Here's a breakdown:
* Water (H2O): MgO can react with water to form magnesium hydroxide (Mg(OH)2). This reaction is particularly relevant when MgO is exposed to humid environments.
* Carbon Dioxide (CO2): MgO can react with CO2 to form magnesium carbonate (MgCO3). This reaction is more likely to occur in the presence of moisture, as water acts as a catalyst.
These reactions can complicate quantitative studies of MgO because:
* They change the composition of the sample: The formation of Mg(OH)2 or MgCO3 alters the chemical makeup of the original MgO, affecting measurements.
* They introduce errors in analysis: If the presence of these compounds is not accounted for, it can lead to inaccurate measurements of the amount of MgO present.
To minimize these problems, researchers often:
* Store MgO in airtight containers: This helps to minimize exposure to moisture and CO2.
* Perform experiments in a controlled atmosphere: This could involve using a dry box or inert gas purging to remove moisture and CO2.
* Account for the presence of these compounds in analysis: This may involve using specific analytical techniques or applying correction factors to account for the presence of Mg(OH)2 and MgCO3.
It's important to be aware of these potential reactions when conducting quantitative studies of MgO to ensure accurate and reliable results.
