2007-08-21 17:07:01 · answer #1 · answered by Flying Dragon 7 · 0⤊ 0⤋
Hg forms compounds in two oxidation states: Hg+ and Hg ++
The atomic mass of Hg is 200.61 amu. The atomic mass of O is 16.00. You should be able to solve the problems with this information.
2007-08-22 00:01:38 · answer #2 · answered by skipper 7 · 0⤊ 0⤋
Hey man! You're hilarious. I always ask for help on here and no one freakin' answers. Try begging people to death. lol. And you actually expect them to show work. lol.
Sorry... I don't know the answer to your difficult question. Bye now! LMAO.
2007-08-21 23:38:16 · answer #3 · answered by Anonymous · 0⤊ 0⤋