When hydrogen gas was passed over $8.08 g$ of heated metal oxide, it was completely reduced and $1.8 g$ of water was formed:
(a) What is weight of oxygen in the metal oxide?
(b) What is the equivalent mass of the metal?

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Solution

(a) When hot metal oxide is treated with hydrogen, $1.8 g$ water is formed.
$18 g H_{2} O$ contains $16 g$ oxygen.
Thus, $1.8 g H_{2} O$ will contain $1.6 g$ oxygen.
(b) Equivalent mass may be defined as weight of the metal that combines with $8$ parts of oxygen to form its oxide.
Mass of metal in its oxide $= 8.08 - 1.6$
$= 6.48 g$
$∵ 1.6 g$ oxygen combines with $6.48 g$ of metal
$∴ 8 g$ oxygen will combine with $= \frac{6.48}{1.6} \times 8 g$ of metal
$= 32.4 g$
Thus, equivalent mass of metal $= 32.4$ .

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When hydrogen gas was passed over 8.08 g of heated metal oxide, it was completely reduced and 1.8 g of water was formed:(a) What is weight of oxygen in the metal oxide?(b) What is the equivalent mass of the metal?

When hydrogen gas was passed over $8.08 g$ of heated metal oxide, it was completely reduced and $1.8 g$ of water was formed:
(a) What is weight of oxygen in the metal oxide?
(b) What is the equivalent mass of the metal?