Question
Given the reactants is 100KJ/mol and product is 300KJ/mol. Calculate the enthalpy change of the energy profile graph
Answers
GPT-4o mini
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.
\[
\Delta H = E_{\text{products}} - E_{\text{reactants}}
\]
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.