What mass of iron(ii) oxide must be used in the reaction given by the equation below to release 44.7 kj? 6feo(s) + o2(g) => 2fe3o4(s) δh° = -635 kj calculate your answer in g. enter it with two decimal places and no units.

The mass of iron (II) oxide that must be used in the reaction is 30.37

Explanation:

The given chemical reaction follows:

By Stoichiometry of the reaction:

When 635 kJ of energy is released, 6 moles of iron (II) oxide is reacted.

So, when 44.7 kJ of energy is released, of iron (II) oxide is reacted.

Now, calculating the mass of iron (II) oxide by using the equation:

Moles of iron (II) oxide = 0.423 moles

Molar mass of iron (II) oxide = 71.8 g/mol

Putting values in above equation, we get:

Hence, the mass of iron (II) oxide that must be used in the reaction is 30.37

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explanation:

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explanation:

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