The Equivalent Weight of Oxygen:
The equivalent weight of a substance is defined as the mass of the substance that combines with or replaces one mole of hydrogen ions (H+). In the case of oxygen, its equivalent weight is half that of a metal.

The Weight of Oxygen's Oxide:
When oxygen reacts with a metal, it forms an oxide. The oxide is composed of oxygen atoms and the metal atoms. To determine the weight of the oxide, we need to consider the atomic masses of both oxygen and the metal.

Weight of Oxygen:
The atomic mass of oxygen is approximately 16 g/mol. Since the equivalent weight of oxygen is half that of a metal, the weight of oxygen involved in the reaction is 8 g/mol.

Weight of Metal:
To find the weight of the metal, we need to know the specific metal involved in the reaction. Let's consider an example with magnesium, whose atomic mass is approximately 24 g/mol. Since the equivalent weight of oxygen is half that of the metal, the weight of magnesium involved in the reaction is 48 g/mol.

Weight of the Oxide:
The weight of the oxide can be calculated by adding the weight of oxygen to the weight of the metal. In this case, the weight of the oxide is 8 g/mol (weight of oxygen) + 48 g/mol (weight of metal) = 56 g/mol.

Comparison:
To determine how many times the weight of the oxide is greater than the weight of the metal, we can calculate the ratio between the two.

Weight of the oxide: 56 g/mol
Weight of the metal: 48 g/mol

The weight of the oxide is 56 g/mol, which is 1.17 times greater than the weight of the metal. Therefore, the weight of the oxide is approximately 1.17 times greater than the weight of the metal.

Summary:
The weight of an oxide formed by the reaction of oxygen with a metal is determined by adding the weight of oxygen to the weight of the metal. In this case, since the equivalent weight of oxygen is half that of the metal, the weight of the oxide is 1.17 times greater than the weight of the metal.