Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN: 9781938168390
Author: Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher: OpenStax
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Chapter 5, Problem 78E
From the data in Table 5.2, determine which of the following fuels produces the greatest amount of heat per gram when burned under standard conditions:
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Chapter 5 Solutions
Chemistry by OpenStax (2015-05-04)
Ch. 5 - A burning match and a bonfire may have the same...Ch. 5 - Prepare a table identifying several energy...Ch. 5 - Explain the difference between heat capacity and...Ch. 5 - Calculate the heat capacity, in joules and in...Ch. 5 - Calculate the heat capacity, in joules and in...Ch. 5 - How much heat, in joules and in calories, must be...Ch. 5 - How much heat, in joules and in calories, is...Ch. 5 - How much would the temperature of 275 g of water...Ch. 5 - If 14.5 kJ of heat were added to 485 g of liquid...Ch. 5 - A piece of unknown substance weighs 44.7 g and...
Ch. 5 - A piece of unknown solid substance weighs 437.2 g,...Ch. 5 - An aluminum kettle weighs 1.05 kg. (a) What is the...Ch. 5 - Most people find waterbeds uncomfortable unless...Ch. 5 - A 500-mL bottle of water at room temperature and a...Ch. 5 - Would the amount of heat measured for the reaction...Ch. 5 - Would the amount of heat absorbed by the...Ch. 5 - Would the amount of heat absorbed by the...Ch. 5 - How many milliliters of water at 23 C with a...Ch. 5 - How much will the temperature of a cup (180 g) of...Ch. 5 - A 45-g aluminum spoon (specific heat 0.88 J/g C)...Ch. 5 - The temperature of the cooling water as it leaves...Ch. 5 - A 70.0-g piece of metal at 80.0 °C is placed in...Ch. 5 - If a reaction produces 1.506 kJ of heat, which is...Ch. 5 - A 0.500-g sample of KCl is added to 50.0 g of...Ch. 5 - Dissolving 3.0 g of CaCl2(s) in 150.0 g of water...Ch. 5 - When 50.0 g of 0.200 M NaCl(aq) at 24.1 C is added...Ch. 5 - The addition of 3.15 g of Ba(OH)28H2O to a...Ch. 5 - The reaction of 50 mL of acid and 50 mL of base...Ch. 5 - If the 3.21 g of NH4NO3 in Example 5.6 were...Ch. 5 - When 1.0 g of fructose, C6H12O6(s), a sugar...Ch. 5 - When a 0.740-g sample of trinitrotoluene (TNT),...Ch. 5 - One method of generating electricity is by burning...Ch. 5 - The amount of fat recommended for someone with a...Ch. 5 - A teaspoon of the carbohydrate sucrose (common...Ch. 5 - What is the maximum mass of carbohydrate in a 6-oz...Ch. 5 - A pint of premium ice cream can contain 1100...Ch. 5 - A serving of a breakfast cereal contains 3 g of...Ch. 5 - Which is the least expensive source of energy in...Ch. 5 - Explain how the heat measured in Example 5.5...Ch. 5 - Using the data in the check your learning section...Ch. 5 - Calculate the enthalpy of solution ( H for the...Ch. 5 - Calculate H for the reaction described by the...Ch. 5 - Calculate the enthalpy of solution ( H for the...Ch. 5 - Although the gas used in an oxyacetylene torch...Ch. 5 - How much heat is produced by burning 4.00 moles of...Ch. 5 - How much heat is produced by combustion of 125 g...Ch. 5 - How many moles of isooctane must be burned to...Ch. 5 - What mass of carbon monoxide must be burned to...Ch. 5 - When 2.50 g of methane burns in oxygen, 125 kJ of...Ch. 5 - How much heat is produced when loo mL of 0.250 M...Ch. 5 - A sample of 0.562 g of carbon is burned in oxygen...Ch. 5 - Before the introduction of chlorofluorocarbons,...Ch. 5 - Homes may be heated by pumping hot water through...Ch. 5 - Which of the enthalpies of combustion in Table 5.2...Ch. 5 - Does the standard enthalpy of formation of H2O(g)...Ch. 5 - Joseph Priestly prepared oxygen in 1774 by heating...Ch. 5 - How many kilojoules of heat will be released when...Ch. 5 - How many kilojoules of heat will be released when...Ch. 5 - The following sequence of reactions occurs in the...Ch. 5 - Both graphite and diamond burn....Ch. 5 - From the molar heats of formation in Appendix G,...Ch. 5 - Which produces more heat?...Ch. 5 - Calculate H298 for the process...Ch. 5 - Calculate H298 for the process...Ch. 5 - Calculate H for the process Hg2Cl2(s)2Hg(l)+Cl2(g)...Ch. 5 - Calculate H298 for the process...Ch. 5 - Calculate the standard molar enthalpy of formation...Ch. 5 - Using the data in Appendix G, calculate the...Ch. 5 - Using the data in Appendix G, calculate the...Ch. 5 - The following reactions can be used to prepare...Ch. 5 - The decomposition of hydrogen peroxide, H2O2, has...Ch. 5 - Calculate the enthalpy of combustion of propane,...Ch. 5 - Calculate the enthalpy of combustion of butane,...Ch. 5 - Both propane and butane are used as gaseous fuels....Ch. 5 - The white pigment TiO2 is prepared by the reaction...Ch. 5 - Water gas, a mixture of H2 and CO, is an important...Ch. 5 - In the early days of automobiles, illumination at...Ch. 5 - From the data in Table 5.2, determine which of the...Ch. 5 - The enthalpy of combustion of hard coal averages...Ch. 5 - Ethanol, C2H5OH, is used as a fuel for motor...Ch. 5 - Among the substances that react with oxygen and...Ch. 5 - How much heat is produced when 1.25 g of chromium...Ch. 5 - Ethylene, C2H2, a byproduct from the fractional...Ch. 5 - The oxidation of the sugar glucose, C6H12O6, is...Ch. 5 - Propane, C3H8, is a hydrocarbon that is commonly...Ch. 5 - During a recent winter month in Sheboygan,...
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- In a bomb calorimeter, the reaction vessel is surrounded by water that must be added for each experiment. Since the amount of water is not constant from experiment to experiment, the mass of water must be measured in each case. The heat capacity of the calorimeter is broken down into two parts: the water and the calorimeter components. If a calorimeter contains 1.00 kg water and has a total heat capacity of 10.84 kJ/C, what is the heat capacity of the calorimeter components?arrow_forwardWhen solid iron burns in oxygen gas (at constant pressure) to produce Fe2O3(s), 1651 kJ of heat is released for every 4 mol of iron burned. How much heat is released when 10.3 g Fe2O3(s) is produced (at constant pressure)? What additional information would you need to calculate the heat released to produce this much Fe2O3(s) if you burned iron in ozone gas, O3(g), instead of 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
- 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). The 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 the reaction. Is the process exothermic or endothermic? (b) Write the chemical equation and evaluate H.arrow_forwardThe equation for the combustion of butane, C4H10, is C4H10(g)+132O2(g)4CO2(g)+5H2O(g) Which one of the following generates the least heat? Why? a Burning one mole of butane b Reacting one mole of oxygen with excess butane c Producing one mole of carbon dioxide by burning butane d Producing one mole of water by burning butanearrow_forwardThe temperature of the cooling water as it leaves the hot engine of an automobile is 240 F. After it passes through the radiator it has a temperature of 175 F. Calculate the amount of heat transferred from the engine to the surroundings by one gallon of water with a specific heat of 4.184 J/g oC.arrow_forward
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