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4 years ago

FeSO4 • 7H2O

Chemistry

2 answers:

ziro4ka [17]4 years ago

8 0

Answer:

The percent by mass of water in the hydrate is 45.4%

The percent by mass of the anhydrous salt in the hydrate is 54.6%

Explanation:

Mrac [35]4 years ago

4 0

Answer:

1. Percent by mass of H₂O = 45.3%

2. Percent by mass of anhydrous Salt (FeSO₄) = 54.7 %

Explanation:

Data Given

Formula of the Molecule = FeSO₄ • 7H₂O

% by mass water (H₂O) = ?

% by mass FeSO₄ = ?

________________________________________

> First of all find the atomic masses of each component in a molecule

For H₂O atomic masses are given below

H = 1 g/mol

O = 16 g/mol

> Then find the total mass of H₂O in haydrated salt

7H₂O = 7 (2x1 +1x16) g/mol

7H₂O = 7 (2+16) g/mol

7H₂O = 7 (18) g/mol

7H₂O = 126 g/mol

> find total Molar Mass of Molecule:

Molar Mass of FeSO₄ • 7H₂O = [56+ 32 + 16x4] + 7(2+16)

Molar Mass of FeSO₄ • 7H₂O = [56+ 32 + 64] + 126

Molar Mass of FeSO₄ • 7H₂O = 278

Now to find the mass by percent of H₂O

Formula used to find the mass by percent of a component

Percent composition of H₂O = mass of H₂O in Molecule / molar mass of FeSO₄ • 7H₂O x 100%

Put the values

Percent by mass of H₂O = 126 (g/mol) / 278 (g/mol) x 100%

Percent by mass of H₂O = 0.4532 x 100%

Percent by mass of H₂O = 45.3%

_______________________________________________

> First of all find the atomic masses of each component in a molecule

For anhydrus salt (FeSO₄) atomic masses are given below

Fe = 56 g/mol

S= 32 g/mol

O = 16 g/mol

> Then find the total mass of FeSO₄ in haydrated salt

FeSO₄ = (56x1 + 32 + 4x16) g/mol

FeSO₄ = ( 56 + 32 + 64) g/mol

FeSO₄ = 152 g/mol

> find total Molar Mass of Molecule:

Molar Mass of FeSO₄ • 7H₂O = [56+ 32 + 16x4] + 7(2+16)

Molar Mass of FeSO₄ • 7H₂O = [56+ 32 + 64] + 126

Molar Mass of FeSO₄ • 7H₂O = 278

Now to find the mass by percent of FeSO₄

Formula used to find the mass by percent of a component

Percent composition of FeSO₄ = mass of FeSO₄ in Molecule / molar mass of FeSO₄ • 7H₂O x 100%

Put the values

Percent by mass of FeSO₄ = 152 (g/mol) / 278 (g/mol) x 100%

Percent by mass of FeSO₄ = 0.547 x 100%

Percent by mass of FeSO₄ = 54.7 %

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bixtya [17]

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(c): $FeCl_3+3NH_4OH\rightarrow Fe(OH)_3+3NH_4CI$

Answer: The net ionic equation is $Fe^{3+}(aq)+3OH^{-}(aq)\rightarrow Fe(OH)_3(s)$

Explanation:

Net ionic equation is defined as the equations in which spectator ions are not included.

Spectator ions are the ones that are present equally on the reactant and product sides. They do not participate in the reaction.

(c):

The balanced molecular equation is:

$FeCl_3(aq)+3NH_4OH(aq)\rightarrow Fe(OH)_3(s)+3NH_4Cl(aq)$

The complete ionic equation follows:

$Fe^{3+}(aq)+3Cl^-(aq)+3NH_4^+(aq)+3OH^{-}(aq)\rightarrow Fe(OH)_3(s)+3NH_4^+(aq)+3Cl^-(aq)$

As ammonium and chloride ions are present on both sides of the reaction. Thus, they are considered spectator ions.

The net ionic equation follows:

$Fe^{3+}(aq)+3OH^{-}(aq)\rightarrow Fe(OH)_3(s)$

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