iii. C6H1206(s)→6C(diamond)+6H2(g)+302(g)b. The standard enthalpy change for the reaction CaCO:(s) → CaO(s) + CO2(g) is178.1 kJ. Use Table 5.3 to calculate the standard enthalpy of formation ofCaCO:(s).TABLE 5.3 · Standard Enthalpies of Formation, AH, at 298 KSubstanceFormulaAH} (kl/mol)SubstanceFormulaAHF (kJ/mol)Hydrogen chlorideHydrogen fluorideHydrogen iodideAcetyleneHC(g)HF(g)226.7-92.30AmmoniaNH3(g)-46.19-268.60BenzeneCH(1)49.0HI(g)25.9Calcium carbonateCaCO,(s)-1207.1MethaneCH,(g)-74.80Calcium oxideCaO(s)-635.5MethanolCH,OH()-238.6Carbon dioxideCO:(g)-393.5PropaneC,Hlg)-103.85Carbon monoxideCOlg)-110.5Silver chlorideAgCI(s)-127.0DiamondC(s)1.88Sodium bicarbonateNAHCO,(s)-947.7EthaneC,Holg)C;H;OH()-84.68Sodium carbonateNa,CO,(s)-1130.9Ethanol-277.7Sodium chlorideNaCl(s)-410.9EthyleneSucroseCHlg)CH120,(s)52.30-2221Glucose-1273WaterH,O()-285.8Hydrogen bromideHBr(g)-36.23Water vaporH;O(g)-241.82012 Pearon Bducation, Inc 5. Enthalpy of formationa. For which of these reactions at 25 °C does the enthalpy change represent astandard enthalpy of formation? For each that does not, what changes are neededto make it an equation whose AH is an enthalpy of formation?i. 2Na(s)+02(g)→Na20(s)ii. 2K(1)+Cl2(g)→2KCI(s)

a) Standard enthalpy of formation is the change in enthalpy when one mole of compound is formed from…

Answered: 5. Enthalpy of formation a. For which…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter5: Thermochemistry

Section: Chapter Questions

Problem 5.99QE

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One step in the manufacturing of sulfuric acid is the conversion of SO2(g) to SO3(g). The thermochemical equation for this process is SO2(g)+12O2(g)SO3(g)H=98.9kJ The second step combines the SO3 with H2O to make H2SO4. (a) Calculate the enthalpy change that accompanies the reaction to make 1.00 kg SO3(g). (b) Is heat absorbed or released in this process?
When one mol of KOH is neutralized by sulfuric acid, q=56 kJ. (This is called the heat of neutralization.) At 23.7C, 25.0 mL of 0.475 M H2SO4 is neutralized by 0.613 M KOH in a coffee-cup calorimeter. Assume that the specific heat of all solutions is 4.18J/gC, that the density of all solutions is 1.00 g/mL, and that volumes are additive. (a) How many mL of KOH is required to neutralize H2SO4? (b) What is the final temperature of the solution?
A 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?
Assume 200. mL of 0.400 M HCl is mixed with 200. mL of 0.400 M NaOH in a coffee-cup calorimeter The temperature of the solutions before mixing was 25.10 C; after mixing and allowing the reaction to occur, the temperature is 27.78 C. What is the enthalpy change when one mole of acid is neutralized? (Assume that the densities of all solutions are 1.00 g/mL and their specific heat capacities are 4.20 J/g K.)
Calculate the standard enthalpy of combustion for benzene, C6H6. C6H6() + 15/2 O2(g) 6 CO2(g) + 3 H2O() rH = ? The enthalpy of formation of benzene is known [rH[C6H6()] = +49.0 kJ/mol], and other values needed can be found in Appendix L.
In a coffee-cup calorimeter, 100.0 mL of 1.0 M NaOH and 100.0 mL of 1.0 M HCI are mixed. Both solutions were originally at 24.6C. After the reaction, the final temperature is 31.3C. Assuming that all the solutions have a density of 1.0 g/cm3 and a specific heat capacity of 4.18 J/Cg, calculate the enthalpy change for the neutralization of HCl by NaOH. Assume that no heat is lost to the surroundings or to the calorimeter.
Consider the reaction 2HCl(aq)+Ba(OH)2(aq)BaCl2(aq)+2H2O(l)H=118KJ Calculate the heat when 100.0 rnL of 0.500 M HCl is mixed with 300.0 mL of 0.100 M Ba(OH)2 Assuming that the temperature of both solutions was initially 25.0C and that the final mixture has a mass of 400.0 g and a specific heat capacity of 4.18 J/C g, calculate the final temperature of the mixture.
The enthalpy of combustion of diamond is -395.4 kJ/mol. C s, dia O2 g CO2 g Determine the fH of C s, dia.
Another reaction that is used to propel rockets is N2O4(l)+2N2H4(l)3N2(g)+4H2O(g) This reaction has the advantage that neither product is toxic, so no dangerous pollution is released. When the reaction consumes 10.0 g liquid N2O4, it releases 124 kJ of heat. (a) Is the sign of the enthalpy change positive or negative? (b) What is the value of H for the chemical equation if it is understood to be written in molar quantities?
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.
Combustion reactions involve reacting a substance with oxygen. When compounds containing carbon and hydrogen are combusted, carbon dioxide and water are the products. Using the enthalpies of combustion for C4H4 ( 2341 kJ/mol), C4H8 (2755 kJ/mol), and H2 (286 kJ/mol), calculate H for the reaction C4H4(g)+2H2(g)C4H8(g)
You want to determine the value for the enthalpy of formation of CaSO4(s), but the reaction cannot be done directly. Ca(s) + S(s) + 2 O2(g) CaSO4(s) You know, however, that (a) both calcium and sulfur react with oxygen to produce oxides in reactions that can be studied calorimetrically, and (b) the basic oxide CaO reacts with the acidic oxide SO3(g) to produce CaSO4(s) with rH = 402.7 kJ. Outline a method for determining fH for CaSO4(s), and identify the information that must be collected by experiment. Using information in Appendix L, confirm that fH for CaSO4(s) = 1433.5 kJ/mol.

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5. Enthalpy of formation a. For which of these reactions at 25 °C does the enthalpy change represent a standard enthalpy of formation? For each that does not, what changes are needed to make it an equation whose AH is an enthalpy of formation? i. 2Na(s)+÷02(g)¬Na20(s) ii. 2K(l)+Cl½(g)→2KCI(s)