Chemistry with Access Code, Hybrid Edition
9th Edition
ISBN: 9781285188492
Author: Steven S. Zumdahl
Publisher: CENGAGE L
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Chapter 6, Problem 14Q
What is the difference between ∆H and ∆E?
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Chapter 6 Solutions
Chemistry with Access Code, Hybrid 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 - For the reaction HgO(s)Hg(l)+12O2(g),H=+90.7kJ:...Ch. 6 - The enthalpy of combustion of CH4(g) when H2O(l)...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. 22QCh. 6 - What is incomplete combustion of fossil fuels? Why...Ch. 6 - Explain the advantages and disadvantages of...Ch. 6 - Prob. 25ECh. 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 - A system releases 125 kJ of heal while 104 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 - 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. 72ECh. 6 - Given the following data 2O3(g) 3O2(g)H = 427 kJ...Ch. 6 - Calculate H for the reaction N2H4(l) + O2(g) ...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. 93ECh. 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. 100AECh. 6 - Consider the following cyclic process carried out...Ch. 6 - Calculate H for the reaction...Ch. 6 - The enthalpy of neutralization for the reaction of...Ch. 6 - Prob. 104AECh. 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 - 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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- How is the sign of q, heat, defined? How does it relate to the total energy of the system?arrow_forward9.42 Why is enthalpy generally more useful than internal energy in the thermodynamics of real world systems?arrow_forwardDefine the term entropy, and give an example of a sample of matter that has zero entropy. What are the units of entropy? How do they differ from the units of enthalpy?arrow_forward
- When a gas expands, what is the sign of w? Why? When a gas contracts, what is the sign of w? Why? What are the signs of q and w for the process of boiling water?arrow_forwardOne statement of the second law of thermodynamics is that heat cannot be turned completely into work. Another is that the entropy of the universe always increases. How are these two statements related?arrow_forwardWhen vapors from hydrochloric acid and aqueous ammonia come in contact, they react, producing a white cloud of solid NH4C1 (Figure 18.9). HCI(g) + NH3(g) NH4Cl(s) Defining the reactants and products as the system under study: (a) Predict whether S(system), S(surroundings), S(universe), rH, and rG (at 298 K) are greater than zero, equal to zero, or less than zero; and explain your prediction. Verify your predictions by calculating values for each of these quantities. (b) Calculate the value of Kp for this reaction at 298 K.arrow_forward
- Coal is used as a fuel in some electric-generating plants. Coal is a complex material, but for simplicity we may consider it to be a form of carbon. The energy that can be derived from a fuel is sometimes compared with the enthalpy of the combustion reaction: C(s)+O2(g)CO2(g) Calculate the standard enthalpy change for this reaction at 25C. Actually, only a fraction of the heat from this reaction is available to produce electric energy. In electric generating plants, this reaction is used to generate heat for a steam engine, which turns the generator. Basically the steam engine is a type of heat engine in which steam enters the engine at high temperature (Th), work is done, and the steam then exits at a lower temperature (Tl). The maximum fraction, f, of heat available to produce useful energy depends on the difference between these temperatures (expressed in kelvins), f = (Th Tl)/Th. What is the maximum heat energy available for useful work from the combustion of 1.00 mol of C(s) to CO2(g)? (Assume the value of H calculated at 25C for the heat obtained in the generator.) It is possible to consider more efficient ways to obtain useful energy from a fuel. For example, methane can be burned in a fuel cell to generate electricity directly. The maximum useful energy obtained in these cases is the maximum work, which equals the free-energy change. Calculate the standard free-energy change for the combustion of 1.00 mol of C(s) to CO2(g). Compare this value with the maximum obtained with the heat engine described here.arrow_forwardWrite the balanced chemical equation for the combustion of methane, CH4(g), to give carbon dioxide and water vapor. Explain why it is difficult to predict whether S is positive or negative for this chemical reaction.arrow_forwardAt 298 K, the standard enthalpies of formation for C2H2(g) and C6H6(l) are 227 kJ/mol and 49 kJ/mol, respectively. a. Calculate H for C6H6(l)3C2H2(g) b. Both acetylene (C2H2) and benzene (C6H6) can be used as fuels. Which compound would liberate more energy per gram when combusted in air?arrow_forward
- Define the following: a. spontaneous process b. entropy c. positional probability d. system e. surroundings f. universearrow_forward9.83 A student performing a calorimetry experiment combined 100.0 mL of 0.50 M HCl and 100.0 mL of 0.50 M NaOH in a coffee cup calorimeter. Both solutions were initially at 20.0°C, but when the two were mixed, the temperature rose to 23.2°C. (a) Suppose the experiment is repeated in the same calorimeter but this time using 200 mL of 0.50 M HCl and 200.0 mL of 0.50 M NaOH. Will the T observed he greater than, less than, or equal to that in the first experiment, and why? (b) Suppose that the experiment is repeated once again in the same calorimeter, this time using 100 mL of 1.00 M HCl and 100.0 mL of 1.00 M NaOH. Will the T observed he greater than, less than, or equal to that in the first experiment, and why?arrow_forwardWhat is entropy? Why is entropy important?arrow_forward
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