Iron(III) oxide reacts with carbon monoxide according to the equation:Fe2O3 (s)3CO (g)+2Fe(s) 3CO2(9)A reaction mixture initially contains 22.05 g Fe2 O3 and 14.00 g COPart AOnce the reaction has occurred as completely as possible, what mass (in g) of the excess reactant remains?Express your answer to three significant figures.

The term limiting reagent in a given reaction is defined as the chemical species which is totally…

Answered: Iron(III) oxide reacts with carbon…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter3: Chemical Reactions

Section: Chapter Questions

Problem 70QRT

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The reaction of methane and water is one way to prepare hydrogen for use as a fuel: CH4(g) + H2O(g) CO(g) + 3 H2(g) If you begin with 995 g of CH4 and 2510 g of water, (a) Which reactant is the limiting reactant? (b) What is the maximum mass of H2 that can be prepared? (c) What mass of the excess reactant remains when the reaction is completed?
Aluminum chloride, Al2Cl6, is an inexpensive reagent used in many industrial processes. It is made by treating scrap aluminum with chlorine according to the balanced equation 2 Al(s) + 3 Cl2(g) Al2Cl6(S) (a) Determine which reactant is limiting if 2.70 g Al and 4.05 g Cl2 are mixed. (b) Calculate what mass of Al2Cl6 can be produced. (c) Calculate what mass of the excess reactant remains when the reaction is complete.
Ammonia can be formed by a direct reaction of nitrogen and hydrogen. N2(g) + 3 H2(g) 2 NH3(g) A tiny portion of the starting mixture is represented by the diagram, where the blue circles represent N and the white circles represent H. Which of these represents the product mixture? For the reaction of the given sample, which of these statements is true? (a) N2 is the limiting reactant. (b) H2 is the limiting reactant. (c) NH, is the limiting reactant. (d) No reactant is limiting: they are present in the correct stoichiometric ratio.
You react nitrogen and hydrogen in a container to produce ammonia, NH3(g). The following figure depicts the contents of the container after the reaction is complete. a Write a balanced chemical equation for the reaction. b What is the limiting reactant? c How many molecules of the limiting reactant would you need to add to the container in order to have a complete reaction (convert all reactants to products)?
Disulfur dichloride, S2Cl2, is used to vulcanize rubber. It can be made by treating molten sulfur with gaseous chlorine: S8(l) + 4 Cl2(g) 4 S2Cl3(l) Starting with a mixture of 32.0 g of sulfur and 71.0 g of Cl2, (a) Which is the limiting reactant? (b) What is the theoretical yield of S2Cl2? (c) What mass of the excess reactant remains when the reaction is completed?
4.69 The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH. The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
The compound SF6 is made by burning sulfur in an atmosphere of fluorine. The balanced equation is Sa(s) + 24 F2(g) SF6(g) Starting with a mixture of 1.6 mol of sulfur. Sg, and 35 mol of F2, (a) Which is the limiting reagent? (b) What amount of SF6 is produced?
A potential fuel for rockets is a combination of B5H9 and 0 2. The two react according to the following balanced equation: 2B5H9(l)+12O2(g)5B2O3(s)+9H2O(g) If one tank in a rocket holds 126 g B5H9 and another tank holds 192 g O2, what mass of water can be produced when the entire contents of each tank react together?
Consider the following unbalanced chemical equation for the combustion of pentane (C5H12): C5H12(l)+O2(g)CO2(g)+H2O(l) If 20.4 g of pentane are burned in excess oxygen, what mass of water can be produced, assuming 100% yield?
The catalytic converter that is standard equipment on American automobiles converts carbon monoxide (CO)to carbon dioxide (CO2) by the reaction 2CO + O2 2CO2 What mass of O2, in grams, is needed to react completely with 25.0 g of CO?
In an experiment designed to produce calcium oxide by the chemical reaction 2Ca + O2 2CaO 177.2 g of CaO was obtained out of a possible 203.9 g ofCaO. a. What is the theoretical yield of CaO? b. What is the actual yield of CaO? c. What is the percent yield of CaO?
4.68 The pictures below show a molecular-scale view of a chemical reaction between the compounds AB2 and B2. (Green balls represent B atoms and orange balls are A atoms). The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.

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