6.72 Many portable gas heaters and grills use propane, CHg(g), as fuel. Using standard enthalpies of formation, calculate the quantity of heat produced when 10.0 g of propane is com- pletely combusted in air under standard conditions. 6.73/Using values from Appendix C, calculate the standard en- 6.8 ae thalpy change for each of the following reactions: (a) 2 SO2(8) + O2(8) → 2 SO3(g) (b) Mg(OH)2(s) – (c) N2O4(8) + 4 H2(8) (d) SiCl4(1) + 2 H20(1) → SiO2(s) + 4 HC1(8) MgO(s) + H2O(1) Bor N2(8) + 4 H20((g) 6 6.74 Using values from Appendix C, calculate the value of AH° for each of the following reactions: (a) CaO(s) + 2 HC1(g) CaCl2(s) + H2O(8) → 2 Fe2O3(s) (b) 4 FeO(s) + O2(8) (c) 2 CuO(s) + NO(g) Cu20(s) + NO2(g) g) + 2 H20(1)

6.72 Many portable gas heaters and grills use propane, CHg(g), as fuel. Using standard enthalpies of formation, calculate the quantity of heat produced when 10.0 g of propane is com- pletely combusted in air under standard conditions. 6.73/Using values from Appendix C, calculate the standard en- 6.8 ae thalpy change for each of the following reactions: (a) 2 SO2(8) + O2(8) → 2 SO3(g) (b) Mg(OH)2(s) – (c) N2O4(8) + 4 H2(8) (d) SiCl4(1) + 2 H20(1) → SiO2(s) + 4 HC1(8) MgO(s) + H2O(1) Bor N2(8) + 4 H20((g) 6 6.74 Using values from Appendix C, calculate the value of AH° for each of the following reactions: (a) CaO(s) + 2 HC1(g) CaCl2(s) + H2O(8) → 2 Fe2O3(s) (b) 4 FeO(s) + O2(8) (c) 2 CuO(s) + NO(g) Cu20(s) + NO2(g) g) + 2 H20(1)

Chemistry: Principles and Practice

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Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

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Chapter5: Thermochemistry

Section: Chapter Questions

Problem 5.86QE: One of the components of jet engine fuel is n-dodecane, C12H26(), which has a standard enthalpy of...

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9.104 An engineer is using sodium metal as a cooling agent in a design because it has useful thermal properties. Looting up the heat capacity, the engineer finds a value of 28.2 J mol-l °C-l. Carelessly, he wrote this number down without units. As a result, it was later taken as specific heat. (a) What would he the difference between these two values? (b) Would the engineer overestimate the ability of sodium to remove heat from the system or underestimate it because of this error? Be sure to explain your reasoning.
Sodium carbonate, Na2CO3, is used to manufacture glass. It is obtained from sodium hydrogen carbonate, NaHCO3, by heating. 2NaHCO3(s)Na2CO3(s)+H2O(g)+CO2(g) Calculate the standard enthalpy of reaction, using enthalpies of formation (Table 6.2).
One of the components of jet engine fuel is n-dodecane, C12H26(), 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 of n-dodecane.
Calcium oxide, CaO, is prepared by heating calcium carbonate (from limestone and seashells). CaCO3(s)CaO(s)+CO2(g) Calculate the standard enthalpy of reaction, using enthalpies of formation. The Hf of CaO(s) is 635 kJ/mol. Other values are given in Table 6.2.
The head of a strike anywhere match contains tetraphosphorus trisulfide, P4S3. In an experiment, a student burned this compound in an excess of oxygen and found that it evolved 3651 kJ of heat per mole of P4S3 at a constant pressure of 1 atm. She wrote the following thermochemical equation: P4S3(s)+8O2(g)P4O10(s)+3SO2(g);H=3651kJ Calculate the standard enthalpy of formation of P4S3, using this students result and the following standard enthalpies of formation: P4O10(s), 3009.9 kJ/mol; SO2(g), 296.8 kJ/mol. How does this value compare with the value given in Appendix C?
Chlorine trifluoride is a toxic, intensely reactive gas. It was used in World War II to make incendiary bombs. It reacts with ammonia and forms nitrogen, chlorine, and hydrogen fluoride gases. When two moles of chlorine trifluoride react, 1196 kJ of heat are evolved. (a) Write a thermochemical equation for the reaction. (b) What is Hf for ClF3?
9.32 The material typically used to heat metal radiators is water. If a boiler generates water at 79.5°C, what mass of water was needed to provide the heat required in the previous problem? Water has a specific heat of 4.184Jg1 C1 .
Ethanol, C2H5OH, is used as a fuel for motor vehicles, particularly in Brazil. (a) Write the balanced equation for the combustion of ethanol to CO2(g) and H2O(g), and, using the data in Appendix G, calculate the enthalpy of combustion of 1 mole of ethanol. (b) The density of ethanol is 0.7893 g/mL. Calculate the enthalpy of combustion of exactly 1 L of ethanol. (c) Assuming that an automobile’s mileage is directly proportional to the heat of combustion of the fuel, calculate how much farther an automobile could be expected to travel on 1 L of gasoline than on 1 L of ethanol. Assume that gasoline has the heat of combustion and the density of n—octane, C8H18(Hf=208.4kJ/mol;density=0.7025g/mL).
When one mol of KOH is neutralized by sulfuric acid, q=56 kJ. (This is called the heat of neutralization.) At 23.7C, 25.0 mL of 0.475 M H2SO4 is neutralized by 0.613 M KOH in a coffee-cup calorimeter. Assume that the specific heat of all solutions is 4.18J/gC, that the density of all solutions is 1.00 g/mL, and that volumes are additive. (a) How many mL of KOH is required to neutralize H2SO4? (b) What is the final temperature of the solution?
Given the following (hypothetical) thermochemical equations: A+B2C;H=447kJA+3D2E;H=484kJ2D+B2F;H=429kJ Calculate H, in kJ, for the equation 4E+5B4C+6F
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 the heat q. Is the precipitation reaction exothermic or endothermic?
Combustion of table sugar produces CO2(g) and H2O( l). When 1.46 g table sugar is combusted in a constant-volume (bomb) calorimeter, 24.00 kJ of heat is liberated. a. Assuming that table sugar is pure sucrose, C12H22O11 (s), write the balanced equation for the combustion reaction. b. Calculate E in kJ/mol C12H22O11 for the combustion reaction of sucrose.

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