Answer:
(a) 1.92 moles of Bi produced.
(b) 80.6 grams
Explanation:
Balanced equation: Bi2O3(s) + 3C(s) → 2Bi(s) + 3CO(g)
1st find moles of Bi2O3:
Bi2O3 has Mr of 466 and mass of 447 g
2nd find moles of Bi:
Bi2O3 : 2Bi
→ 1 : 2 ------ this is molar ratio.
→ 0.959227 : (0.959227)*2
→ 0.959227 : 1.91845
→ 0.959227 : 1.92
Therefore 1.92 moles of Bi was produced.
3rd Find moles of 3CO:
Bi2O3 : 3CO
1 : 3
0.959227 : (0.959227 )*3
0.959227 : 2.87768
3CO has 2.87768 moles and we know the Mr is 28.
g
Therefore 80.575 grams of CO was produced.
Answer:
Magnesium oxide
Explanation:
When magnesium reacts with oxygen, the magnesium atoms donate electrons to O2 molecules and thereby reduce the oxygen. Magnesium therefore acts as a reducing agent in this reaction. The O2 molecules, on the other hand, gain electrons from magnesium atoms and thereby oxidize the magnesium.
he could heat up the mixture
hope this help :)
Answer:
1) SO₄
²⁻ : (+6)
H₂S : (-2)
Explanation:
a) <u>Sulfate reducers</u> are widespread in muds and other sediments, water-logged soils, etc., environments that contain SO₄ ²⁻ and become anoxic as a result of microbial decomposition.
Sulfate (SO₄ ²⁻), the most oxidized form of sulfur (+6), <u>is reduced</u> by these
sulfate-reducing bacteria. The end product of sulfate reduction is hydrogen sulfide, H₂S, (oxidation number -2) an important natural product that participates in many biogeochemical processes. The H₂S they generate is responsible for the pungent smell (like that of rotten eggs) often encountered near coastal ecosystems. When sulfate-reducing bacteria grow, the H₂S formed from SO₄ ²⁻ reduction combines with the ferrous iron to form black, insoluble ferrous sulfide, which is not toxic. This is important for the conservation of the environment.
b) The net ionic equation under acidic conditions is:
4 H₂ + SO₄²⁻ + H⁺ → HS⁻ + 4 H₂O
Global reaction: SO₄²⁻ + 2H⁺ → H₂S + O₂