Calcium carbonate decomposes to lime according to the following reaction: CaCO3(s) = CaO(s) + CO2(g) %3D What is the enthalpy change of the reaction at standard conditions? Substance AH° (kJ/mol) S° U/mol.K) Cp (U/mol.K) AHm U/mol) Cu (s) 33.4 22.65+0.00628T 13000 @ 1356 K Cu (1) 41.6 31.40 CaCO, (s) -1207 88.7 104.57+0.02193T-2595000/T CaO(s) -635.5 38.2 49.95+0.00489T-352000/T -393.5 213.6 22.24+0.0598T-349900/T 205.1 33.44 Cu O(s) -167.4 93.1 83.6 O a. 98 kJ O b. -98 kl Oc. 178 k) O d. O e -178 ki

Calcium carbonate decomposes to lime according to the following reaction: CaCO3(s) = CaO(s) + CO2(g) %3D What is the enthalpy change of the reaction at standard conditions? Substance AH° (kJ/mol) S° U/mol.K) Cp (U/mol.K) AHm U/mol) Cu (s) 33.4 22.65+0.00628T 13000 @ 1356 K Cu (1) 41.6 31.40 CaCO, (s) -1207 88.7 104.57+0.02193T-2595000/T CaO(s) -635.5 38.2 49.95+0.00489T-352000/T -393.5 213.6 22.24+0.0598T-349900/T 205.1 33.44 Cu O(s) -167.4 93.1 83.6 O a. 98 kJ O b. -98 kl Oc. 178 k) O d. O e -178 ki

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter8: Thermochemistry

Section: Chapter Questions

Problem 12QAP: The heat of neutralization, Hneut, can be defined as the amount of heat released (or absorbed), q,...

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9.102 A runner generates 418 kJ of energy per kilometer from the cellular oxidation of food. The runner's body must dissipate this heat or the body will overheat. Suppose that sweat evaporation is the only important cooling mechanism. If you estimate the enthalpy of evaporation of water as 44 kJ/mol and assume that sweat can he treated as water, describe how you would estimate the volume of sweat that would have to be evaporated if the runner runs a 10-km race.
A student is asked to calculate the amount of heat involved in changing 10.0 g of liquid bromine at room temperature (22.5C) to vapor at 59.0C.To do this, one must use Tables 8.1 and 8.2 for information on the specific heat, boiling point, and heat of vaporization of bromine. In addition, the following step-wise process must be followed. (a) Calculate H for: Br2(l,22.5C)Br2(l,59.0C) (b) Calculate H for: Br2(l,59.0C)Br2(g,59.0C) (c) Using Hess's law, calculate H for: Br2(l,22.5C)Br2(g,59.0C)
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
The enthalpy of combustion of hard coal averages 35 kJ/g, that of gasoline, 1.28105 kJ/gal. How many kilograms of hard coal provide the same amount of heat as is available from 1.0 gallon of gasoline? Assume that the density of gasoline is 0.692 g/mL (the same as the density of isooctane).
The thermite reaction was once used to weld rails: 2Al(s)+Fe2O3(s)Al2O3(s)+2Fe(s)(a) Using heat of formation data, calculate H for this reaction. (b) Take the specific heats of Al2O3 and Fe to be 0.77 and 0.45 J/g C, respectively. Calculate the temperature to which the products of this reaction will be raised, starting at room temperature, by the heat given off in the reaction. (c) Will the reaction produce molten iron (mpFe=1535C,Hfus=270J/g)?
9.56 Using heats of formation tabulated in Appendix E, calculate the heats of reaction for the following. (a) C2H2(g)+52O2(g)2CO2(g)+H2O(l) (b) PCl3(g)+Cl2(g)PCl5(g) (c) C2H4(g)+H2O(g)C2H5OH(g) (d) Fe2O3(s)+2Al(s)Al2O3(s)+2Fe(l)
A gaseous hydrocarbon reacts completely with oxygen gas to form carbon dioxide and water vapour. Given the following data, determine Hf for the hydrocarbon: Hreaction=2044.5KJ/molhydrocarbonHf(CO2)=393.5KJ/molHf(H2O)=242KJ/mol Density of CO2 and H2O product mixture at 1.00 atm, 200.c = 0.751g/L. The density of the hydrocarbon is less than the density of Kr at the same conditions.
Water gas is produced from the reaction of steam with coal: C(s)+H2O(g)H2(g)+CO(g) Assuming that coal is pure graphite, calculate H for this reaction.
9.95 How much heat is required to convert 250 g of water from liquid at 23°C: into steam at 107°C? (The necessary heat capacities and enthalpy changes can be found in the chapter or online.)
The heat of neutralization, Hneut, can be defined as the amount of heat released (or absorbed), q, per mole of acid (or base) neutralized. Hneut for nitric acid is -52 kJ/mol HNO3. At 27.3C, 50.00 mL of 0.743M HNO3 is neutralized by 1.00 M Sr(OH)2 in a coffee-cup calorimeter. (a) How many mL of Sr(OH)2 were used in the neutralization? (b) What is the final temperature of the resulting solution? (Use the assumptions in Question 11.)
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The addition of 3.15 g of Ba(OH)28H2O to a solution of 1.52 g of NH4SCN in loo g of water in a calorimeter caused the temperature to fall by 3.1 C. Assuming the specific heat of the solution and products is 4.20 J/g C, calculate the approximate amount of heat absorbed by the reaction, which can be represented by the following equation: Ba(OH)28H2O(s)+2NH4SCN(aq)Ba(SCN)2(aq)+2NH3(aq)+10H2O(l)