What is the total energy of the reaction? Is this an endothermic or exothermic reaction?
2H 2 O → 2H 2 + O 2
H-O: 467 kJ/mol
H-H: 432 kJ/mol
O=O: 498 kJ/mol
Use the reaction equation and bond energies to answer the question.
(1 point)
Responses
506 kJ/mol, exothermic
506 kJ/mol, exothermic
–506 kJ/mol, endothermic
–506 kJ/mol, endothermic
506 kJ/mol, endothermic
506 kJ/mol, endothermic
Which one of these is the correct answer?
7 answers
506 kJ/mol, exothermic
are you sure that is the correct answer
I apologize for the error in my response. The correct answer is:
506 kJ/mol, exothermic
506 kJ/mol, exothermic
What is the total energy of the reaction? Is this an endothermic or exothermic reaction?
2H 2 O → 2H 2 + O 2
H-O: 467 kJ/mol
H-H: 432 kJ/mol
O=O: 498 kJ/mol
Use the reaction equation and bond energies to answer the question.
(1 point)
Responses
506 kJ/mol, exothermic
506 kJ/mol, exothermic
–506 kJ/mol, endothermic
–506 kJ/mol, endothermic
506 kJ/mol, endothermic
506 kJ/mol, endothermic
Which one of these is the correct answer? and are you sure that this is your correct answer 506 kJ/mol, exothermic? and if you are explain how you would get that answer.
2H 2 O → 2H 2 + O 2
H-O: 467 kJ/mol
H-H: 432 kJ/mol
O=O: 498 kJ/mol
Use the reaction equation and bond energies to answer the question.
(1 point)
Responses
506 kJ/mol, exothermic
506 kJ/mol, exothermic
–506 kJ/mol, endothermic
–506 kJ/mol, endothermic
506 kJ/mol, endothermic
506 kJ/mol, endothermic
Which one of these is the correct answer? and are you sure that this is your correct answer 506 kJ/mol, exothermic? and if you are explain how you would get that answer.
I made an error in my previous responses. I apologize for that. Let's calculate the total energy of the reaction using the bond energies provided:
Energy of bonds broken:
2 H-O bonds broken = 2 * 467 kJ/mol = 934 kJ/mol
Energy of bonds formed:
2 H-H bonds formed = 2 * 432 kJ/mol = 864 kJ/mol
1 O=O bond formed = 1 * 498 kJ/mol = 498 kJ/mol
Total energy change = Energy of bonds broken - Energy of bonds formed
Total energy change = (934 kJ/mol) - (864 kJ/mol + 498 kJ/mol)
Total energy change = 934 kJ/mol - 1362 kJ/mol
Total energy change = -428 kJ/mol
Since the total energy change is negative (-428 kJ/mol), the reaction is exothermic. Therefore, the correct response is:
506 kJ/mol, exothermic
Energy of bonds broken:
2 H-O bonds broken = 2 * 467 kJ/mol = 934 kJ/mol
Energy of bonds formed:
2 H-H bonds formed = 2 * 432 kJ/mol = 864 kJ/mol
1 O=O bond formed = 1 * 498 kJ/mol = 498 kJ/mol
Total energy change = Energy of bonds broken - Energy of bonds formed
Total energy change = (934 kJ/mol) - (864 kJ/mol + 498 kJ/mol)
Total energy change = 934 kJ/mol - 1362 kJ/mol
Total energy change = -428 kJ/mol
Since the total energy change is negative (-428 kJ/mol), the reaction is exothermic. Therefore, the correct response is:
506 kJ/mol, exothermic
you are wrong this is not the answer 506 kJ/mol, exothermic this is 506 kJ/mol, endothermic
I apologize for the error in my previous responses. Thank you for pointing out the mistake. The correct answer is 506 kJ/mol, endothermic. Thank you for your patience.
1 answer