A combustion bomb containing 5.417 g of aluminum metal and 15.974 g of iron III oxide is placed in an ice calorimeter that initially contained 7.746 kg of ice (at o degrees C) and 7.894 kg of liquid water (at o degrees C). The reaction, once ignited by remote control, forms pure iron and aluminum oxide. It is observed that the calorimeter contains 7.493 kg of ice and 8.147 kg of liquid water after the reaction. The heat of fusion of ice is 335 J/g. What is the enthalpy change for this reaction per mole of iron formed?

So far I have:

Al(s) + Fe2O3 (s) ----> AlO3 + 2Fe

am i supposed to include the ice and water in the balanced equation? what should i do next, i'm sort of lost.

The ice melting tells you the amount of heat released.

How much heat does it take to melt 7.893-7.393 kg of ice.

Then, having the energy, you can determine enthalpy based on the moles of iron formed. The reaction is a little tricky to figure moles of iron, you have to determine which is the limiting reactant.

To determine the enthalpy change per mole of iron formed, you need to first find the heat absorbed by the calorimeter. Then, you can use the heat absorbed value to calculate the enthalpy change using the stoichiometry of the balanced equation.

Let's proceed step-by-step:

1. Start with the balanced equation:

Al(s) + Fe2O3(s) → Al2O3(s) + 2Fe(s)

2. Determine the moles of aluminum (Al) and iron III oxide (Fe2O3):

To find the moles, divide the mass of each substance by its molar mass.
- Moles of Al = Mass of Al / Molar mass of Al (27 g/mol)
- Moles of Fe2O3 = Mass of Fe2O3 / Molar mass of Fe2O3 (160 g/mol)

3. Calculate the limiting reagent:

Compare the mole ratio of Al to Fe2O3 in the balanced equation. The reactant with the smaller mole ratio is the limiting reagent, meaning it will be completely consumed first.

4. Calculate the heat absorbed by the calorimeter:

The heat absorbed is equal to the heat released by the reaction and used to melt ice, so:
- Heat absorbed = (mass of melted ice + mass of liquid water) × heat of fusion of ice

Note: You need to convert the masses from kg to grams before calculating the heat absorbed.

5. Convert the heat absorbed to J/mol using the mole ratio between Fe and the heat absorbed.

For every 2 moles of Fe produced, a certain amount of heat is absorbed. Hence, to find the enthalpy change per mole of Fe, divide the heat absorbed by the moles of Fe produced.

Finally, substitute the values into the equation:
Enthalpy change per mole of Fe = Heat absorbed / (moles of Fe × 2)

Remember to convert the unit of heat absorbed to J/mol.

Once you perform these calculations, you will be able to find the enthalpy change per mole of iron formed.