in the reaction of aluminium and iron (III) oxide to form iron and aluminium oxide, H-850 kJ. how many grams of aluminium oxide are formed when 350 kJ are released?

2Al(s) + Fe2O3 -- Fe(s) + Al2O3(s) H=-850 kJ

Is that delta H for the reaction as written? If so then,

molar mass Al2O3 x (350/850) = ?

84g is one of the options.

To determine the grams of aluminium oxide formed when 350 kJ are released in the reaction, we need to calculate the moles of aluminium oxide formed and then convert it to grams using the molar mass of aluminium oxide.

Step 1: Determine the moles of aluminium oxide formed.
From the balanced chemical equation:
2Al(s) + Fe2O3(s) → Fe(s) + Al2O3(s)

The balanced equation shows that for every 2 moles of aluminium, 1 mole of aluminium oxide is formed. However, we don't know how many moles of aluminium are initially present. So, we need to calculate it.

Step 2: Calculate the moles of aluminium.
To calculate the moles of aluminium, we need to know the molar mass of aluminium. The molar mass of aluminium (Al) is approximately 27 g/mol.

Step 3: Calculate the grams of aluminium.
To calculate the grams of aluminium, divide the given energy change by the enthalpy change per mole (850 kJ/mol) and multiply by the molar mass of aluminium (27 g/mol).
Grams of aluminium = (350 kJ / -850 kJ/mol) * 27 g/mol

Step 4: Calculate the moles of aluminium oxide formed.
Since 2 moles of aluminium oxide are formed for every 2 moles of aluminium, the moles of aluminium oxide formed will be equal to the moles of aluminium.

Step 5: Calculate the grams of aluminium oxide formed.
Multiply the moles of aluminium oxide formed by the molar mass of aluminium oxide. The molar mass of aluminium oxide (Al2O3) is approximately 101.96 g/mol.
Grams of aluminium oxide = moles of aluminium oxide * molar mass of aluminium oxide

Now, let's perform the calculations:

Grams of aluminium = (350 kJ / -850 kJ/mol) * 27 g/mol
Grams of aluminium = -10.294 g (rounded to 3 decimal places)

Since the moles of aluminium oxide formed are equal to the moles of aluminium, the grams of aluminium oxide formed will also be -10.294 g (rounded to 3 decimal places).

Therefore, when 350 kJ are released in this reaction, approximately 10.294 grams of aluminium oxide are formed.

To determine the number of grams of aluminum oxide formed when 350 kJ of energy are released, we need to calculate the amount of energy released per mole of reaction and then use the energy change to find the number of moles of reaction. Finally, we can convert moles of aluminum oxide to grams using its molar mass.

Here's how you can calculate it:

1. Calculate the moles of reaction that correspond to the energy change:
- The energy change for the reaction is ΔH = -850 kJ.
- Use the balanced equation to determine the stoichiometry of the reaction:
2Al + Fe2O3 → Fe + Al2O3
The stoichiometric ratio between the reactant (Fe2O3) and the product (Al2O3) is 1:1.
- Since the reaction produces 1 mole of Al2O3 to release 850 kJ, for every -850 kJ released, you have 1 mole of Al2O3.

2. Calculate the moles of reaction for the given energy change (350 kJ):
- Determine the moles of reaction using the energy change ratio:
Moles of reaction = (Energy change of interest ÷ Energy per mole of reaction)
Moles of reaction = (350 kJ ÷ -850 kJ/mole)

3. Convert moles of reaction to grams of aluminum oxide:
- Determine the molar mass of Al2O3:
Molar mass of Al2O3 = (2 x Molar mass of Al) + (3 x Molar mass of O)
Molar mass of Al2O3 = (2 x 26.98 g/mol) + (3 x 16.00 g/mol)
- Multiply moles of reaction by the molar mass of Al2O3 to get the mass:
Mass of Al2O3 = Moles of reaction x Molar mass of Al2O3

By following these steps, you should be able to calculate the grams of aluminum oxide formed.