The material which is used as source for commercial production aluminum is bauxite.
The aluminum can be extracted from bauxite ore by the process of Bayer process.
In the Bayer process, bauxite ore is heated in the pressure vessel along with a caustic soda solution (sodium hydroxide) at a temperature between 150 to 200 °C. At this temperatures, the aluminium is dissolved in the solution as sodium aluminate in the extraction process. After separation of the residue by filtering, when the liquid is cooled gibbsite is precipitated and then it is seeded with fine-grained aluminum hydroxide crystals from previous extractions. The precipitation take 7-19 days without the addition of seed crystals.
This extraction process converts the aluminium oxide to soluble sodium aluminate, NaAlO2, which afterward converted into aluminum hydroxide and then into aluminum oxide.
Thus, we concluded that the material which is used as source for commercial production aluminum is bauxite ore.
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We’re going to use the mass percent formula shown below:
For the percent by mass N, we’re going to rewrite the equation as:
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Problem Details
Calculate the mass percent composition of nitrogen in each nitrogen-containing compound:
c. NO2
Answer:
linear
Explanation:
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dilution
V₁M₁=V₂M₂
V₁.12 = 100.6
V₁=50 ml
Add water 50 ml to 50 ml 12 M
Answer:
<u>Volume versus temperature, because they are also directly proportional</u>
Explanation:
The <u>Ideal Gas Equation</u> is :
<u>Evaluating the options</u>
- V ∝ P [Incorrect, because V ∝ 1/P, and graph will be a parabola]
- V ∝ T [Correct, because V ∝ T, and graph is a straight line]
- V ∝ 1/P [Incorrect, because graph is not similar]
- V ∝ 1/T [Incorrect, because V ∝ T]