Consider the reaction represented by the following equation: H 2(g) + \(\frac{1}{2}\) O(g) → H 2O(g) ∆H =-285.8 KJmo -1 ∆H represents the enthalpy of

Consider the reaction represented by the following equation: H _2(g) + \(\frac{1}{2}\) O_(g) → H ₂O_(g) ∆H =-285.8 KJmo ^-1 ∆H represents the enthalpy of

Answer Details

∆H represents the enthalpy change of a chemical reaction, which is defined as the difference between the enthalpy of the products and the enthalpy of the reactants. In this case, the equation given is the reaction of hydrogen gas and oxygen gas to form water, so ∆H represents the enthalpy change of the formation of water. Therefore, the correct answer is "formation".