Question

(iii) iodine and chlorine react at high temperatures to form iodine monochloride, \\(\text{icl}\\).

the equation for the reaction is shown.

\\\text{i}_2(\text{g}) + \text{cl}_2(\text{g}) \
ightarrow 2\text{icl}(\text{g})\\

the structures of the molecules involved in the reaction are \\(\text{i}-\text{i}\\), \\(\text{cl}-\text{cl}\\) and \\(\text{i}-\text{cl}\\).

table 6.1

bond	bond energy in kj/mol
\\(\text{cl}-\text{cl}\\)	242
\\(\text{i}-\text{cl}\\)	218

calculate the enthalpy change, \\(\delta h\\), for the reaction using the bond energies in table 6.1.

use the following steps.

• calculate the total amount of energy required to break the bonds in 1 mol of \\(\text{i}_2(\text{g})\\) and 1 mol of \\(\text{cl}_2(\text{g})\\).

.................................................. kj

• calculate the total amount of energy released when the bonds in 2 mol of \\(\text{icl}(\text{g})\\) are formed.

.................................................. kj

• calculate the enthalpy change, \\(\delta h\\), for the reaction.

your answer should include a sign.

.................................................. kj/mol

Explanation:

Calculate energy required to break reactant bonds

$$
LATEXBLOCK0
$$

Calculate energy released when product bonds form

$$
LATEXBLOCK1
$$

Calculate the overall enthalpy change

$$
LATEXBLOCK2
$$

Answer:

Question 1

Calculate the total amount of energy required to break the bonds in \(1\text{ mol}\) of \(\text{I}_2\text{(g)}\) and \(1\text{ mol}\) of \(\text{Cl}_2\text{(g)}\).
<blank>392</blank> \(\text{kJ}\)

Question 2

Calculate the total amount of energy released when the bonds in \(2\text{ mol}\) of \(\text{ICl(g)}\) are formed.
<blank>436</blank> \(\text{kJ}\)

Question 3

Calculate the enthalpy change, \(\Delta H\), for the reaction. Your answer should include a sign.
<blank>-44</blank> \(\text{kJ/mol}\)