If in Part B.2, the burning of the magnesium is uncontrolled (burns brightly), how will this procedural error affect the reported mass of:

a Magnesium in the magnesium oxide? Explain.
B. oxygen in the magnesium oxide? Explain.

Let me explain and you do the rest.

Burning Mg in air leads both to MgO and Mg3N2.You want the MgO; you don't want the Mg3N2. The amount of MgO is reduced; the amount of oxygen in the MgO is reduced.

Ok, I think I get it now. Thank you so much!

If the burning of magnesium in Part B.2 is uncontrolled and burns brightly, it will affect the reported mass of both the magnesium and the oxygen in the magnesium oxide.

a) Magnesium in the magnesium oxide:
When magnesium burns in air, it reacts with oxygen to form magnesium oxide (MgO). The reaction can be represented as follows:
2Mg + O2 -> 2MgO

Magnesium oxide (MgO) is formed by the combination of one magnesium atom (Mg) with one oxygen atom (O). Therefore, the stoichiometric ratio of magnesium to magnesium oxide is 1:1. This means that for every one atom of magnesium, one atom of oxygen is required to form magnesium oxide.

Now, if the burning of magnesium is uncontrolled, it means that some of the magnesium may not react completely with oxygen to form magnesium oxide. Instead, it may partially burn or form other magnesium compounds. As a result, the reported mass of magnesium in the magnesium oxide will be lower than the actual amount present because some of the magnesium will be lost due to incomplete reaction or side reactions.

To obtain an accurate measurement of the mass of magnesium in the magnesium oxide, it is important to ensure that the burning is controlled and complete, allowing all the magnesium to react with oxygen to form magnesium oxide.

b) Oxygen in the magnesium oxide:
Since magnesium oxide is formed by the combination of one magnesium atom with one oxygen atom, the stoichiometric ratio of magnesium to oxygen in magnesium oxide is 1:1. This means that the mass of oxygen in the magnesium oxide can be determined by subtracting the mass of magnesium from the total mass of magnesium oxide.

If the burning of magnesium is uncontrolled, it can lead to incomplete reaction or side reactions. This means that the amount of magnesium oxide formed may not be accurate. Consequently, the reported mass of oxygen in the magnesium oxide will also be affected. It may be higher or lower than the actual amount present, depending on the extent of the incomplete reactions or side reactions that occur during the uncontrolled burning.

To obtain an accurate measurement of the mass of oxygen in the magnesium oxide, it is essential to ensure that the burning of magnesium is controlled and complete, allowing all the magnesium to react with oxygen and form magnesium oxide accurately.