To calculate the enthalpy change (ΔH) of a reaction using the energy of the reactants and products, you can use the following formula:
\[ \Delta H = E_{\text{products}} - E_{\text{reactants}} \]
Where:
- \(E_{\text{products}}\) is the energy of the products
- \(E_{\text{reactants}}\) is the energy of the reactants
Given:
- \(E_{\text{reactants}} = 100 \text{ kJ/mol}\)
- \(E_{\text{products}} = 300 \text{ kJ/mol}\)
Now plug the values into the formula:
\[ \Delta H = 300 \text{ kJ/mol} - 100 \text{ kJ/mol} = 200 \text{ kJ/mol} \]
Therefore, the enthalpy change (ΔH) for this reaction is \(+200 \text{ kJ/mol}\). This indicates that the reaction is endothermic, as the products have higher energy than the reactants.
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