Part A) Use bond enthalpies from the table below to determine whether CH4(g), CH3OH(g), H2CO(g), or HCOOH(g) produces the most energy per gram when burned completely in O2(g) to give CO2(g) and H2O(g).

a. CH4(g)

b. CH3OH(g)

c. HCOOH(g)

d. H2CO(g)

e. none of these

Part B) Describe the relationship between the oxidation state of carbon and the heat of combustion (in kJkg1kJkg1 or kJmol1kJmol1)?

The more the oxidation state of the carbon, the energy that is generated per gram of that material.

options: negative, positive, less, more

TABLE 10.3 Some Average Bond Energiesa Bond Energy, Bond Energy, Bond Energy Bond kJ mol-1 Bond kJ mol-1 Bond kJ mol-1 H-H 436 C-C 347 N-N 163 H-C 414 C=C 611 N=N 418 H-N 389 C=C 837 N=N 946 H-O 464 C-N 305 N-O 222 H-S 368 CEN 615 N=0 590 H-F 565 CON 891 0-0 142 H-CI 431 C-0 360 O=O 498 H- Br 364 CEO 736b F-F 159 H-1 297 C-Cl 339 C1-C1 243 Br-Br 193 I-I 151 a Although all data are listed with about the same precision (three significant figures), some values are actually known more precisely. Specifically, the values for the diatomic mole- cules H2, HF, HC, HBr, HI, N2 (N=N), 02 (O=O), F2, Cl, Bry, and I are actually bond-dissociation energies, rather than average bond energies. bThe value for the C=O bonds in CO2 is 799 kJ moll