Chemistry For Changing Times (14th Edition)
14th Edition
ISBN: 9780321972026
Author: John W. Hill, Terry W. McCreary
Publisher: PEARSON
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Chapter 15, Problem 79AP
Production of gasoline from tar sands requires natural gas. If the ratio between the energy needed to generate the gasoline and the energy content of the gasoline itself is very low, why is this production methane pursued?
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Chapter 15 Solutions
Chemistry For Changing Times (14th Edition)
Ch. 15 - Prob. 1RQCh. 15 - Prob. 2RQCh. 15 - Prob. 3RQCh. 15 - Prob. 4RQCh. 15 - Prob. 5PCh. 15 - Prob. 6PCh. 15 - Prob. 7PCh. 15 - Prob. 8PCh. 15 - Prob. 9PCh. 15 - Prob. 10P
Ch. 15 - Prob. 11PCh. 15 - Prob. 12PCh. 15 - Prob. 13PCh. 15 - Prob. 14PCh. 15 - Prob. 15PCh. 15 - Prob. 16PCh. 15 - Prob. 17PCh. 15 - Prob. 18PCh. 15 - Prob. 19PCh. 15 - Prob. 20PCh. 15 - Prob. 21PCh. 15 - Prob. 22PCh. 15 - Prob. 23PCh. 15 - Prob. 24PCh. 15 - Prob. 25PCh. 15 - Prob. 26PCh. 15 - Which has higher entropy, potassium in solid...Ch. 15 - Prob. 28PCh. 15 - Prob. 29PCh. 15 - Prob. 30PCh. 15 - Prob. 31PCh. 15 - Prob. 32PCh. 15 - Prob. 33PCh. 15 - Prob. 34PCh. 15 - Prob. 35PCh. 15 - Prob. 36PCh. 15 - Prob. 37PCh. 15 - Prob. 38PCh. 15 - Prob. 39PCh. 15 - Prob. 40PCh. 15 - Prob. 41PCh. 15 - Prob. 42PCh. 15 - Prob. 43PCh. 15 - Prob. 44PCh. 15 - Prob. 45PCh. 15 - Prob. 46PCh. 15 - Prob. 47PCh. 15 - Prob. 48PCh. 15 - Prob. 49PCh. 15 - Prob. 50PCh. 15 - Prob. 51PCh. 15 - Prob. 52PCh. 15 - Prob. 53PCh. 15 - Prob. 54PCh. 15 - Prob. 55PCh. 15 - Prob. 56PCh. 15 - Prob. 57PCh. 15 - What are some problems associated with the use of...Ch. 15 - Prob. 59PCh. 15 - Prob. 60PCh. 15 - Prob. 61PCh. 15 - Prob. 62PCh. 15 - Prob. 63PCh. 15 - Prob. 64PCh. 15 - Prob. 65PCh. 15 - Prob. 66APCh. 15 - Prob. 67APCh. 15 - Prob. 68APCh. 15 - Prob. 69APCh. 15 - Prob. 70APCh. 15 - Both a banana and a hand grenade have about 170...Ch. 15 - Prob. 72APCh. 15 - Prob. 73APCh. 15 - Prob. 74APCh. 15 - Prob. 75APCh. 15 - Prob. 76APCh. 15 - Prob. 77APCh. 15 - Prob. 78APCh. 15 - Production of gasoline from tar sands requires...Ch. 15 - Prob. 80APCh. 15 - Prob. 15.1CTECh. 15 - Prob. 15.2CTECh. 15 - Prob. 15.3CTECh. 15 - Prob. 15.4CTECh. 15 - Prob. 15.5CTECh. 15 - Prob. 15.6CTECh. 15 - Prob. 1CGPCh. 15 - Prepare a PowerPoint, poster, or other...Ch. 15 - Prob. 3CGPCh. 15 - Prob. 4CGPCh. 15 - Prob. 5CGPCh. 15 - Prob. 6CGPCh. 15 - Prob. 7CGPCh. 15 - Prob. 8CGPCh. 15 - Prob. 9CGPCh. 15 - Prob. 1CHQCh. 15 - Prob. 2CHQCh. 15 - Prob. 3CHQCh. 15 - Prob. 4CHQCh. 15 - Prob. 5CHQ
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- Water gas, a mixture of carbon monoxide and hydrogen, is produced by treating carbon (in the form of coke or coal) with steam at high temperatures. (See Study Question 83.) C(s) + H2O(g) CO(g) + H2(g) Not all of the carbon available is converted to water gas since some is burned to provide the heat for the endothermic reaction of carbon and water. What mass of carbon must be burned (to CO2 gas) to provide the energy to convert 1.00 kg of carbon to water gas?arrow_forwardA rebreathing gas mask contains potassium superoxide, KO2, which reacts with moisture in the breath to give oxygen. 4KO2(s)+2H2O(l)4KOH(s)+3O2(g) Estimate the grams of potassium superoxide required to supply a persons oxygen needs for one hour. Assume a person requires 1.00 102 kcal of energy for this time period. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 1.00 102 kcal of heat, calculate the amount of oxygen consumed and hence the amount of KO2 required. The ff0 for glucose(s) is 1273 kJ/mol.arrow_forwardEthylene, C2H2, a byproduct from the fractional distillation of petroleum, is fourth among the 50 chemical compounds produced commercially in the largest quantities. About 80% of synthetic ethanol is manufactured from ethylene by its reaction with water in the presence of a suitable catalyst. C2H2(g)+H2O(g)C2H5OH(l) Using the data in the table in Appendix G, calculate H for the reaction.arrow_forward
- The equation for the fermentation of glucose to alcohol and carbon dioxide is: C6H12O6(aq) 2C2H5OH(aq) + 2CO2(g) The enthalpy change for the reaction is 67 kJ. Is this reaction exothermic or endothermic? Is energy, in the form of heat, absorbed or evolved as the reaction occurs?arrow_forwardWhat is incomplete combustion of fossil fuels? Why can this be a problem?arrow_forwardWhen one mole of ethylene gas, C2H4, reacts with fluorine gas, hydrogen fluoride and carbon tetrafluoride gases are formed and 2496.7 kJ of heat are given off. What is Hf for CF4(g)?arrow_forward
- When 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_forwardThe carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.arrow_forwardConsider the two space shuttle fuel reactions in Exercises 81 and 82. Which reaction produces more energy per kilogram of reactant mixture (stoichiometric amounts)? 81. The reusable booster rockets of the space shuttle use a mixture of aluminum and ammonium perchlorate as fuel. A possible reaction is 3Al(s)+3NH4ClO4(s)Al2O3(s)+AlCl3(s)+3NO(g)+6H2O(g) Calculate H for this reaction 82. The space shuttle Orbiter utilizes the oxidation of methylhydrazine by dinitrogen tetroxide for propulsion: 4N2H3CH3(l)+5N2O4(l)12H2O(g)+9N2(g)+4CO2(g) Calculate H for this reactionarrow_forward
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