Use the reaction and bond information to answer the question.
C2H6 → C2H4 + H2
Reactant bond energies: H–C = 413 kJ/mol, C–C single bond = 347 kJ/mol
Product bond energies: H–C = 413 kJ/mol, C=C double bond = 614 kJ/mol, H–H = 432 kJ/mol
Based on the bond energies, is this reaction endothermic or exothermic? Why or why not?
A) This reaction is exothermic, because stronger bonds are broken than formed.
B) The reaction is endothermic, because stronger bonds are broken than formed.
C) The reaction is exothermic, because stronger bonds are formed than broken.
D) The reaction is endothermic, because stronger bonds are formed than broken.
9 answers
The reaction is endothermic, because stronger bonds are broken than formed.
1
In order to break a bond, energy must be... (absorbed)
2
H2 + O2 → H2O2
H–H + O=O → H–O–O–H
The energy of the H–H bond is 432 kJ/mol. The energy of the O=O bond is 495 kJ/mol. The energy of the O–H bond is 467 kJ/mol. The energy of the O–O bond is 146 kJ/mol.
Which bond is the strongest? (O=O)
3
H2 + CO2 → CH2O2
Reactant bond energies: H–H is 432 kJ/mol, C=O is 799 kJ/mol
Product bond energies: C–H is 413 kJ/mol, C=O is 745 kJ/mol, C–O is 358 kJ/mol, O–H is 467 kJ/mol
How much energy must this system absorb before the reaction can begin? (2,030 kJ)
4
C2H2 + 3H2 → 2CH4
Reactant bond energies: H–C = 413 kJ/mol, C–C triple bond = 839 kJ/mol, H–H = 432 kJ/mol
Product bond energies: H–C = 413 kJ/mol
Based on the bond energies, would this reaction occur without the addition of energy? Why or why not? (Yes, it would occur without additional energy because the reaction is exothermic.)
5
C2H6 → C2H4 + H2
Reactant bond energies: H–C = 413 kJ/mol, C–C single bond = 347 kJ/mol
Product bond energies: H–C = 413 kJ/mol, C=C double bond = 614 kJ/mol, H–H = 432 kJ/mol
Based on the bond energies, is this reaction endothermic or exothermic? Why or why not? (The reaction is endothermic, because stronger bonds are broken than formed.)
100%
No one
In order to break a bond, energy must be... (absorbed)
2
H2 + O2 → H2O2
H–H + O=O → H–O–O–H
The energy of the H–H bond is 432 kJ/mol. The energy of the O=O bond is 495 kJ/mol. The energy of the O–H bond is 467 kJ/mol. The energy of the O–O bond is 146 kJ/mol.
Which bond is the strongest? (O=O)
3
H2 + CO2 → CH2O2
Reactant bond energies: H–H is 432 kJ/mol, C=O is 799 kJ/mol
Product bond energies: C–H is 413 kJ/mol, C=O is 745 kJ/mol, C–O is 358 kJ/mol, O–H is 467 kJ/mol
How much energy must this system absorb before the reaction can begin? (2,030 kJ)
4
C2H2 + 3H2 → 2CH4
Reactant bond energies: H–C = 413 kJ/mol, C–C triple bond = 839 kJ/mol, H–H = 432 kJ/mol
Product bond energies: H–C = 413 kJ/mol
Based on the bond energies, would this reaction occur without the addition of energy? Why or why not? (Yes, it would occur without additional energy because the reaction is exothermic.)
5
C2H6 → C2H4 + H2
Reactant bond energies: H–C = 413 kJ/mol, C–C single bond = 347 kJ/mol
Product bond energies: H–C = 413 kJ/mol, C=C double bond = 614 kJ/mol, H–H = 432 kJ/mol
Based on the bond energies, is this reaction endothermic or exothermic? Why or why not? (The reaction is endothermic, because stronger bonds are broken than formed.)
100%
No one
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