You measured out 0.101g of Mg. You heat the sample and measure out 0.234 of the magnesium oxide compound. Given your data, what us the empirical formula for the Mg(x)O(y)? x and y are ratio x:y
If I'm doing this correctly, I divided 0.101g of Mg/24.31g of Mg = .00415 mol Mg
But I'm stuck on what to do next or even if my first step is correct or not. Help please?
mass of O2: .234-.101 grams=.131g
moles O2: .131/32=.004
Moles Mg= .101/24=.004
divide both by the lower
Moles O2= 1
moles Mg=1
MgO2 is what you got.
I understand your math, but where did Oxygen started with 2 of them to be O2? Is it because of the charges?
If you had used mols O
you would have had .13/.16 = .008
or two mols of O for every one of Mg
so it would have been MgO2 anyway :)
I mean .131/16 = .008 mols O
IT STATE THAT IF A CHEMICAL IS IN EQUILIBRIUM AND ARE OF THE FACTORS INVOLVED IN THE EQUILIBRIUM WILL SHIFT.
Your first step is correct. You correctly converted the mass of magnesium (Mg) to moles of Mg by dividing by the molar mass of Mg (24.31 g/mol).
Now, to determine the empirical formula, you need to find the ratio of moles of Mg to moles of oxygen (O).
You stated that the mass of the magnesium oxide (MgO) compound formed is 0.234 g. First, we need to find the mass of oxygen (O) in this compound:
Mass of oxygen (O) = Mass of magnesium oxide (MgO) - Mass of magnesium (Mg)
Mass of oxygen (O) = 0.234 g - 0.101 g = 0.133 g
Now, we can convert the mass of oxygen (O) to moles of oxygen (O) using the molar mass of oxygen (O, 16.00 g/mol):
Moles of oxygen (O) = Mass of oxygen (O) / Molar mass of oxygen (O)
Moles of oxygen (O) = 0.133 g / 16.00 g/mol = 0.00831 mol O
Now, we have the moles of magnesium (Mg) and the moles of oxygen (O). To find the ratio of moles, we need to divide both by the smaller value.
Dividing both moles of magnesium (Mg) and moles of oxygen (O) by 0.00831 mol (the smaller value), we get:
Moles of Mg: Moles of O = 0.00415 mol Mg / 0.00831 mol O : 0.00831 mol O / 0.00831 mol O
Simplifying, we have:
Moles of Mg: Moles of O = 0.5 : 1
This means the ratio of moles of magnesium (Mg) to oxygen (O) is 1:2, and the empirical formula for the magnesium oxide compound is MgO.
The empirical formula MgO indicates that for every magnesium atom, there are two oxygen atoms.