I am pretty sure it’s five and six
I am pretty sure it’s not three and four
I don’t know about one and two
Hope this helps
The strategy here would be to convert mass to moles and then from moles to the number of atoms.
100.0 g of iron(iii) oxide, or Fe2O3, has a molar mass of 159.687 g/mol. To convert the mass into the number of moles, divide the mass by the molar mass: (100.0 g)(159.687) = 0.6262 moles Fe2O3.
1 mole of any substance is, by definition, equal to 6.022 • 10^23 units of that substance. So to compute the number atoms contained in 0.6262 moles of Fe2O3, multiply (0.6262)(6.022 • 10^23) = 3.771 • 10^23 atoms of iron(iii) oxide, which is your answer (given to four significant figures).
Answer:
There are three possible chemical equations for the combustion of sulfur:
- 2S (s) + O₂ (g) → 2SO (g)
- 2S (s) + 3O₂ (g) → 2SO₃ (g)
Explanation:
<em>Combustion</em> is a reaction with oxygen. The products of the reaction are oxides, and energy is released in the form of heat and light.
<em>Sulfur</em> iis a nonmetal, so the oxide formed is a nonmetal oxide.
The most common oxidation numbers of sulfur are -2, + 2, + 4, and + 6.
The combination of sulfur with oxygen may be only with the positive oxidation numbers (+2, + 4, and +6).
Then you have three different equations for sulfur combustion:
<u>1) Oxidation number +2:</u>
Which when balanced is: 2S(g) + O₂(g) → 2SO(g)
<u>2) Oxitation number +4:</u>
That equation is already balanced.
<u>3) Oxidation number +6:</u>
Which when balanced is: 2S(s) + 3O₂(g) → 2SO₃(g)
Loses 1 atom. in this case, the silver atom achieves a <span>pseudo-noble-gas electron configuration.</span>