Part B An iron ore sample contains Fe2 03 together with other substances. Reacti

Question

Part B An iron ore sample contains Fe2 03 together with other substances. Reaction of the ore with CO produces iron metal Fe3O3(s) + CO(g) Fe(s) + CO2 (g) Calculate the number of grams of CO that can react with 0.320 kg of Fe203 Express your answer in grams to three significant figures. You may want to reference (Pages 103-105) Section 3.6 while completing this problem. Submit Previous Answers Request Answer XIncorrect; Try Again; 18 attempts remaining Since the mass of the oxide is given in kg, first convert kg to g. Recall that 1 kg 1000 g. Next, convert grams of Fe2O3 to moles of Fe2 03 using its molar mass. Then, convert to moles of CO using the molar ratio, which can be determined using the balanced chemical equation. Finally, convert moles of CO to grams of CO using its molar mass. All units should cancel out except for g CO Part C Calculate the number of grams of Fe formed when 0.320 kg of Fe2O3 reacts Express your answer in grams to three significant figures Submit Request Answer

Explanation / Answer

Ans

b) The balanced reaction is given as :

Fe2O3 + 3CO = 2Fe + 3CO2

0.320 kg = 320 g of Fe2O3

Number of moles of Fe2O3 = 320 / molar mass

= 320 / 159.6882

= 2 .0 mol

1 mol of Fe2O3 requires 3 mol of Fe2O3

So 2.0 mol of Fe2O3 will require 2.0 x 3= 6.0 mol of CO2

The mass of CO = 6.0 x molar mass

= 6.0 x 28.01

= 168 grams

Part c) 1 mol of Fe2O3 makes 2 moles of Fe

So 2.0 mol of Fe2O3 will produce 2.0 x 2 = 4.0 mol of Fe

Mass of Fe produced = 4.0 x molar mass

= 4.0 x 55.845

= 224 g

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