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3 years ago

How many moles of aluminum oxide would form if 12.5 moles of aluminum burned

Chemistry

1 answer:

jarptica [38.1K]3 years ago

7 0

Balance it:

So you need 2 Al and 3 O2 to make 2 Al2O3 (aluminum oxide).

I'm going to assume you have all the O2 you need.

Since 2 mols of Al is needed to make 2 mols of the product, it's a 1:1 ratio. You get as much aluminum oxide for as much aluminum you burn.

So 12.5 mols if there is not a lack of the O2.

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FeSO4 • 7H2O

Mrac [35]

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 %

4 0

4 years ago

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Can anyone answer this question?

-Dominant- [34]

Hello! Those are called the isotopes of those elements!! They have more than just one form and each has it’s own AMU’s so the multiple numbers above different elements, represent the isotopes of those elements. Carbon is a good one just for one example.

Hope this helps you out! Questions please just ask! Thanks!

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(a) what product or products would you expect to obtain by the addition of bromine to cis-cinnamic acid, assuming that it reacts

Free_Kalibri [48]

If the totaling of bromine to cis-cinnamic acid uses the same mechanism or device as the addition to trans-cinnamic acid, addition of bromine only transpires on the top (syn) and not the bottommost face (anti). Therefore, bromine added to cis-cinnamic only adds to the same face (syn addition) as a result producing only threo dibromides.

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Convert 256.3 g sodium carbonate to formula units

nalin [4]

Answer:

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Explanation:

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3 years ago

How many moles of aluminum oxide would form if 12.5 moles of aluminum burned​

How many moles of aluminum oxide would form if 12.5 moles of aluminum burned