Question

question 8 (1 point)
use the following information to answer the next question.
the energy required to break one mole of bonds of particular type between atoms is called bond energy. consider the reaction:
h₂(g) + ½ o₂(g) → h₂o(l)
the bond energy of an o - h bond is 449.08 kj/mol, when one mole of water is formed.
what is the amount of energy required to be absorbed/released in the dissociation of 1 mole of water?
898.16 kj is released
898.16 kj is absorbed
989.16 kj is released
989.16 kj is absorbed
449.07 kj is released

Explanation:

Step1: Analyze the bond - breaking and bond - forming in water dissociation

When water (\(H_2O\)) dissociates, the \(O - H\) bonds are broken. One molecule of \(H_2O\) has 2 \(O - H\) bonds.

Step2: Calculate the energy for 1 mole of water dissociation

For 1 mole of \(H_2O\), the number of \(O - H\) bonds is \(2N_A\) (where \(N_A\) is Avogadro's number). Given the bond energy of one \(O - H\) bond is \(449.08\ kJ/mol\).
The energy required to break the bonds in 1 mole of \(H_2O\) is \(E=2\times449.08\ kJ/mol\)

$$E = 898.16\ kJ/mol$$

Since bond - breaking is an endothermic process (energy is absorbed).

Answer:

898.16 kJ is absorbed