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8.7g of pure ...

Question

$8.7 g$ of pure $M n O_{2}$ is heated with an excess of $H C l$ and the gas evolved is passed into a solution of $K I$ . Calculate the weight of the iodine librated $(M n = 55, C l = 35.5. I = 127)$

7.77 g

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16.41 g

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12.70 g

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25.4 g

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Solution

The correct option is D $25.4 g$
The chemical equation for the reaction between $M n O_{2}$ and HCl can be written as:
$M n O_{2} + 4 H C l \to C l_{2} + M n C l_{2} + 2 H_{2} O$
Now molecular weight of $M n O_{2}$ = 87g
87g of $M n O_{2}$ produces = 71g 0f $C l_{2}$
$∴$ 8.7g $M n O_{2}$ produces = 7.1g 0f $C l_{2}$
Now chlorine gas reacts with KI as:
$C l_{2} + 2 K I \to I_{2} + 2 K C l$
71g of $C l_{2}$ liberates = 254g of $I_{2}$
$∴$ 7.1g of $C l_{2}$ liberates = 25.4g of $I_{2}$

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