a metal x with relative atomic mass 56 forms an oxide with formula X2O3. how many grams of the metal will combine 10g of oxygen (o=16)

8:48 = 5/3 : 10

4X + 3O2 ==> 2X2O3

mols O2 = 10/32 = 0.31
mols X = 0.31 x (4 mols X/3 mols O2) = about 0.42
g X = mols X*56 = ?

23.3

To find out how many grams of the metal will combine with 10g of oxygen in the oxide X2O3, we need to use the concept of molar ratios.

First, let's calculate the molar mass of oxygen (O) by using its atomic mass, which is 16 g/mol.

Now, we can calculate the number of moles of oxygen present in 10g of oxygen by using the formula:
Number of moles = Mass / Molar mass

Number of moles of oxygen = 10g / 16 g/mol = 0.625 mol

Next, let's determine the ratio between the moles of oxygen and the moles of metal in the oxide X2O3. From the formula X2O3, we can see that there are two moles of metal (X) for every three moles of oxygen (O).

Therefore, the molar ratio of metal to oxygen is 2:3. So, for every 2 moles of metal, we have 3 moles of oxygen.

Now, let's set up a proportion using the molar ratio and the moles of oxygen we calculated earlier:

(2 moles of metal / 3 moles of oxygen) = (x moles of metal / 0.625 moles of oxygen)

Simplifying the proportion, we get:

2 / 3 = x / 0.625

Cross-multiplying and solving for x:

x = 2 * 0.625 / 3 = 0.4167 mol

To convert moles of metal to grams, we multiply by its molar mass. Since we know the relative atomic mass of the metal is 56, the molar mass of the metal will also be 56 g/mol.

Therefore, the mass of the metal that combines with 10g of oxygen will be:

Mass of metal = Number of moles * Molar mass = 0.4167 mol * 56 g/mol = 23.334 g

Therefore, approximately 23.334 grams of the metal will combine with 10g of oxygen.