General Chemistry - Standalone book (MindTap Course List) 11th Edition
ISBN: 9781305580343
Author: Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher: Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
1 Chemistry And Measurement 2 Atoms, Molescules, And Ions 3 Calculations With Chemical Formulas And Equaitons 4 Chemical Reactions 5 The Gaseous State 6 Thermochemisty 7 Quantum Theory Of The Atom 8 Electron Configurations And Periodicity 9 Ionic And Covalent Bonding 10 Molecular Geometry And Chemical Bonding Theory 11 States Of Matter; Liquids And Solids 12 Solutions 13 Rates Of Reaction 14 Chemical Equilibirum 15 Acids And Bases 16 Acid-base Equilibria 17 Solubility And Complex-ion Equilibria 18 Thermodynamics And Equilibrium 19 Electrochemistry 20 Nuclear Chemistry 21 Chemistry Of The Main-group Elements 22 The Transition Elements And Coordination Compounds 23 Organic Chemistry 24 Polymer Materials: Synthetic And Biological A.1 Scientific (exponential) Notation A.2 Logarithms A.3 Algebraic Operations And Graphing Chapter6: Thermochemisty
6.1 Energy And Its Units 6.2 First Law Of Thermodynamics; Work And Heat 6.3 Heat Of Reaction; Enthalpy Of Reaction 6.4 Thermochemical Equaitons 6.5 Applying Stoichiometry To Heats Of Reaction 6.6 Measuring Heats Of Reaction 6.7 Hess's Law 6.8 Standard Enthalpies Of Formation 6.9 Fuels-food, Commercial Fuels And Rocket Fuels Chapter Questions Section: Chapter Questions
Problem 6.1QP: Define energy, kinetic energy, potential energy, and internal energy. Problem 6.2QP: Define the joule in terms of SI base units. Problem 6.3QP Problem 6.4QP: Describe the interconversions of potential and kinetic energy in a moving pendulum. A moving... Problem 6.5QP: Suppose heat flows into a vessel containing a gas. As the heat flows into the gas, what happens to... Problem 6.6QP: Define an exothermic reaction and an endothermic reaction. Give an example of each. Problem 6.7QP Problem 6.8QP: Under what condition is the enthalpy change equal to the heat of reaction? Problem 6.9QP Problem 6.10QP: Why is it important to give the states of the reactants and products when giving an equation for H? Problem 6.11QP: If an equation for a reaction is doubled and then reversed, how is the value of H changed? Problem 6.12QP Problem 6.13QP Problem 6.14QP: Describe a simple calorimeter. What measurements are needed to determine the heat of reaction? Problem 6.15QP Problem 6.16QP: You discover that you cannot carry out a particular reaction for which you would like the enthalpy... Problem 6.17QP Problem 6.18QP Problem 6.19QP Problem 6.20QP Problem 6.21QP: Is the following reaction the appropriate one to use in determining the enthalpy of formation of... Problem 6.22QP Problem 6.23QP Problem 6.24QP Problem 6.25QP: The equation for the combustion of 2 mol of butane can be written 2C4H10(g)+O2(g)8CO2(g)+10H2O(g);HO... Problem 6.26QP: A 5.0-g sample of water starting at 60.0C loses 418 J of energy in the form of heat. What is the... Problem 6.27QP: Hypothetical elements A2 and B2 react according to the following equation, forming the compound AB.... Problem 6.28QP: Consider the following specific heats of metals. Metal Specific Heat copper 0.385 J/(gC) magnesium... Problem 6.29QP: Thermal Interactions Part 1: In an insulated container, you mix 200. g of water at 80C with 100. g... Problem 6.30QP: Enthalpy a A 100.-g sample of water is placed in an insulated container and allowed to come to room... Problem 6.31QP: Chemical reactions are run in each of the beakers depicted below (labeled A, B, and C). The... Problem 6.32QP: Shown below is a diagram depicting the enthalpy change of a chemical reaction run at constant... Problem 6.33QP: A small car is traveling at twice the speed of a larger car, which has twice the mass of the smaller... Problem 6.34QP: The equation for the combustion of butane, C4H10, is C4H10(g)+132O2(g)4CO2(g)+5H2O(g) Which one of... Problem 6.35QP: A 250-g sample of water at 20.0C is placed in a freezer that is held at a constant temperature of... Problem 6.36QP: A 20.0-g block of iron at 50.0C and a 20.0 g block of aluminum at 45C are placed in contact with... Problem 6.37QP Problem 6.38QP: A block of aluminum and a block of iron, both having the same mass, are removed from a freezer and... Problem 6.39QP: You have two samples of different metals, metal A and metal B, each having the same mass. You heat... Problem 6.40QP: Consider the reactions of silver metal, Ag(s), with each of the halogens: fluorine, F2(g), chlorine,... Problem 6.41QP Problem 6.42QP: A soluble salt, MX2, is added to water in a beaker. The equation for the dissolving of the salt is:... Problem 6.43QP: Methane, CH4, is a major component of marsh gas. When 0.5000 mol methane burns to produce carbon... Problem 6.44QP: Hydrogen sulfide, H2S, is produced during decomposition of organic matter. When 0.5000 mol H2S burns... Problem 6.45QP Problem 6.46QP Problem 6.47QP: Chlorine dioxide, ClO2, is a reddish yellow gas used in bleaching paper pulp. The average speed of a... Problem 6.48QP: Nitrous oxide, N2O, has been used as a dental anesthetic. The average speed of an N2O molecule at... Problem 6.49QP: A gas is cooled and loses 82 J of heat. The gas contracts as it cools, and work done on the system... Problem 6.50QP: An ideal gas expands isothermally (at constant temperature). The internal energy of an ideal gas... Problem 6.51QP: The process of dissolving ammonium nitrate, NH4NO3, in water is an endothermic process. What is the... Problem 6.52QP: The decomposition of ozone, O3, to oxygen, O2, is an exothermic reaction. What is the sign of q? If... Problem 6.53QP: Nitric acid, a source of many nitrogen compounds, is produced from nitrogen dioxide. An old process... Problem 6.54QP: Hydrogen cyanide is used in the manufacture of clear plastics such as Lucite and Plexiglas. It is... Problem 6.55QP: What is U when 1.00 mol of liquid water vaporizes at 100C? The heat of vaporization, Hvap, of water... Problem 6.56QP: What is U for the following reaction at 25C? 2H2(g)+O2(g)2H2O(l) Problem 6.57QP: When 1 mol of iron metal reacts with hydrochloric acid at constant temperature and pressure to... Problem 6.58QP: When 2 mol of potassium chlorate crystals decompose to potassium chloride crystals and oxygen gas at... Problem 6.59QP: When white phosphorus burns in air, it produces phosphorus(V) oxide. P4(s)+5O2(g)P4O10(s);H=3010kJ... Problem 6.60QP: Carbon disulfide burns in air, producing carbon dioxide and sulfur dioxide.... Problem 6.61QP: Phosphoric acid, H3PO4, can be prepared by the reaction of phosphorus(V) oxide, P4O10, with water.... Problem 6.62QP: With a platinum catalyst, ammonia will burn in oxygen to give nitric oxide, NO.... Problem 6.63QP: Colorless nitric oxide, NO, combines with oxygen to form nitrogen dioxide, NO2, a brown gas.... Problem 6.64QP: Hydrogen, H2, is used as a rocket fuel. The hydrogen is burned in oxygen to produce water vapor.... Problem 6.65QP: Ammonia burns in the presence of a copper catalyst to form nitrogen gas.... Problem 6.66QP: Hydrogen sulfide, H2S, is a foul-smelling gas. It burns to form sulfur dioxide.... Problem 6.67QP: Propane, C3H8, is a common fuel gas. Use the following to calculate the grams of propane you would... Problem 6.68QP: Ethanol, C2H5OH, is mixed with gasoline and sold as gasohol. Use the following to calculate the... Problem 6.69QP: You wish to heat water to make coffee. How much heat (in joules) must be used to raise the... Problem 6.70QP: An iron skillet weighing 1.63 kg is heated on a stove to 178C. Suppose the skillet is cooled to room... Problem 6.71QP: When steam condenses to liquid water, 2.26 kJ of heat is released per gram. The heat from 168 g of... Problem 6.72QP: When ice at 0C melts to liquid water at 0C, it absorbs 0.334 kJ of heat per gram. Suppose the heat... Problem 6.73QP: When 15.3 g of sodium nitrate, NaNO3, was dissolved in water in a constant-pressure calorimeter, the... Problem 6.74QP: When 23.6 g of calcium chloride, CaCl2, was dissolved in water in a constant-pressure calorimeter,... Problem 6.75QP: A sample of ethanol, C2H5OH, weighing 2.84 g was burned in an excess of oxygen in a bomb... Problem 6.76QP: A sample of benzene, C6H6, weighing 3.51 g was burned in an excess of oxygen in a bomb calorimeter.... Problem 6.77QP: Hydrazine, N2H4, is a colorless liquid used as a rocket fuel. What is the enthalpy change for the... Problem 6.78QP: Hydrogen peroxide, H2O2, is a colorless liquid whose solutions are used as a bleach and an... Problem 6.79QP: Ammonia will burn in the presence of a platinum catalyst to produce nitric oxide, NO.... Problem 6.80QP: Hydrogen cyanide is a highly poisonous, volatile liquid. It can be prepared by the reaction... Problem 6.81QP: Compounds with carboncarbon double bonds, such as ethylene, C2H4, add hydrogen in a reaction called... Problem 6.82QP: Acetic acid, CH3COOH, is contained in vinegar. Suppose acetic acid was formed from its elements,... Problem 6.83QP: The cooling effect of alcohol on the skin is due to its evaporation. Calculate the heat of... Problem 6.84QP: Carbon tetrachloride, CCl4, is a liquid used as an industrial solvent and in the preparation of... Problem 6.85QP: Hydrogen sulfide gas is a poisonous gas with the odor of rotten eggs. It occurs in natural gas and... Problem 6.86QP: Carbon disulfide is a colorless liquid. When pure, it is nearly odorless, but the commercial product... Problem 6.87QP: Iron is obtained from iron ore by reduction with carbon monoxide. The overall reaction is... Problem 6.88QP: The first step in the preparation of lead from its ore (galena, PbS) consists of roasting the ore.... Problem 6.89QP: Hydrogen chloride gas dissolves in water to form hydrochloric acid (an ionic solution).... Problem 6.90QP: Carbon dioxide from the atmosphere weathers, or dissolves, limestone (CaCO3) by the reaction... Problem 6.91QP: The Group 2A carbonates decompose when heated. For example, MgCO3(s)MgO(s)+CO2(g) Use enthalpies of... Problem 6.92QP: The Group 2A carbonates decompose when heated. For example, BaCO3(s)BaO(s)+CO2(g) Use enthalpies of... Problem 6.93QP Problem 6.94QP Problem 6.95QP: Liquid hydrogen peroxide has been used as a propellant for rockets. Hydrogen peroxide decomposes... Problem 6.96QP: Hydrogen is an ideal fuel in many respects; for example, the product of its combustion, water, is... Problem 6.97QP: Niagara Falls has a height of 167 ft (American Falls). What is the potential energy in joules of... Problem 6.98QP Problem 6.99QP: When calcium carbonate, CaCO3 (the major constituent of limestone and seashells), is heated, it... Problem 6.100QP: Calcium oxide (quicklime) reacts with water to produce calcium hydroxide (slaked lime).... Problem 6.101QP: Formic acid, HCHO2, was first discovered in ants (formica is Latin for ant). In an experiment, 5.48... Problem 6.102QP: Acetic acid, HC2H3O2, is the sour constituent of vinegar (acetum is Latin for vinegar). In an... Problem 6.103QP: Suppose you mix 19.8 g of water at 80.0C with 54.7 g of water at 29.0C in an insulated cup. What is... Problem 6.104QP: Suppose you mix 23.6 g of water at 66.2C with 45.4 g of water at 35.7C in an insulated cup. What is... Problem 6.105QP: A piece of lead of mass 121.6 g was heated by an electrical coil. From the resistance of the coil,... Problem 6.106QP: The specific heat of copper metal was determined by putting a piece of the metal weighing 35.4 g in... Problem 6.107QP: A 44.3 g sample of water at 100.00C was placed in an insulated cup. Then 25.4 g of zinc metal at... Problem 6.108QP: A 19.6-g sample of a metal was heated to 61.67C. When the metal was placed into 26.7 g of water in a... Problem 6.109QP: A 21.3-mL sample of 0.977 M NaOH is mixed with 29.5 mL of 0.918 M HCl in a coffee-cup calorimeter... Problem 6.110QP: A 29.1-mL sample of 1.05 M KOH is mixed with 20.9 mL of 1.07 M HBr in a coffee-cup calorimeter (see... Problem 6.111QP: In a calorimetric experiment, 6.48 g of lithium hydroxide, LiOH, was dissolved in water. The... Problem 6.112QP: When 21.45 g of potassium nitrate, KNO3, was dissolved in water in a calorimeter, the temperature... Problem 6.113QP: A 10.00-g sample of acetic acid, HC2H3O2, was burned in a bomb calorimeter in an excess of oxygen.... Problem 6.114QP: The sugar arabinose, C5H10O5, is burned completely in oxygen in a calorimeter.... Problem 6.115QP: Hydrogen sulfide, H2S, is a poisonous gas with the odor of rotten eggs. The reaction for the... Problem 6.116QP: Ethylene glycol, HOCH2CH2OH, is used as antifreeze. It is produced from ethylene oxide, C2H4O, by... Problem 6.117QP: Hydrogen, H2, is prepared by steam reforming, in which hydrocarbons are reacted with steam. For CH4,... Problem 6.118QP: Hydrogen is prepared from natural gas (mainly methane, CH4) by partial oxidation.... Problem 6.119QP: Calcium oxide, CaO, is prepared by heating calcium carbonate (from limestone and seashells).... Problem 6.120QP: Sodium carbonate, Na2CO3, is used to manufacture glass. It is obtained from sodium hydrogen... Problem 6.121QP: Calculate the heat released when 2,395 L O2 with a density of 1.11 g/L at 25C reacts with an excess... Problem 6.122QP Problem 6.123QP: Sucrose, C12H22O11, is common table sugar. The enthalpy change at 25C and 1 atm for the complete... Problem 6.124QP Problem 6.125QP: Ammonium nitrate is an oxidizing agent and can give rise to explosive mixtures. A mixture of 2.00... Problem 6.126QP Problem 6.127QP Problem 6.128QP Problem 6.129QP Problem 6.130QP Problem 6.131QP Problem 6.132QP Problem 6.133QP: Dry ice is solid carbon dioxide; it vaporizes at room temperature and normal pressures to the gas.... Problem 6.134QP Problem 6.135QP Problem 6.136QP: Sulfur dioxide gas reacts with oxygen, O2(g), to produce SO3(g). This reaction releases 99.0 kJ of... Problem 6.137QP: When solid iron burns in oxygen gas (at constant pressure) to produce Fe2O3(s), 1651 kJ of heat is... Problem 6.138QP: Calculate the grams of oxygen gas required to produce 7.60 kJ of heat when hydrogen gas burns at... Problem 6.139QP: Hydrogen is burned in oxygen to release heat (see equation below). How many grams of hydrogen gas... Problem 6.140QP Problem 6.141QP Problem 6.142QP Problem 6.143QP: You heat 1.000 quart of water from 25.0C to its normal boiling point by burning a quantity of... Problem 6.144QP: A piece of iron was heated to 95.4C and dropped into a constant-pressure calorimeter containing 284... Problem 6.145QP: The enthalpy of combustion, H, for benzoic acid, C6H5COOH, is 3226 kJ/mol. When a sample of benzoic... Problem 6.146QP: Given the following (hypothetical) thermochemical equations:... Problem 6.147QP: The head of a strike anywhere match contains tetraphosphorus trisulfide, P4S3. In an experiment, a... Problem 6.148QP: Toluene C6H5CH3, has an enthalpy of combustion of 3908 kJ/mol. Using data from Appendix C, calculate... Problem 6.149QP: What will be the final temperature of a mixture made from 25.0 g of water at 15.0C, 45.0 g of water... Problem 6.150QP: What will be the final temperature of a mixture made from equal masses of the following: water at... Problem 6.151QP: Graphite is burned in oxygen to give carbon monoxide and carbon dioxide. If the product mixture is... Problem 6.152QP: A sample of natural gas is 80.0% CH4 and 20.0% C2H6 by mass. What is the heat from the combustion of... Problem 6.153QP Problem 6.154QP Problem 6.155QP: How much heat is released when a mixture containing 10.0 g NH3 and 20.0 g O2 reacts by the following... Problem 6.156QP: How much heat is released when a mixture containing 10.0 g CS2 and 10.0 g Cl2 reacts by the... Problem 6.157QP: Consider the Haber process: N2(g)+3H2(g)2NH3(g);H=91.8kJ The density of ammonia at 25C and 1.00 atm... Problem 6.158QP: An industrial process for manufacturing sulfuric acid, H2SO4, uses hydrogen sulfide, H2S, from the... Problem 6.159QP: The carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by... Problem 6.160QP: A rebreathing gas mask contains potassium superoxide, KO2, which reacts with moisture in the breath... Problem 6.161QP Problem 6.94QP
Related questions
Concept explainers
Consider the following series of balanced chemical reactions in the production of potassium bicarbonate, KHCO3:
K2S + CaCO3 -----------> CaS + K2CO3
K2CO3 + H2O + CO2 ------------> 2 KHCO3
If potassium sulfate, K2SO4, is the limiting reactant, how many grams of KHCO3 (F.M. = 100.12) can be produced from 65.00 g of K2SO4 (F.M. = 174.27)?
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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