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3 years ago

How many grams of iron can be produced from 3.65g of Iron (III) Sulfate? 3Mg + Fe2(SO4)3 --> 3MgSO4 + 2Fe

Chemistry

1 answer:

Tasya [4]3 years ago

3 0

Answer:

Option A. 1.02g of Fe.

Explanation:

Step 1:

The balanced equation for the reaction.

3Mg + Fe2(SO4)3 —> 3MgSO4 + 2Fe

Step 2:

Determination of the mass Fe2(SO4)3 that reacted and the mass of Fe produced from the balanced equation. This is illustrated below:

Molar Mass of of Fe2(SO4)3 = (2x56) + 3[32 + (16x4)] = 112 + 3[32 + 64] = 112 + 3[96] = 400g/mol

Mass of Fe2(SO4)3 from the balanced equation = 1 x 400 = 400g

Molar Mass of Fe = 56g/mol

Mass of Fe from the balanced equation = 2 x 56 = 112g

From the balanced equation above,

400g of Fe2(SO4)3 reacted to produce 112g Fe.

Step 3:

Determination of the mass of Fe produced by reacting 3.65g of Fe2(SO4)3.

This is illustrated below:

From the balanced equation above,

400g of Fe2(SO4)3 reacted to produce 112g Fe.

Therefore, 3.65g of Fe2(SO4)3 will react to produce = (3.65 x 112)/400 = 1.02g of Fe.

Therefore, 1.02g of Fe is produced from 3.65g of Fe2(SO4)3.

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Answer:

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4 years ago

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Answer:

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Explanation:

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