The maximum mass of B₄C that can be formed from 2.00 moles of boron (III) oxide is 55.25 grams.
<h3>What is the stoichiometry?</h3>
Stoichiometry of the reaction gives idea about the relative amount of moles of reactants and products present in the given chemical reaction.
Given chemical reaction is:
2B₂O₃ + 7C → B₄C + 6CO
From the stoichiometry of the reaction, it is clear that:
2 moles of B₂O₃ = produces 1 mole of B₄C
Now mass of B₄C will be calculated by using the below equation:
W = (n)(M), where
- n = moles = 1 mole
- M = molar mass = 55.25 g/mole
W = (1)(55.25) = 55.25 g
Hence required mass of B₄C is 55.25 grams.
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The higher the velocity the faster it moves
To answer this item, we assume that oxygen behaves ideally such that it is able to fulfill the following equation,
PV = nRT
If we are to retain constant the variable n and V.
The percent yield can therefore be solved through the following calculation,
n = (10.5 L)/(22.4 L) x 100%
Simplifying,
n = 46.875%
Answer: 48.87%
The pounds of alum produced when 0.26 g of hydrogen was produced are 0.0434 lb.
First, let's convert 0.126 g of hydrogen to moles using its molar mass (2.02 g/mol).
Let's consider the steps to make alum (KAl(SO₄)₂⋅12H₂O) from aluminum (Al).
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2 Al(s) + 2 KOH(aq) + 6 H₂O(l) →2 KAl(OH)₄(aq) + 3 H₂(g)
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2 KAl(OH)₄(aq) + H₂SO₄(aq) → 2 Al(OH)₃(s) + K₂SO₄(aq) + 2 H₂O(l)
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2 Al(OH)₃(s) + H₂SO₄(aq) → Al₂(SO₄)₃(aq) + 6 H₂O(l)
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K₂SO₄(aq) + Al₂(SO₄)₃(aq) + 24 H₂O(l) → 2 KAl(SO₄)₂⋅12H₂O(s)
To relate H₂ to KAl(SO₄)₂⋅12H₂O, we need to consider the appropriate molar ratios:
- In step 1, the molar ratio of H₂ to KAl(OH)₄ is 3:2.
- In step 2, the molar ratio of KAl(OH)₄ to Al(OH)₃ is 2:2.
- In step 3, the molar ratio of Al(OH)₃ to Al₂(SO₄)₃ is 2:1.
- In step 4, the molar ratio of Al₂(SO₄)₃ to KAl(SO₄)₂⋅12H₂O is 1:2.
The moles of KAl(SO₄)₂⋅12H₂O produced from 0.0624 moles of H₂ are:
The molar mass of alum is 474.38 g/mol. The mass corresponding to 0.0416 moles is:
Finally, we convert 19.7 grams to pounds using the conversion factor 1 lb = 454 g.
The pounds of alum produced when 0.26 g of hydrogen was produced are 0.0434 lb.
You can learn more about molar ratios here: brainly.com/question/15973092