1.0g of the oxide of metal x(atomic mass =64)gave 0.08g of the mental when reduced with hydrogen. the formula of oxide is?
.08 g of the metal combined with 0.92 g of oxygen
convert the grams to moles to find the oxide formula
it looks like the post-reduction metal mass may not have the correct decimal point
To find the formula of the oxide of metal x, we first need to determine the number of moles of metal produced when 1.0g of the oxide is reduced with hydrogen.
1. Calculate the number of moles of metal produced:
- Given: Mass of metal produced = 0.08g
- Atomic mass of metal x = 64g/mol
Number of moles of metal = mass of metal produced / atomic mass of metal x
Number of moles of metal = 0.08g / 64g/mol
2. Determine the molar ratio of the metal and oxygen in the oxide:
- From the balanced chemical equation, we know that 1 mole of metal corresponds to 1 mole of oxygen in the oxide.
3. Calculate the number of moles of oxygen in the oxide:
Number of moles of oxygen = Number of moles of metal
4. Determine the mass of oxygen in the oxide:
Mass of oxygen in the oxide = number of moles of oxygen x atomic mass of oxygen
- Given: atomic mass of oxygen = 16g/mol
5. Determine the empirical formula of the oxide:
The empirical formula shows the simplest whole-number ratio of atoms in a compound.
For the empirical formula, we divide the number of moles of each element by the smallest number of moles calculated in the previous steps. This will give us a ratio from which we can determine the empirical formula.
6. Determine the molecular formula of the oxide:
To obtain the molecular formula, we need the molar mass of the compound.
Given that the molar mass of the oxide is known, we can calculate the ratio of the molar mass to the empirical formula mass. This ratio will tell us how many empirical formulas are present in the molecular formula.
By following these steps, you should be able to determine the formula of the oxide of metal x.