Exam 5: Thermochemistry: Energy Changes in Reactions
Exam 1: Matter and Energy: The Origin of the Universe99 Questions
Exam 2: Atoms, Ions, and Molecules: Matter Starts Here131 Questions
Exam 3: Stoichiometry: Mass, Formulas, and Reactions133 Questions
Exam 4: Solution Chemistry: The Hydrosphere126 Questions
Exam 5: Thermochemistry: Energy Changes in Reactions132 Questions
Exam 6: Properties of Gases: the Air We Breathe138 Questions
Exam 7: A Quantum Model of Atoms: Waves and Particles143 Questions
Exam 8: Chemical Bonds: What Makes a Gas a Greenhouse Gas139 Questions
Exam 9: Molecular Geometry: Shape Determines Function136 Questions
Exam 10: Intermolecular Forces: The Uniqueness of Water140 Questions
Exam 11: Solutions: Properties and Behavior130 Questions
Exam 12: Solids: Structures and Applications144 Questions
Exam 13: Organic Chemistry: Fuels, Pharmaceuticals, Materials, and Life129 Questions
Exam 14: Chemical Kinetics: Reactions in the Air We Breathe164 Questions
Exam 15: Chemical Equilibrium: How Much Product Does a Reaction Really Make91 Questions
Exam 16: Acid-Base and Solubility Equilibria: Reactions in Soil and Water179 Questions
Exam 17: Metal Ions: Colorful and Essential144 Questions
Exam 18: Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes157 Questions
Exam 19: Electrochemistry: the Quest for Clean Energy143 Questions
Exam 20: Biochemistry: the Compounds of Life108 Questions
Exam 21: Nuclear Chemistry: Applications to Energy and Medicine144 Questions
Exam 22: Life and the Periodic Table95 Questions
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The integrated circuits in your cell phone and computer are made from the semiconductor silicon. The silicon is obtained from a really inexpensive starting material, sand, which is primarily SiO2. One step in the purification of silicon is to separate it from solid impurities by forming the gas silicon tetrachloride. Given the following reactions, what is the overall enthalpy change in converting 1.00 mol of silicon dioxide into pure silicon? Reaction () (s)+2(s)\rightarrow (impure s +2(g) +690 ()+2(g)\rightarrow(g) -657 (g)+2(s)\rightarrow2(s)+(s) -625
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When ammonium nitrate (NH4NO3)(s) is used in explosives, it decomposes to N2(g), O2(g), and H2O(g). Write a balanced reaction equation for the decomposition of ammonium nitrate, and determine the standard enthalpy of reaction using standard enthalpies of formation:
solid ammonium nitrate = -366 kJ/mol and water vapor = -242 kJ/mol.
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The kinetic energy associated with the random motion of molecules is called ________
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You have a summer job in a lead foundry. Your task is to identify how energy efficiency can be improved. You therefore need to know the minimum amount of energy it takes to raise 1 pound of lead (454 g) from room temperature (25°C) to its melting point (327°C) and then melt it. The specific heat capacity of lead is 0.159 J/(g .°C), the enthalpy of fusion is 24.7 J/g, and the molar mass is 207 g/mol.
(Multiple Choice)
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Which statement regarding combustion of a sample of gasoline in a bomb calorimeter is correct?
(Multiple Choice)
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Lightweight camping stoves typically use a mixture of C5 and C6 hydrocarbons, which is called white gas. Assuming white gas is 100% C6H14 with an enthalpy of combustion of -4,150 kJ/mol, how many grams of it must be used to heat 1.50 L of water from 20°C to 90°C? Assume all the energy is used to heat the water.
(Multiple Choice)
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A 15 g piece of iron (CP = 25.09 J/(mol · °C)) is heated to a temperature of 95°C and placed into a bucket containing 4.5 gal of water (CP = 75.38 J/(mol · °C)) initially at 25°C. Eventually,
(Multiple Choice)
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Which of the following fuels has the highest fuel value (kJ/g)?
(Multiple Choice)
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How much work does a gas do when it expands against a constant pressure of 0.500 atm from a volume of 50.00 mL to a volume of 350.00 mL? (101.3 J = 1 L atm)
(Multiple Choice)
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The inside of a perfectly insulated capped thermos bottle is an example of ________
(Multiple Choice)
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Energy that an object has by virtue of its position is called ________
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Isooctane is a good model compound for gasoline. When 1.14 g of isooctane (114 g/mol) reacts with excess oxygen in a constant pressure calorimeter, the temperature of the calorimeter increases by 10.0oC. The heat capacity of the calorimeter is 5.46 kJ/oC. Determine the molar enthalpy of combustion of isooctane.
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