Question

The enthalpy of formation for \( \text{H}_2(g) \), \( \text{O}_2(g) \), and \( \text{H}_2O(l) \) are 0, 0, and -285.8 kJ/mol, respectively. What is the enthalpy change for the following reaction: \[ \text{2H}_2(g) + \text{O}_2(g) \rightarrow 2\text{H}_2O(l) \]

• A. \( -571.6 \, \text{kJ/mol} \)
• B. \( -285.8 \, \text{kJ/mol} \)
• C. \( 0 \, \text{kJ/mol} \)
• D. \( 571.6 \, \text{kJ/mol} \)

Hint:

The enthalpy change of a reaction can be calculated by subtracting the enthalpy of formation of the reactants from the enthalpy of formation of the products.