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Nsubuga writes down the hazards of the investigation. Complete the table to show how to control these risks.

\begin{tabular}{|l|l|}
\hline
Hazard & How to Control \\
\hline
Magnesium is highly flammable and can catch fire & \\
\hline
Burning magnesium has a very bright flame & \\
\hline
\end{tabular}

Nsubuga writes down his results as follows:
- Mass of crucible + lid = [tex]$32.00 \, \text{g}$[/tex]
- Mass of magnesium = [tex]$0.24 \, \text{g}$[/tex]
- Mass of crucible + lid + magnesium oxide = [tex]$32.40 \, \text{g}$[/tex]

i) Calculate the mass of magnesium oxide formed (2 marks)



Answer :

GinnyAnswer
Alright, let's go through the steps to calculate the mass of magnesium oxide formed.

### Given Data:
1. Mass of crucible and lid = 32.00 g
2. Mass of magnesium = 0.24 g
3. Mass of crucible, lid, and magnesium oxide = 32.40 g

### Calculation Steps:

1. First, determine the combined mass of the crucible and lid.
[tex]\[ \text{Mass of crucible + lid} = 32.00 \, \text{g} \][/tex]

2. Next, find the total mass after the reaction, which includes the mass of crucible, lid, and the newly formed magnesium oxide.
[tex]\[ \text{Mass of crucible + lid + magnesium oxide} = 32.40 \, \text{g} \][/tex]

3. To find the mass of the magnesium oxide formed, subtract the mass of the crucible and lid from the total mass.
[tex]\[ \text{Mass of magnesium oxide} = (\text{Mass of crucible + lid + magnesium oxide}) - (\text{Mass of crucible + lid}) \][/tex]

4. Plug in the given values to solve for the mass of magnesium oxide:
[tex]\[ \text{Mass of magnesium oxide} = 32.40 \, \text{g} - 32.00 \, \text{g} \][/tex]

5. Subtract the values:
[tex]\[ \text{Mass of magnesium oxide} = 0.40 \, \text{g} \][/tex]

### Final Answer:
The mass of magnesium oxide formed is 0.40 g.

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