Part A Consider the hypothetical reaction between two diatomic molecules in the gas phase: X-X(g)+Y–Y(g)→ 2X–Y(g) Based on the bond enthalpies in the table shown, how many of the following combinations of X and Y are predicted to lead to exothermic reactions? (i) X = H, Y = F; (ii) X = H, Y = Br; (ii)X = F, Y = Cl; (iv) X = CI, Y = 1.

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Chapter1: Chemical Foundations
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Average Bond Enthalpies (kJ/mol)
Part A
C-H 413 N-H 391 0-H 463 F-F 155
C-C 348 N-N
C=C 614 N-O 201 O=0
163 0-0 146
Consider the hypothetical reaction between two diatomic molecules in the gas phase:
495 Cl-F 253
C-N 293 N-F 272 0-F 190 Cl-CI 242
X-X(g)+ Y-Y(g)→ 2X-Y(g)
C-0 358 N-Cl 200 0-Cl 203 Br-F 237
C=0 799 N-Br 243 0-I
Based on the bond enthalpies in the table shown, how many of the following combinations of X and Y are
predicted to lead to exothermic reactions? (i) X = H, Y = F; (ii) X = H, Y = Br; (iii) X = F, Y = Cl; (iv) X = CI,
Y = .
234 Br-Cl 218
С -F 485 | Н-Н 436
C-Cl 328 H–F
Br-Br 193
567
C-Br 276 H-CI 431
I-C 208
240 H-Br 366
H-I 299
C-I
I-Br 175
O 1
I-I
151
O 2
combinations will lead to an exothermic reaction.
O 3
O 4
Transcribed Image Text:Average Bond Enthalpies (kJ/mol) Part A C-H 413 N-H 391 0-H 463 F-F 155 C-C 348 N-N C=C 614 N-O 201 O=0 163 0-0 146 Consider the hypothetical reaction between two diatomic molecules in the gas phase: 495 Cl-F 253 C-N 293 N-F 272 0-F 190 Cl-CI 242 X-X(g)+ Y-Y(g)→ 2X-Y(g) C-0 358 N-Cl 200 0-Cl 203 Br-F 237 C=0 799 N-Br 243 0-I Based on the bond enthalpies in the table shown, how many of the following combinations of X and Y are predicted to lead to exothermic reactions? (i) X = H, Y = F; (ii) X = H, Y = Br; (iii) X = F, Y = Cl; (iv) X = CI, Y = . 234 Br-Cl 218 С -F 485 | Н-Н 436 C-Cl 328 H–F Br-Br 193 567 C-Br 276 H-CI 431 I-C 208 240 H-Br 366 H-I 299 C-I I-Br 175 O 1 I-I 151 O 2 combinations will lead to an exothermic reaction. O 3 O 4
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