- 9.9.1: You are calculating DE in a chemistry problem. What if you confuse ...
- 9.9.2: What if Hesss law were not true? What are some possible repercussio...
- 9.9.3: For DHreaction calculations we define DH8f for an element in its st...
- 9.9.4: Objects placed together eventually reach the same temperature. When...
- 9.9.5: What is meant by the term lower in energy? Which is lower in energy...
- 9.9.6: A fire is started in a fireplace by striking a match and lighting c...
- 9.9.7: Liquid water turns to ice. Is this process endothermic or exothermi...
- 9.9.8: Consider the following statements: Heat is a form of energy, and en...
- 9.9.9: Photosynthetic plants use the following reaction to produce glucose...
- 9.9.10: Photosynthetic plants use the following reaction to produce glucose...
- 9.9.11: Predict the signs of q and w for the process of boiling water.
- 9.9.12: Hesss law is really just another statement of the first law of ther...
- 9.9.13: In the equation w 5 2PDV, why is there a negative sign?
- 9.9.14: Why is Cp larger than Cv? Provide a conceptual rationale
- 9.9.15: You have an ideal gas with an initial volume of 1.0 L and initial p...
- 9.9.16: When is DH 5 5 2RT? When is DE 5 5 2RT? When is DH 5 3 2RT? When is...
- 9.9.17: For a liquid, which would you expect to be larger: DHvaporization o...
- 9.9.18: Consider the accompanying diagram. Ball A is allowed to fall and st...
- 9.9.19: Consider the following potential energy diagrams for two different ...
- 9.9.20: Consider an airplane trip from Chicago, Illinois, to Denver, Colora...
- 9.9.21: Assuming gasoline is pure C8H18(l), predict the signs of q and w fo...
- 9.9.22: Consider 2.00 moles of an ideal gas that is taken from state A (PA ...
- 9.9.23: A sample of an ideal gas at 15.0 atm and 10.0 L is allowed to expan...
- 9.9.24: A piston performs work of 210. L ? atm on the surroundings, while t...
- 9.9.25: A system undergoes a process consisting of the following two steps:...
- 9.9.26: Calculate the internal energy change for each of the following. a. ...
- 9.9.27: A balloon filled with 39.1 moles of helium has a volume of 876 L at...
- 9.9.28: Consider a mixture of air and gasoline vapor in a cylinder with a p...
- 9.9.29: One mole of H2O(g) at 1.00 atm and 100.8C occupies a volume of 30.6...
- 9.9.30: As a system increases in volume, it absorbs 52.5 J of energy in the...
- 9.9.31: What is the difference between DH and DE at constant P?
- 9.9.32: The enthalpy change for a reaction is a state function and it is an...
- 9.9.33: One of the components of polluted air is NO. It is formed in the hi...
- 9.9.34: Are the following processes exothermic or endothermic? a. the combu...
- 9.9.35: The reaction SO3(g) 1 H2O(l) 88n H2SO4(aq) is the last step in the ...
- 9.9.36: Consider the following reaction: 2H2(g) 1 O2(g) 88n 2H2O(l) DH 5 25...
- 9.9.37: The overall reaction in a commercial heat pack can be represented a...
- 9.9.38: Consider the combustion of propane: C3H8(g) 1 5O2(g) 88n 3CO2(g) 1 ...
- 9.9.39: For the process H2O(l) 88n H2O(g) at 298 K and 1.0 atm, DH is more ...
- 9.9.40: For the following reactions at constant pressure, predict if DH . D...
- 9.9.41: Calculate the energy required to heat 1.00 kg of ethane gas (C2H6) ...
- 9.9.42: Calculate q, w, DE, and DH for the process in which 88.0 g of nitro...
- 9.9.43: Consider 111 J of heat added to 30.3 g of Ne on STP. Determine w, D...
- 9.9.44: Consider a sample containing 2.00 moles of a monatomic ideal gas th...
- 9.9.45: Explain how calorimetry works to calculate DH or DE for a reaction....
- 9.9.46: The specific heat capacity of silver is 0.24 J 8C21 g21. a. Calcula...
- 9.9.47: Consider the substances in Table 9.3. Which substance requires the ...
- 9.9.48: A 150.0-g sample of a metal at 75.08C is added to 150.0 g of H2O at...
- 9.9.49: A 150.0-g sample of a metal at 75.08C is added to 150.0 g of H2O at...
- 9.9.50: A biology experiment requires the preparation of a water bath at 37...
- 9.9.51: A 5.00-g sample of aluminum pellets (specific heat capacity 5 0.89 ...
- 9.9.52: A sample of nickel is heated to 99.88C and placed in a coffee cup c...
- 9.9.53: Hydrogen gives off 120. J/g of energy when burned in oxygen, and me...
- 9.9.54: In a coffee cup calorimeter, 50.0 mL of 0.100 M AgNO3 and 50.0 mL o...
- 9.9.55: In a coffee cup calorimeter, 100.0 mL of 1.0 M NaOH and 100.0 mL of...
- 9.9.56: A coffee cup calorimeter initially contains 125 g water at 24.28C. ...
- 9.9.57: In a coffee cup calorimeter, 1.60 g of NH4NO3 is mixed with 75.0 g ...
- 9.9.58: Consider the dissolution of CaCl2: CaCl2(s) 88n Ca21(aq) 1 2Cl2(aq)...
- 9.9.59: Consider the reaction 2HCl(aq) 1 Ba(OH)2(aq) 88n BaCl2(aq) 1 2H2O(l...
- 9.9.60: The heat capacity of a bomb calorimeter was determined by burning 6...
- 9.9.61: The combustion of 0.1584 g benzoic acid increases the temperature o...
- 9.9.62: Combustion of table sugar produces CO2(g) and H2O(l). When 1.46 g o...
- 9.9.63: Calculate w and DE when 1 mole of a liquid is vaporized at its boil...
- 9.9.64: Calculate DH for the reaction 2NH3(g) 1 1 2O2(g) 88n N2H4(l) 1 H2O(...
- 9.9.65: Given the following data: C2H2(g) 1 5 2O2(g) 88n 2CO2(g) 1 H2O(l) D...
- 9.9.66: Given the following data: 2ClF(g) 1 O2(g) 88n Cl2O(g) 1 F2O(g) DH 5...
- 9.9.67: Given the following data: Ca(s) 1 2C(graphite) 88n CaC2(s) DH 5 262...
- 9.9.68: Given the following data: Fe2O3(s) 1 3CO(g) 88n 2Fe(s) 1 3CO2(g) DH...
- 9.9.69: Combustion reactions involve reacting a substance with oxygen. When...
- 9.9.70: Given the following data: 2O3(g) 88n 3O2(g) DH 5 2427 kJ O2(g) 88n ...
- 9.9.71: The bombardier beetle uses an explosive discharge as a defensive me...
- 9.9.72: Given the definition of the standard enthalpy of formation for a su...
- 9.9.73: The combustion of methane can be represented as follows: Reactants ...
- 9.9.74: Use the values of DH8f in Appendix 4 to calculate DH8 for the follo...
- 9.9.75: The Ostwald process for the commercial production of nitric acid fr...
- 9.9.76: Calculate DH8 for each of the following reactions using the data in...
- 9.9.77: The reusable booster rockets of the space shuttle use a mixture of ...
- 9.9.78: The space shuttle Orbiter utilizes the oxidation of methylhydrazine...
- 9.9.79: Does the reaction in Exercise 76 or that in Exercise 77 produce mor...
- 9.9.80: At 298 K, the standard enthalpies of formation for C2H2(g) and C6H6...
- 9.9.81: occur in the atmosphere. a. C2H4(g) 1 O3(g) n CH3CHO(g) 1 O2(g) b. ...
- 9.9.82: Use the reaction 2ClF3(g) 1 2NH3(g) 88n N2(g) 1 6HF(g) 1 Cl2(g) DH8...
- 9.9.83: The standard enthalpy of combustion of ethene gas [C2H4(g)] is 2141...
- 9.9.84: What is incomplete combustion of fossil fuels? Why can this be a pr...
- 9.9.85: Explain the advantages and disadvantages of hydrogen as an alternat...
- 9.9.86: The complete combustion of acetylene [C2H2(g)] produces 1300. kJ of...
- 9.9.87: Assume that 4.19 3 106 kJ of energy is needed to heat a home. If th...
- 9.9.88: Syngas can be burned directly or converted to methanol. Calculate D...
- 9.9.89: Ethanol (C2H5OH) has been proposed as an alternative fuel. Calculat...
- 9.9.90: Methanol (CH3OH) has also been proposed as an alternative fuel. Cal...
- 9.9.91: Some automobiles and buses have been equipped to burn propane (C3H8...
- 9.9.92: Consider the following cyclic process carried out in two steps on a...
- 9.9.93: Determine DE for the process H2O(l) 88n H2O(g) at 258C and 1 atm
- 9.9.94: The standard enthalpy of formation of H2O(l) at 298 K is 2285.8 kJ/...
- 9.9.95: A piece of chocolate cake contains about 400 Calories. A nutritiona...
- 9.9.96: It has been determined that the body can generate 5500 kJ of energy...
- 9.9.97: Nitromethane, CH3NO2, can be used as a fuel. When the liquid is bur...
- 9.9.98: In a bomb calorimeter, the bomb is surrounded by water that must be...
- 9.9.99: The bomb calorimeter in Exercise 97 is filled with 987 g of water. ...
- 9.9.100: When 1.00 L of 2.00 M Na2SO4 solution at 30.08C is added to 2.00 L ...
- 9.9.101: If a student performs an endothermic reaction in a calorimeter, how...
- 9.9.102: The enthalpy of neutralization for the reaction of a strong acid wi...
- 9.9.103: Three gas-phase reactions were run in a constant-pressure piston ap...
- 9.9.104: Consider the following changes: a. N2(g) n N2(l) b. CO(g) 1 H2O(g) ...
- 9.9.105: Nitrogen gas reacts with hydrogen gas to form ammonia gas . Conside...
- 9.9.106: Using the following data, calculate the standard heat of formation ...
- 9.9.107: High-quality audio amplifiers generate large amounts of heat. To di...
- 9.9.108: Write reactions that correspond to the following enthalpy changes: ...
- 9.9.109: Consider a balloon filled with helium at the following conditions. ...
- 9.9.110: In which of the following systems is(are) work done by the surround...
- 9.9.111: Which of the following processes are exothermic? a. N2 1g2 h 2N1g2 ...
- 9.9.112: Consider the reaction B2H6 1g2 1 3O2 1g2 h B2O3 1s2 1 3H2O1g2 DH 5 ...
- 9.9.113: A swimming pool, 10.0 m by 4.0 m, is filled with water to a depth o...
- 9.9.114: In a coffee-cup calorimeter, 150.0 mL of 0.50 M HCl is added to 50....
- 9.9.115: Calculate DH for the reaction N2H4 1l2 1 O2 1g2 h N2 1g2 1 2H2O1l2 ...
- 9.9.116: Which of the following substances have an enthalpy of formation equ...
- 9.9.117: The heat required to raise the temperature from 300.0 K to 400.0 K ...
- 9.9.118: When water is supercooled, it freezes at a temperature below 0.08C....
- 9.9.119: The sun supplies energy at a rate of about 1.0 kilowatt per square ...
- 9.9.120: The heat of vaporization of water at the normal boiling point, 373....
- 9.9.121: Consider the following reaction at 2488C and 1.00 atm: CH3Cl(g) 1 H...
- 9.9.122: The best solar panels currently available are about 19% efficient i...
- 9.9.123: You have 2.4 moles of a gas contained in a 4.0-L bulb at a temperat...
- 9.9.124: An isothermal process is one in which the temperatures of the syste...
- 9.9.125: You have a 1.00-mole sample of water at 230.8C, and you heat it unt...
- 9.9.126: Consider a sample containing 5.00 moles of a monatomic ideal gas th...
- 9.9.127: A gaseous hydrocarbon reacts completely with oxygen gas to form car...
Solutions for Chapter 9: Energy, Enthalpy, and Thermochemistry
Full solutions for Chemical Principles | 8th Edition
ISBN: 9781305581982
Solutions for Chapter 9
28
2
Since 127 problems in chapter 9: Energy, Enthalpy, and Thermochemistry have been answered, more than 66964 students have viewed full step-by-step solutions from this chapter. This expansive textbook survival guide covers the following chapters and their solutions. This textbook survival guide was created for the textbook: Chemical Principles, edition: 8. Chemical Principles was written by and is associated to the ISBN: 9781305581982. Chapter 9: Energy, Enthalpy, and Thermochemistry includes 127 full step-by-step solutions.
Key Chemistry Terms and definitions covered in this textbook
-
allylic bromination
A radical reaction that achieves installation of a bromine atom at an allylic position.
-
amino sugars
Carbohydrate derivatives in which an OH group has been replaced with an amino group.
-
band
An array of closely spaced molecular orbitals occupying a discrete range of energy. (Section 12.4)
-
Charles’ law.
The volume of a fixed amount of gas maintained at constant pressure is directly proportional to the absolute temperature of the gas. (5.3)
-
coordination-sphere isomers
Structural isomers of coordination compounds in which the ligands within the coordination sphere differ. (Section 23.4)
-
Correlation tables
Tables of data on absorption patterns of functional groups.
-
coupling constant
When signal splitting occurs in NMR spectroscopy, the distance between the individual peaks of a signal.
-
dihydroxylation
A reaction characterized by the addition of two hydroxyl groups (OH) across an alkene.
-
enantiomers
Two mirror-image molecules of a chiral substance. The enantiomers are nonsuperimposable. (Section 23.4)
-
Entropy (S)
Measures chaos versus order and chaos is favorable
-
Haloalkene (vinylic halide)
A compound containing a halogen atom bonded to one of the carbons of a carbon-carbon double bond.
-
molecularity
The number of molecules that participate as reactants in an elementary reaction. (Section 14.6)
-
pericylic reactions
Reactions that occur via a concerted process and do not involve either ionic or radical intermediates.
-
phase change
The conversion of a substance from one state of matter to another. The phase changes we consider are melting and freezing 1solid ? liquid2, sublimation and deposition, and vaporization and condensation 1liquid ? gas2. (Section 11.4)
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photon
When electromagnetic radiation is viewed as a particle, an individual packet of energy.
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polar covalent bond
A covalent bond in which the electrons are not shared equally. (Section 8.4)
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racemic mixture
A solution containing equal amounts of both enantiomers.
-
Reaction coordinate diagram
A graph showing the energy changes that occur during a chemical reaction; energy is plotted on the vertical axis and reaction progress is plotted on the horizontal axis.
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thiols
Compounds containing a mercapto group (SH).
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valence bond theory
A theory that treats a bond as the sharing of electrons that are associated with individual atoms, rather than being associated with the entire molecule.