2HgO (s) --> 2Hg(l) + O2 (g)
2HgO(s) + heat ---> 2Hg + O2
I'm pretty sure you have your formula wrong. Oxygen has a net charge of -2. So therefore, the equation must be written as 2Hg with a net charge of 2+ plus CO3 with a net charge of 2-. So, you do your math here, and the answer should be Hg3CO3
Dimethylmercury = (CH3)2Hg and molar mass = 230.7 g/moleatomic mass Hg = 200.6Percent Hg by mass = 200.6/230.7 (x100) = 87.0 %.This is the percent in 4.75 g or 47.5 g or in 475 g. It won't change. If you need the mass of mercury in 4.75 g of diemthyl mercury, then it will be 4.75 g x 0.87 = 4.13 g4.13 g/4.75 g (x100) = 87% Hg
well, you know the basic H2 + O2 ---> H2O right? so, if you balance it, it will be 2H2 + O2 ---> 2H2O. So, you just take the front numbers out so, it will be H2 + O2 ---> H2O. easy. ^_^ !
2HgO (s) --> 2Hg(l) + O2 (g)
2HgO(s) + heat ---> 2Hg + O2
2HgO(heat) ----> 2Hg + O2
The chemical formula (NOT: equation) for mercury oxide is (there are two possibillities):Mercury(I) oxide (mercurous oxide), Hg2O.Mercury(II) oxide (mercuric oxide), HgO
2HgO------->2Hg+O2
2 molecules of mercuric oxide yields 2 atoms of mercury and 2 of oxygen.
hgo is decomposed when exposed to light of 500 degrees
2Hg atoms and 2Cl atoms for a total of 4 atoms.
The formula for mercurous peroxide is Hg2O2.
Mercuric oxide will decompose into elemental Mercury and gaseous oxygen
This equation is 2 H2O (liquid) = 2 H2 (gas) + O2 (gas)There must be 4 atoms / 2 diatomic molecules of hydrogen on each side to yield O2This is the electrolysis of water.
I'm pretty sure you have your formula wrong. Oxygen has a net charge of -2. So therefore, the equation must be written as 2Hg with a net charge of 2+ plus CO3 with a net charge of 2-. So, you do your math here, and the answer should be Hg3CO3