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.
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%
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The reaction is endothermic, because stronger bonds are broken than formed.
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To determine whether the reaction is endothermic or exothermic based on the bond energies, we need to compare the amount of energy required to break the bonds in the reactants with the amount of energy released when new bonds are formed in the products.
In the given reaction, the reactant C2H6 (ethane) is converted into C2H4 (ethylene) and H2 (hydrogen).
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
To find the total energy change in the reaction, we need to subtract the energy needed to break the bonds in the reactants from the energy released when new bonds are formed in the products.
Reactant energy = 413 kJ/mol (H–C) + 347 kJ/mol (C–C single bond) = 760 kJ/mol
Product energy = 413 kJ/mol (H–C) + 614 kJ/mol (C=C double bond) + 432 kJ/mol (H–H) = 1459 kJ/mol
Energy change = Product energy - Reactant energy
Energy change = 1459 kJ/mol - 760 kJ/mol = 699 kJ/mol
The energy change in the reaction is positive (699 kJ/mol), indicating that the reaction requires an input of energy. This means the reaction is endothermic because it absorbs energy from the surroundings.
Therefore, the correct answer is:
B) The reaction is endothermic, because stronger bonds are broken than formed.