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Assoli18 [71]
3 years ago
10

How many grams of iron metal do you expect to be produced when 325 grams of an 87.5 percent by mass iron (II) nitrate solution r

eact with excess aluminum metal? Show all of the work needed to solve this problem.
2Al (s) + 3Fe(NO3)2 (aq) yields 3Fe (s) + 2Al(NO3)3 (aq
Chemistry
1 answer:
Basile [38]3 years ago
6 0
2Al (s) + 3Fe(NO3)2 (aq) → 3Fe (s) + 2Al(NO3)3 (aq)

Find the pure amount of iron nitrate solution:

325 g x 87.5% = 284.375 g

Convert 284.375g into mols by dividing by molar mass of the iron nitrate solution

Molar mass of iron nitrate =  55.85 g/mol + 2x14g/mol + 6x16g/mol = 179.85 g/mol

Moles of iron nitrate = 284.375 g / 179.85 g/mol = 1.58

Stoichiometry

3 mols of iron nitrate / 3 mols of iron = 1.58 mols of iron nitrate / x mols of iron

x = 1.58 mols of iron.

Convert that in grams by multiplying by the molar mass of iron

grams of iron = 1.58 mol x 55.85 g/mol = 88.24 g
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Answer:

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Molecular formula = C₆H₁₂O₆

Explanation:

Given data:

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Empirical formula = ?

Molecular formula = ?

Solution:

Empirical formula:

It is the simplest formula gives the ratio of atoms of different elements in small whole number

Number of gram atoms of H = 3.36 / 1.01 = 3.3

Number of gram atoms of O = 26.64 / 16 = 1.7

Number of gram atoms of C = 20 / 12 = 1.7

Atomic ratio:

            C                      :        H            :         O

           1.7/1.7                :     3.3/1.7       :       1.7/1.7

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C : H : O = 1 : 2 : 1

Empirical formula is CH₂O.

Molecular formula:

Molecular formula = n (empirical formula)

n = molar mass of compound / empirical formula mass

Empirical formula mass = CH₂O = 12×1 + 2× + 16

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n = 180.156 / 30

n = 6

Molecular formula = n (empirical formula)

Molecular formula = 6 (CH₂O)

Molecular formula = C₆H₁₂O₆

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