To calculate the enthalpy change (ΔH) for the reaction, you can use the following formula:
\[ \Delta H = H_{\text{products}} - H_{\text{reactants}} \]
Given:
- Enthalpy of the reactants = 100 kJ/mol
- Enthalpy of the products = 300 kJ/mol
Now, substituting the values into the formula:
\[ \Delta H = 300 \text{ kJ/mol} - 100 \text{ kJ/mol} = 200 \text{ kJ/mol} \]
Answer to (1):
\[ \Delta H = 200 \text{ kJ/mol} \]
Answer to (2):
The enthalpy change of +200 kJ/mol indicates that the reaction is endothermic. This means that the reaction absorbs energy from the surroundings. In an endothermic reaction, the energy of the products is higher than that of the reactants. The positive value of ΔH shows that energy input is required for the reaction to proceed, which is often associated with processes that involve breaking bonds in the reactants and forming new bonds in the products. This energy requirement can be observed in reactions that involve heat absorption, such as the melting of ice or the dissolution of certain salts in water.