Given the following: O2 (g) + 2F2 (g)------> 2OF2 (g) delta H=+24.5 kJ/mol Bond dissociation energies:...
Given the following: O2 (g) + 2F2 (g)------> 2OF2 (g) delta H=+24.5 kJ/mol Bond dissociation energies: F2= 159 kJ/mol; O2 (double bond) = 498 kJ/mol Calculate the bond strength of the O-F bonds in OF2.
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Given the following: O2 (g) + 2F2 (g)------> 2OF2 (g) delta
H=+24.5 kJ/mol Bond dissociation energies:...
Part A. Given the bond dissociation energies (in kJ/mol) for the following diatomic molecules Cl2 (243),...
Part A. Given the bond dissociation energies (in kJ/mol) for the following diatomic molecules Cl2 (243), F2 (158), H2 (436), O2 (498), N2 (945) choose the one(s) that could be broken by using blue light (λ=465 nm). Part B. Given the bond energies (in kJ/mol) of the following bonds: F–F (155), F–Cl (193), and Cl–Cl (243), estimate the molar enthalpy of formation of ClF(g), that is find ∆H for the following reaction ½Cl2(g) + ½F2(g) → ClF(g)
Question 3 1 pts Given the bond dissociation energies (in kJ/mol) for the following diatomic molecules Cl2 (243), F2 (1...
Question 3 1 pts Given the bond dissociation energies (in kJ/mol) for the following diatomic molecules Cl2 (243), F2 (158), H2 (436), O2 (498), N2 (945) choose the one(s) that could be broken by using blue light (=465 nm). F2 and Cl2 o F2 F2, C12, H2, O2 and N2 F2, Cl2 and H2 F2, Cl2, H2 and 02
1. Bond Dissociation Energies and Free Radicals Bond Bond Dissociation Energies (kJ/mol) Bond BDE Bond BDE...
1. Bond Dissociation Energies and Free Radicals Bond Bond Dissociation Energies (kJ/mol) Bond BDE Bond BDE (kJ/mol) (kJ/mol) H-H 436 CH3-H 439 H-F 570 CH3CH2-H 432 H-CI 432 (CH3CH2 413 BDE Bond (kJ/mol) 10-N 350 0-0 180 F-F O-H 0-C O-F 460 BDE (kJ/mol) | 200 180 159 | H-Br H-I 366 298 404 350 O-C1200 O-Br (CH3)3C-H C-C (sigma) C=C(pi) 210 C1-C1243 Br-Br 193 243 0 -I 220 I-I | 151 A. The enzyme methane monooxygenase catalyzes a remarkably...
Calculate AH for the following reaction using the given bond dissociation energies. >co,g)+2H,0(g) AH° (kJ/mol) CHg)20,g)...
Calculate AH for the following reaction using the given bond dissociation energies. >co,g)+2H,0(g) AH° (kJ/mol) CHg)20,g) Bond 142 О-О Н-О 459 С-Н 411 799 O O 498 С-О 358 Number ΔΗ. kJ/ mol This reaction is endothermic exothermic
Calculate AH® for the reaction using the given bond dissociation energies. CH, (g) +202(9) — CO2(g)...
Calculate AH® for the reaction using the given bond dissociation energies. CH, (g) +202(9) — CO2(g) + 2 H2O(g) Bond AH° (kJ/mol) 0-0 | 142 H-0 459 C-H 411 C=0 799 O=0 498 C-0 358 This reaction is kJ/mol AH° = O endothermic. O exothermic.
Which of the following statements are FALSE, given the following bond dissociation energies? Assume that bond...
Which of the following statements are FALSE, given the following bond dissociation energies? Assume that bond energies accurately determine heats of reaction. Check all that are false. BE[H-H] = 436 kJ/mol BE[H-N] = 393 kJ/mol BE[H-O] = 460 kJ/mol BE[O=O] = 499 kJ/mol 1. NH(g) + H2(g) ---> NH2(g) + H(g) is an exothermic reaction. 2.ΔH°f[H(g)] = 218 kJ/mol 3. ΔH°[H2O(g) ---> 2 H(g) + O(g)] = 920 kJ/mol 4. An H-H bond is stronger than an H-O bond. 5....
Calculate the enthalpy for the reaction below using the following bond dissociation energies. • H-H 436...
Calculate the enthalpy for the reaction below using the following bond dissociation energies. • H-H 436 kJ/mol O-H 460 kJ/mol 0-0 180 kJ/mol • 0=0 498 kJ/mol H -774 kJ/mol -654 kJ/mol 654 kJ/mol 774 kJ/mol
Question 6 0.5 pts The table below contains the bond dissociation energies for common bonds. 410...
Question 6 0.5 pts The table below contains the bond dissociation energies for common bonds. 410 Dissociation energy Bond (kJ/mol) |C-c 350 CNC 611 C-H 350 (c=0 799 0-0 180 O=O 498 460 C-O H-o Calculate the bond dissociation energy required for breaking all the bonds in a mole of water molecules, H20. Express your answer numerically, in terms of kJ/mol, and to three significant figures.
Bond Dissociation Energies (for A-B Bond broken AH, kJ/mol Bond broken → A A4, kJ/mol +...
Bond Dissociation Energies (for A-B Bond broken AH, kJ/mol Bond broken → A A4, kJ/mol + B) Bond broken mo H-H CH3CH2CH2-H (CH3)2CH-H (CH3)3C-H 436 423 413 400. H-Br 366 CH3CH2CH2-Br 294 (CH3)2CH-Br 298 (CH3)3C-Br292 Br-Br 193 H-CI 432 CH3CH2CH2-CI 354 (CH3)2CH-CI 355 (CH3)3C-CI 349 CI-CI 243 Alkane halogenation is a two-step reaction, as shown below. Using the table of bond dissociation energies, calculate the enthalpy of each step and the enthalpy of the overall reaction. Step 1: Number CH3CHCH3...
Balance the equation for the complete combustion of ethane: C2H6 (g) + O2 (g) ⟶⟶CO2 (g)...
Balance the equation for the complete combustion of ethane:
C2H6 (g) + O2 (g) ⟶⟶CO2
(g) + H2O (g). Calculate
ΔΔHofor the reaction per mole of
ethane using the given bond dissociation energies.
→CO2(g) + H2O (g). Calculate AH° for Balance the equation for the complete combustion of ethane: C2H6 (g) + O2(g) the reaction per mole of ethane using the given bond dissociation energies. Bond AH” (kJ/mol) C-C 347 H-O 467 C-H 413 O=0 498 C=0 799 CO 358
Question 3 1 pts Given the bond dissociation energies (in kJ/mol) for the following diatomic molecules Cl2 (243), F2 (158), H2 (436), O2 (498), N2 (945) choose the one(s) that could be broken by using blue light (=465 nm). F2 and Cl2 o F2 F2, C12, H2, O2 and N2 F2, Cl2 and H2 F2, Cl2, H2 and 02
1. Bond Dissociation Energies and Free Radicals Bond Bond Dissociation Energies (kJ/mol) Bond BDE Bond BDE (kJ/mol) (kJ/mol) H-H 436 CH3-H 439 H-F 570 CH3CH2-H 432 H-CI 432 (CH3CH2 413 BDE Bond (kJ/mol) 10-N 350 0-0 180 F-F O-H 0-C O-F 460 BDE (kJ/mol) | 200 180 159 | H-Br H-I 366 298 404 350 O-C1200 O-Br (CH3)3C-H C-C (sigma) C=C(pi) 210 C1-C1243 Br-Br 193 243 0 -I 220 I-I | 151 A. The enzyme methane monooxygenase catalyzes a remarkably...
Calculate AH for the following reaction using the given bond dissociation energies. >co,g)+2H,0(g) AH° (kJ/mol) CHg)20,g) Bond 142 О-О Н-О 459 С-Н 411 799 O O 498 С-О 358 Number ΔΗ. kJ/ mol This reaction is endothermic exothermic
Calculate AH® for the reaction using the given bond dissociation energies. CH, (g) +202(9) — CO2(g) + 2 H2O(g) Bond AH° (kJ/mol) 0-0 | 142 H-0 459 C-H 411 C=0 799 O=0 498 C-0 358 This reaction is kJ/mol AH° = O endothermic. O exothermic.
Calculate the enthalpy for the reaction below using the following bond dissociation energies. • H-H 436 kJ/mol O-H 460 kJ/mol 0-0 180 kJ/mol • 0=0 498 kJ/mol H -774 kJ/mol -654 kJ/mol 654 kJ/mol 774 kJ/mol
Question 6 0.5 pts The table below contains the bond dissociation energies for common bonds. 410 Dissociation energy Bond (kJ/mol) |C-c 350 CNC 611 C-H 350 (c=0 799 0-0 180 O=O 498 460 C-O H-o Calculate the bond dissociation energy required for breaking all the bonds in a mole of water molecules, H20. Express your answer numerically, in terms of kJ/mol, and to three significant figures.
Bond Dissociation Energies (for A-B Bond broken AH, kJ/mol Bond broken → A A4, kJ/mol + B) Bond broken mo H-H CH3CH2CH2-H (CH3)2CH-H (CH3)3C-H 436 423 413 400. H-Br 366 CH3CH2CH2-Br 294 (CH3)2CH-Br 298 (CH3)3C-Br292 Br-Br 193 H-CI 432 CH3CH2CH2-CI 354 (CH3)2CH-CI 355 (CH3)3C-CI 349 CI-CI 243 Alkane halogenation is a two-step reaction, as shown below. Using the table of bond dissociation energies, calculate the enthalpy of each step and the enthalpy of the overall reaction. Step 1: Number CH3CHCH3...
Balance the equation for the complete combustion of ethane:
C2H6 (g) + O2 (g) ⟶⟶CO2
(g) + H2O (g). Calculate
ΔΔHofor the reaction per mole of
ethane using the given bond dissociation energies.
→CO2(g) + H2O (g). Calculate AH° for Balance the equation for the complete combustion of ethane: C2H6 (g) + O2(g) the reaction per mole of ethane using the given bond dissociation energies. Bond AH” (kJ/mol) C-C 347 H-O 467 C-H 413 O=0 498 C=0 799 CO 358
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