This problem explores the vibrational and rotational energy levels of the hydrogen halides. Experimental data are given below. Hydrogen halides kf (kg/s²) R (pm) HF 970.0 91.7 HCI 480.0 127.5 HBr 410.0 141.4 HI 320.0 160.9 For one mole of each HF, determine the following quantities. AE10 = 8.29 x10-20 J b. The number of vibrational energy levels occupied at 300 K j = 2 levels c. The spacing between the two lowest rotational energy levels –32 7.73 x10° ΔΕ10 - J Incorrect d. The number of rotational energy levels occupied at 300 K j = levels

ThermoDynamic Data C2H5OH = delta H = -278 KJ/mol, delta G = -175 KJ/mol, S = 161 J/K mol 3O2 = delta H = 0 KJ/mol, 3(0 KJ/mol), S = 205.152 J/K mol 2Co2 = delta H = -393.5 KJ/mol, 2(-394 KJ/mol), S = 214 J/K mol 3H2O = delta H = -242 KJ/mol, 3(-229 KJ/mol), S = 189 J/K mol

Use the table below to determine ΔH for the following reactionN 2H 4(g) + H 2O(g) ↔ NH 2OH(g) + NH 3(g) Bond Energies, kJ/mol Single Bonds   H C N O S F Cl Br I H 432                 C 411 346               N 386 305 167             O 459 358 201 142           S 363 272 --- --- 286         F 565 485 283 190 284 155       Cl 428 327 313 218 255 249 240     Br 362 285 243 201 217 249 216 190   I 295 213 --- 201 --- 278 208 175 149 Multiple Bonds C=C 602 C=N 615 C=O 799 C≡C 835 C≡N 887 C≡O 1072 N=N 418 N=O 607 S=O (in SO2) 532 N≡N 942 O2 494 S=O (in SO3) 469

predict ΔrH for the following reaction in kj/mol HCΞCH  +  2 H2  →  H3C-CH3