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Question
Use the reaction and bond information to answer the question.

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

Triple bonds are hard to break and require a lot of energy. The reaction would likely not occur without adding energy to the system if it took more energy to break the bonds than would be produced. Based on the bond energies, would this reaction occur without the addition of energy? Why or why not?

No, it would not occur without additional energy because the reaction is exothermic.

No, it would not occur without additional energy because the reaction is endothermic.

Yes, it would occur without additional energy because the reaction is exothermic.

Yes, it would occur without additional energy because the reaction is endothermic.

Respuesta :

ANswer:-

Yes, it would occur without additional energy because the reaction is exothermic.

Explanation :-

Find Hydrogen enthalpies of both sides

Reactant=413+839+432=1684KJ/mol

Product=413KJ/mol

Clearly shown

[tex]\\ \bull\sf\dashrightarrow \Delta H=-ve[/tex]

Hence its an exothermic reaction.

pstnonsonjoku

Yes, the reaction would occur without additional energy because the reaction is exothermic.

We have to calculate the reaction enthalpy using the values of bond energy provided as follows;

ΔH(reaction) = ∑bond energies of bonds being broken - ∑bond energies of the bonds being formed.

Hence;

ΔH(reaction) =∑[839 + 3 (432)) + 2(413)] kJ/mol - ∑2(4×413) kJ/mol

ΔH(reaction) = (839 + 1296 + 826) kJ/mol - 3304  kJ/mol

ΔH(reaction) = 2961 kJ/mol - 3304  kJ/mol = -343 kJ/mol

Yes, the reaction would occur without additional energy because the reaction is exothermic.

Learn more about exothermic reaction:https://brainly.com/question/14969584

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