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2 years ago

In the oxidation of iron; how many grams of iron (III) oxide will be produced from 6.20 mol of Fe?

Chemistry

1 answer:

Flura [38]2 years ago

8 0

Answer:

496 g of Fe₂O₃.

Explanation:

The balanced equation for the reaction is given below:

4Fe + 3O₂ —> 2Fe₂O₃

From the balanced equation above,

4 moles of Fe reacted to produce 2 moles of Fe₂O₃.

Therefore, 6.20 moles of Fe will react to produce = (6.20 × 2)/4 = 3.1 moles of Fe₂O₃

Finally, we shall determine the mass of 3.1 moles of Fe₂O₃. This can be obtained as follow:

Mole of Fe₂O₃ = 3.1 moles

Molar mass of Fe₂O₃ = (56 × 2) + (3×16)

= 112 + 48

= 160 g/mol

Mass of Fe₂O₃ =?

Mass = mole × molar mass

Mass of Fe₂O₃ = 3.1 × 160

Mass of Fe₂O₃ = 496 g

Therefore, 496 g of Fe₂O₃ were produced from the reaction.

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Answer:

Explanation:

From the given information:

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$= 2.00 L \times 0.007118 \dfrac{mol}{L} \times \dfrac{24.31 \ g}{1 \ mol}$

= 0.3461 g

Mass of Mg²⁺ = 346.1 mg

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2 years ago

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posledela

6.00g because it is a balanced equation

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Read 2 more answers

Rutherford used a gold foil experiment and discovered what part of an atom

slamgirl [31]

Hihi!

During Rutherford's experiment of shooting particles through a sheet of gold foil he had discovered that some were deflected! This had proved that an atom is actually a small dense nucleus surrounded by orbiting electrons!

I hope I helped!
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Answer:

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