Student Solutions Manual for Zumdahl/Zumdahl/DeCoste?s Chemistry, 10th Edition
10th Edition
ISBN: 9781305957510
Author: ZUMDAHL, Steven S.; Zumdahl, Susan A.; DeCoste, Donald J.
Publisher: Cengage Learning
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Chapter 6, Problem 2ALQ
What is meant by the term lower in energy? Which is lower in energy, a mixture of hydrogen and oxygen gases or liquid water? How do you know? Which of the two is more stable? How do you know?
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Chapter 6 Solutions
Student Solutions Manual for Zumdahl/Zumdahl/DeCoste?s Chemistry, 10th Edition
Ch. 6 - Define the following terms: potential energy,...Ch. 6 - Consider the following potential energy diagrams...Ch. 6 - What is the first law of thermodynamics? How can a...Ch. 6 - When a gas expands, what is the sign of w? Why?...Ch. 6 - What is the heat gained/released at constant...Ch. 6 - High-quality audio amplifiers generate large...Ch. 6 - Explain how calorimetry works to calculate H or E...Ch. 6 - What is Hesss law? When a reaction is reversed,...Ch. 6 - Define the standard enthalpy of formation. What...Ch. 6 - Objects placed together eventually reach the same...
Ch. 6 - What is meant by the term lower in energy? Which...Ch. 6 - A fire is started in a fireplace by striking a...Ch. 6 - Liquid water turns to ice. Is this process...Ch. 6 - Consider the following statements: ''Heat is a...Ch. 6 - Consider 5.5 L of a gas at a pressure of 3.0 atm...Ch. 6 - Consider 5.5 L of a gas at a pressure of 3.0 atm...Ch. 6 - What if energy was not conserved? How would this...Ch. 6 - Hesss law is really just another statement of the...Ch. 6 - In the equation w = P V, why is there a negative...Ch. 6 - Consider an airplane trip from Chicago, Illinois,...Ch. 6 - How is average bond strength related to relative...Ch. 6 - Assuming gasoline is pure C8H18(l), predict the...Ch. 6 - What is the difference between H and E?Ch. 6 - The enthalpy change for the reaction...Ch. 6 - Explain why oceanfront areas generally have...Ch. 6 - The equation for the fermentation of glucose to...Ch. 6 - Explain why H is obtained directly from coffee-cup...Ch. 6 - The enthalpy of combustion of CH4(g) when H2O (1)...Ch. 6 - The enthalpy change for a reaction is a state...Ch. 6 - Standard enthalpies of formation are relative...Ch. 6 - The combustion of methane can be represented as...Ch. 6 - Why is it a good idea to rinse your thermos bottle...Ch. 6 - Prob. 26QCh. 6 - What is incomplete combustion of fossil fuels? Why...Ch. 6 - Explain the advantages and disadvantages of...Ch. 6 - Prob. 29ECh. 6 - Which has the greater kinetic energy, an object...Ch. 6 - Consider the following diagram when answering the...Ch. 6 - A gas absorbs 45 kJ of heat and does 29 kJ of...Ch. 6 - Calculate E for each of the following. a. q = 47...Ch. 6 - A system undergoes a process consisting of the...Ch. 6 - If the internal energy of a thermodynamic system...Ch. 6 - Calculate the internal energy change for each of...Ch. 6 - A sample of an ideal gas at 15.0 atm and 10.0 L is...Ch. 6 - A piston performs work of 210. L atm on the...Ch. 6 - Consider a mixture of air and gasoline vapor in a...Ch. 6 - As a system increases in volume, it absorbs 52.5 J...Ch. 6 - A balloon filled with 39.1 moles of helium has a...Ch. 6 - One mole of H2O(g) at 1.00 atm and 100.C occupies...Ch. 6 - One of the components of polluted air is NO. It is...Ch. 6 - The reaction SO3(g)+H2O(l)H2SO4(aq) is the last...Ch. 6 - Are the following processes exothermic or...Ch. 6 - Are the following processes exothermic or...Ch. 6 - The overall reaction in a commercial heat pack can...Ch. 6 - Consider the following reaction:...Ch. 6 - Consider the combustion of propane:...Ch. 6 - Consider the following reaction:...Ch. 6 - For the process H2O(l) H2O(g) at 298 K and 1.0...Ch. 6 - For the following reactions at constant pressure,...Ch. 6 - Consider the substances in Table 7-1. Which...Ch. 6 - The specific heat capacity of silver is 0.24 J/Cg....Ch. 6 - A 500-g sample of one of the substances listed in...Ch. 6 - It takes 585 J of energy to raise the temperature...Ch. 6 - A 30.0-g sample of water at 280. K is mixed with...Ch. 6 - A biology experiment requires the preparation of a...Ch. 6 - A 5.00-g sample of aluminum pellets (specific heat...Ch. 6 - Hydrogen gives off 120. J/g of energy when burned...Ch. 6 - A 150.0-g sample of a metal at75.0C is added to...Ch. 6 - A 110.-g sample of copper (specific heat capacity...Ch. 6 - In a coffee-cup calorimeter, 50.0 mL of 0.100 M...Ch. 6 - In a coffee-cup calorimeter, 100.0 mL of 1.0 M...Ch. 6 - A coffee-cup calorimeter initially contains 125 g...Ch. 6 - In a coffee-cup calorimeter, 1.60 g NH4NO3 is...Ch. 6 - Consider the dissolution of CaCl2:...Ch. 6 - Consider the reaction...Ch. 6 - Quinone is an important type of molecule that is...Ch. 6 - The energy content of food is typically determined...Ch. 6 - The heat capacity of a bomb calorimeter was...Ch. 6 - The combustion of 0.1584 g benzoic acid increases...Ch. 6 - The enthalpy of combustion of solid carbon to form...Ch. 6 - Combustion reactions involve reacting a substance...Ch. 6 - Given the following data calculate H for the...Ch. 6 - Prob. 78ECh. 6 - The bombardier beetle uses an explosive discharge...Ch. 6 - Calculate H for the reaction...Ch. 6 - Given the following data...Ch. 6 - Given the following data...Ch. 6 - Give the definition of the standard enthalpy of...Ch. 6 - Write reactions for which the enthalpy change will...Ch. 6 - Use the values ofHf in Appendix 4 to calculate H...Ch. 6 - Use the values of Hf in Appendix 4 to calculate H...Ch. 6 - The Ostwald process for the commercial production...Ch. 6 - Calculate H for each of the following reactions...Ch. 6 - The reusable booster rockets of the space shuttle...Ch. 6 - The space shuttle Orbiter utilizes the oxidation...Ch. 6 - Consider the reaction...Ch. 6 - The standard enthalpy of combustion of ethene gas,...Ch. 6 - Water gas is produced from the reaction of steam...Ch. 6 - Syngas can be burned directly or converted to...Ch. 6 - Ethanol (C2H5OH) has been proposed as an...Ch. 6 - Methanol (CH3OH) has also been proposed as an...Ch. 6 - Some automobiles and buses have been equipped to...Ch. 6 - Acetylene (C2H2) and butane (C4H10) are gaseous...Ch. 6 - Prob. 99ECh. 6 - The complete combustion of acetylene, C2H2(g),...Ch. 6 - It has been determined that the body can generate...Ch. 6 - One way to lose weight is to exercise! Walking...Ch. 6 - Three gas-phase reactions were run in a...Ch. 6 - Nitrogen gas reacts with hydrogen gas to form...Ch. 6 - Combustion of table sugar produces CO2(g) and H2O(...Ch. 6 - Prob. 106AECh. 6 - A serving size of six cookies contains 4 g of fat,...Ch. 6 - Calculate H for the reaction...Ch. 6 - The enthalpy of neutralization for the reaction of...Ch. 6 - Given the following data: NO2(g) NO(g) + O(g)H =...Ch. 6 - If a student performs an endothermic reaction in a...Ch. 6 - In a bomb calorimeter, the reaction vessel is...Ch. 6 - The bomb calorimeter in Exercise 102 is filled...Ch. 6 - Consider the two space shuttle fuel reactions in...Ch. 6 - Consider the following equations:...Ch. 6 - Given the following data...Ch. 6 - At 298 K, the standard enthalpies of formation for...Ch. 6 - Using the following data, calculate the standard...Ch. 6 - A sample of nickel is heated to 99.8C and placed...Ch. 6 - Given: 2Cu2O(s) + O2(g) 4CuO(s)H = 288 kJ Cu2O(s)...Ch. 6 - Calculate H for each of the following reactions,...Ch. 6 - Consider a balloon filled with helium at the...Ch. 6 - In which of the following systems is(are) work...Ch. 6 - Which of the following processes are exothermic?...Ch. 6 - Consider the reaction...Ch. 6 - A swimming pool, 10.0 m by 4.0 m, is filled with...Ch. 6 - In a coffee-cup calorimeter, 150.0 mL of 0.50 M...Ch. 6 - Calculate H for the reaction...Ch. 6 - Which of the following substances have an enthalpy...Ch. 6 - Consider 2.00 moles of an ideal gas that are taken...Ch. 6 - For the process H2O(l)H2O(g) at 298 K and 1.0 atm,...Ch. 6 - The sun supplies energy at a rate of about 1.0...Ch. 6 - The best solar panels currently available are...Ch. 6 - On Easter Sunday, April 3, 1983, nitric acid...Ch. 6 - A piece of chocolate cake contains about 400...Ch. 6 - The standard enthalpies of formation for S(g),...Ch. 6 - You have a l.00-mole sample of water at 30.C and...Ch. 6 - A 500.0-g sample of an element at 195C is dropped...Ch. 6 - When 1.00 L of 2.00 M Na2SO4 solution at 30.0c is...Ch. 6 - The preparation of NO2(g) from N2(g) and O2(g) is...Ch. 6 - Nitromethane, CH3NO2, can be used as a fuel. When...Ch. 6 - A cubic piece of uranium metal (specific heat...Ch. 6 - A gaseous hydrocarbon reacts completely with...
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- You discover that you cannot carry out a particular reaction for which you would like the enthalpy change. Does this mean that you will be unable to obtain this enthalpy change? Explain.arrow_forwardWhat quantity of heat energy must have en applied to a block of aluminum weighing 42.7 g if the temperature of the block of aluminum increased by 15.2 °C? (See Table 10.1.)arrow_forward9.41 Under what conditions does the enthalpy change equal the heat of a process?arrow_forward
- For the reaction HgO(s)Hg(l)+12O2(g),H=+90.7kJ: a.What quantity of heat is required to produce 1 mole of mercury by this reaction? b.What quantity of heat is required to produce 1 mole of oxygen gas by this reaction? c.What quantity of heat would be released in the following reaction as written? 2Hg(l) + O2(g) 2HgO(s)arrow_forwardHow much heat is produced by combustion of 125 g of methanol under standard state conditions?arrow_forward9.59 For the reaction N2(g)+O2(g)2NO(g),H=180.5kJ . How much energy is needed to generate 35 moles of NO(g)?arrow_forward
- The following reactions can be used to prepare samples of metals. Determine the enthalpy change under standard state conditions for each. (a) 2Ag2O(s)4Ag(s)+O2(g) (b) SnO(s)+CO(g)Sn(s)+CO2(g) (c) Cr2O3(s)+3H2(g)2Cr(s)+3H2O(l) (d) 2Al(s)+Fe2O3(s)Al2O(s)+2Fe(s)arrow_forwardDescribe the interconversions of potential and kinetic energy in a moving pendulum. A moving pendulum eventually comes to rest. Has the energy been lost? If not, what has happened to it?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
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