(ii) iodine and bromine react at high temperatures to form iodine monobromide, $\text{ibr}$.

the equation is shown.

\\text{i}_2(\text{g}) + \text{br}_2(\text{g}) \
ightarrow 2\text{ibr}(\text{g})\

the structures of the molecules involved in the reaction are $\text{i}-\text{i}$, $\text{br}-\text{br}$ and $\text{i}-\text{br}$.

table 6.1

| bond | bond energy in $\text{kj/mol}$ |
| :---: | :---: |
| $\text{i}-\text{i}$ | 150 |
| $\text{br}-\text{br}$ | 193 |
| $\text{i}-\text{br}$ | 175 |

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 $1\text{ mol}$ of $\text{i}_2(\text{g})$ and $1\text{ mol}$ of $\text{br}_2(\text{g})$.

........................... $\text{kj}$

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

........................... $\text{kj}$

* calculate the enthalpy change, $\delta h$, for the reaction.
your answer should include a sign.

........................... $\text{kj/mol}$
3

Question

(ii) iodine and bromine react at high temperatures to form iodine monobromide, $\text{ibr}$.

the equation is shown.

\\text{i}_2(\text{g}) + \text{br}_2(\text{g}) \
ightarrow 2\text{ibr}(\text{g})\

the structures of the molecules involved in the reaction are $\text{i}-\text{i}$, $\text{br}-\text{br}$ and $\text{i}-\text{br}$.

table 6.1

| bond | bond energy in $\text{kj/mol}$ |
| :---: | :---: |
| $\text{i}-\text{i}$ | 150 |
| $\text{br}-\text{br}$ | 193 |
| $\text{i}-\text{br}$ | 175 |

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 $1\text{ mol}$ of $\text{i}_2(\text{g})$ and $1\text{ mol}$ of $\text{br}_2(\text{g})$.

........................... $\text{kj}$

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

........................... $\text{kj}$

* calculate the enthalpy change, $\delta h$, for the reaction.
your answer should include a sign.

........................... $\text{kj/mol}$
3

Accepted Answer

{ "quality": "clear", "question_count": 3, "skills_matched": [ "step_cot", "table_formatter", "explain_then_answer", "quick" ], "needs_drawing": false, "concepts_used": [], "new_concepts": [], "current_concepts": [ "Bond Energy", "Enthalpy Change" ] } ## Calculate energy required to break bonds $$ \begin{aligned} E_{\text{break}} &= \text{Bond Energy}(\text{I-I}) + \text{Bond Energy}(\text{Br-Br}) \ E_{\text{break}} &= 150\text{ kJ/mol} + 193\text{ kJ/mol} = 343\text{ kJ} \end{aligned} $$ ## Calculate energy released when bonds are formed $$ \begin{aligned} E_{\text{form}} &= 2 \times \text{Bond Energy}(\text{I-Br}) \ E_{\text{form}} &= 2 \times 175\text{ kJ/mol} = 350\text{ kJ} \end{aligned} $$ ## Calculate enthalpy change $$ \begin{aligned} \Delta H &= E_{\text{break}} - E_{\text{form}} \ \Delta H &= 343\text{ kJ} - 350\text{ kJ} = -7\text{ kJ/mol} \end{aligned} $$ | No. | Problem | Answer | |---|---|---| | 1 | Energy required to break bonds | $343\text{ kJ}$ | | 2 | Energy released when bonds form | $350\text{ kJ}$ | | 3 | Enthalpy change, $\Delta H$ | $-7\text{ kJ/mol}$ | { "subject": "Natural Science", "question_type": "Multi-part", "knowledge_point": [ "Natural Science", "Chemistry", "Enthalpy Change" ] }

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QUESTION IMAGE

Question

Explanation:

Calculate energy required to break bonds

Calculate energy released when bonds are formed

Calculate enthalpy change

Answer:

No.	Problem	Answer
2	Energy released when bonds form	\(350\text{ kJ}\)
3	Enthalpy change, \(\Delta H\)	\(-7\text{ kJ/mol}\)