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 62E
Which produces more heat?
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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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- The formation of aluminum oxide from its elements is highly exothermic. If 2.70 g Al metal is burned in pure O2 to give A12O3, calculate how much thermal energy is evolved in the process (at constant pressure).arrow_forwardWhich of the following processes will lead to a decrease in the internal energy of a system? (1) Energy is transferred as heat to the system; (2) energy is transferred as heat from the system; (3) energy is transferred as work done on the system; or (4) energy is transferred as work done by the system. (a) 1 and 3 (b) 2 and 4 (c) 1 and 4 (d) 2and3arrow_forwardAn industrial process for manufacturing sulfuric acid, H2SO4, uses hydrogen sulfide, H2S, from the purification of natural gas. In the first step of this process, the hydrogen sulfide is burned to obtain sulfur dioxide, SO2. 2H2S(g)+3O2(g)2H2O(l)+2SO2(g);H=1124kJ The density of sulfur dioxide at 25C and 1.00 atm is 2.62 g/L, and the molar heat capacity is 30.2 J/(mol C). (a) How much heat would be evolved in producing 1.00 L of SO2 at 25C and 1.00 atm? (b) Suppose heat from this reaction is used to heat 1.00 L of the SO2 from 25C to 500C for its use in the next step of the process. What percentage of the heat evolved is required for this?arrow_forward
- The decomposition of ozone, O3, to oxygen, O2, is an exothermic reaction. What is the sign of q? If you were to touch a flask in which ozone is decomposing to oxygen, would you expect the flask to feel warm or cool?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_forwardIndicate which state function is equal to heat, q, for each process described. a. The ignition of a sample in a bomb calorimeter, an unyielding, heavy metal chamberin which samples are burned for heat content analysis b.The melting of an icecube in a cup c.The cooling down ofthe inside of arefrigerator d.A fire in a fireplacearrow_forward
- Dissolving 6.00 g CaCl2 in 300 mL of water causes the temperature of the solution to increase by 3.43 C. Assume that the specific heat of the solution is 4.18 J/g K and its mass is 306 g. (a) Calculate the enthalpy change when the CaCl2 dissolves. Is the process exothermic or endothermic? (b) Determine H on a molar basis for CaCl2(s)H2OCa2+(aq)+2Cl(aq)arrow_forwardAlloys When a 58.8-g piece of hot alloy is placed in125 g of cold water in a calorimeter, the temperature ofthe alloy decreases by 106.1°C, while the temperature ofthe water increases by 10.5°C. What is the specific heat ofthe alloy?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_forward
- Gasohol, a mixture of gasoline and ethanol, C2H5OH, is used as automobile fuel. The alcohol releases energy in a combustion reaction with O2. C2H5OH(l)+3O2(g)2CO2(g)+3H2O(l) If 0.115 g ethanol evolves 3.62 kJ when burned at constant pressure, calculate the combustion enthalpy for ethanol.arrow_forward2. In which of the following reactions is there a significant transfer of energy as work from the system to the surroundings? This occurs if there is a change in the number of moles of gases. C(s) + O2(g) → CO2(g) CH4(g) + 2 O2(g) → CO2g) + 2 H2O(g) 2 C(s) + O2(g) → 2 CO(g) 2 Mg(s) + O2(g) → 2 MgO(s)arrow_forwardThe process of dissolving ammonium nitrate, NH4NO3, in water is an endothermic process. What is the sign of q? If you were to add some ammonium nitrate to water in a flask, would you expect the flask to feel warm or cool?arrow_forward
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