To solve this problem, we need to understand the basic concepts of bond energy in chemical reactions:
1. When bonds are broken, energy is absorbed.
2. When bonds are formed, energy is released.
In the given chemical reaction:
[tex]\[ H_2(g) + I_2(g) \rightarrow 2 HI(g) \][/tex]
- Breaking bonds requires energy. Here, the bonds in the reactants [tex]\( H_2 \)[/tex] and [tex]\( I_2 \)[/tex] are broken. When [tex]\( H_2 \)[/tex] breaks, energy is absorbed to break the [tex]\( H-H \)[/tex] bond. Similarly, energy is also absorbed to break the [tex]\( I-I \)[/tex] bond in [tex]\( I_2 \)[/tex].
- Forming bonds releases energy. In this reaction, [tex]\( HI \)[/tex] is formed by creating new bonds between hydrogen and iodine atoms. Therefore, energy is released when the [tex]\( H-I \)[/tex] bonds are formed in [tex]\( HI \)[/tex].
Based on these principles, the statement that correctly describes the energy changes taking place in the reaction [tex]\( H_2(g) + I_2(g) \rightarrow 2 HI(g) \)[/tex] is:
(4) Energy is absorbed as bonds are broken, and energy is released as bonds are formed.
Thus, the correct option is 4.
