Problem 5.88 Review 1 Constants Periodic Table Consider the reaction: Ha(&) +I2(s)-2HI(g) Ub st E...
Constants Periodic Table Consider the reaction: H2(g) +12(s) + 2HI(g) Average Bond Enthalpies (kJ/mol) Part A Use the bond enthalpies in the table to estimate AH for this reaction, ignoring the fact that iodine is in the solid state. Express your answer in kilojoules to two significant figures. IVO AQ R o 21 ? C-H 413 N-H 391 0-H 463 F-F 155 C-C 348 N-N 163 0-0 146 C=C 614 N-O 201 0=0 495 Cl-F 253 C-N 293 N-F 272...
Need help on part C!
Without doing a calculation, predict whether your estimase in Part A is more negative or less negative than the true reaction enthalpy Consider the reaction: B(R) + 1:(s)2HI(R) o The actual enthalpy change for the reactants as wniten wil be more exothermie (more negative. smaler) han the value we essma n Part A Average Bond Enthalpies (k.Jimol o The actual enthalpy chamge fer the reactants as witen wi be mone endothermi (more negative. smaerj than...
Problem 5.83
Use bond enthalpies in the table below to estimate ?H
for each of the following reactions.
Problem 5.83 Part A Use bond enthalpies in the table below to estimate ? 1 for each of the following reactions H-H(g) + Br-Br(g) ? 2H-Br(g) Express your answer in kilojoules to 3 significant figures Average Bond Enthalpies (kJ/mol) 103 kJ C-H 413 N-H 391 O-H 463 F-F 155 C-C 348 N-N 163 O-O 146 C-C 614 N-O 201 O O 495...
Problem 5.84
Use bond enthalpies in the table below to estimate ΔH
for each of the following reactions
.
Average Bond Enthalpies
(kJ/mol)
C−H413
N−H391
O−H463
F−F155
C−C348
N−N163
O−O146
C=C614
N−O201
O=O495
Cl−F253
C−N293
N−F272
O−F190
Cl−Cl242
C−O358
N−Cl200
O−Cl203
Br−F237
C=O799
N−Br243
O−I234
Br−Cl218
C−F485
H−H436
Br−Br193
C−Cl328
H−F567
C−Br276
H−Cl431
I−Cl208
C−I240
H−Br366
I−Br175
H−I299
I−I151
Part A
Express your answer in kilojoules to 3 significant figures.
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Part B
Express your answer in kilojoules...
Use the bond enthalpies in the table below to determine the enthalpy of reaction in the following questions: Average Bond-Enthalpies- (kJ/mol) Single Bonds -H 41 3 348 293 358 485 N- 391 -H 463 -O 146 F-F 155 N-N 163 N-O 201 272 N-CI 200 N-Br 243 CI-P 253 N-I CI-CI 242 O-CI 203 -I 234 C-C Br-p 237 B-CI 218 Br-Br 193 339 327 S-Cl 253 S-Br 218 S-H 240 259 -X-H 436 567 431 366 299 208 175...
2CH4(g)→C2H6(g)+H2(g)
C2H6(g)+Cl2(g)→C2H5Cl(g)+HCl(g)
N2(g)+3H2(g)→2NH3(g)
Express your answer as a whole number and include the
appropriate units.
ΔHrxn∘=
Use the average bond dissociation energies in the table given below to calculate approximate reaction enthalpies in kilojoules for the following processes: TABLE. Average Bond Dissociation Energies, D (kJ/mol) Н - н 436а | С — н |410 N— H 390| О — F I-I 151a 180 Н- С |410 C 350 N- C |300|O C Cl S - F 200 310 H -F...
Part B?
Review | Constants Periodic Table H2NH3 Consider the following reaction: 2NH3(g) = N2(g) + 3H2(g) Submit Previous Answers Correct The equilibrium constant is equal to the concentrations of the products divided by the concentrations of the reactants. The concentrations of both the reactants and the products are raised to a power of the respective coefficient from the balanced chemical reaction. K.= [N] [H] [NH3] Part B What is the numerical value of Kc for the reaction if the...
Using Table 9.4, calculate an approximate enthalpy (in kJ) for
the reaction of 1.10 g gaseous methanol (CH3OH) in excess molecular
oxygen to form gaseous carbon dioxide and gaseous water. (Hint,
remember to first write the balanced equation.)
TABLE 9.4 Bond Energies (kJ/mol)* Single Bonds C-H 414 C-C 348 C-N 293 C-O 351 C-F 439 C-CI 328 C-Br 276 C-1 238 C-S 259 N-H 889O H 463 FF 159 N-N 163OO 146 C F 253 N-O 201O-F 190 CCI 242...
< Chapter 8 HW Problem 8.70 - Enhanced - with Feedback < 12 of 15 > Using bond enthalpies in the table, estimate Al for the following gas-phase reactions. un Review | Constants Periodic Table Part A Estimate AH for the reaction. Br-c-H+CI-C1B -C-CI+H-CI 463 146 190 203 234 Express your answer using three significant figures. IVO AL O 2 ? Average Bond Enthalpies (kJ/mol) Single Bonds C-H 413 N-H 391 0-H C-C 348 N-N 163 0-0 C-N 293 N-...
< 9 of 13 Review Constants Periodic Table Part A A calorimeter contains 28.0 mL of water at 11.0 °C. When 250 g of X (a substance with a molar mass of 60.0 g/mol) is added, it dissolves via the reaction X(s) + H2O(1) X(aq) and the temperature of the solution increases to 30.0 °C. Calculate the enthalpy change, AH, for this reaction per mole of X. Assume that the specific heat of the resulting solution is equal to that...