A metal X with relative atomic mass 56 form an oxide with formula X2O3.how many grams of the metal will combine with 10g of oxygen
To find out how many grams of the metal will combine with 10g of oxygen, we need to use the formula of the oxide and find the atomic ratio between the metal and the oxygen.
The formula of the oxide is X2O3, which means that for every 2 atoms of metal X, there are 3 atoms of oxygen.
Using relative atomic masses, we can find the mass of 1 mole of oxygen (O), which is 16 g. Therefore, the mass of 1 mole of X2O3 is:
2 x atomic mass of X + 3 x 16g = 2 x 56g + 3 x 16g = 184g
This means that 184g of X2O3 contains 2 x 56g of metal X.
To find out how many grams of the metal will combine with 10g of oxygen, we need to use the atomic ratio between the metal and the oxygen in the oxide formula. Since there are 3 atoms of oxygen for every 2 atoms of metal, we can write:
2g of metal X combines with 3 x 16g = 48g of oxygen
Therefore, we can use a proportion to find out how many grams of metal X will combine with 10g of oxygen:
2g / 48g = x / 10g
Cross-multiplying, we get:
48g x = 2g x 10g
x = 0.417g
Therefore, 0.417g of metal X will combine with 10g of oxygen.