Chemistry: Structure and Properties (2nd Edition)
2nd Edition
ISBN: 9780134293936
Author: Nivaldo J. Tro
Publisher: PEARSON
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Textbook Question
Chapter 9, Problem 41E
How much heat is required to warm 1.50 L of water from 25.0 °C to 100.0 °C? (Assume a density of 1.00 g/mL for the water.)
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Chapter 9 Solutions
Chemistry: Structure and Properties (2nd Edition)
Ch. 9 - What is thermochemistry? Why is it important?Ch. 9 - What is energy? What is work? List some examples...Ch. 9 - Prob. 3ECh. 9 - What is the law of conservation of energy? How...Ch. 9 - A friend claims to have constructed a machine that...Ch. 9 - What is a state function? List some examples of...Ch. 9 - What is internal energy? Is internal energy a...Ch. 9 - If energy flows out of a chemical system and into...Ch. 9 - If the internal energy of the products of a...Ch. 9 - What is heat? Explain the difference between heat...
Ch. 9 - How is the change in internal energy of a system...Ch. 9 - Explain how the sum of heat and work can be a...Ch. 9 - What is heat capacity? Explain the difference...Ch. 9 - Explain how the high specific heat capacity of...Ch. 9 - If two objects, A and B, of different temperature...Ch. 9 - What is pressure-volume work? How is it...Ch. 9 - What is calorimetry? Explain the difference...Ch. 9 - What is the change in enthalpy ( H) for a...Ch. 9 - Explain the difference between an exothermic and...Ch. 9 - From a molecular viewpoint where does the energy...Ch. 9 - From a molecular viewpoint, where does the energy...Ch. 9 - Is the change in enthalpy for a reaction an...Ch. 9 - Explain how the value of H for a reaction changes...Ch. 9 - What is Hess's law? Why is it useful?Ch. 9 - What is a standard state? What is the standard...Ch. 9 - How can bond energies be used to estimate H for a...Ch. 9 - Explain the difference between exothermic and...Ch. 9 - What is the standard enthalpy of formation for a...Ch. 9 - How do you calculate Hrxn from tabulated standard...Ch. 9 - What is lattice energy? How does lattice energy...Ch. 9 - Which statement is true of the internal energy of...Ch. 9 - During an energy exchange, a chemical system...Ch. 9 - Identify each energy exchange as primarily heat or...Ch. 9 - Identify each energy exchange as primarily heat or...Ch. 9 - A system releases 622 kJ of heat and does 105 kJ...Ch. 9 - A system absorbs 196 kJ of heat, and the...Ch. 9 - The gas in a piston (defined as the system) warms...Ch. 9 - The air in an inflated balloon (defined as the...Ch. 9 - A person packs two identical coolers for a picnic,...Ch. 9 - A kilogram of aluminum metal and a kilogram of...Ch. 9 - How much heat is required to warm 1.50 L of water...Ch. 9 - How much heat is required to warm 1.50 kg of sand...Ch. 9 - Suppose that 25 g of each substance is initially...Ch. 9 - An unknown mass of each substance, initially at...Ch. 9 - How much work (in J) is required to expand the...Ch. 9 - The average human lung expands by about 0.50 L...Ch. 9 - The air within a piston equipped with a cylinder...Ch. 9 - A gas is compressed from an initial volume of 5.55...Ch. 9 - When 1 mol of a fuel burns at constant pressure,...Ch. 9 - The change in internal energy for the combustion...Ch. 9 - Is each process exothermic or endothermic?...Ch. 9 - Is each process exothermic or endothermic?...Ch. 9 - Consider the thermochemical equation for the...Ch. 9 - What mass of natural gas (CH4) must bum to emit...Ch. 9 - Nitromethane (CH3NO2) burns in air to produce...Ch. 9 - Titanium reacts with iodine to form titanium (III)...Ch. 9 - The propane fuel (C3H8) used in gas barbeques bums...Ch. 9 - Charcoal is primarily carbon. Determine the mass...Ch. 9 - We submerge a silver block, initially at 58.5 °C...Ch. 9 - We submerge a 32.5-g iron rod, initially at 22.7...Ch. 9 - We submerge a 31.1-g wafer of pure gold initially...Ch. 9 - We submerge a 2.85-g lead weight, initially at...Ch. 9 - Two substances, A and B, initially at different...Ch. 9 - A 2.74-g sample of a substance suspected of being...Ch. 9 - Exactly 1.5 g of a fuel burns under conditions of...Ch. 9 - In order to obtain the largest possible amount of...Ch. 9 - When 0.514 g of biphenyl (C12H10) undergoes...Ch. 9 - Mothballs are composed primarily of the...Ch. 9 - Zinc metal reacts with hydrochloric acid according...Ch. 9 - Instant cold packs used to ice athletic injuries...Ch. 9 - For each generic reaction, determine the value of...Ch. 9 - Consider the generic reaction: A+2BC+3DH=155kJ...Ch. 9 - Calculate Hrxn for the reaction:...Ch. 9 - Calculate Hrxn for the reaction:...Ch. 9 - Calculate Hrxn for the reaction:...Ch. 9 - Calculate Hrxn for the reaction:...Ch. 9 - Hydrogenation reactions are used to add hydrogen...Ch. 9 - Ethanol is a possible fuel. Use average bond...Ch. 9 - Hydrogen, a potential future fuel, can be produced...Ch. 9 - Hydroxyl radicals react with and eliminate many...Ch. 9 - Write an equation for the formation of each...Ch. 9 - Prob. 82ECh. 9 - S3. Hydrazine (N2H4) is a fuel used by some...Ch. 9 - Prob. 84ECh. 9 - Prob. 85ECh. 9 - Prob. 86ECh. 9 - Prob. 87ECh. 9 - Prob. 88ECh. 9 - Top fuel dragsters and funny cars burn...Ch. 9 - Prob. 90ECh. 9 - Prob. 91ECh. 9 - Rubidium iodide has a lattice energy of-617...Ch. 9 - Prob. 93ECh. 9 - Prob. 94ECh. 9 - Use the Born-Haber cycle and data from Appendix...Ch. 9 - Prob. 96ECh. 9 - The kinetic energy of a rolling billiard ball is...Ch. 9 - A100-W light bulb is placed in a cylinder equipped...Ch. 9 - Evaporating sweat cools the body because...Ch. 9 - LP gas burns according to the exothermic reaction:...Ch. 9 - Use standard enthalpies of formation to calculate...Ch. 9 - Dry ice is solid carbon dioxide. Instead of...Ch. 9 - A 25.5-g aluminum block is warmed to 65.4 °C and...Ch. 9 - We mix 50.0 mL of ethanol (density = 0.789 g/mL)...Ch. 9 - Prob. 105ECh. 9 - Prob. 106ECh. 9 - One tablespoon of peanut butter has a mass of 16...Ch. 9 - Prob. 108ECh. 9 - Prob. 109ECh. 9 - When we burn 10.00 g of phosphorus in O2 (g) to...Ch. 9 - The H for the oxidation of S in the gas phase to...Ch. 9 - The Hfo of TiI3(s) is -328 kJ/mol; and the Ho for...Ch. 9 - A copper cube measuring 1.55 cm on edge and an...Ch. 9 - A pure gold ring and pure silver ring have a total...Ch. 9 - The reaction of Fe2O3(s) with Al(s) to form...Ch. 9 - Prob. 116ECh. 9 - Prob. 117ECh. 9 - Prob. 118ECh. 9 - Prob. 119ECh. 9 - Calculate the heat of atomization (see previous...Ch. 9 - Prob. 121ECh. 9 - Prob. 122ECh. 9 - Prob. 123ECh. 9 - Prob. 124ECh. 9 - Prob. 125ECh. 9 - Find H, E, q, and w for the freezing of water at...Ch. 9 - The heat of vaporization of water at 373 K is 40.7...Ch. 9 - Prob. 128ECh. 9 - Prob. 129ECh. 9 - Prob. 130ECh. 9 - Prob. 131ECh. 9 - Prob. 132ECh. 9 - Prob. 133ECh. 9 - Which expression describes the heat emitted in a...Ch. 9 - Prob. 135ECh. 9 - Prob. 136ECh. 9 - Prob. 137ECh. 9 - Prob. 138ECh. 9 - Prob. 139ECh. 9 - Which statement is true of a reaction in which V...Ch. 9 - Which statement is true of an endothermic...Ch. 9 - When a firecracker explodes, energy is obviously...Ch. 9 - Prob. 143ECh. 9 - Classify each process as endothermic or...Ch. 9 - A propane tank on a home barbeque contains 10.4 x...Ch. 9 - Prob. 146ECh. 9 - Consider the decomposition of liquid hydrogen...Ch. 9 - Prob. 148ECh. 9 - A chemical system produces 155 kJ of heat and does...Ch. 9 - Which sample is most likely to undergo the...Ch. 9 - Prob. 3SAQCh. 9 - A 12.5-g sample of granite initially at 82.0 C is...Ch. 9 - A cylinder with a moving piston expands from an...Ch. 9 - When a 3.80-g sample of liquid octane (C8H18)...Ch. 9 - Hydrogen gas reacts with oxygen to form water....Ch. 9 - Manganese reacts with hydrochloric acid to produce...Ch. 9 - Consider the reactions: A2BH1A3CH2 What is H for...Ch. 9 - Use standard enthalpies of formation to determine...Ch. 9 - Prob. 11SAQCh. 9 - Prob. 12SAQCh. 9 - Prob. 13SAQCh. 9 - Which set of compounds is arranged in order of...Ch. 9 - Prob. 15SAQ
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- Enthalpy a A 100.-g sample of water is placed in an insulated container and allowed to come to room temperature at 21C. To heat the water sample to 41C, how much heat must you add to it? b Consider the hypothetical reaction,2X(aq)+Y(l)X2Y(aq)being run in an insulated container that contains 100. g of solution. If the temperature of the solution changes from 21C to 31C, how much heat does the chemical reaction produce? How does this answer compare with that in part a? (You can assume that this solution is so dilute that it has the same heat capacity as pure water.) c If you wanted the temperature of 100. g of this solution to increase from 21C to 51C, how much heat would you have to add to it? (Try to answer this question without using a formula.) d If you had added 0.02 mol of X and 0.01 mol of Y to form the solution in part b, how many moles of X and Y would you need to bring about the temperature change described in part c. e Judging on the basis of your answers so far, what is the enthalpy of the reaction 2X(aq) + Y(l) X2Y(aq)?arrow_forwardHow much heat is evolved when 1255 g of water condensesto a liquid at 100°C?arrow_forwardHow much would the temperature of 275 g of water increase if 36.5 U of heat were added?arrow_forward
- Calcium oxide (quicklime) reacts with water to produce calcium hydroxide (slaked lime). CaO(s)+H2O(l)Ca(OH)2(s);H=65.2kJ The heat released by this reaction is sufficient to ignite paper. How much heat is released when 28.6 g of calcium oxide reacts?arrow_forwardCopper is used in building the integrated circuits, chips, and printed circuit boards for computers. When 228 J of heat are absorbed by 125 g of copper at 22.38C, the temperature rises to 27.12C. What is the specific heat of copper?arrow_forwardIf 125 J of heat energy is applied to a block of silver weighing 29.3 g, by how many degrees will the temperature of the silver increase? (See Table 10.1.)arrow_forward
- Alloys 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_forwardWhich molecule, HF, HCl, HBr, or HI, has the strongest chemical bond?arrow_forwardHow much heat, in joules and in calories, must be added to a 75.0g iron block with a specific heat of 0.449 Jig C to increase its temperature from 25 C to its melting temperature of 1535 C?arrow_forward
- 9.45 What happens to the temperature of a material as it undergoes an endothermic phase change? If heat is added, how can the temperature behave in this manner?arrow_forwardA student used a coffee-cup calorimeter to determine the enthalpy of solution for NH4NO3.When NH4NO3 is added to water, there is a decrease in temperature of the solution. Is the solution process exothermic or endothermic? (a) endothermic (b) exothermicarrow_forwardHow much heat is required to raise the temperature of 100. grams of water from 25C near room temperature to 100.C its boiling point? The specific heat of water is approximately 4.2Jperg-K. a.3.2104J b.32J c.4.2104J d.76Jarrow_forward
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