Introductory Chemistry: A Foundation
8th Edition
ISBN: 9781285199030
Author: Steven S. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Chapter 6, Problem 6QAP
If you’ve ever left bread in a toaster too long, you know that the bread eventually burns and turns black. What evidence is there that this represents a chemical process?
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Chapter 6 Solutions
Introductory Chemistry: A Foundation
Ch. 6.2 - Prob. 6.1SCCh. 6.3 - Prob. 1CTCh. 6.3 - One part of the problem-solving strategy for...Ch. 6.3 - Prob. 6.2SCCh. 6.3 - Prob. 6.3SCCh. 6 - The following are actual student responses to the...Ch. 6 - Prob. 2ALQCh. 6 - Given the equation for the reaction:N2+H2NH3 ,...Ch. 6 - Prob. 4ALQCh. 6 - Can the subscripts in a chemical formula be...
Ch. 6 - Prob. 6ALQCh. 6 - Changing the subscripts of chemicals can...Ch. 6 - Table 6.1 lists some clues that a chemical...Ch. 6 - Use molecular-level drawings to show the...Ch. 6 - It is stated in Section 6.3 of the text that to...Ch. 6 - Prob. 11ALQCh. 6 - Consider the generic chemical equationaA+bBcC+dD...Ch. 6 - Prob. 13ALQCh. 6 - Which of the following correctly describes the...Ch. 6 - Which of the following correctly balances the...Ch. 6 - The reaction of an element X() with element Y() is...Ch. 6 - Prob. 1QAPCh. 6 - Prob. 2QAPCh. 6 - Although these days many people have...Ch. 6 - Prob. 4QAPCh. 6 - You have probably had the unpleasant experience of...Ch. 6 - If you’ve ever left bread in a toaster too long,...Ch. 6 - What are the substances to theleftof the arrow in...Ch. 6 - Prob. 8QAPCh. 6 - In a chemical reaction, the total number of atoms...Ch. 6 - Prob. 10QAPCh. 6 - Prob. 11QAPCh. 6 - The notation “(l)” after a substance’s formula...Ch. 6 - A common experiment to determine the relative...Ch. 6 - If calcium carbonate is heated strongly, carbon...Ch. 6 - If a sample of pure hydrogen gas is ignited very...Ch. 6 - Liquid hydrazine, has been used as a fuel for...Ch. 6 - If electricity of sufficient voltage is passed...Ch. 6 - Silver oxide may be decomposed by strong heating...Ch. 6 - Elemental boron is produced in one industrial...Ch. 6 - Many over-the-counter antacid tablets are now...Ch. 6 - Phosphorus trichloride is used in the manufacture...Ch. 6 - Pure silicon, which is needed in the manufacturing...Ch. 6 - Nitrous oxide gas (systematic name: dinitrogen...Ch. 6 - Solid zinc is added to an aqueous solution...Ch. 6 - Acetylene gas (C2H2) is often used by plumbers,...Ch. 6 - The burning of high-sulfur fuels has been shown to...Ch. 6 - The Group 2 metals (Ba, Ca, Sr) can be produced in...Ch. 6 - There are fears that the protective ozone layer...Ch. 6 - Carbon tetrachloride was widely used for many...Ch. 6 - When elemental phosphorus, P4, burns in oxygen...Ch. 6 - Calcium oxide is sometimes very challenging to...Ch. 6 - Prob. 32QAPCh. 6 - The element tin often occurs in nature as the...Ch. 6 - Nitric acid, HNO3 , can be produced by reacting...Ch. 6 - When balancing chemical equations, beginning...Ch. 6 - The “Chemistry in Focus” segment The Beetle That...Ch. 6 - Balance each of the following chemical equations....Ch. 6 - Balance the equations for the reaction of...Ch. 6 - Balance each of the following chemical equations....Ch. 6 - Balance each of the following chemical equations....Ch. 6 - Balance each of the following chemical equations....Ch. 6 - Prob. 42QAPCh. 6 - Prob. 43QAPCh. 6 - Prob. 44QAPCh. 6 - Acetylene gas, C2H2 , is used in welding because...Ch. 6 - When balancing a chemical equation, which of the...Ch. 6 - Crude gunpowders often contain a mixture of...Ch. 6 - Prob. 48APCh. 6 - Methanol (methyl alcohol), CH3OH , is a very...Ch. 6 - The Hall process is an important method by which...Ch. 6 - Iron oxide ores, commonly a mixture of FeO and...Ch. 6 - True or false? Coefficients can be fractions when...Ch. 6 - When steel wool (iron) is heated in pure oxygen...Ch. 6 - One method of producing hydrogen peroxide is to...Ch. 6 - When elemental boron, B, is burned in oxygen gas,...Ch. 6 - A common experiment in introductory chemistry...Ch. 6 - A common demonstration in chemistry courses...Ch. 6 - Prob. 58APCh. 6 - Prob. 59APCh. 6 - Prob. 60APCh. 6 - If you had a “sour stomach,” you might try an...Ch. 6 - When iron wire is heated in the presence of...Ch. 6 - When finely divided solid sodium is dropped into a...Ch. 6 - If aqueous solutions of potassium chromate and...Ch. 6 - When hydrogen sulfide, H2S , gas is bubbled...Ch. 6 - If an electric current is passed through aqueous...Ch. 6 - When a strip of magnesium metal is heated in...Ch. 6 - Prob. 68APCh. 6 - When solid red phosphorus, is burned in air, the...Ch. 6 - When copper (II) oxide is boiled in an aqueous...Ch. 6 - When lead(II) sulfide is heated lo high...Ch. 6 - Which of the following statements about chemical...Ch. 6 - Prob. 73APCh. 6 - Prob. 74APCh. 6 - Prob. 75APCh. 6 - Using different shapes to distinguish between...Ch. 6 - Which of the following statements about chemical...Ch. 6 - Prob. 78CPCh. 6 - Balance the following chemical equations....
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- A rebreathing gas mask contains potassium superoxide, KO2, which reacts with moisture in the breath to give oxygen. 4KO2(s)+2H2O(l)4KOH(s)+3O2(g) Estimate the grams of potassium superoxide required to supply a persons oxygen needs for one hour. Assume a person requires 1.00 102 kcal of energy for this time period. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 1.00 102 kcal of heat, calculate the amount of oxygen consumed and hence the amount of KO2 required. The ff0 for glucose(s) is 1273 kJ/mol.arrow_forwardlist at least three quantities that must be conserved in chemical reactions.arrow_forwardThe carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.arrow_forward
- Carbon dioxide from the atmosphere weathers, or dissolves, limestone (CaCO3) by the reaction CaCO3(s)+CO2(g)+H2O(l)Ca2(aq)+2HCO3(aq) Obtain H for this reaction. See Table 6.2 for the data.arrow_forward4.60 Why are fuel additives used?arrow_forwardYou have probably had the unpleasant experience of discovering that a flashlight battery has gotten old and begun to leak. Is there evidence that this change is due to a chemical reaction?arrow_forward
- A newspaper article states that biomass has actually been used as an energy source throughout human history. Do you agree or disagree with this statement? Defend your answer.arrow_forwardMany over-the-counter antacid tablets are now formulated using calcium carbonate as the active ingredient, which enables such tablets to also be used as dietary calcium supplements. As an antacid for gastric hyperacidity, calcium carbonate reacts by combining with hydrochloric acid found in the stomach, producing a solution of calcium chloride, converting the stomach acid to water, and releasing carbon dioxide gas (which the person suffering from stomach problems may feel as a “burp”). Write the unbalanced chemical equation for this process.arrow_forwardEnthalpy a A 100.-g sample of water is placed in an insulated container and allowed to come to room temperature at 21C. To heat the water sample to 41C, how much heat must you add to it? b Consider the hypothetical reaction,2X(aq)+Y(l)X2Y(aq)being run in an insulated container that contains 100. g of solution. If the temperature of the solution changes from 21C to 31C, how much heat does the chemical reaction produce? How does this answer compare with that in part a? (You can assume that this solution is so dilute that it has the same heat capacity as pure water.) c If you wanted the temperature of 100. g of this solution to increase from 21C to 51C, how much heat would you have to add to it? (Try to answer this question without using a formula.) d If you had added 0.02 mol of X and 0.01 mol of Y to form the solution in part b, how many moles of X and Y would you need to bring about the temperature change described in part c. e Judging on the basis of your answers so far, what is the enthalpy of the reaction 2X(aq) + Y(l) X2Y(aq)?arrow_forward
- Table 6.1 lists some clues that a chemical reaction has occurred. However, these events do not necessarily prove the existence of a chemical change. Give an example for each of the clues that is not a chemical reaction but a physical change.arrow_forwardWrite a chemical equation representing the decomposition of water into two gaseous products. What are the products?arrow_forwardIron oxide ores, commonly a mixture of FeO and Fe2O3, are given the general formula Fe3O4. They yield elemental iron when heated to a very high temperature with either carbon monoxide or elemental hydrogen. Balance the following equations for these processes: Fe3O4(s)+H2(g)Fe(s)+H2O(g)Fe3O4(s)+CO(g)Fe(s)+CO2(g)arrow_forward
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