Question
Asked Feb 15, 2020
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What mass of iron(III) oxide must be used to produce 64.28 g of iron?

What is the maximum mass of aluminum oxide that could be produced along with 79.76 g iron?

What mass of aluminum must be used to produce 80.05 g of iron?

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Expert Answer

Step 1

The equation required to produce iron from iron(III)oxide is as follows,

Chemistry homework question answer, step 1, image 1

Given grams of iron is converted into moles as follows,

Chemistry homework question answer, step 1, image 2

Step 2

Observing the balanced equation shows that 2 moles of Fe is obtained from 1 mole of iron(III)oxide moles. Therefore, 1.151 moles of Fe is obtained from 0.5755 moles of Fe2O3.

Now, the moles of Fe2O3 is converted into mass as follows,

Chemistry homework question answer, step 2, image 1

Step 3

The equation required to produce iron from iron(III)oxide is as follows,

Chemistry homework question answer, step 3, image 1

Given grams of iron is converted into moles as follows,

Chemistry homework question answer, step 3, image 2

Observing the balanced equation shows that 2 moles of Fe is produced along with 1 mole of Al2O3. Therefore, the mole of Al2O3 produced along with given grams of iron are 0.714 moles.

 

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