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chemistry principles and practice

Chemistry Principles And Practice 3rd Edition Daniel L. Reger, Scott R. Goode, David W. Ball - Solutions

What are the two factors about a system that relate the heat of a process and the temperature change that the process causes the system?
A perpetual motion machine of the first kind generates more energy than it uses. Explain why this violates the first law of thermodynamics.
A chemical reaction occurs and gives off 32,500 J. How many calories is this? Is the reaction endothermic or exothermic?
The enthalpy change for the following reaction is -393.5 kJ.(a) Is energy released from or absorbed by the system in this reaction?(b) What quantities of reactants and products are assumed?(c) Predict the enthalpy change observed when 3.00 g carbon burns in an excess of oxygen. C(s, graphite) +
The enthalpy change for the following reaction is +131.3 kJ.(a) Is energy released from or absorbed by the system in this reaction?(b) What quantities of reactants and products are assumed if ΔH =+131.3 kJ?(c) What is the enthalpy change when 6.00 g carbon is reacted with excess H2O(g)? C(s,
A chemical reaction occurs and absorbs 64.7 cal. How many joules is this? Is the reaction endothermic or exothermic?
The thermochemical equation for the burning of methane, the main component of natural gas, is(a) Is this reaction endothermic or exothermic?(b) What quantities of reactants and products are assumed if ΔH = -890 kJ?(c) What is the enthalpy change when 1.00 g methane burns in an excess of oxygen?
When lightning strikes, the energy can force atmospheric nitrogen and oxygen to react to make NO:(a) Is this reaction endothermic or exothermic?(b) What quantities of reactants and products are assumed if ΔH = +181.8 kJ?(c) What is the enthalpy change when 3.50 g nitrogen is reacted with excess
If nitric acid were sufficiently heated, it can be decomposed into dinitrogen pentoxide and water vapor:(a) Calculate the enthalpy change that accompanies the reaction of 1.00 kg(b) Is heat absorbed or released during the course of the reaction? 2HNO3()→ N₂O(g) + H₂O(g) AHrxn = +176 kJ
One step in the manufacturing of sulfuric acid is the conversion of SO2 (g) to SO3(g). The thermochemical equation for this process isThe second step combines the SO3 with H2O to make H2SO4.(a) Calculate the enthalpy change that accompanies the reaction to make 1.00 kg SO3(g).(b) Is heat absorbed
The thermite reaction produces a large quantity of heat, enough to melt the iron metal that is a product of the reaction:What is the enthalpy change if 50.0 g Al reacts with excess iron(III) oxide? 2Al(s) + Fe2O3(s) → AlO3(s) + 2Fe(s) ΔΗ, · ΓΥΠ –852 kJ
Hydrazine, N2H4, is used as a fuel in some rockets:What is the enthalpy change if 110.0 g N2H4 reacts with excess oxygen? N₂H4(l) + O₂(g) → N₂(g) + 2H₂O(l) ΔΗ = −622 kJ
The combustion of 1.00 mol liquid octane (C8H18), a component of gasoline, in excess oxygen is exothermic, producing 5.46 × 103 kJ of heat.(a) Write the thermochemical equation for this reaction.(b) Calculate the enthalpy change that accompanies the burning of 10.0 g octane.
Another reaction that is used to propel rockets isThis reaction has the advantage that neither product is toxic, so no dangerous pollution is released. When the reaction consumes 10.0 g liquid N2O4, it releases 124 kJ of heat.(a) Is the sign of the enthalpy change positive or negative?(b) What is
The combustion of 1.00 mol liquid methyl alcohol (CH3OH) in excess oxygen is exothermic, giving 727 kJ of heat.(a) Write the thermochemical equation for this reaction.(b) Calculate the enthalpy change that accompanies the burning 10.0 g methanol.(c) Compare this with the amount of heat produced
Ammonia is produced commercially by the direct reaction of the elements. The formation of 5.00 g gaseous NH3 by this reaction releases 13.56 kJ of heat.(a) What is the sign of the enthalpy change for this reaction?(b) Calculate ΔH for the reaction, assuming molar amounts of reactants and products.
The reaction of 1 mol O2(g) and 1 mol N2(g) to yield 2 mol NO(g) is endothermic, with ΔH = +181.8 kJ. Calculate the enthalpy change observed when 2.20 g N2(g) reacts with an excess of oxygen.
The reaction of 1 mol C(s, graphite) with 0.5 mol O2(g) to yield 1 mol CO(g) gives off 110.5 kJ. Calculate the enthalpy change when 52.0 g CO(g) is formed.
The reaction of 2 mol H2(g) with 1 mol O2(g) to yield 2 mol is exothermic, with ΔH = -572 kJ. Calculate the enthalpy change observed when 10.0 g O2(g) reacts with an excess of hydrogen. H₂O(l)
The reaction of 2 mol Fe(s) with 1 mol O2(g) to make 2 mol FeO(s) gives off 544 kJ. Calculate the enthalpy change that accompanies the formation of 100.0 g FeO.
Gasohol, a mixture of ethyl alcohol and gasoline, has been proposed as a fuel to help conserve our petroleum resources. It is available on a limited basis. The thermochemical equation for the burning of ethyl alcohol isCalculate the enthalpy change observed when burning 2.00 g ethyl alcohol.
Isooctane (2,2,4-trimethylpentane), one of the many hydrocarbons that makes up gasoline, burns in air to give water and carbon dioxide.What is the enthalpy change if you burn 1.00 L of isooctane (density = 0.69 g/mL)? 2C8H18 () + 250₂(g) → 16CO2(g) + 18H₂O(l) AH° -10,922 kJ
It takes 6.01 kJ to melt 1 mol of ice at 0 °C. Based on the data given in Exercise 5.51, how many grams of CH4 must be burned to melt an ice cube having a mass of 35.0 g? وه دار ر کار ران 000
The enthalpy change when 1 mol methane (CH4) is burned is -890 kJ. It takes 44.0 kJ to vaporize 1 mol water. What mass of methane must be burned to provide the heat needed to vaporize 1.00 g water?
How much heat, in kilojoules, must be added to increase the temperature of 500 g water from 22.5 °C to 39.1 °C?
How much energy is required to raise the temperature of 50.00 mL of water from 25.52 °C to 28.75 °C? (The density of water at this temperature is 0.997 g/mL.)
How much heat, in kilojoules, must be removed to decrease the temperature of a 20.0-g bar of aluminum from 34.2 °C to 22.5 °C?
How much heat, in kilojoules, must be removed to reduce the temperature of a 300-g bar of gold from 800 °C to 24.5 °C?
A 50.0-g sample of metal at 100.00 °C is added to 40.0 g water that is initially 23.50 °C. The final temperature of both the water and the metal is 28.46 °C.(a) Use the specific heat of water to fi nd the heat absorbed by the water.(b) How much heat did the metal sample lose?(c) Calculate the
A 40.0-g sample of gold powder at 91.50 °C is dissolved into 51.2 g mercury that is initially 22.00 °C. Using the specific heats given in Table 5.1, calculate the final temperature of the resulting solution, called an amalgam.Table 5.1 TABLE 5.1 Specific Heats of Some Common
A 50.0-g sample of metal at 100.00 °C is added to 60.0 g water that is initially 25.00 °C. The final temperature of both the water and the metal is 31.51 °C.(a) Use the specific heat of water to fi nd the heat absorbed by the water.(b) How much heat did the metal sample lose?(c) Calculate the
A 59.9-g sample of ethyl alcohol at 70.30 °C is mixed with 40.1 g water that is initially 22.00 °C. The specific heat of ethyl alcohol is 2.419 J/g · °C. What is the final temperature of the resulting solution?
When 7.11 g NH4NO3 is added to 100 mL water, the temperature of the calorimeter contents decreases from 22.1 °C to 17.1 °C. Assuming that the mixture has the same specific heat as water and a mass of 107 g, calculate the heat q. Is the dissolution of ammonium nitrate exothermic or endothermic?
A 50-mL solution of a dilute AgNO3 solution is added to 100 mL of a base solution in a coffee-cup calorimeter. As Ag2O(s) precipitates, the temperature of the solution increases from 23.78 °C to 25.19 °C. Assuming that the mixture has the same specific heat as water and a mass of 150 g, calculate
Dissolving 6.00 g CaCl2 in 300 mL of water causes the temperature of the solution to increase by 3.43 °C. Assume that the specific heat of the solution is 4.18 J/g · K and its mass is 306 g.(a) Calculate the enthalpy change when the CaCl2 dissolves. Is the process exothermic or
Draw an energy-level diagram based on each of the following thermochemical equations. Label each level with the amounts of substances present, and use an arrow between levels for the given enthalpy change. (a) C(s, graphite) + HO(g) → CO(g) + H2(g) ΔΗ = +131.3 kJ (b) CO(g) + H,O(g) → CO2(g) +
A 0.470-g sample of magnesium reacts with 200 g dilute HCl in a coffee-cup calorimeter to form MgCl2(aq) and H2(g). Th e temperature increases by 10.9 °C as the magnesium reacts. Assume that the mixture has the same specific heat as water and a mass of 200 g.(a) Calculate the enthalpy change for
Draw an energy-level diagram based on each of the following thermochemical equations. Label each level with the amounts of substances present, and use an arrow between levels for the given enthalpy change. (a) Zn(s) + 2HC1(aq) → ZnCl₂(aq) + H₂(g) (b) N₂(g) + 20₂(g) →2NO₂(g) (c)
Using the following thermochemical equations 7 C₂H6(g) + O₂(g)→2CO₂(g) + 3H₂O(l) 2C₂H₂(g) + 50₂(g) → 4CO2(g) +2H₂O(l) H₂(g) + 0₂(g) → H₂O(l) calculate AH for AH = -1560 kJ C₂H₂(g) + 2H₂(g) → C₂H6(g) ΔΗ = -2599 kJ ΔΗ = -286 kJ AH = ?
Using the thermochemical equations in Exercise 5.67 as needed and in additionExercise 5.67Using the following thermochemical equations CH4(g) + 20₂(g) → CO₂(g) + 2H₂O(l) C₂H4(g) + 30₂(g) →2CO₂(g) + 2H₂O(l) calculate AH for ΔΗ = -890 kJ C₂H4(g) + 2H₂(g) → 2CH4(g) AH = -1411
Calculate ΔH for the reaction Zn(s) + -—-0₂(g) → ZnO(s) 2 given the equations AH = ? Zn(s) + 2HC1(aq) → ZnCl₂ (aq) + H₂(g) 2H₂(g) + O₂(g) → 2H₂O(l) ΔΗ = -152.4 kJ ZnO(s) + 2HC1(aq) →ZnCl₂(aq) + H₂O(0) AH = -90.2 kJ AH = -571.6 kJ
In the process of isolating iron from its ores, carbon monoxide reacts with iron(III) oxide, as described by the following equation: Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO₂(g) ΔΗ = -24.8 kJ The enthalpy change for the combustion of carbon mon- oxide is 2CO(g) + O₂(g) → 2CO₂(g) AH = -566
Given the thermochemical equations 2Cu(s) + Cl₂(g) → 2CuCl(s) 2CuCl(s) + Cl₂(g) →2CuCl2(s) find the enthalpy change for Cu(s) + Cl₂(g) → CuCl₂(s) AH = -274.4 kJ AH = -165.8 kJ AH = ?
Draw an energy-level diagram that represents the Hess’s law calculation in Exercise 5.71.Exercise 5.71Given the thermochemical equations 2Cu(s) + Cl₂(g) → 2CuCl(s) 2CuCl(s) + Cl₂(g) →2CuCl2(s) find the enthalpy change for Cu(s) + Cl₂(g) → CuCl₂(s) AH = -274.4 kJ AH = -165.8 kJ AH = ?
Draw an energy-level diagram that represents the Hess’s law calculation in Exercise 5.72.Exercise 5.72In the process of isolating iron from its ores, carbon monoxide reacts with iron(III) oxide, as described by the following equation: Fe2O3(s) + 3CO(g) →2Fe(s) + 3CO₂(g) ΔΗ = -24.8 kJ The
What does an energy-level diagram for the reverse reaction from Exercise 5.71 look like?Exercise 5.71Given the thermochemical equations 2Cu(s) + Cl₂(g) → 2CuCl(s) 2CuCl(s) + Cl₂(g) →2CuCl2(s) find the enthalpy change for Cu(s) + Cl₂(g) → CuCl₂(s) AH = -274.4 kJ AH = -165.8 kJ AH = ?
What does an energy-level diagram for the reverse reaction from Exercise 5.72 look like?Exercise 5.72In the process of isolating iron from its ores, carbon monoxide reacts with iron(III) oxide, as described by the following equation: Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO₂(g) ΔΗ = -24.8 kJ The
Write the formation reaction for each of the following substances. (a) HBr(g) (b) H₂SO4(l) (c) 03(g) (d) NaHSO4(s)
Write the chemical equation for the reaction whose energy change is the standard enthalpy of formation of each of the following substances. (a) CH₂COOH(e) (b) H₂PO4(0) (c) CaSO4 2H₂O(s) (d) C(s, diamond)
Use standard enthalpies of formation to calculate the enthalpy change for each of the following reactions at 298.15 K and 1 atm. Label each as endothermic or exothermic.(a) The fermentation of glucose to ethyl alcohol and carbon dioxide:(b) The combustion of normal (straight-chain) butane:
Use the standard enthalpies of formation from Appendix G to calculate the enthalpy change for each of the following reactions at 298.15 K and 1 atm. Label each as endothermic or exothermic.(a) The photosynthesis of glucose:(b) The reduction of iron(III) oxide with carbon: 6CO₂(g) +6H₂O(l) →
Use the standard enthalpies of formation from Appendix G to calculate the enthalpy change for each of the following reactions at 298.15 K and 1 atm. Label each as endothermic or exothermic. (a) NaHCO3(s) → NaOH(s) + CO₂(g) (b) H₂O(l) + SO3(g) →H₂SO4(0) (c) H₂O(g) + SO3(g) → H₂SO4(l)
Use data in Appendix G to find the enthalpy of reaction for (a) CaCO3(s)→ CaO(s) + CO₂(g) (b) 2HI(g) + F2(g) → 2HF(g) + I₂(s) (c) SF6(g) + 3H₂O()→ 6HF(g) + SO3(g)
Calculate ΔH ° when a 38-g sample of glucose, C6H12O6(s), burns in excess O2(g) to form CO2(g) and in a reaction at constant pressure and 298.15 K. H₂O(l)
Calculate the amount of heat evolved or absorbed when a 0.2045-g sample of acetylene, C2H2(g), burns in excess oxygen to form CO2 (g) and in a reaction at constant pressure and 298.15 K. H₂O(l)
The octane number of gasoline is based on a comparison of the gasoline’s behavior with that of 2,2,4-trimethylpentane, which is arbitrarily assigned an octane number of 100. The standard enthalpy of combustion of this compound is -5456.6 kJ/mol.(a) Write the thermochemical equation for the
One of the components of jet engine fuel is n-dodecane, which has a standard enthalpy of combustion of -8080.1 kJ/mol.(a) Write the thermochemical equation for the combustion of n-dodecane.(b) Use the standard enthalpies of formation in Appendix G to calculate the standard enthalpy of formation
Propane, C3H8(g), and n-octane, are important components of the widely used fossil fuels. The enthalpy change for combustion of 1 mol propane is -2219 kJ, and that for 1 mol octane is -5466 kJ. Calculate the enthalpy change per gram for each compound. CgH18(e),
A fission nuclear reactor produces about 8.1 × 107 kJ of energy for each gram of uranium consumed. One kilogram of high-grade coal produces about 2.8 × 104 kJ of energy when it is burned.(a) How many metric tons (1 metric ton = 1000 kg) of coal must be burned to produce the same energy as
When a 2.30-g sample of magnesium dissolves in dilute hydrochloric acid, 16.25 kJ of heat is released. Determine the enthalpy change for the thermochemical equation Mg(s) + 2HCl(aq) → MgCl(aq) + H2(g) ΔΗ = ?
A 1:1 mole ratio of CO (g) and H2 (g) is called water gas. It is used as a fuel because it can be burned in air:(a) Find the number of moles of CO (g) and H2 (g) Present in 10.0 g water gas. (Remember that they are present in a 1:1 mole ratio.)(b) Use the preceding thermochemical equations to
What mass of ethylene, C2H4(g), must be burned to produce 3420 kJ of heat, given that its enthalpy of combustion is -1410.1 kJ/mol?
What mass of acetylene, C2H2(g), must be burned to produce 3420 kJ of heat, given that its enthalpy of combustion is -1301 kJ/mol? Compare this with the answer to Exercise 5.91 and determine which substance produces more heat per gram.Exercise 5.91What mass of ethylene, C2H4(g), must be burned to
100.0 J of heat is added to a 3.45-g sample of an unknown metal. The temperature of the metal increases from 22.37 °C to 54.58 °C. Use the date in Table 5.1 to identify the metal.Table 5.1 TABLE 5.1 Specific Heats of Some Common
It takes 677 J of heat to increase the temperature of 25.0 g liquid ethanol (C2H5OH) from 23.5 °C to 34.7 °C. What is the specific heat of this substance?
The enthalpy of combustion of liquid n-hexane, C6H14, is -4159.5 kJ/mol, and that of gaseous n-hexane is -4191.1 kJ/mol. Use Hess’s law to determine ΔH for the vaporization of 1 mol of n-hexane: C6H14()→ C6H14(g)
When 50.0 g water at 41.6 °C was added to 50.0 g water at 24.3 °C in a calorimeter, the temperature increased to 32.7 °C. When 4.82 g KClO3(s) was added to 100.0 g water in the calorimeter (at 24.3 °C), the temperature decreased to 20.6 °C.(a) What is the heat capacity of this
A typical waterbed measures 84 in. × 60 in. × 9 in. How many kilocalories are required to heat the water in the waterbed from 55 °F (cold water from the faucet) to 85 °F, the operating temperature of the waterbed?
What is ΔHrxn for reaction of iron(III) oxide and carbon monoxide to give iron metal and carbon dioxide gas? Use the following reactions: 4Fe(s) + 30₂(g) → 2Fe₂O3(s) 2CO(g) + O₂(g) → 2CO₂(g) AH-1648.4 kJ ΔΗ = -565.98 kJ
Ammonium nitrate, a common fertilizer, has been used by terrorists to construct car bombs. The products of the explosion of ammonium nitrate are nitrogen gas, oxygen gas, and water vapor. or ammonium nitrate is -87.37 kcal/mol.(a) Write the balanced chemical reaction for the decomposition of
In the 1880s, Frederick Trouton noted that the enthalpy of vaporization of 1 mol pure liquid is approximately 88 times the boiling point, Tb, of the liquid on the Kelvin scale. This relationship is called Trouton’s rule and is represented by the thermochemical equationCombined with an empirical
Cyclopropane, C3H6(g), is a flammable compound that has been used in the past as an anesthetic. It has an enthalpy of combustion of -2091 kJ/mol.(a) Write the thermochemical equation for the combustion of cyclopropane.(b) Use the standard enthalpies of formation in Appendix G to calculate the
A compound that contains only carbon, hydrogen, and oxygen is 54.5% C and 9.15% H. Its enthalpy of vaporization is 388 J/g, and it boils at a temperature of 374 K.(a) What is the empirical formula of this compound?(b) Use Trouton’s rule to calculate the approximate enthalpy of vaporization of
The price of silver is $16.74 per troy ounce at this writing (1 troy oz = 31.10 g).(a) Calculate the cost of 1 mol silver.(b) How much heat is needed to increase the temperature of $1000.00 worth of silver from 15.0 °C to 99.0 °C? Cs(Ag) = 0.235 J/g · °C. .999 FINE SILVER 10 TROY OUNCES
The law of Dulong and Petit states that the heat capacity of metallic elements is approximately 25 J/mol · °C at 25 °C. In the 19th century, scientists used this relationship to obtain approximate atomic masses of metals, from which they determined the formulas of compounds. Once the formula of
See Exercise 5.104 for a description of the law of Dulong and Petit.(a) Experimentally, the specific heat of a metal is found to be 0.460 J/g · °C. Use the law of Dulong and Petit to calculate the approximate atomic mass of the metal.(b) A chloride of this element is 67.2% chlorine by mass. Use
A compound is 82.7% carbon and 17.3% hydrogen, and has a molar mass of approximately 60 g/mol. When 1.000 g of this compound burns in excess oxygen, the enthalpy change is -49.53 kJ.(a) What is the empirical formula of this compound?(b) What is the molecular formula of this compound?(c) What is
When wood is burned we may assume that the reaction is the combustion of cellulose (empirical formula, CH2O).How much energy is released when a 10-lb wood log burns completely? (Assume the wood is 100% dry and burns via the reaction above.) CH,O(s) + Oz(g) → CO2(g) + H,O(g) ΔΗ° = −425 kJ
You want to heat the air in your house with natural gas (CH4). Assume your house has 275 m2 (about 2960 ft2) of floor area and that the ceilings are 2.50 m from the floors. The air in the house has a molar heat capacity of 29.1 J/mol K. (The number of moles of air in the house can be found by
Write a balanced equation for the reaction pictured below. Nitrogen Oxygen +
Describe the steps needed to write balanced equations.
Using solid circles for H atoms and open circles for O atoms, make a drawing that shows the molecular level representation for the balanced equation of H2 and O2 reacting to form H2O.
The chapter introduction indicates that a backup oxygen source for the ISS is a Solid Fuel Oxygen Generator. The main compound in the generator is solid sodium chlorate, NaClO3. Heating this compound produces oxygen gas and solid sodium chloride, NaCl. Write the balanced equation for this reaction.
Using solid circles for H atoms and open circles for O atoms, make a drawing that shows the molecular level representation for the balanced equation of H2 and O2 reacting to form H2O2. The two oxygen atoms are bonded to each other, and a hydrogen atom is bonded to each oxygen.
Write the equation for sodium hydroxide dissolving in water.
Give the name and definition of the SI unit for amount of substance.
Write the balanced chemical equation for the reaction of hydrochloric acid with calcium hydroxide.
How many objects are in 1 mol? What is the common name for this number of objects?
Write the equation for the combustion of liquid methanol, CH3OH.
When writing and balancing a chemical equation, we generally count the number of molecules that are present, but when carrying out reactions in the laboratory, we think of the equation in terms of moles. Why is the unit of moles more convenient on the laboratory scale?
The reaction of magnesium metal, Mg(s), with oxygen, O2(g), yields magnesium oxide, MgO(s). Write the balanced equation for this reaction, assign an oxidation number to each element in the reactants and products, and indicate which element is oxidized and which is reduced.
What are the units for molecular mass, formula mass, and molar mass?
How many molecules are present in 0.241 mol N2O?
Draw a diagram that outlines the conversion of number of atoms into moles.
What is the mass of 43.1 mol phosphorus pentachloride?
Draw a flow diagram that outlines the conversion of moles to number of atoms.
How many moles are present in a 12.7-g sample of NO?
Describe an experiment that would enable someone to determine the percentages of carbon and hydrogen in a sample of a newly prepared hydrocarbon.
How many moles of C are present in 0.22 mol CH3NH2?
Explain how a combustion analysis is used to determine the percentage of oxygen in a new compound that contains only carbon, hydrogen, and oxygen.

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