To predict the mass of magnesium oxide (MgO) produced from the complete reaction of magnesium (Mg) and oxygen (O₂), we need to know the mass of the magnesium used in the experiment.
Here's a general approach to calculate the mass of magnesium oxide produced:
-
Determine the molar mass of reactants:
- Molar mass of magnesium (Mg) = ~24.31 g/mol
- Molar mass of oxygen (O₂) = ~32.00 g/mol
- Molar mass of magnesium oxide (MgO) = 24.31 g/mol + 16.00 g/mol = ~40.31 g/mol
-
Write the balanced chemical equation: \[ 2 , \text{Mg} + \text{O}_2 \rightarrow 2 , \text{MgO} \]
-
Calculate the amount of magnesium used: If you have the mass of magnesium (let's say it's \( m \) grams):
\[ \text{Moles of Mg} = \frac{m}{24.31} \]
-
Use the mole ratio from the balanced equation: From the equation, 2 moles of Mg produce 2 moles of MgO. This means 1 mole of Mg produces 1 mole of MgO.
-
Calculate the moles of MgO produced: The moles of MgO produced will equal the moles of magnesium used: \[ \text{Moles of MgO produced} = \text{Moles of Mg} = \frac{m}{24.31} \]
-
Calculate the mass of MgO produced: \[ \text{Mass of MgO} = \text{Moles of MgO} \times 40.31 \] \[ = \left(\frac{m}{24.31}\right) \times 40.31 \]
Once you have the mass \( m \) of the magnesium used, you can plug in that value to find the predicted mass of magnesium oxide produced.
If you provide the mass of magnesium, I can calculate the exact mass of magnesium oxide produced.