How many moles of magnesium are needed to react with 16 g of O2?
2 MgO (s) + O2 (g) → 2 MgO (s)
Well, let's do some mole math, shall we? The molar mass of O2 is 32 g/mol and the molar mass of Mg is 24.31 g/mol. So, the number of moles of O2 can be calculated by dividing the mass by the molar mass:
16 g O2 / 32 g/mol = 0.5 moles of O2
According to the balanced equation, the ratio of moles between Mg and O2 is 2:1. Since magnesium reacts with oxygen in a 1:1 ratio, we need the same number of moles of magnesium as moles of oxygen:
0.5 moles of O2 × 2 moles of Mg / 1 mole of O2 = 1 mole of Mg
So, you would need 1 mole of magnesium to react with 16 g of O2. Just be careful not to mix up the moles with furry little underground mammals. Moles the unit, not moles the burrowing creature.
To determine the number of moles of magnesium needed to react with 16 g of O2, we need to use the balanced equation and the molar masses of the substances involved.
1. First, find the molar mass of O2 (oxygen gas):
- The molar mass of oxygen (O) is 16.00 g/mol.
- Since there are two oxygen atoms in O2, the molar mass of O2 is 2 * 16.00 g/mol = 32.00 g/mol.
2. Next, use the molar mass of O2 to convert the given mass to moles:
- Moles of O2 = Mass of O2 / Molar mass of O2
- Moles of O2 = 16 g / 32.00 g/mol = 0.50 mol
3. According to the balanced equation, the stoichiometric ratio between magnesium (Mg) and O2 is 2:1. This means that 2 moles of Mg react with 1 mole of O2.
4. Use the stoichiometric ratio to determine the number of moles of magnesium required:
- Moles of Mg = (Moles of O2) * (2 moles of Mg / 1 mole of O2)
- Moles of Mg = 0.50 mol * (2/1) = 1.00 mol
Therefore, 1 mol of magnesium is needed to react with 16 g of O2.
To determine the number of moles of magnesium required to react with 16 g of O2, we will follow these steps:
1. Determine the molar mass of O2.
The molar mass of O2 is calculated by adding the atomic masses of oxygen (O). Since O2 has two oxygen atoms, the atomic mass of oxygen (O) is 16 g/mol. So, the molar mass of O2 is 16 g/mol x 2 = 32 g/mol.
2. Convert the given mass of O2 to moles.
We can use the formula: Moles = Mass / Molar mass
Moles of O2 = 16 g / 32 g/mol = 0.5 moles
3. Use the stoichiometry ratio from the balanced equation to determine the number of moles of magnesium required.
From the balanced equation, we can see that 1 mole of O2 reacts with 2 moles of Mg. Therefore, the number of moles of magnesium (Mg) required will be twice the moles of O2.
Moles of Mg = Moles of O2 x 2 = 0.5 moles x 2 = 1 mole
So, 1 mole of magnesium is needed to react with 16 g of O2.
I think I worked this for you last night. First you need to correct the equation to
2Mg + O2 --> 2MgO
mols O2 = grams/molar mass = 16/32 = 0.5
0.5 mol O2 x (2 mol Mg/1 mol O2) = 0.5 x 2/1 = 1 mol Mg