Answer:
The atomic weight in g/mole of the metal (molar mass) is 8.87.
Explanation:
To begin, it is possible to assume that, as a sample, it has 100 g of the compound. This means that:
Using the molar mass of oxygen, which is 16 g / mol, it is possible to calculate the amount of moles of oxygen present in the sample using the rule of three:
[tex]moles of oxygen=\frac{47.8g*1mol}{16g}[/tex]
moles of oxygen=2.9875
The chemical formula of metal oxide tells you that:
2 M⁺³ + 3 O²⁻ ⇒ M₂O₃
In the previous equation you can see that you need 3 oxygen anions to react with two metal cations. Then:
[tex]2.9875 moles of oxygen*\frac{2 moles of metal M}{1 mol of oxygen} = 5.975 moles of metal M[/tex]
You have 52.92 g of metal in the sample, then the molar mass of the metal is:
[tex]molar mass=\frac{52.92 g}{5.975 mol}[/tex]
molar mass≅ 8.87 g/mol
The atomic weight in g/mole of the metal (molar mass) is 8.87.
The closest match to this value is Beryllium (Be), which has an atomic mass of 9.0122 g / mol.
The atomic weight in g/mole of the metal (M) is 27 g/mol
From the question given above, the following data were obtained:
Metal (M) = 52.92%
Oxygen (O) = 100 – 52.92 = 47.08%
Let the mass of the compound (M₂O₃) = 100 g.
Thus,
Metal (M) = 52.92 g
Oxygen (O) = 47.08 g
Mass of O = 47.08 g
Molar mass of O = 16 g/mol
Mole = mass / molar mass
Mole of O = 47.08 / 16
Formula of compound => M₂O₃
From the formula of the compound,
3 moles of Oxygen required 2 moles of the metal
Therefore,
2.94 moles of oxygen will require = (2.94 × 2)/3 = 1.96 mole of the metal
Mole of metal = 1.96
Mass of metal = 52.92 g
Molar mass = mass / mole
Molar mass of metal = 52.92 / 1.96
Therefore, the atomic weight in g/mole of the metal (M) is 27 g/mol
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