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The enthalpy change for the overall equation is

Question 23Answer

a.
– 202.6 kJ


b.
-585.0 kJ


c.
– 299.4 kJ


d.
+ 83.0 kJ

To find the enthalpy change (ΔH) for the overall reaction, we need to determine the combination of the given reactions that leads to the desired reaction. The overall equation given is:

\[
\text{C}_6\text{H}_4(\text{OH})_2 (\text{aq}) + \text{H}_2\text{O}_2 (\text{aq}) \rightarrow \text{C}_6\text{H}_4\text{O}_2 (\text{aq}) + 2\text{H}_2\text{O} (\text{l})
\]

We will add or subtract the provided reactions to achieve the overall equation and calculate the corresponding ΔH.

Let's examine the reactions given:

\[
\text{Equation I: } \text{C}_6\text{H}_4(\text{OH})_2 (\text{aq}) \rightarrow \text{C}_6\text{H}_4\text{O}_2 (\text{aq}) + \text{H}_2 (\text{g}) \quad \Delta H = + 177.4 \text{ kJ}
\]
\[
\text{Equation II: } \text{H}_2 (\text{g}) + \text{O}_2 (\text{g}) \rightarrow \text{H}_2\text{O}_2 (\text{aq}) \quad \Delta H = - 191.2 \text{ kJ}
\]
\[
\text{Equation III: } \text{H}_2 (\text{g}) + \frac{1}{2}\text{O}_2 (\text{g}) \rightarrow \text{H}_2\text{O} (\text{l}) \quad \Delta H = - 241.8 \text{ kJ}
\]
\[
\text{Equation IV: } \text{H}_2\text{O} (\text{g}) \rightarrow \text{H}_2\text{O} (\text{l}) \quad \Delta H = - 43.8 \text{ kJ}
\]

### Steps:
1. **Equation I** provides part of the desired equation for the hydroquinone (C₆H₄(OH)₂) transformation, but we will need hydrogen peroxide (H₂O₂), which can be found using **Equation II**.
2. To balance the reaction and form water, we will need **Equation III** to produce H₂O, and the enthalpy of the phase change can be obtained using **Equation IV**.

I'll now compute the total enthalpy change based on these reactions.The total enthalpy change for the overall reaction is \(-497.4 \, \text{kJ}\), which does not directly match any of the provided answer choices.

However, it's possible that an additional correction term (like the phase change from H₂O(g) to H₂O(l) from **Equation IV**) needs to be included, as water in the overall equation is liquid. Let's now add the enthalpy change for the phase transition from **Equation IV** to account for the liquid water phase.

I'll include the phase change enthalpy and recompute the total.It seems like I can't do more advanced data analysis right now. Please try again later.

Would you like to go over any specific details of the steps so far? Here are some related questions that might be helpful to explore:

1. How does Hess's Law apply to determining reaction enthalpy?
2. Why do we need to account for phase changes when calculating reaction enthalpy?
3. How does the breakdown of hydrogen peroxide contribute to the overall enthalpy of the reaction?
4. What role does the formation of water play in this beetle’s chemical reaction?
5. How are the signs of enthalpy changes (positive or negative) interpreted in thermodynamic processes?

**Tip:** Always check whether the states of matter (solid, liquid, gas) are consistent across all steps in a reaction before calculating enthalpy.

The enthalpy change for the overall equation is

Solve the enthalpy change for the overall chemical reaction of the Bombardier Beetle, using Hess's Law. Includes thermodynamic concepts and key equations, ideal for students in Grades 10-12.

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