Chemistry for Engineering Students
3rd Edition
ISBN: 9781285199023
Author: Lawrence S. Brown, Tom Holme
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 9, Problem 9.31PAE
9.31 A metal radiator is made from 26.0 kg of iron. The specific heat of iron is
Expert Solution & Answer
Trending nowThis is a popular solution!
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
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Graphite is burned in oxygen to give carbon monoxide and carbon dioxide. If the product mixture is 33% CO and 67% CO2 by mass, what is the heat from the combustion of 1.00 g of graphite?arrow_forwardHow much heat is absorbed by a 44.7-g piece of leadwhen its temperature increases by 65.4°C?arrow_forwardChlorine dioxide, ClO2, is a reddish yellow gas used in bleaching paper pulp. The average speed of a ClO2 molecule at 25C is 306 m/s. What is the kinetic energy (in joules) of a ClO2 molecule moving at this speed?arrow_forward
- When steam condenses to liquid water, 2.26 kJ of heat is released per gram. The heat from 168 g of steam is used to heat a room containing 6.44 104 g of air (20 ft 12 ft 8 ft). The specific heat of air at normal pressure is 1.015 J/(gC). What is the change in air temperature, assuming the heat from the steam is all absorbed by air?arrow_forwardIn a calorimetric experiment, 6.48 g of lithium hydroxide, LiOH, was dissolved in water. The temperature of the calorimeter rose from 25.00C to 36.66C. What is H for the solution process? LiOH(s)Li(aq)+OH(aq) The heat capacity of the calorimeter and its contents is 547 J/C.arrow_forwardThe thermochemical equation for the burning of methane, the main component of natural gas, is CH4(g)+2O2(g)CO2(g)+2H2O(l)H=890kJ (a) Is this reaction endothermic or exothermic? (b) What quantities of reactants and products are assumed if H = 890 kJ? (c) What is the enthalpy change when 1.00 g methane burns in an excess of oxygen?arrow_forward
- A piece of lead of mass 121.6 g was heated by an electrical coil. From the resistance of the coil, the current, and the Time the current flowed, it was calculated that 235 J of heat was added to the lead. The temperature of the lead rose from 20.4C to 35.5C. What is the specific heat of the lead?arrow_forwardWhen lightning strikes, the energy can force atmospheric nitrogen and oxygen to react to make NO: N2(g)+O2(g)2NO(g)H=+181.8kJ (a) Is this reaction endothermic or exothermic? (b) What quantities of reactants and products are assumed if H = +181.8 kJ? (c) What is the enthalpy change when 3.50 g nitrogen is reacted with excess O2(g)?arrow_forwardWhat 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.arrow_forward
- Hydrogen sulfide, H2S, is produced during decomposition of organic matter. When 0.5000 mol H2S burns to produce SO2(g) and H2O(l), 281.0 kJ of heat is released. What is this heat in kilocalories?arrow_forwardA 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?arrow_forwardWhen a 0.740-g sample of trinitrotoluene (TNT), C7H5N2O6, is burned in a bomb calorimeter, the temperature increases from 23.4 C to 26.9 C. The heat capacity of the calorimeter is 534 J/C, and it contains 675 mL of water. How much heat was produced by the combustion of the TNT sample?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning
World of ChemistryChemistryISBN:9780618562763Author:Steven S. ZumdahlPublisher:Houghton Mifflin College Div
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
General Chemistry - Standalone book (MindTap Cour...
Chemistry
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:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
World of Chemistry
Chemistry
ISBN:9780618562763
Author:Steven S. Zumdahl
Publisher:Houghton Mifflin College Div
Calorimetry Concept, Examples and Thermochemistry | How to Pass Chemistry; Author: Melissa Maribel;https://www.youtube.com/watch?v=nSh29lUGj00;License: Standard YouTube License, CC-BY