Chemistry for Engineering Students
3rd Edition
ISBN: 9781285199023
Author: Lawrence S. Brown, Tom Holme
Publisher: Cengage Learning
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Chapter 9, Problem 9.72PAE
9.68 What are some features of petroleum that make it such an attractive fuel?
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8. Determine the enthalpy for the following reaction, given AH, (NH3(g)) = -46.1 kJ/mol, AH; (NO(g)) =
+90.3 kJ/mol, and AH (H20(g)) = -241.8 kJ/mol.
%3D
4NH3(g) + 502(g) → 4NO(g) + 6H20(g)
AHn = ? kJ
%3D
a.
-1274 kJ/mol
d. -905.2 kJ/mol
b. -1,996 kJ/mol
+1,274 kJ/mol
е.
-105.4 kJ/mol
с.
Write a balanced equation for the formation of CO2(g) from C(s) and O2(g). Calculate the enthalpy change for this reaction using the following data (at 25 degrees Celsius):
C(s) + 1/2 O2(g) --> CO(g) change in H = -111 kJ
CO(g) + 1/2 O2(g) --> CO2(g) change in H = -394 kJ
Is the reaction endothermic or exothermic?
[1] Benzoic acid (C;H,O2) is used as a standard to measure the heat capacity of a bomb calorimeter. (The energy
released by combustion of benzoic acid is 3.23x10° kJ/mol.) The combustion of 0.5000 g benzoic acid increases the
temperature of a bomb calorimeter by 6.94 °C. Calculate the heat capacity of the calorimeter.
Chapter 9 Solutions
Chemistry for Engineering Students
Ch. 9 - Explain the economic importance of conversions...Ch. 9 - • define work and beat using the standard sign...Ch. 9 - • define state functions and explain their...Ch. 9 - • state the first law of thermodynamics in words...Ch. 9 - • use calorimetric data to obtain values for E and...Ch. 9 - • define Hfo and write formation reactions for...Ch. 9 - • explain Hess’s law in your own words.Ch. 9 - • calculate H for chemical reactions from...Ch. 9 - Prob. 9.1PAECh. 9 - Prob. 9.2PAE
Ch. 9 - Prob. 9.3PAECh. 9 - Prob. 9.4PAECh. 9 - Prob. 9.5PAECh. 9 - Prob. 9.6PAECh. 9 - Define the term internal energy.Ch. 9 - How fast (in meters per second) must an iron ball...Ch. 9 - What is the kinetic energy of a single molecule of...Ch. 9 - 9.10 The kinetic energy of molecules is often used...Ch. 9 - 9.11 Analyze the units of the quantity...Ch. 9 - 9.12 How many kilojoules are equal to 3.27 L atm...Ch. 9 - Prob. 9.13PAECh. 9 - Prob. 9.14PAECh. 9 - 9.15 Carry out the following conversions of energy...Ch. 9 - 9.16 According to Figure 9.2, the total energy...Ch. 9 - 9.17 If a machine does 4.8103kJ of work after an...Ch. 9 - 9.18 Calculate (a) q when a system does 54J of...Ch. 9 - 9.19 If the algebraic sign of E is negative, in...Ch. 9 - 9.20 State the first law of thermodynamics briefly...Ch. 9 - 9.21 Which type of energy heat or work, is valued...Ch. 9 - 9.12 PV-work occurs when volume changes and...Ch. 9 - 9.23 Which system does not work: (a) E=436J ,...Ch. 9 - 9.29 In which case is heat added to the system:...Ch. 9 - Prob. 9.25PAECh. 9 - 9.26 Gas furnaces have achieved impressive...Ch. 9 - Prob. 9.27PAECh. 9 - 9.28 When an electrical appliance whose power...Ch. 9 - Prob. 9.29PAECh. 9 - 9.30 For the example of shallow water and sandy...Ch. 9 - 9.31 A metal radiator is made from 26.0 kg of...Ch. 9 - 9.32 The material typically used to heat metal...Ch. 9 - 9.33 Copper wires used to transport electrical...Ch. 9 - 9.34 A copper nail and an iron nail of the same...Ch. 9 - 9.35 A piece of titanium metal with a mass of 20.8...Ch. 9 - 9.36 Define the term calibration.Ch. 9 - 9.37 A calorimeter contained 75.0 g of water at...Ch. 9 - 9.38 The energy densities of various types of coal...Ch. 9 - 9.39 How much thermal energy is required to heat...Ch. 9 - Prob. 9.40PAECh. 9 - 9.41 Under what conditions does the enthalpy...Ch. 9 - 9.42 Why is enthalpy generally more useful than...Ch. 9 - Prob. 9.43PAECh. 9 - Prob. 9.44PAECh. 9 - 9.45 What happens to the temperature of a material...Ch. 9 - 9.46 The heat of fusion of pure silicon is 43.4...Ch. 9 - 9.47 If 14.8 kJ of heat is given off when 1.6 g of...Ch. 9 - 9.48 Calculate the energy required to convert 1.70...Ch. 9 - 9.49 Hvap=31.3 kJ/mol for acetone. If 1.40 kg of...Ch. 9 - 9.50 When a 13.0-g sample of NaOH(s) dissolves in...Ch. 9 - Prob. 9.51PAECh. 9 - 9.52 Write the formation reaction for each of the...Ch. 9 - Explain why each of the following chemical...Ch. 9 - Which of the following are state functions? (a)...Ch. 9 - 9.53 Using these reactions, find the standard...Ch. 9 - 9.54 The phase change between graphite and diamond...Ch. 9 - 9.55 Hydrogen gas will react with either acetylene...Ch. 9 - 9.56 Using heats of formation tabulated in...Ch. 9 - 9.57 The heat of combustion of butane is —2877...Ch. 9 - Prob. 9.60PAECh. 9 - When a reaction is exothermic, is the sum of bond...Ch. 9 - 9.58 For the reaction C2H2(g)+2H2(g)C2H6,H=136 kJ....Ch. 9 - 9.59 For the reaction N2(g)+O2(g)2NO(g),H=180.5kJ...Ch. 9 - 9.60 Nitroglycenne, C3H5(NO3)3( l ), is an...Ch. 9 - 9.61 Silane, SiH4, burns according to the...Ch. 9 - 9.62 Sulfur trioxide can be removed from the...Ch. 9 - 9.63 Reactions of hydrocarhons are often studied...Ch. 9 - Prob. 9.68PAECh. 9 - 9.65 When 0.0157 g of a compound with a heat of...Ch. 9 - Prob. 9.70PAECh. 9 - Prob. 9.71PAECh. 9 - 9.68 What are some features of petroleum that make...Ch. 9 - 9.69 How are the roles of transmission substations...Ch. 9 - 9.70 Residential electric service in the United...Ch. 9 - 9.71 In recent years, the notion of a “smart grid”...Ch. 9 - 9.72 Although it can be a nuisance when a laptop...Ch. 9 - 9.85 The figure below shows a "self-cooling"...Ch. 9 - 9.86 You make some iced tea by dropping 134 g of...Ch. 9 - A student performing a calorimetry experiment...Ch. 9 - The specific heat of gold is 0.13 J g-1K-1, and...Ch. 9 - 9.87 What will be the final temperature of a...Ch. 9 - Prob. 9.82PAECh. 9 - 9.89 A sample of gas is 80.0% CH4 and 20.0% C2H6...Ch. 9 - 9.90 Many engineering designs must incorporate...Ch. 9 - 9.91 You want to heat the air in your house with...Ch. 9 - Prob. 9.86PAECh. 9 - Prob. 9.87PAECh. 9 - Prob. 9.88PAECh. 9 - 9.95 How much heat is required to convert 250 g of...Ch. 9 - 9.96 Most first aid "cold packs" are based on the...Ch. 9 - 9.97 Suppose that the working fluid inside an...Ch. 9 - 9.98 Hydrogen combines with oxygen in fuel cells...Ch. 9 - 9.99 The chemical reaction...Ch. 9 - 9.100 Two baking sheets are made of different...Ch. 9 - Prob. 9.95PAECh. 9 - 9.102 A runner generates 418 kJ of energy per...Ch. 9 - 9.103 One reason why the energy density of a fuel...Ch. 9 - 9.104 An engineer is using sodium metal as a...Ch. 9 - Prob. 9.99PAECh. 9 - Prob. 9.100PAECh. 9 - Prob. 9.101PAECh. 9 - Prob. 9.102PAECh. 9 - Prob. 9.103PAECh. 9 - Prob. 9.104PAE
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- Calculate the standard enthalpy change for the following reaction: CH4(g) + 2 O₂(g) → CO₂(g) + 2 H₂O(g) O-243 kJ/mol O 188 kJ/mol O 166 kJ/mol O-802 kJ/mol O-166 kJ/molarrow_forwardTo a test tube containing 5.0 ml of 1.00 M NaOH at 27°C in a calorimeter, 5.0 ml of 2.00 M HNO3 at the same temperature was added, the heat generated by the reaction was monitored. Which of the following is TRUE? a.Reaction is exothermic; solution will turn pink upon addition of phenolphthalein. b.Heat is absorbed by the system; no color change will be observed upon addition of phenolphthalein. c.Heat is released by the system; no color change will be observed upon addition of phenolphthalein. d.Reaction is endothermic; solution will turn pink upon addition of phenolphthalein.arrow_forwardGiven the following reactions: Fe2O3(s) + 3 CO(g)→2 Fe(s) + 3 CO2(g); ΔH = −28.0kJ 3 Fe(s)+ 4 CO2(g) →4 CO(g) + Fe3O4(s); ΔH = +12.5 kJ the enthalpy of the reaction of Fe2O3 with CO 3 Fe2O3(s) + CO(g) → CO2(g) + 2 Fe3O4(s) is which of the following? -109 kJ -15.5 kJ +109 kJ -59.0 kJarrow_forward
- The enthalpy of formation of CF4(g) is -679.9 kJ/mol. Based on the enthalpy of formation of two reactions, which is more exothermic? (See attached image)arrow_forward8 Consider the combustion of liquid CH in oxygen gas to produce carbon dioxide gas and water vapor. In an experiment, 0.1063 g of CH is combusted to produce enough heat to raise the temperature of 150.0 g of water by 7.630 °C. 8 If-4789 J of heat was produced from the combustion of 0.001561 moles of C₂H₂, what is the enthalpy change (in kJ/mol) for the 8⁹ combustion of CH?arrow_forwardIt is interesting to compare the “fuel value” of a hydrocarbonin a hypothetical world where oxygen is not thecombustion agent. The enthalpy of formation of CF4(g) is-679.9 kJ/mol. Which of the following two reactions is themore exothermic?CH4(g) + 2 O2(g) ----->CO2(g) + 2 H2O(g)CH4(g) + 4 F2(g) ------> CF4(g) + 4 HF(g)arrow_forward
- 26. When a mixture of hydrogen and bromine is maintained at normal atmospheric pressure and heated above 200°C in a closed container, the hydrogen and bromine react to form hydrogen bromide and a gas-phase equilibrium is established. a) Write a balanced chemical equation for the equilibrium reaction. b) Use bond enthalpies to estimate the enthalpy change for the reaction. c) Based on your answers to parts (a) and (b), which is more important in determining the position of this equilibrium, the entropy effect or the energy effect? d) In which direction will the equilibrium shift as the temperature increases above 200°C? Explain. e) Suppose that the pressure were increased to triple its initial value. In which direction would the equilibrium shift? f) Why is the equilibrium not established at room temperature?arrow_forwardIf the enthalpy change for the reaction below is 46.72 kJ, how many grams of ammonia can be produced if 50.7 kJ of heat energy are provided to the reaction? 4 NO + 6 H2O --> 4 NH3 + 5 O2arrow_forward12. Consider the following process. AH = -802 kJ + 202 (2) 2 CO2 (g) + 2H,O(3) CHAIB) + 2H,O(g) A) Is the reaction exothermic or endothermic? B) What is the enthalpy change for the following reaction? + H2O(e) 1/2CH4 () + O2 () O 1/2 CO2 (8) + H,0R)arrow_forward
- GO and O-H bonds are stronger than C-C and C-H bonds, because C-O bonds and O-H bonds e polar. The partial charges on the atoms result in stronger attraction between the atoms. This is why combustion reactions are exothermic and why fossil fuels are so valuable Which of the following reactions would you predict to be endothermic? a) 200 + 4H2 > CHạ + 02 b) 2H2(8) + Oz(8) → 2H;O(1) c) Na(s) + Chie) → 2NACI(s) d) paper burning to form CO; and H20 6) Consider the reaction CH3OH + HBr > CH,Br + H;0 Draw the Lewis structures for reactants and products. Which bonds are broken in this reaction? Which bonds are formed? Use the table below to determine if this reaction is exothermic or endothermic and the value for AH. Table 5.4 Average Bond Enthalpies (kJ/mol) C-H 413 N-H 391 0-H 463 155 C-C 348 N-N 163 0-0 146 614 N-O 201 495 d-F 253 C-N 293 N-F 272 0-F 190 C-a 242 C-O 358 N-C 200 2113 799 N-ir 24.1 0-1 234 lir- 237 C-F 485 218 C-a 328 H-H 436 Br-Br 193 C-Br 276 H-F 567 C-I 240 H-CI 431 208…arrow_forwardFf.203. what is meant by a hydrogenated oil? Why is this potentially dangerous to human health?arrow_forward33.9 Given the following two reactions and their enthalpy changes, 2 ClO2 (g) --> Cl2 (g) + 2 O2 (g) Delta H = – 204 kJ 2 TiCl4 (l) + 2 O2 (g) --> 2 TiO2 (s) + 4 Cl2 Delta H = – 139.8 kJ What is the value of the enthalpy change for the reaction that is the sum of these two reactions? 2 ClO2 (g) + 2 TiCl4 (l) --> 2 TiO2 (s) + 5 Cl2 Delta H = ? Select one: a. – 64 kJ b. – 344 kJ c. 64.2 kJ d. 64 kJ e. 344 kJ f. – 204 kJ g. none of thesearrow_forward
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