As a result of the reduction with hydrogen of 18.2 g of the oxide, a pentavalent metal, 0.5 mol

As a result of the reduction with hydrogen of 18.2 g of the oxide, a pentavalent metal, 0.5 mol of water was formed. Determine the metal.

Let’s implement the solution:
1. The oxide formula is R2O5 (5);
2. Let’s write down the recovery process:
R2O5 + 5H2 = 2R + 5H2O;
3. Let’s make the proportion:
X mol (R2O5) – 0.5 mol H2O;
-1 mol -5 mol hence, X mol (R2O5) = 1 * 0.5 / 5 = 0.1 mol;
Determine the molar mass of the metal oxide:
Y (R2O5) = m / M;
M (R2O5) = 18.2 / 0.1 = 182 g.
Let’s make calculations using the formula:
RxOy; R2O5
2x + 16 * 5 = 182;
2x = 102;
X = 51;
Ar (V) = 50.9 = 51;
V2O5 is the oxide formula; M (V2O5) = 2 * 51 + 16 * 5 = 182 g / mol.
Answer: the oxide formula is V2O5, the metal is vanadium.