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Aliun [14]
3 years ago
8

How many grams of aluminum in required to produce 17.5 g of hydrogen

Chemistry
1 answer:
azamat3 years ago
6 0

Mass of Aluminum = 157.5 g

<h3>Further explanation</h3>

Given

17.5 g of Hydrogen

Required

Mass of Aluminum

Solution

Reaction

2Al + 3H₂SO₄ → Al₂(SO₄)₃ + 3H₂

mol Hydrogen :

= mass : molar mass

= 17.5 g : 2 g/mol

= 8.75

From the equation, mol Al :

= 2/3 x mol H₂

= 2/3 x 8.75

= 5.83

Mass Al :

= 5.83 x 27 g/mol

= 157.5 g

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Answer:

6.25 μg/mL

Explanation:

When a dilution is made, the mass of the solute is conserved (Lavoiser's law), so the mass pipetted will be the mass in the assay. The mass is the concentration (C) multiplied by the volume (V). If the pipet solution is called 1, and the assay 2:

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3 years ago
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Answer:

Explanation:

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