Question

Use the information below to answer the question that follows.

CO(g)+H2(g)⟶CH2O(g)Bond energy of (C≡O)=1072 kJBond energy of (C=O)=802 kJBond energy of (H−H)=436 kJBond energy of (C−H)=413 kJ

What is the enthalpy of the reaction using bond energies?

Answer 1

The enthalpy change of the reaction can be calculated using bond energies. In this reaction, the C≡O bond in CO is broken, the H−H bond in H2 is also broken, and a C−H bond is formed in CH2O. Substituting the given bond energy values, the enthalpy change is calculated to be 293 kJ.

Step-by-step explanation:

The enthalpy of the reaction can be calculated using bond energies. In this reaction, the C≡O bond in CO is broken, requiring 1072 kJ. The H−H bond in H2 is also broken, requiring 436 kJ. At the same time, a C−H bond is formed in CH2O, releasing 413 kJ. Therefore, the enthalpy change of the reaction can be calculated as:

ΔH = (bond energy of C≡O + bond energy of H−H) - (bond energy of C=O + bond energy of C−H)

Substituting the given values:

ΔH = (1072 + 436) - (802 + 413) = 293 kJ