Question

The oxide of an element possess the molecular formula M2O3. If the equivalent mass of the metal is 9, the molecular mass of the oxide will be-

Answer 1

Since valancy factor of metal is 3 so
Atomic weight of metal = 3*equivalent mass
. . . . = 3*9=27
Atomic mass of O= 16 so O3 = 48
So the molecular weight of M2O3 = 2*27+3*16=102

Answer 2

Given:

Formula of the Oxide = $M_2O_3$

Equivalent mass of the metal = 9

To find:

Molecular mass of the oxide = ?

Formula to be used:

$Equivalent weight = \frac{Atomic weight}{Valency}$

Calculation:

The valency of metal in given oxide is 3

As the equivalent weight and valency are known, atomic weight of the metal M can be calculated by the following method

$\frac{Atomic weight}{Valency} = Equivalent weight$

Atomic weight = Equivalent weight × Valency

Atomic weight = 9× 3 = 27

∴ Atomic weight of 1 metal = 27, and for 1 oxygen = 16

As 2 atoms of metal M is involved, atomic weight of metal will be:

27×2 = 54

As 3 atoms of oxygen is involved, atomic weight of oxygen will be:

16×3 = 48

Thus the molecular mass of the oxide is

Molecular mass of oxide = Atomic weight of Metal + Atomic weight of Oxygen

Molecular mass of oxide = 54 + 48

Molecular mass of oxide = 102

Conclusion:

Thus the molecular mass of the oxide will be 102.

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