The thermite reaction, used for welding iron, is the reaction of Fe3O4 with Al. 8 Al (s) + 3 Fe3O4 (s) ⟶ 4 Al2O3 (s) + 9 Fe (s) Δ H° = -3350. kJ/mol rxn. Because this large amount of heat cannot be rapidly dissipated to the surroundings, the reacting mass may reach temperatures near 3000. °C. How much heat (in kJ) is released by the reaction of 19.3 g of Al with 63.2 g of Fe3O4?

The amount of heat released by the reaction is -2395.25 kJ

Explanation:

To calculate the number of moles, we use the equation:

Given mass of aluminium = 19.3 g

Molar mass of aluminium = 27 g/mol

Putting values in equation 1, we get:

Given mass of = 63.2 g

Molar mass of = 231.5 g/mol

Putting values in equation 1, we get:

The given chemical equation follows:

By Stoichiometry of the reaction:

8 moles of aluminium reacts with 3 moles of

So, 0.715 moles of aluminium will react with = of

As, given amount of is more than the required amount. So, it is considered as an excess reagent.

Thus, aluminium is considered as a limiting reagent because it limits the formation of product.

To calculate the enthalpy change of the reaction, we use the equation:

where,

= amount of heat absorbed = ? J

n = number of moles of aluminium = 0.715 moles

= enthalpy change of the reaction  = -3350 kJ/mol

Putting values in above equation, we get:

Hence, the amount of heat released by the reaction is -2395.25 kJ

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