3. Chemical Formulas and Thermodynamics (continued)From the bond energy data given below, (a) write a balanced equation for the formation ofC.liquid formic acid from its elements (solid carbon, hydrogen gas and oxygen gas) and (b) calculate itsreaction energy in kJ.415 kJ/mol345 kl/mol460 kJ/mol490 kJ/mol436 kJ/molC-HO-HC-o360 kl/molO=0800 kJ/mol799 kl/molC-CC=CH-HC=0a. Write the equation for formation of Formic Acid from its elements:b. Show your AHrmx calculations. It may help to review the Lewis Structure of formic acid on page 4. Boxyour final answer.

#3: #(a): The chemical formula of formic acid is HCOOH or CH2O2. The standard state elements, C, H,…

3. Chemical Formulas and Thermodynamics (continued) C. From the bond energy data given below, (a) write a balanced equation for the formation of liquid formic acid from its elements (solid carbon, hydrogen gas and oxygen gas) and (b) calculate its reaction energy in kJ. C-H 415 kl/mol O-H 460 kJ/mol 360 kl/mol 800 kl/mol C=0 799 kl/mol C-o 345 kl/mol O=0 490 kJ/mol 436 kJ/mol C-C C=C H-H a. Write the equation for formation of Formic Acid from its elements: b. Show your AHmau calculations. It may help to review the Lewis Structure of formic acid on page 4. Box your final answer.

3. Chemical Formulas and Thermodynamics (continued) C. From the bond energy data given below, (a) write a balanced equation for the formation of liquid formic acid from its elements (solid carbon, hydrogen gas and oxygen gas) and (b) calculate its reaction energy in kJ. C-H 415 kl/mol O-H 460 kJ/mol 360 kl/mol 800 kl/mol C=0 799 kl/mol C-o 345 kl/mol O=0 490 kJ/mol 436 kJ/mol C-C C=C H-H a. Write the equation for formation of Formic Acid from its elements: b. Show your AHmau calculations. It may help to review the Lewis Structure of formic acid on page 4. Box your final answer.

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter12: Chemical Bonding

Section: Chapter Questions

Problem 8CR

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Similar questions

Given the following data: NO2(g) NO(g) + O(g)H = 233 kJ 2O3(g) 3O2(g)H = 427 kJ NO(g) + O3(g) NO2(g) + O2(g)H = 199 kJ Calculate the bond energy for the O2 bond, that is, calculate H for: O2(g) 2O(g)H = ?
The standard enthalpies of formation for S(g), F(g), SF4(g), and SF6(g) are +278.8, +79.0, 775, and +1209 KJ/mol, respectively. a. Use these data to estimate the energy of an SF bond. b. Compare your calculated value to the value given in Table 3-3. What conclusions can you draw? c. Why are the Hf values for S(g) and F(g) not equal to zero, since sulfur and fluorine are elements?
Explain the decomposition of nitroglycerin in terms of relative bond enthalpies.
hat is the enthalpy change for a process? Is enthalpy a state function? In what experimental apparatus are enthalpy changes measured?
Estimate H for the following reactions using bond energies given in Table 8.5. 3CH2=CH2(g) + 3H2(g) 3CH2CH3(g) The enthalpies of formation for C6H6(g) and C6H12 (g) are 82.9 and 90.3 kJ/mol. respectively. Calculate H for the two reactions using standard enthalpies of formation from Appendix 4. Account for any differences between the results obtained from the two methods.
Calculate the enthalpy of reaction for HCN(g)H(g)+C(g)+N(g) from enthalpies of formation (see Appendix C). Given that the CH bond enthalpy is 411 kJ/mol, obtain a value for the CN bond enthalpy. Compare your result with the value given in Table 9.5.
When a reaction is exothermic, is the sum of bond energies of products or of reactants greater?
Using the bond dissociation enthalpies in Table 8.8, estimate the enthalpy of combustion of gaseous methane, CH4, to give water vapor and carbon dioxide gas.
Estimate ΔrH° for forming 2 mol ammonia from molecular nitrogen and molecular hydrogen. Is this reaction exothermic or endothermic?
Although nitrogen trifluoride (NF3) is a thermally stable compound, nitrogen triiodide (NI3) is known to be a highly explosive material. NI3 can be synthesized according to the equation BN(s) + 3IF(g) BF3(g) + NI3(g) a. What is the enthalpy of formation for NI3(s) given the enthalpy of reaction (307 kJ) and the enthalpies of formation for BN(s) (254 kJ/mol), IF(g) (96 kJ/mol), and BF3(g) (1136 kJ/mol)? b. It is reported that when the synthesis of NI3 is conducted using 4 moles of IF for every 1 mole of BN, one of the by-products isolated is [IF2]+[BF4]. What are the molecular geometries of the species in this by-product? What are the hybridizations of the central atoms in each species in the by-product?
When boron hydrides burn in air, the reactions are very exothermic (a) Write a balanced equation for the combustion of B5H9(g) in air to give B2O3(s) and H2O(g). (b) Calculate the enthalpy of combustion for B5H9(g) (fH = 73.2 kJ/mol), and compare it with the enthalpy of combustion of B2H6 (2038 kJ/mol). (The enthalpy of formation of B2O3(s) is 1271.9 kJ/mol.) (c) Compare the enthalpy of combustion of C2H6(g) with that of B2H6(g). Which transfers more energy as heat per gram?
Compare your answers from parts a and b of Exercise 69 of Chapter 3 with H values calculated for each reaction using standard enthalpies of formation in Appendix 4. Do enthalpy changes calculated from bond energies give a reasonable estimate of the actual values?