2.08g of metal Y react with 0.96g of oxygen to form a metal oxide.The empirical formula of the metal oxide is Y2O3.What is the relative atomic mass of metal Y.
.96g of O2 is .03 moles
So, since it takes 2 moles of Y to combine with 3 moles of O, and we have .03 moles of O2 (.06 moles of O), we have .04 moles of Y.
So, the molar mass of Y is 2.08/.04 = 52
Thanks a lot^^
To find the relative atomic mass of metal Y, we need to use the given information about the reactants and the empirical formula of the metal oxide.
First, let's calculate the moles of metal Y and oxygen:
Moles of metal Y = Mass of metal Y / Molar mass of metal Y
Moles of metal Y = 2.08g / Molar mass of metal Y (1)
Moles of oxygen = Mass of oxygen / Molar mass of oxygen
Moles of oxygen = 0.96g / Molar mass of oxygen (2)
According to the balanced chemical equation for the reaction, the ratio of moles of metal Y to moles of oxygen is 2:3 (based on the empirical formula Y2O3).
Therefore, from equation (1) and (2), we can set up the following equation:
(2.08g / Molar mass of metal Y) / (0.96g / Molar mass of oxygen) = 2 / 3
Now, we can solve this equation to find the relative atomic mass of metal Y.
Cross-multiplying the equation:
2.08g x Molar mass of oxygen = 0.96g x Molar mass of metal Y x (2/3)
Simplifying:
2.08g x Molar mass of oxygen = 0.64g x Molar mass of metal Y
Now, we need to find the molar mass of oxygen, which is 16g/mol (since oxygen has an atomic mass of 16 g/mol).
Substituting the values:
2.08g x 16g/mol = 0.64g x Molar mass of metal Y
33.28g/mol = 0.64g x Molar mass of metal Y
Dividing both sides by 0.64g:
33.28g/mol / 0.64g = Molar mass of metal Y
Molar mass of metal Y = 52g/mol
Therefore, the relative atomic mass of metal Y is 52g/mol.