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Given the equation representing a reaction:

[tex]\[ H_2(g) + I_2(g) \rightarrow 2HI(g) \][/tex]

Which statement describes the energy changes that occur in this reaction?

A. Energy is absorbed as bonds are formed.
B. Energy is released as bonds are broken.
C. Energy is absorbed as bonds are formed, and energy is released as bonds are broken.
D. Energy is absorbed as bonds are broken, and energy is released as bonds are formed.

Sagot :

GinnyAnswer
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.
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