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madam [21]
3 years ago
6

The heat of formation of Fe2O3(s) is –826.0 kJ/mol. Calculate the heat of the reaction 4Fe(s) + 3O2(g) → 2Fe2 O3(s) when a 53.99

-g sample of iron is reacted.
Chemistry
1 answer:
ira [324]3 years ago
7 0

Answer : The heat of the reaction is, 399.784 kJ

Explanation :

The given balanced chemical reaction is,

4Fe(s)+3O_2(g)\rightarrow 2Fe_2O_3(s)

First we have to calculate the moles of iron.

\text{Moles of }Fe=\frac{\text{Mass of }Fe}{\text{Molar mass of }Fe}=\frac{53.99g}{55.8g/mole}=0.968moles

Now we have to calculate the moles of Fe_2O_3

From the reaction we conclude that,

As, 4 moles of Fe react to give 2 moles of Fe_2O_3

So, 0.968 moles of Fe react to give \frac{2}{4}\times 0.968=0.484 moles of Fe_2O_3

Now we have to calculate the heat of the reaction.

As, 1 mole of Fe_2O_3 produce heat = 826.0 kJ

So, 0.484 mole of Fe_2O_3 produce heat = 0.484\times 826.0=399.784kJ

Therefore, the heat of the reaction is, 399.784 kJ

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