A solid element burns in oxygen without any change in volume (of gas) under similar conditions of temperature and pressure. If the vapour density of pure gaseous product is 32, what is the equivalent mass of the element?

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Solution

The correct option is B 8
Given in this question $M + O_{2} \to M O$
Then molecular weight is $2 \times V . D$ So MO mass is 64

If we take 2 atoms of $O_{2}$ then mass of M will be 32 So sulphur mass is 32
AND n-factor is 2
Now equivalent weight is $\frac{16}{2}$ = 8

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A solid element burns in oxygen without any change in volume (of gas) under similar conditions of temperature and pressure. If the vapour density of pure gaseous product is 32, what is the equivalent mass of the element?

The correct option is B 8Given in this question M+O2→MO Then molecular weight is 2×V.D So MO mass is 64 If we take 2 atoms of O2 then mass of M will be 32 So sulphur mass is 32 AND n-factor is 2 Now equivalent weight is 162 = 8

The correct option is B 8
Given in this question $M + O_{2} \to M O$
Then molecular weight is $2 \times V . D$ So MO mass is 64

If we take 2 atoms of $O_{2}$ then mass of M will be 32 So sulphur mass is 32
AND n-factor is 2
Now equivalent weight is $\frac{16}{2}$ = 8