Use the References to access important vafues if needed for this question. The following thermochemical equation is for the reaction of Fe3O4( s) with hydrogen( g) to form iron(s) and water (g). Fe3O4( s)+4H2( g)⟶3Fe(s)+4H2O(g) ΔH=151 kJ When 66.9 grams of Fe3O4( s) react with excess hydrogen( g), __ kJ of energy are _

Hint: An arnount of energy is expressed as a positive number. The sign of aH in the thermochemical nguation indicates whether the energy is absorbed of Evolved.

In the given thermochemical equation, the reaction of 66.9 grams of Fe3O4 with excess hydrogen gas releases a certain amount of energy. The value of ΔH, which is the enthalpy change, is given as 151 kJ. The question asks for the amount of energy released in kJ during the reaction.

The ΔH value in the thermochemical equation represents the enthalpy change of the reaction. It indicates whether energy is absorbed or evolved during the reaction. In this case, the value of ΔH is given as 151 kJ, which means that the reaction releases 151 kJ of energy.

Since the reaction is stated to occur with 66.9 grams of Fe3O4, it is important to note that the ΔH value given is for the specified amount of reactant. If the amount of reactant were different, the energy released would also be different.

To determine the energy released during the reaction, we can directly use the given value of ΔH, which is 151 kJ. This value represents the amount of energy released when the specified amount of reactants react completely.

Therefore, when 66.9 grams of Fe3O4 react with excess hydrogen gas, 151 kJ of energy are released.

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