Ammonium nitrate is an oxidizing agent and can give rise to explosive mixtures of mixture of two moles of powdered aluminum and 3 moles of ammonium nitrate crystals react exothermically yielding nitrogen gas water vapor and aluminum oxide how many grams of the mixture are required to provide 245 kilojoules of heat see appendix C for data.

I pretty much don't really know where to start or how to do it at all.... Also, could you use domino format please? (It's the only format she'll accept)

THANK YOU SO MUCH FOR HELPING♡♡

I have no idea what the domino format is.

To solve this problem, we will follow these steps:

Step 1: Write and balance the chemical equation.
Step 2: Calculate the molar mass of the mixture.
Step 3: Convert heat energy to moles.
Step 4: Use stoichiometry to relate moles of reactants and products.
Step 5: Convert moles of the mixture to grams.

Now let's go through each step in a domino format:

Step 1: Write and balance the chemical equation.
2Al (s) + 3NH4NO3 (s) → Al2O3 (s) + 3N2 (g) + 6H2O (g)

Step 2: Calculate the molar mass of the mixture.
The molar mass of aluminum (Al) is 26.98 g/mol.
The molar mass of ammonium nitrate (NH4NO3) is 80.04 g/mol.
To calculate the molar mass of the mixture, we need to consider the number of moles of aluminum and ammonium nitrate used in the reaction.

Step 3: Convert heat energy to moles.
We need to use the data provided in Appendix C to convert kilojoules of heat to moles of the mixture.

Step 4: Use stoichiometry to relate moles of reactants and products.
Using the balanced chemical equation, we can determine the mole ratio between the mixture and the heat produced. In this case, the mole ratio is 245 kilojoules of heat to the mole ratio of the mixture.

Step 5: Convert moles of the mixture to grams.
With the mole ratio obtained in the previous step, we can convert moles of the mixture to grams using the molar mass of the mixture.

I hope this explanation helps! Please let me know if you need further assistance.