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Introduction and Degree of Hydrolysis

When one mole...

Question

When one mole of anhydrous $F e S O_{4}$ is dissolved in excess of water, there in evolution of $58.2 k J$ of heat. But when one mole of $F e S O_{4}$ . $5 H_{2} O$ is dissolved in water, the heat change is $+ 8.6 k J$ calculate the enthalpy of hydration of anhydrous $F e S O_{4}$ .

- 49.6 k J

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- 66.8 k J

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+ 49.6 k J

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+ 66.8 k J

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Solution

The correct option is C $+ 49.6 k J$
Given, for $F e S O_{4}, △_{s o l} H^{o} = + 58.2 k J$
$△_{l a t t i c e} H^{o} = + 8.6 k J$
$∴ △_{h y d} H^{o}$ of $F e S O_{4} = △_{s o l} H^{o} - △_{h y d} H^{o}$
$= 59.2 k J - 8.6 k J = + 49.6 k J$

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