A certain metal sulphide, $M S_{2}$ , is used extensively as a high-temperature lubricant. If $M S_{2}$ has $40.06$ % sulphur by weight, atomic mass of $M$ will be:

100 a m u

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96 a m u

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60 a m u

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30 a m u

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Solution

The correct option is A $96 a m u$
Weight percentage of sulphur $= \frac{Mass of sulphur}{Mass of compound} \times 100$

$\Rightarrow 40.06 = \frac{64}{M + 64} \times 100$

$M =$ Atomic mass of metal

$M = 96 a m u$

Hence, option B is correct.

Suggest Corrections

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