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Given the diagram below, what is the
H in kJ/mol for the decomposition of CO to produce 2 moles of C (graphite)? Please report answer as a whole number. If negative make sure to use the sign in answer.

To determine the enthalpy change (\( \Delta H \)) for the decomposition of CO to produce 2 moles of C (graphite), we can analyze the provided thermochemical diagram with the following enthalpy changes for reactions:

1. \( \Delta H_{R1} = -393 \, \text{kJ/mol} \)
2. \( \Delta H_{R2} = -111 \, \text{kJ/mol} \)
3. \( \Delta H_{R3} = -282 \, \text{kJ/mol} \)

Let's assume the overall equation we want to achieve is:
\[ \text{2 CO} \rightarrow \text{2 C} + \text{O}_2 \]

We can apply Hess's Law by manipulating the given reactions to match this overall equation. The key is to find a pathway that correctly balances the decomposition of CO into graphite and oxygen. Let's work through the reaction steps:

- \( R1 \) is the formation of CO from C and \( \frac{1}{2} \)O₂.
- \( R2 \) might involve similar species.
- \( R3 \) might also involve these species in some form.

Let's now determine the relationship between these reactions to decompose CO. 

\( R1 \) is already a formation equation for CO, so reversing it will give us the decomposition of CO. Since we need 2 moles of C (graphite), we should consider reversing \( R1 \) and multiplying it by 2 to get:
\[ 2 \text{CO} \rightarrow 2 \text{C} + \text{O}_2 \]
This would reverse the sign of \( \Delta H_{R1} \), giving \( \Delta H = 2 \times (+393 \, \text{kJ/mol}) = +786 \, \text{kJ/mol} \).

The calculated \( \Delta H \) for the decomposition of 2 moles of CO to produce 2 moles of C (graphite) is \( +786 \, \text{kJ/mol} \).

Would you like to explore any details of this solution or have further questions about thermochemistry or Hess's Law? Here are some follow-up topics we can discuss:
1. How to use Hess's Law to determine enthalpy changes for other complex reactions.
2. Why reversing a reaction changes the sign of \( \Delta H \).
3. The importance of stoichiometry in thermochemical equations.
4. How enthalpy changes relate to bond energies.
5. The difference between endothermic and exothermic reactions.

**Tip:** Always ensure that the stoichiometry of your reactions matches that of the desired overall reaction when using Hess's Law to avoid errors in calculating \( \Delta H \).

Given the diagram below, what is the H in kJ/mol for the decomposition of CO to produce 2 moles of C (graphite)? Please report answer as a whole number. If negative make sure to use the sign in answer.

Learn how to calculate the enthalpy change (ΔH) for the decomposition of CO to produce 2 moles of graphite using Hess's Law. This advanced chemistry problem involves stoichiometry, thermochemistry, and proper application of enthalpy concepts. Perfect for Grades 11-12.

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