12) What mass of Fe₂O3 would react with 20.00 g of Zn? The chemical equation for this reacti 3 Zn + Fe₂O3 → 2 Fe + 3 ZnO is: 13) x moles of C4H10 reacts with oxygen according to the following equation: 2 C4H10 + 13 0₂ →8 CO₂ +¹10 H₂O a) How many moles of water are formed? b) How many moles of oxygen are consumed? 14) 10.00 g of N₂ is mixed with 33.61 g of F2, and the elements react according to the following equation: N₂ + 3 F2 → 2 NF3 a) Which element is the limiting reactant? b) What is the theoretical yield of NF3? c) If the reaction goes to completion, how many grams of the excess reactant will remain? d) Set up an ICE table for this reaction. 15) a) If 58.26 g of iodine reacts with excess aluminum, what is the theoretical yield of aluminum iodide? The reaction is 2 Al +3 12 → 2 All 3. FEB 7 22

12) What mass of Fe₂O3 would react with 20.00 g of Zn? The chemical equation for this reacti 3 Zn + Fe₂O3 → 2 Fe + 3 ZnO is: 13) x moles of C4H10 reacts with oxygen according to the following equation: 2 C4H10 + 13 0₂ →8 CO₂ +¹10 H₂O a) How many moles of water are formed? b) How many moles of oxygen are consumed? 14) 10.00 g of N₂ is mixed with 33.61 g of F2, and the elements react according to the following equation: N₂ + 3 F2 → 2 NF3 a) Which element is the limiting reactant? b) What is the theoretical yield of NF3? c) If the reaction goes to completion, how many grams of the excess reactant will remain? d) Set up an ICE table for this reaction. 15) a) If 58.26 g of iodine reacts with excess aluminum, what is the theoretical yield of aluminum iodide? The reaction is 2 Al +3 12 → 2 All 3. FEB 7 22

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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Similar questions

Many cereals are made with high moisture content so that the cereal can be formed into various shapes before it is dried. A cereal product containing 58% H2O by mass is produced at the rate of 1000. kg/h. What mass of water must be evaporated per hour if the final product contains only 20.% water?
Many cereals are made with high moisture content so that the cereal can be formed into various shapes before it is dried. A cereal product containing 58% H2O by mass is produced at the rate of 1000. kg/h. What mass of water must be evaporated per hour if the final product contains only 20.% water?
(a) Butane gas, C4H10, can burn completely in air [use O2(g) as the other reactant] to give carbon dioxide gas and water vapor. Write a balanced equation for this combustion reaction. (b) Write a balanced chemical equation for the complete combustion of C3H7BO3, a gasoline additive. The products of combustion are CO2(g), H2O(g), and B2O3(s).
4.8 In an experiment carried out at very low pressure, 13x1015 molecules of H2 are reacted with acetylene, C2H2, to form ethane, C2H6, on the surface of a catalyst. Write a balanced chemical equation for this reaction. How many molecules of acetylene are consumed?
Nitric acid is produced commercially by the Ostwald process, represented by the following equations: 4NH3(g)+5O24NO(g)+6H2O(g)2NO(g)+O2(g)2NO2(g)3NO2(g)+H2O(l)2HNO3(aq)+NO(g) What mass of NH3 must be used to produce 1.0 106 kg HNO3 by the Ostwald process? Assume 100% yield in each reaction, and assume that the NO produced in the third step is not recycled.
ou know that chemical A reacts with chemical B. You react 10.0 g A with 10.0 g B. What information do you need to know to determine the amount of product that will be produced? Explain.
4.106 An ore sample with a mass of 670 kg contains 27.7% magnesium carbonate, MgCO3. If all of the magnesium carbonate in this ore sample is decomposed to form carbon dioxide, describe how to determine what mass of CO2 is evolved during the process.
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.
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.