How many kilocalories are required to produce 12.7g of aluminum?

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12 To calculate the number of kilocalories required to produce 12.7g of aluminum, we need to know the heat of formation value for aluminum. The heat of formation is the amount of energy released or absorbed during the formation of 1 mole of a substance from its pure elements under standard conditions.

However, since we're given the mass of aluminum (12.7g) instead of the number of moles, we need to convert it to moles first. To do this, we need the molar mass of aluminum, which is 26.98 g/mol.

By using the formula:

moles = mass / molar mass

we can calculate the number of moles of aluminum:

moles = 12.7g / 26.98 g/mol

Now, we can proceed to calculate the energy required. Since the heat of formation is given per mole, we can use the following formula:

energy = heat of formation × moles

However, the heat of formation for aluminum is not readily available. Instead, we can estimate the energy required using the heat of fusion. The heat of fusion tells us the amount of energy needed to melt one mole of a substance. For aluminum, the heat of fusion is approximately 10.7 kilocalories per mole.

So, the estimation of the energy required would be:

energy ≈ heat of fusion × moles

Now we can substitute the values:

energy ≈ 10.7 kcal/mol × (12.7g / 26.98 g/mol)

By performing the calculation, we find:

energy ≈ 5.032 kilocalories