Bond H-H* H-N H-O H-S H-P H-F H-Cl H-Br H-I C-H C-C C=C C=C C-N C=N C=N C-0 C=0¹ C=0 C-P C-S C=S C-F C-CI C-Br C-I Bond enthalpy (kJ/mol) 436.4 393 460 368 326 568.2 431.9 366.1 298.3 414 347 620 812 276 615 891 351 745 1070 263 255 477 453 339 276 216 "Bond enthalpies shown in red are for diatomic molecules. The CO bond enthalpy in CO₂ is 799 kJ/mol. Bond N-N N=N N=N N-O N=0 N-F N-CI N-Bri N-I 0-0 0=0 O-P O=S 0-F O-CI 0-Br 0-1 P-P P=P S-S S=S F-F CI-CI CI-F Br-Br 1-I a) Give your answer here. work. Bond enthalpy (kJ/mol) 193 418 941.4 176 607 272 Use bond enthalpies to calculate the enthalpy of the reaction given below, in kJ per mole N₂O4. 2N2O4 (g) + N₂H4 (g) 6NO (g) + 2H₂O (g) Be sure to draw the best Lewis structure. 200 243 159 142 498.7 502 469 190 203 234 234 197 489 268 352 156.9 242.7 193 192.5 151.0 You must draw Lewis structures, show detailed work, and give your answer with the correct units and significant figures. b) Is the reaction exothermic or endothermic? , and you will be asked to upload your
Bond H-H* H-N H-O H-S H-P H-F H-Cl H-Br H-I C-H C-C C=C C=C C-N C=N C=N C-0 C=0¹ C=0 C-P C-S C=S C-F C-CI C-Br C-I Bond enthalpy (kJ/mol) 436.4 393 460 368 326 568.2 431.9 366.1 298.3 414 347 620 812 276 615 891 351 745 1070 263 255 477 453 339 276 216 "Bond enthalpies shown in red are for diatomic molecules. The CO bond enthalpy in CO₂ is 799 kJ/mol. Bond N-N N=N N=N N-O N=0 N-F N-CI N-Bri N-I 0-0 0=0 O-P O=S 0-F O-CI 0-Br 0-1 P-P P=P S-S S=S F-F CI-CI CI-F Br-Br 1-I a) Give your answer here. work. Bond enthalpy (kJ/mol) 193 418 941.4 176 607 272 Use bond enthalpies to calculate the enthalpy of the reaction given below, in kJ per mole N₂O4. 2N2O4 (g) + N₂H4 (g) 6NO (g) + 2H₂O (g) Be sure to draw the best Lewis structure. 200 243 159 142 498.7 502 469 190 203 234 234 197 489 268 352 156.9 242.7 193 192.5 151.0 You must draw Lewis structures, show detailed work, and give your answer with the correct units and significant figures. b) Is the reaction exothermic or endothermic? , and you will be asked to upload your
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Types of Chemical Bonds
The attractive force which has the ability of holding various constituent elements like atoms, ions, molecules, etc. together in different chemical species is termed as a chemical bond. Chemical compounds are dependent on the strength of chemical bonds between its constituents. Stronger the chemical bond, more will be the stability in the chemical compounds. Hence, it can be said that bonding defines the stability of chemical compounds.
Polarizability In Organic Chemistry
Polarizability refers to the ability of an atom/molecule to distort the electron cloud of neighboring species towards itself and the process of distortion of electron cloud is known as polarization.
Coordinate Covalent Bonds
A coordinate covalent bond is also known as a dative bond, which is a type of covalent bond. It is formed between two atoms, where the two electrons required to form the bond come from the same atom resulting in a semi-polar bond. The study of coordinate covalent bond or dative bond is important to know about the special type of bonding that leads to different properties. Since covalent compounds are non-polar whereas coordinate bonds results always in polar compounds due to charge separation.
Question
I need help calculating the enthalpy of the reaction and whether the reaction is endothermic or exothermic.
Transcribed Image Text:TABLE 10.4 Bond Enthalpies
Bond enthalpy (kJ/mol)
436.4
393
460
368
326
568.2
431.9
366.1
298.3
414
347
620
812
Bond
H-H*
H-N
H-O
H-S
H-P
H-F
Copygma-cocation. Prignits reserved. No reproducono
distribution without the prior written consent of McGraw-Hill Education.
H-CI
H-Br
H-I
C-H
C-C
C=C
C=C
C-N
C=N
C=N
C-0
C=0*
C=0
C-P
C-S
C=S
C-F
C-CI
C-Br
C-I
*Bond enthalpies shown in red are for diatomic molecules.
'The C=0 bond enthalpy in CO₂ is 799 kJ/mol.
276
615
891
351
745
1070
263
255
477
453
339
276
216
work.
Bond
a) Give your answer here
N-N
N=N
N=N
N-O
N=0
N-F
N-CI
N-Br
N-I
0-0
0=0
O-P
O=S
O-F
O-CI
0-Br
0-1
P-P
P=P
S-S
S=S
F-F
CI-CI
CI-F
Br-Br
I-I
Bond enthalpy (kJ/mol)
193
418
941.4
176
607
272
200
243
159
142
498.7
502
469
190
203
234
Use bond enthalpies to calculate the enthalpy of the reaction given below, in kJ per mole
N₂O4.
2N₂O4 (g) + N₂H4 (g) →6NO (g) + 2H₂O (g)
Be sure to draw the best Lewis structure.
b) Is the reaction exothermic or endothermic?
234
197
489
268
352
You must draw Lewis structures, show detailed work, and give your answer with the correct.
units and significant figures.
156.9
242.7
193
192.5
151.0
, and you will be asked to upload your
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