A chemical reaction occurs when aluminum oxide (Al2O3) is exposed to oxygen, resulting in the format...

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As a university professor, the first step is to carefully read and understand the given information. We are given a chemical reaction where aluminum oxide (Al2O3) is exposed to oxygen, resulting in the formation of aluminum oxide (Al2O3) and the release of energy. We are also given the amount of aluminum oxide (Al2O3) that is being oxidized, which is 2 moles. Additionally, we are given the standard enthalpy change for the formation of aluminum oxide (Al2O3), which is -1676 kJ/mol.

Step 2: Write the balanced chemical equation
The next step is to write the balanced chemical equation for the given reaction. This will help us determine the mole ratio between aluminum oxide (Al2O3) and oxygen. The balanced chemical equation for the reaction is:

2Al2O3 + 3O2 → 4Al2O3

Step 3: Determine the mole ratio
From the balanced chemical equation, we can see that for every 2 moles of aluminum oxide (Al2O3) that is oxidized, 3 moles of oxygen are required. This means that the mole ratio between aluminum oxide (Al2O3) and oxygen is 2:3.

Step 4: Calculate the moles of oxygen required
Since we are given 2 moles of aluminum oxide (Al2O3), we can use the mole ratio to calculate the moles of oxygen required for the reaction to reach completion. This can be done using the following calculation:

2 moles Al2O3 x (3 moles O2 / 2 moles Al2O3) = 3 moles O2

Therefore, 3 moles of oxygen are required for the reaction to reach completion.

Step 5: Calculate the energy released
To calculate the energy released during the oxidation process, we will use the standard enthalpy change given to us (-1676 kJ/mol). The energy released can be calculated using the following formula:

Energy released = Standard enthalpy change x Moles of reactant

Substituting the values, we get:

Energy released = -1676 kJ/mol x 2 moles Al2O3 = -3352 kJ

Therefore, the energy released during the oxidation process is -3352 kJ or 3352 kJ (since the negative sign indicates that energy is being released).

Step 6: Convert energy to joules
The energy released is given in kilojoules (kJ), but we can convert it to joules (J) for easier understanding. This can be done by multiplying the energy released by 1000. Therefore, the energy released in joules is:

3352 kJ x 1000 = 3,352,000 J

Step 7: Final answer
To summarize, 3 moles of oxygen are required for the reaction to reach completion and the energy released during the oxidation process is 3,352,000 joules.

Final Answer:
3 moles of oxygen are required for the reaction to reach completion and the energy released during the oxidation process is 3,352,000 joules.