How many moles of Fe3O4 are required to supply enough iron to prepare 0.472mol Fe2O3 ?
1 answer:
The combustion reaction for Fe₃O₄ in an oxygen molecule O₂ yields Fe₂O₃.
The number of moles of Fe₃O₄ required to prepare 0.472 moles of Fe₂O₃ is:
0.315 moles
The reaction equation is:
From the above reaction;
4 moles of Fe₃O₄ react with oxygen to produce 6 moles Fe₂O₃.
i.e.
Fe₃O₄ : Fe₂O₃ = 4 : 6
Fe₃O₄ : Fe₂O₃ = 2 : 3
= 0.315 moles
Therefore, we can conclude that 0.472 moles of Fe₂O₃ are prepared from 0.315 moles of Fe₃O₄.
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2.083 Liters of 6.0 M solution sulfuric acid is required. This solved using molecular calculations and Titration.
Solution:
Moles of hydrogen gas =
Then 12.5 moles of hydrogen will be obtained from Moles of Sulfuric acid = 12.5 mol
Molarity of the sulfuric acid solution = 6.0 M = 6 mol/ l
6M =
where V is the volume needed
V = 2.083 l
<h3>What is Titration?</h3>- Titration, commonly referred to as titrimetry, is a typical quantitative chemical analysis method used in laboratories to ascertain the unidentified quantity of an analyte .
- Titration is frequently referred to as volumetric analysis because it relies heavily on volume measurements. The titrant or titrator is a reagent that is prepared as a standard solution.
- To determine concentration, a solution of the analyte or titrand reacts with a known concentration and volume of the titrant. The titration volume is the amount of titrant that has responded.
- Titrations come in a variety of forms with various protocols and objectives. Redox and acid-base titrations are the two most typical types of qualitative titrations.
To learn more about titration with the given link
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Answer:
Idk if this is right but i hope it helps... sorry if it's wrong
Explanation:
