When $4.0$ g of iron is burnt at high temperature, to ferric oxide, at constant pressure, $29.28$ kJ of heat is evolved. The amount of heat evolved for producing one mole of ferric oxide is:

819.84

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40.99

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81.98

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409.0

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Solution

The correct option is B $819.84$ kJ
The reaction is $2 F e + \frac{3}{2} O_{2} \to F e_{2} O_{3}$ .

$2$ moles ( $112$ g) of iron produces $1$ mole of ferric oxide.

When $4.0$ g iron is burnt, the heat evolved is $29.28$ kJ.

Thus, when $112$ g iron is burnt, the heat evolved is $\frac{29.28}{4.0} \times 112 = 819.84$ kJ.

Hence, option A is correct.

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When 4.0 g of iron is burnt at high temperature, to ferric oxide, at constant pressure, 29.28 kJ of heat is evolved. The amount of heat evolved for producing one mole of ferric oxide is:

The correct option is B 819.84 kJThe reaction is 2Fe+32O2→Fe2O3.2 moles (112 g) of iron produces 1 mole of ferric oxide.When 4.0 g iron is burnt, the heat evolved is 29.28 kJ.Thus, when 112 g iron is burnt, the heat evolved is 29.284.0×112=819.84 kJ.Hence, option A is correct.

When $4.0$ g of iron is burnt at high temperature, to ferric oxide, at constant pressure, $29.28$ kJ of heat is evolved. The amount of heat evolved for producing one mole of ferric oxide is: