9.03 of Mg combine completely with 3.48g of N to form compound. what is the percent composition of each element in this compound?

To find the percent composition of each element in a compound, follow these steps:

1. Determine the molar masses of each element:
- The molar mass of Mg (Magnesium) is 24.305 g/mol.
- The molar mass of N (Nitrogen) is 14.007 g/mol.

2. Calculate the number of moles for each element:
- Divide the given mass of each element by its molar mass.
- Moles of Mg = 9.03 g / 24.305 g/mol = 0.371 mol
- Moles of N = 3.48 g / 14.007 g/mol ≈ 0.249 mol

3. Determine the total moles of the compound:
- Since the compound is formed by the combination of Mg and N, the total moles will be the sum of the individual moles.
- Total moles of the compound = Moles of Mg + Moles of N = 0.371 mol + 0.249 mol = 0.620 mol

4. Calculate the percent composition of each element:
- Percent composition = (moles of element / total moles of the compound) x 100%
- For Mg: (0.371 mol / 0.620 mol) x 100% ≈ 59.8%
- For N: (0.249 mol / 0.620 mol) x 100% ≈ 40.2%

Therefore, the percent composition of Mg in the compound is approximately 59.8%, and the percent composition of N is approximately 40.2%.

%Mg = (grams Mg/total mass)*100 = ?

Note: total mass is 9.03 + 3.48 = ?

%N = (3.48/total mass)*100 = ?