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Ch.3 - Chemical Reactions and Reaction Stoichiometry
All textbooksBrown 14th EditionCh.3 - Chemical Reactions and Reaction StoichiometryProblem 63b
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Chapter 3, Problem 63b

Several brands of antacids use Al1OH23 to react with stomach acid, which contains primarily HCl: Al1OH231s2 + HCl1aq2¡AlCl31aq2 + H2O1l2 (b) Calculate the number of grams of HCl that can react with 0.500 g of Al1OH23.

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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 converting between grams and moles. In this case, stoichiometry will help us find out how much HCl can react with a given mass of Al(OH)3.
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Molar Mass

Molar mass is the mass of one mole of a substance, typically expressed in grams per mole (g/mol). It is crucial for converting between the mass of a substance and the number of moles. To solve the problem, we need to calculate the molar mass of Al(OH)3 to determine how many moles correspond to 0.500 g.
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Limiting Reactant

The limiting reactant is the substance that is completely consumed in a chemical reaction, thus determining the maximum amount of product that can be formed. Identifying the limiting reactant is important in stoichiometric calculations, as it affects how much HCl can react with the available Al(OH)3. In this scenario, understanding which reactant limits the reaction will be key to finding the grams of HCl that can react.
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Textbook Question

Hydrofluoric acid, HF(aq), cannot be stored in glass bottles because compounds called silicates in the glass are attacked by the HF(aq). Sodium silicate 1Na2SiO32, for example, reacts as follows: Na2SiO31s2 + 8 HF1aq2¡ H2SiF61aq2 + 2 NaF1aq2 + 3 H2O1l2 (b) How many grams of NaF form when 0.500 mol of HF reacts with excess Na2SiO3?

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Textbook Question

The reaction between potassium superoxide, KO2, and CO2, 4 KO2 + 2 CO2¡2K2CO3 + 3 O2 is used as a source of O2 and absorber of CO2 in selfcontained breathing equipment used by rescue workers. (a) How many moles of O2 are produced when 0.400 mol of KO2 reacts in this fashion?

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Textbook Question

The reaction between potassium superoxide, KO2, and CO2, 4 KO2 + 2 CO2¡2K2CO3 + 3 O2 is used as a source of O2 and absorber of CO2 in selfcontained breathing equipment used by rescue workers. (b) How many grams of KO2 are needed to form 7.50 g of O2?

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Textbook Question

An iron ore sample contains Fe2O3 together with other substances. Reaction of the ore with CO produces iron metal: Fe2O31s2 + CO1g2¡Fe1s2 + CO21g2 (b) Calculate the number of grams of CO that can react with 0.350 kg of Fe2O3.

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Textbook Question

Aluminum sulfide reacts with water to form aluminum hydroxide and hydrogen sulfide. (a) Write the balanced chemical equation for this reaction. (b) How many grams of aluminum hydroxide are obtained from 14.2 g of aluminum sulfide?

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Textbook Question

Calcium hydride reacts with water to form calcium hydroxide and hydrogen gas. (a) Write a balanced chemical equation for the reaction.

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