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3.d) Determine the formula of the white powder.

The empirical formula is determined using the percentage composition of each element and their atomic masses.

Write down the percentage of each element.
Percentage of Magnesium (Mg) = $60.3\%$
Percentage of Oxygen (O) = $100\% - 60.3\% = 39.7\%$
Convert percentages to mass (assume 100 g of the compound).
Mass of Mg = $60.3 \text{ g}$
Mass of O = $39.7 \text{ g}$
Calculate the number of moles for each element.
Atomic mass of Mg = 24
Atomic mass of O = 16
$\text{Moles of Mg} = \frac{60.3 \text{ g}}{24 \text{ g/mol}} = 2.5125 \text{ mol}$ $\text{Moles of O} = \frac{39.7 \text{ g}}{16 \text{ g/mol}} = 2.48125 \text{ mol}$
Find the simplest mole ratio by dividing each number of moles by the smallest number of moles.
The smallest number of moles is $2.48125 \text{ mol}$ .
$\text{Ratio for Mg} = \frac{2.5125}{2.48125} \approx 1.01$ $\text{Ratio for O} = \frac{2.48125}{2.48125} = 1$
The simplest mole ratio is approximately $1:1$ .
Write the empirical formula.
The empirical formula is MgO.
The formula mass of MgO = $24 + 16 = 40$ . This matches the given RFM of 40. Therefore, the molecular formula is also MgO.

The formula of the white powder is: $\boxed{\text{MgO}}$

3.a) State and explain the name of the white powder formed.

The name of the white powder is Magnesium Oxide.
This powder is formed when magnesium (a metal) burns in air, reacting with oxygen (a gas) to form an ionic compound.

3.b) State four properties of the white powder.

Four properties of magnesium oxide are:
- It is a white solid.
- It has a very high melting point.
- It is a basic oxide (reacts with acids).
- It is a refractory material, meaning it can withstand extremely high temperatures.
3.c) State the application of the white powder in medical industry.

In the medical industry, magnesium oxide is used as an antacid to relieve heartburn and indigestion by neutralizing stomach acid.

3.e) Write down one environmental impact of the white powder and suggest the mitigation.

Environmental impact: The production of magnesium oxide is an energy-intensive process, often relying on fossil fuels, which leads to greenhouse gas emissions contributing to climate change.
Mitigation: Utilizing renewable energy sources (such as solar or wind power) and improving energy efficiency in production processes.

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Step-by-step solution

Write down the percentage of each element.

Convert percentages to mass (assume 100 g of the compound).

Calculate the number of moles for each element.

Find the simplest mole ratio by dividing each number of moles by the smallest number of moles.

Write the empirical formula.

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