Answered

Welcome to Westonci.ca, where finding answers to your questions is made simple by our community of experts. Our platform provides a seamless experience for finding precise answers from a network of experienced professionals. Explore comprehensive solutions to your questions from a wide range of professionals on our user-friendly platform.

A 3.6 g sample of iron (III) oxide reacts with sufficient aluminum to be entirely used up.
How much iron is produced?

Sagot :

dsdrajlin

Answer:

0.046 mol

Explanation:

Step 1: Write the balanced equation

Fe₂O₃ + 2 Al ⇒ 2 Fe + Al₂O₃

Step 2: Calculate the moles corresponding to 3.6 g of Fe₂O₃

The molar mass of Fe₂O₃ is 159.69 g/mol.

3.6 g × 1 mol/159.69 g = 0.023 mol

Step 3: Calculate the moles of Fe produced from 0.023 moles of Fe₂O₃

The molar ratio of Fe₂O₃ to Fe is 1:2.

0.023 mol  Fe₂O₃ × 2 mol Fe/1 mol Fe₂O₃ = 0.046 mol Fe

Thanks for stopping by. We are committed to providing the best answers for all your questions. See you again soon. We hope our answers were useful. Return anytime for more information and answers to any other questions you have. Discover more at Westonci.ca. Return for the latest expert answers and updates on various topics.