1 Chemical Foundations 2 Atomic Structure And Periodicity 3 Bonding: General Concepts 4 Molecular Structure And Orbitals 5 Stoichiometry 6 Types Of Chemical Reactions And Solution Stoichiometry 7 Chemical Energy 8 Gases 9 Liquids And Solids 10 Properties Of Solutions 11 Chemical Kinetics 12 Chemical Equilibrium 13 Acids And Bases 14 Acid- Base Equilibria 15 Solubility And Complex Lon Equilibria 16 Spontaneity, Entropy, And Free Energy 17 Electrochemistry 18 The Nucleus: A Chemist's View 19 The Representative Elements 20 Transition Metals And Coordination Chemistry 21 Organic And Biological Molecules Chapter7: Chemical Energy
Chapter Questions Section: Chapter Questions
Problem 1RQ: Define the following terms: potential energy, kinetic energy, path-dependent function, state... Problem 2RQ: Consider the following potential energy diagrams for two different reactions. Which plot represents... Problem 3RQ: What is the first law of thermodynamics? How can a system change its internal energy, E? What are... Problem 4RQ: When a gas expands, what is the sign of w? Why? When a gas contracts, what is the sign of w? Why?... Problem 5RQ Problem 6RQ: High-quality audio amplifiers generate large amounts of heat. To dissipate the heat and prevent... Problem 7RQ: Explain how calorimetry works to calculate H or E for a reaction. Does the temperature of the... Problem 8RQ: What is Hesss law? When a reaction is reversed, what happens to the sign and magnitude of H for that... Problem 9RQ: Define the standard enthalpy of formation. What are standard states for elements and for compounds?... Problem 1ALQ Problem 2ALQ Problem 3ALQ: A fire is started in a fireplace by striking a match and lighting crumpled paper under some logs.... Problem 4ALQ: Liquid water turns to ice. Is this process endothermic or exothermic? Explain what is occurring... Problem 5ALQ Problem 6ALQ Problem 7ALQ: Consider 5.5 L of a gas at a pressure of 3.0 atm in a cylinder with a movable piston. The external... Problem 8ALQ: Explain why oceanfront areas generally have smaller temperature fluctuations than inland areas. Problem 9ALQ: Hesss law is really just another statement of the first law of thermodynamics. Explain. Problem 10ALQ Problem 11Q Problem 12Q Problem 13Q: Assuming gasoline is pure C8H18(l), predict the signs of q and w for the process of combusting... Problem 14Q Problem 15Q: The enthalpy change for the reaction CH4(g)+2O2(g)CO2(g)+2H2O(l) is 891 kJ for the reaction as... Problem 16Q: For the reaction HgO(s)Hg(l)+12O2(g),H=+90.7KJ: a. What quantity of heat is required to produce 1... Problem 17Q Problem 18Q: The enthalpy change for a reaction is a state function and it is an extensive property. Explain. Problem 19Q: Standard enthalpies of formation are relative values. What are Hfvalues relative to? Problem 20Q: The combustion of methane can be represented as follows: a. Use the information given above to... Problem 21Q Problem 22Q Problem 23Q Problem 24Q Problem 25E Problem 26E Problem 27E: Consider the following diagram when answering the questions below. a. Compare balls A and B in terms... Problem 28E: Consider the accompanying diagram. Ball A is allowed to fall and strike ball B. Assume that all of... Problem 29E: A gas absorbs 45 kJ of heat and does 29 kJ of work. Calculate E. Problem 30E: A system releases 125 kJ of heat while 104 kJ of work is done on it. Calculate E. Problem 31E: Calculate E for each of the following. a. q = 47 kJ, w = + 88 kJ b. q = +82 kJ, w = 47 kJ c. q = +... Problem 32E: A system undergoes a process consisting of the following two steps: Step 1: The system absorbs 72 J... Problem 33E: If the internal energy of a thermodynamic system is increased by 300. J while 75 J of expansion work... Problem 34E: Calculate the internal energy change for each of the following. a. One hundred (100.) joules of work... Problem 35E: A sample of an ideal gas at 15.0 atm and 10.0 L is allowed to expand against a constant external... Problem 36E Problem 37E: Consider a mixture of air and gasoline vapor in a cylinder with a piston. The original volume is 40.... Problem 38E: As a system increases in volume, it absorbs 52.5 J of energy in the form of heat from the... Problem 39E: A balloon filled with 39.1 moles of helium has a volume of 876 L at 0.0C and 1.00 atm pressure. The... Problem 40E Problem 41E: One of the components of polluted air is NO. It is formed in the high-temperature environment of... Problem 42E Problem 43E: Are the following processes exothermic or endothermic? a. When solid KBr is dissolved in water, the... Problem 44E: Are the following processes exothermic or endothermic? a. the combustion of gasoline in a car engine... Problem 45E: The overall reaction in a commercial heat pack can be represented as 4Fe(s)+3O2(g)2Fe2O3(s)H=1652KJ... Problem 46E: Consider the following reaction: 2H2(g)+O2(g)2H2O(l)H=572KJ a. How much heat is evolved for the... Problem 47E: Consider the combustion of propane: C3H8(g)+5O2(g)3CO2(g)+4H2O(l)H=2221KJ Assume that all the heat... Problem 48E: Consider the following reaction: CH4(g)+2O2(g)CO2(g)+2H2O(l)H=891KJ Calculate the enthalpy change... Problem 49E Problem 50E: The specific heat capacity of silver is 0.24 J/Cg. a. Calculate the energy required to raise the... Problem 51E: A 500-g sample of one of the substances listed in Table 7-1 was heated from 25.2C to 55.1C,... Problem 52E Problem 53E: A 30.0-g sample of water at 280. K is mixed with 50.0 g water at 330. K. Calculate the final... Problem 54E: A biology experiment requires the preparation of a water bath at 37.0C (body temperature). The... Problem 55E: A 5.00-g sample of aluminum pellets (specific heat capacity = 0.89 J/C g) and a 10.00-g sample of... Problem 56E: Hydrogen gives off 120. J/g of energy when burned in oxygen, and methane gives off 50. J/g under the... Problem 57E Problem 58E: A 110.-g sample of copper (specific heat capacity = 0.20 J/C g) is heated to 82.4C and then placed... Problem 59E: In a coffee-cup calorimeter, 50.0 mL of 0.100 M AgNO3 and 50.0 mL of 0.100 M HCl are mixed to yield... Problem 60E: In a coffee-cup calorimeter, 100.0 mL of 1.0 M NaOH and 100.0 mL of 1.0 M HCI are mixed. Both... Problem 61E: A coffee-cup calorimeter initially contains 125 g water at 24.2C. Potassium bromide (10.5 g), also... Problem 62E: In a coffee-cup calorimeter, 1.60 g NH4NO3 is mixed with 75.0 g water at an initial temperature of... Problem 63E: Consider the dissolution of CaCl2: CaCl2(s)Ca2+(aq)+2Cl(aq)H=81.5KJ An 11.0-g sample of CaCl2 is... Problem 64E: Consider the reaction 2HCl(aq)+Ba(OH)2(aq)BaCl2(aq)+2H2O(l)H=118KJ Calculate the heat when 100.0 rnL... Problem 65E: The heat capacity of a bomb calorimeter was determined by burning 6.79 g methane (energy of... Problem 66E: The combustion of 0.1584 g benzoic acid increases the temperature of a bomb calorimeter by 2.54C.... Problem 67E: The enthalpy of combustion of solid carbon to form carbon dioxide is 393.7 KJ/mol carbon, and the... Problem 68E: Combustion reactions involve reacting a substance with oxygen. When compounds containing carbon and... Problem 69E: Given the following data calculate H for the reaction On the basis of the enthalpy change, is this a... Problem 70E: Given the following data... Problem 71E Problem 72E: Calculate H for the reaction 2NH3(g)+12O2(g)N2H4(l)+H2O(l) given the following data:... Problem 73E: Given the following data... Problem 74E: Given the following data... Problem 75E: Give the definition of the standard enthalpy of formation for a substance. Write separate reactions... Problem 76E: Write reactions for which the enthalpy change will be a. Hf for solid aluminum oxide. b. the... Problem 77E Problem 78E: Use the values of Hf in Appendix 4 to calculate H for the following reactions. (See Exercise 77 .)... Problem 79E: The Ostwald process for the commercial production of nitric acid from ammonia and oxygen involves... Problem 80E: Calculate H for each of the following reactions using the data in Appendix 4:... Problem 81E: The reusable booster rockets of the space shuttle use a mixture of aluminum and ammonium perchlorate... Problem 82E: The space shuttle Orbiter utilizes the oxidation of methylhydrazine by dinitrogen tetroxide for... Problem 83E: Consider the reaction 2ClF3(g)+2NH3(g)N2(g)+6HF(g)+Cl2(g)H=1196KJ Calculate H for CIF3(g). Problem 84E: The standard enthalpy of combustion of ethene gas, C2H4(g), is 1411.1 kJ/mol at 298 K. Given the... Problem 85E: Water gas is produced from the reaction of steam with coal: C(s)+H2O(g)H2(g)+CO(g) Assuming that... Problem 86E Problem 87E Problem 88E Problem 89E: Some automobiles and buses have been equipped to bum propane (C3H8). Compare the amounts of energy... Problem 90E: The complete combustion of acetylene, C2H2(g), produces 1300. kJ of energy per mole of acetylene... Problem 91AE Problem 92AE: One way to lose weight is to exercise! Walking briskly at 4.0 miles per hour for an hour consumes... Problem 93AE: Three gas-phase reactions were run in a constant-pressure piston apparatus as shown in the following... Problem 94AE: Nitrogen gas reacts with hydrogen gas to form ammonia gas .Consider the reaction between nitrogen... Problem 95AE: Combustion of table sugar produces CO2(g) and H2O( l). When 1.46 g table sugar is combusted in a... Problem 96AE Problem 97AE: Consider the following cyclic process carried out in two steps on a gas: Step 1: 45 J of heat is... Problem 98AE: Calculate H for the reaction 2K(s)+2H2O(l)2KOH(aq)+H2(g) A 5.00-g chunk of potassium is dropped into... Problem 99AE: The enthalpy of neutralization for the reaction of a strong acid with a strong base is 56 kJ/mol... Problem 100AE Problem 101AE: If a student performs an endothermic reaction in a calorimeter, how does the calculated value of H... Problem 102AE: In a bomb calorimeter, the reaction vessel is surrounded by water that must be added for each... Problem 103AE: The bomb calorimeter in Exercise 102 is filled with 987 g water. The initial temperature of the... Problem 104AE Problem 105AE: Consider the following equations: 3A+6B3DH=403KJ/molE+2FAH=105.2KJ/molCE+3DH=64.8KJ/mol Suppose the... Problem 106AE Problem 107AE: At 298 K, the standard enthalpies of formation for C2H2(g) and C6H6(l) are 227 kJ/mol and 49 kJ/mol,... Problem 108AE Problem 109AE: A sample of nickel is heated to 99.8C and placed in a coffee-cup calorimeter containing 150.0 g... Problem 110AE: Quinone is an important type of molecule that is involved in photosynthesis. The transport of... Problem 111AE: Calculate H for each of the following reactions, which occur in the atmosphere. a.... Problem 112AE: Compare your answers from parts a and b of Exercise 69 of Chapter 3 with H values calculated for... Problem 113AE: Compare your answer from Exercise 72 of Chapter 3 to the H value calculated from standard enthalpies... Problem 114CWP: Consider a balloon filled with helium at the following conditions. 313 g He 1.00 atm 1910. L Molar... Problem 115CWP Problem 116CWP Problem 117CWP Problem 118CWP: A swimming pool, 10.0 m by 4.0 m, is filled with water to a depth of 3.0 m at a temperature of... Problem 119CWP Problem 120CWP: Calculate H for the reaction N2H4(l)+O2(g)N2(g)+2H2O(l) given the following data: Equation H(KJ)... Problem 121CWP: Which of the following substances have an enthalpy of formation equal to zero? a. Cl2(g) b. H2(g) c.... Problem 122CP: Consider 2.00 moles of an ideal gas that are taken from state A (PA = 2.00 atm, vA = 10.0 L) to... Problem 123CP: For the process H2O(l)H2O(g) at 298 K and 1.0 atm, H is more positive than E by 2.5 kJ/mol. What... Problem 124CP: The sun supplies energy at a rate of about 1.0 kilowatt per square meter of surface area (1 watt = 1... Problem 125CP Problem 126CP: The standard enthalpies of formation for S(g), F(g), SF4(g), and SF6(g) are +278.8, +79.0, 775, and... Problem 127CP: Use the following standard enthalpies of formation to estimate the N-H bond energy in ammonia: N(g),... Problem 128CP: The standard enthalpy of formation for N2H4(g) is 95.4 kJ/mol. Use this and the data in Exercise 127... Problem 129CP: The standard enthalpy of formation for NO(g) is 90. kJ/mol. Use this and the values for the O 9 O... Problem 130CP: A piece of chocolate cake contains about 400 calories. A nutritional calorie is equal to 1000... Problem 131CP: You have a l.00-mole sample of water at 30.C and you heat it until you have gaseous water at 140.C.... Problem 132CP: A 500.0-g sample of an element at 195C is dropped into an ice--water mixture; 109.5 g ice melts and... Problem 133IP: A cubic piece of uranium metal (specific heat capacity = 0.117 J/C g) at 200.0C is dropped into... Problem 134IP: On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado.... Problem 135IP: Using data from Chapter 2, calculate the change in energy expected for each of the following... Problem 136IP: In Exercise 89 in Chapter 3, the Lewis structures for benzene (C6H6) were drawn. Using one of the... Problem 137MP: A gaseous hydrocarbon reacts completely with oxygen gas to form carbon dioxide and water vapour.... Problem 134IP: On Easter Sunday, April 3, 1983, nitric acid spilled from a tank car near downtown Denver, Colorado....
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A. What type of chemical reaction ?
B. Write the net ionic equation for the chemical reaction.
Transcribed Image Text: Consider the following chemical reaction
HCI (aq) + H&N03 (aq) → Hg2Cl2 (s) + HNO3 (aq)
If 20.0 grams of HCI is mixed with 30.0 grams of HgNO,. Determine
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Definition Definition Transformation of a chemical species into another chemical species. A chemical reaction consists of breaking existing bonds and forming new ones by changing the position of electrons. These reactions are best explained using a chemical equation.
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