Using your mass of Mg (0.101g), and assuming all of the Mg burns in oxygen and forms the theoretical predicted product, calculate the theoretical yield of magnesium oxide.
I wrote out the equation and it turned out to be:
2Mg+O2->2MgO
I have my mass of Mg but how do I get to the theoretical yield of how much MgO is formed? Thanks in advance!
I tried doing some conversion factors and came up with this:
(0.101g Mg)(1mol MgO) |(40.31g MgO)
----------------------
(24.31g Mg)|(1mol MgO)
=~0.167g MgO as my theoretical yield if I had a mass of 0.101g of Mg
Did I do this correctly?
To calculate the theoretical yield of magnesium oxide (MgO), you need to follow these steps:
1. Determine the molar mass of magnesium (Mg) and magnesium oxide (MgO).
- The molar mass of Mg is approximately 24.305 g/mol.
- The molar mass of MgO is approximately 40.304 g/mol.
2. Convert the given mass of Mg to moles.
- Divide the mass of Mg (0.101 g) by its molar mass (24.305 g/mol) to get the number of moles of Mg.
- Moles of Mg = Mass of Mg / Molar mass of Mg
3. Use the balanced equation to determine the stoichiometry.
- According to the balanced equation, 2 moles of Mg react with 1 mole of O2 to produce 2 moles of MgO.
- This implies that the mole ratio of Mg to MgO is 2:2 (or 1:1).
4. Calculate the theoretical yield of MgO.
- Since the mole ratio of Mg to MgO is 1:1, the number of moles of Mg is equal to the number of moles of MgO.
- The theoretical yield of MgO is the same as the number of moles of MgO formed.
- Moles of MgO = Number of moles of Mg
5. Convert moles of MgO to grams.
- Multiply the number of moles of MgO by its molar mass to obtain the mass of MgO.
- Mass of MgO = Moles of MgO * Molar mass of MgO
So, to calculate the theoretical yield of MgO, follow these steps:
1. Divide the given mass of Mg (0.101 g) by its molar mass (24.305 g/mol) to find the number of moles of Mg.
2. The number of moles of Mg corresponds to the number of moles of MgO formed.
3. Multiply the number of moles of MgO by the molar mass of MgO (40.304 g/mol) to determine the mass of MgO formed.
Keep in mind that the theoretical yield assumes ideal conditions and complete conversion of the reactants. In practice, the actual yield may be lower due to various factors like incomplete reactions and side reactions.