Fe3O4 + --gt; Fe + H2Oa) Iron ore, in the form of hte mized iron oxide shown, can be reduced by the addition of hydrogen gas. How many grams of Iron metal will be produced in the proces, if 411 g of Fe3O4 are reacted completely with hydrogen gas?b) Determine the amount of water produced in this reaction in moles, if 1201 g of iron ore are reacted with sufficient hydrogen to convert it to products, in such a way that the reaction has a 48.22% yield.Can you please help me just set up the problem? Your help will be greatly appreciated.
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For (a) look up the atomic weights of Iron and Oxygen and calculate the fraction by weight of Iron in Fe3O4. Then since you know that the Fe3O4 is 411g you will know how much of that is Iron. For (b) you will need to balance your original equation, so that you will know how many moles of Iron Ore produce how many moles of water. Use the atomic weight of Iron Ore that you calculated in (a) to figure the moles of Iron Ore in 1201g. Then using the balanced equation you can figure the moles of water. I am not sure how to calculate a 48.22% yield? However I am almost sure your textbook has an example with the yield of something discussed.
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