Question

Experiment 3:%0D%0A%0D%0A%0D%0A%0D%0A(1 point)%0D%0A6. Assuming the magnesium and oxygen will react completely with one another, predict the mass of magnesium oxide that will be produced. %0D%0A%0D%0AMagnesium Oxide:

Answer 1

the magnesium is 12.2g

Answer 2

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:

1. **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

2. **Write the balanced chemical equation**:
\[
2 \, \text{Mg} + \text{O}_2 \rightarrow 2 \, \text{MgO}
\]

3. **Calculate the amount of magnesium used**:
If you have the mass of magnesium (let's say it's \( m \) grams):

\[
\text{Moles of Mg} = \frac{m}{24.31}
\]

4. **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.

5. **Calculate the moles of MgO produced**:
The moles of MgO produced will equal the moles of magnesium used:
\[
\text{Moles of MgO produced} = \text{Moles of Mg} = \frac{m}{24.31}
\]

6. **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.

Answer 3

Given that you have 12.2 g of magnesium (Mg), we can calculate the mass of magnesium oxide (MgO) produced from its reaction with oxygen using the steps outlined earlier.

### Step 1: Calculate moles of magnesium
The molar mass of magnesium (Mg) is approximately 24.31 g/mol.

\[
\text{Moles of Mg} = \frac{\text{mass}}{\text{molar mass}} = \frac{12.2 \, \text{g}}{24.31 \, \text{g/mol}} \approx 0.502 \, \text{mol}
\]

### Step 2: Use the mole ratio
From the balanced chemical equation:
\[
2 \, \text{Mg} + \text{O}_2 \rightarrow 2 \, \text{MgO}
\]
1 mole of Mg produces 1 mole of MgO. Thus, the moles of MgO produced will also be approximately 0.502 moles.

### Step 3: Calculate the mass of magnesium oxide produced
The molar mass of magnesium oxide (MgO) is approximately 40.31 g/mol.

\[
\text{Mass of MgO} = \text{moles of MgO} \times \text{molar mass of MgO}
\]
\[
\text{Mass of MgO} = 0.502 \, \text{mol} \times 40.31 \, \text{g/mol} \approx 20.23 \, \text{g}
\]

### Conclusion
Approximately **20.23 g** of magnesium oxide (MgO) will be produced from the complete reaction of 12.2 g of magnesium.