Iron(III) oxide reacts with carbon monoxide according to the equation: Fe 2 O 3 (s) + 3 CO(g) → 2 Fe(s) + 3 CO 2 (g) A reaction mixture initially contains 22.55 g Fe 2 O 3 and 14.78 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?

Hi everyone today, we have a question asking us at the beginning of the reaction, there are 34.67g of copper oxide and 9.87 g of carbon monoxide. And we want to calculate the amount in grams of excess reactant that remains after the reaction has come to the completion and our reaction is copper copper oxide solid plus three carbon monoxide gashes forms to copper solid plus three carbon carbon dioxide gashes. So let's start out with our three 34 0.67 grams of copper oxide times one mole of copper oxide, divided by 175. g of copper oxide. And our grams here are canceling out, Leaving us with 0. moles of copper oxide. Next we have 9.17 g of carbon monoxide. And we're going to multiply that by one mole of carbon monoxide over .01g of carbon monoxide and our grams of carbon monoxide are going to cancel out. And that's going to leave us with 0.35- moles of carbon monoxide. And for our next step, we want to take our lowest number of moles, which is our 0.1980 and see how many moles of carbon monoxide we get. So we're going to have 0. moles of copper Times 1. 3 moles of carbon monoxide over two moles of copper Times are molar mass of carbon monoxide. So 28.01 g of carbon monoxide over one mole. So our moles of copper are canceling out, and our moles of carbon monoxide are canceling out, and that gives us 8. 1897 grams of carbon monoxide. And our last step is to take our 9.87 g -R 8. 1897, And that equals 1.55 g of carbon monoxide. So our answer here is B. Thank you for watching. Bye.

Ch.4 - Chemical Reactions and Chemical Quantities

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Tro 5th Edition

Ch.4 - Chemical Reactions and Chemical Quantities

Problem 45

Chapter 4, Problem 45

Iron(III) oxide reacts with carbon monoxide according to the equation: Fe₂O₃(s) + 3 CO(g) → 2 Fe(s) + 3 CO₂(g) A reaction mixture initially contains 22.55 g Fe₂O₃ and 14.78 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?

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Calculate the molar mass of Fe_2O_3 and CO using the periodic table.

Convert the given masses of Fe_2O_3 and CO to moles by dividing by their respective molar masses.

Determine the limiting reactant by comparing the mole ratio of Fe_2O_3 to CO from the balanced equation with the mole ratio from the initial amounts.

Use the stoichiometry of the reaction to calculate how much of the excess reactant is consumed by the limiting reactant.

Subtract the moles of the excess reactant consumed from the initial moles to find the remaining moles, then convert this back to grams using the molar mass.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows us to determine the proportions of substances involved in a reaction, which is essential for identifying limiting and excess reactants. In this case, stoichiometry will help us calculate how much of each reactant is consumed and how much remains after the reaction.

Limiting Reactant

The limiting reactant is the substance that is completely consumed first in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is crucial for calculating the amounts of products and any excess reactants left over. In this reaction, we will need to find out which reactant, Fe2O3 or CO, limits the formation of iron and carbon dioxide.

Excess Reactant

The excess reactant is the substance that remains after the reaction has gone to completion, as it is not completely consumed. Understanding the concept of excess reactants is important for calculating how much of a reactant is left over after the reaction. In this scenario, once we identify the limiting reactant, we can determine the mass of the excess reactant that remains unreacted.

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Iron(II) sulfide reacts with hydrochloric acid according to the reaction: FeS(s) + 2 HCl(aq) → FeCl₂(s) + H₂S(g) A reaction mixture initially contains 0.223 mol FeS and 0.652 mol HCl. Once the reaction has occurred as completely as possible, what amount (in moles) of the excess reactant remains?

For the reaction shown, calculate the theoretical yield of product (in grams) for each initial amount of reactants. 2 Al(s) + 3 Cl₂(g) → 2 AlCl₃(s) c. 0.235 g Al, 1.15 g Cl₂

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Textbook Question

For the reaction shown, calculate the theoretical yield of the product (in grams) for each initial amount of reactants. Ti(s) + 2 F₂( g) → TiF₄(s) c. 0.233 g Ti, 0.288 g F₂

Elemental phosphorus reacts with chlorine gas according to the equation: P₄(s) + 6 Cl₂( g) → 4 PCl₃(l) A reaction mixture initially contains 45.69 g P₄ and 131.3 g Cl₂. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?

Magnesium oxide can be made by heating magnesium metal in the presence of oxygen. The balanced equation for the reaction is: 2 Mg(s) + O₂(g) → 2 MgO(s) When 10.1 g of Mg reacts with 10.5 g O₂, 11.9 g MgO is collected. Determine the limiting reactant, theoretical yield, and percent yield for the reaction.

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Textbook Question

Urea (CH₄N₂O) is a common fertilizer that is synthesized by the reaction of ammonia (NH₃) with carbon dioxide: 2 NH₃(aq) + CO₂(aq) → CH₄N₂O(aq) + H₂O(l) In an industrial synthesis of urea, a chemist combines 136.4 kg of ammonia with 211.4 kg of carbon dioxide and obtains 168.4 kg of urea. Determine the limiting reactant, theoretical yield of urea, and percent yield for the reaction.

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Iron(III) oxide reacts with carbon monoxide according to the equation: Fe2O3(s) + 3 CO(g) → 2 Fe(s) + 3 CO2(g) A reaction mixture initially contains 22.55 g Fe2O3 and 14.78 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?

Verified video answer for a similar problem:

Key Concepts

Stoichiometry

Limiting Reactant

Excess Reactant

Iron(III) oxide reacts with carbon monoxide according to the equation: Fe₂O₃(s) + 3 CO(g) → 2 Fe(s) + 3 CO₂(g) A reaction mixture initially contains 22.55 g Fe₂O₃ and 14.78 g CO. Once the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?