Question

How much heat is liberated when 3.21 g of iron (III) oxide are reduced by aluminum
at constant pressure (at 298.15 K)?
2Al + Fe2O3 = Al2O3 + 2Fe

Answer 1

Thermite reaction iron(III)oxide reacts with aluminum and gives molten iron aluminium oxide ...write a balaced equation and identify the reaction involved


2 Al(s) + Fe2O3(s) --> 2Fe(s) + Al2O3(s)  + 850 kJ/mol

The reaction of iron (III) oxide and aluminum is initiated by heat released from a small amount "starter mixture".  This reaction is an oxidation-reduction reaction, a single replacement reaction, producing great quantities of heat (flame and sparks) and a stream of molten iron and aluminum oxide which pours out of a hole in the bottom of the pot into sand.

Answer 2

Hey dear,

● Answer -
∆H = 124 J

● Explaination -
For the reaction,
2Al + Fe2O3 = Al2O3 +
2Fe

No of moles is given by -
n = W / M
n = 3.21 / 162
n = 0.05

Heat energy liberated in the reaction -
∆H = ∆nRT
∆H = 0.05 × 8.314 × 298
∆H = 124 J

Therefore, heat liberated in the reaction is 124 J.

Hope this helps...