How many moles of magnesium are needed to react with 16 g of O2?
2 MgO (s) + O2 (g) → 2 MgO (s)
mols O2 = grams/molar mass = ?
Use the coefficients in the balanced equation to convert mols O2 to mols Mg.
To determine the number of moles of magnesium (Mg) needed to react with 16 g of O2, we can use the balanced chemical equation provided.
The equation states that 2 moles of Mg react with 1 mole of O2 to produce 2 moles of MgO.
To find the number of moles of O2, we need to convert the given mass of O2 (16 g) to moles using the molar mass of O2.
The molar mass of O2 can be calculated by adding the atomic masses of two oxygen atoms (16 g/mol x 2 = 32 g/mol).
Now we can proceed with the calculation:
Number of moles of O2 = mass of O2 / molar mass of O2
= 16 g / 32 g/mol
= 0.5 mol
According to the balanced equation, the ratio of moles of Mg to moles of O2 is 2:1. Therefore, to calculate the number of moles of Mg required, we multiply the number of moles of O2 by the ratio:
Number of moles of Mg = 0.5 mol O2 x 2 mol Mg / 1 mol O2
= 1 mol
Hence, 1 mole of magnesium is needed to react with 16 g of O2.