**Question:**How many grams of CO₂ can you produce by reacting 10.85 g of Fe₂O₃ with excess CO according to the reaction\[ \text{Fe}_2\text{O}_3(s) + 3\text{CO}(g) \rightarrow 2\text{Fe}(s) + 3\text{CO}_2(g) \]**Explanation:**This question involves a chemical reaction where iron(III) oxide (Fe₂O₃) reacts with carbon monoxide (CO) to produce iron (Fe) and carbon dioxide (CO₂). The task is to calculate the mass of CO₂ produced from the given mass of Fe₂O₃ when CO is in excess.**Key Points:**- **Given:** 10.85 g of Fe₂O₃ - **Reaction:** Fe₂O₃ + 3CO → 2Fe + 3CO₂- **Objective:** Determine the mass of CO₂ produced.The calculation will involve converting the mass of Fe₂O₃ to moles, using the stoichiometry of the balanced equation to find the moles of CO₂ produced, and then converting that to grams.

No. of moles of Fe2O3 is calculated using given mass as follows: No. of moles = massmolar massof moles =10.85 g159.69 g/mol=0.06794 molGiven that CO is excess. Therefore, limiting reagent will be Fe2O3. Thus, the number of moles of carbon dioxide can be calculated using the balanced chemical equation: Fe2O3 + 3 CO→2 Fe+3 CO21 mol Fe2O3 gives 3 mol CO20.06794 mol Fe2O3 gives x mol CONo. of moles of CO2 = 0.06794 mol Fe2O3×3 mol CO21 mol Fe2O3No. of moles of CO2=0.2038 mol CO2Mass of carbon dioxide produced is calculated as follows: Mass=No.of moles×Molar massMass=0.2038 mol×44 g/molMass=8.967 g

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Chemistry

How many grams of CO2 can you produce by reacting 10.85 g of Fe:Os with excess CO according to the reaction Fe:Os(s) + 3CO(g) → 2Fe(s) + 3CO:(g)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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