LL R How many grams of Al,0, can form from 36.3 g of Al? 4 Al(s) + 3 O,(g) –→ 2 Al,O3(s) Step 1: Show the strategy for solving this problem. grams Al → → grams Al, O3 Answer Bank grams Al,O3 grams Al moles Al,O3 grams O, moles Al moles O, Step 2: Show the conversions required to solve this problem and calculate the grams of Al, O,. = g Al,O3 36.3 g Al × %D MacBook Pro Q Search or enter website name 巴 4 8. 9- 7. 7. H. R 36.3 g Al x = g Al,O3 %3D Answer Bank 26.98 g Al 1 mole Al 4 moles Al 32.00 g O2 1 mole O, 3 moles O, 101.96 g Al,O3 1 mole Al,O3 2 moles Al,O3 grams of Al,O3: MacBook Pro Q Search or enter website name %3D %24 7. 0. 5. 6. 4. E. K.

LL R How many grams of Al,0, can form from 36.3 g of Al? 4 Al(s) + 3 O,(g) –→ 2 Al,O3(s) Step 1: Show the strategy for solving this problem. grams Al → → grams Al, O3 Answer Bank grams Al,O3 grams Al moles Al,O3 grams O, moles Al moles O, Step 2: Show the conversions required to solve this problem and calculate the grams of Al, O,. = g Al,O3 36.3 g Al × %D MacBook Pro Q Search or enter website name 巴 4 8. 9- 7. 7. H. R 36.3 g Al x = g Al,O3 %3D Answer Bank 26.98 g Al 1 mole Al 4 moles Al 32.00 g O2 1 mole O, 3 moles O, 101.96 g Al,O3 1 mole Al,O3 2 moles Al,O3 grams of Al,O3: MacBook Pro Q Search or enter website name %3D %24 7. 0. 5. 6. 4. E. K.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter3: Equation, The Mole, And Chemical Formulas

Section: Chapter Questions

Problem 3.159QE

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3.75 The following pictures show a molecular-scale view of a chemical reaction between the compounds AB2 and B2. (A atoms are shown in blue and B atoms in white). 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 reac- tion has gone to completion. Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.
4.71 The particulate scale drawing shown depict the products of a reaction between N2 and O2 molecules. (a) Draw a similar representation for the reactants that must have been present before the reaction took place. (b) Write a balanced chemical equation for the reaction, using the smallest possible whole number coefficients. (c) Identify the limiting reactant, and explain how the pictures allow you to do so.
Write an equation from the following description: reactants are gaseous NH3 and O2, products are gaseous NO2 and liquid H2O, and the stoichiometric coefficients are 4, 7, 4, and 6, respectively.
4.70 The particulate scale drawing shown depicts the products of a reaction between H2 and O2 molecules. (a) Draw a similar representation for the reactants that must have been present before the reaction took place. (b) Write a balanced chemical equation for the reaction, using the smallest possible whole number coefficients. (c) identify the limiting reactant, and explain how the pictures allow you to do so.
What is meant by a limiting reactant in a particular reaction? In what way is the reaction “limited”? What does it mean to say that one or more of the reactants are present in excess? What happens to a reaction when the limiting reactant is used up?
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?
Fig. 5-5 illustrates a schematic diagram of a combustion device used to analyze organic compounds. Given that a certain amount of a compound containing carbon, hydrogen, and oxygen is combusted in this device, explain how the data relating to the mass of CO2 produced and the mass of H2O produced can be manipulated to determine the empirical formula.
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.
A titanium ore contains rutile (TiO2) plus some iron oxide and silica. When it is heated with carbon in the presence of chlorine, titanium tetrachloride, TiCl4, is formed. TiO2(s)+C(s)+2Cl2(g)TiCl4(g)+CO2(g) Titanium tetrachloride, a liquid, can be distilled from the mixture. If 35.4 g of titanium tetrachloride is recovered from 18.1 g of crude ore, what is the mass percentage of TiO2 in the ore (assuming all TiO2 reacts)?
Urea is used as a fertilizer because it can react with water to release ammonia, which provides nitrogen to plants. (NH2)2CO(s) + H2O() 2 NH3(aq) + CO2(g) (a) When 300. g urea and 100. g water are combined, calculate the mass of ammonia and the mass of carbon dioxide that form. (b) Calculate the mass of the excess reactant that remains after reaction.
How many molecules of the sweetener saccharin can be prepared from 30 C atoms, 25 H atoms, 12 0 atoms, 8 S atoms, and 14 N atoms?
The principal component of mothballs is naphthalene, a compound with a molecular mass of about 130 amu, containing only carbon and hydrogen. A 3.000-mg sample of naphthalene burns to give 10.3 mg of CO2. Determine its empirical and molecular formulas.