Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: In a particular experiment, the reaction of 2.5 g of Al with 2.5 g of O2 produced 3.5 g of Al2O3. The % yield of the reaction is __________.
Answers
Answer:
The % yield of the reaction is 73.8 %
Explanation:
To solve this, we list out the given variables thus
Mass of aluminium in the experiment = 2.5 g
mass of oxygen gas in the experiment = 2.5 g
Molar mass of aluminium = 26.98 g/mol
molar mass of oxygen O₂ = 32 g/mol
The reaction between aluminium and gaseous oxygen can be written as follows
4Al + 3O₂ → 2Al₂O₃
Thus four moles of aluminium forms two moles of aluminium oxide
Thus (2.5 g)÷(26.98 g/mol) = 0.093 mole of aluminium and
(2.5 g)÷(32 g/mol) = 0.078125 moles of oxygen
However four moles of aluminium react with three moles of oxygen gas O₂
1 mole of aluminum will react with 3/4 moles of oxygen O₂ and 0.093 mole of aluminium will react with 0.093*3/4 moles of O₂ = 0.0695 moles of Oxygen hence aluminium is the limiting reagent and we have
1 mole of oxygen will react with 4/3 mole of aluminium
∴ 0.078125 mole of oxygen will react with 0.104 moles of aluminium
Therefore 0.093 mole of aluminium will react with O₂ to produce 2/4×0.093 or 0.0465 moles of 2Al₂O₃
The molar mass of 2Al₂O₃ = 101.96 g/mol
Hence the mass of 0.0465 moles = number of moles × (molar mass)
= 0.0465 moles × 101.96 g/mol = 4.74 g
The of aluminium oxide Al₂O₃ is 4.74 g, but the actual yield = 3.5 g
Therefore the Percentage yield = ×100 =
× 100 = 73.8 % yield
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When the temperature of a substance decreases, the average kinetic energy of its particles also decreases. This is because the temperature of a substance is proportional to the average kinetic energy of its particles. The slower the particles move, the lower the kinetic energy.
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The question refers to the relationship between the temperature of a substance and the average kinetic energy of its particles. According to the kinetic-molecular theory, the temperature of a substance is proportional to the average kinetic energy of its particles. When the temperature of a substance rises, the particles vibrate more in solids or move more rapidly in liquids and gases, indicating an increase in kinetic energy. Conversely, if the temperature decreases, the kinetic energy also decreases, and the particles move more slowly.
For instance, when the temperature of a gas increases, its average kinetic energy increases, more molecules have higher speeds and fewer molecules have lower speeds. The distribution shifts towards higher speeds overall. If the temperature decreases, the opposite happens: the average kinetic energy decreases, more molecules have lower speeds and fewer molecules have higher speeds. The distribution shifts towards lower speeds overall.
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