To determine how much heat (in kJ) is produced by the decomposition of 1.25 moles of hydrogen peroxide (\(H_2O_2\)) under standard conditions, we can use the standard enthalpy change of reaction (\(ΔH^0_{rxn}\)) provided in the Supplemental Data.
The decomposition of hydrogen peroxide is represented by the following balanced chemical equation:
\[2H_2O_2(l) → 2H_2O(l) + O_2(g)\]
From the data, we can find \(ΔH^0_{rxn}\) for this reaction. It's important to note that the coefficients in the balanced equation represent moles of substances reacting, so the \(ΔH^0_{rxn}\) value applies to the reaction of 2 moles of \(H_2O_2\).
Now, we'll calculate the heat produced when 1.25 moles of \(H_2O_2\) decompose:
1. Calculate \(ΔH^0_{rxn}\) for the decomposition of 2 moles of \(H_2O_2\) using the data provided.
2. Divide the calculated \(ΔH^0_{rxn}\) by 2 to find \(ΔH^0_{rxn}\) for the decomposition of 1 mole of \(H_2O_2\).
3. Multiply \(ΔH^0_{rxn}\) by 1.25 to find the heat produced when 1.25 moles of \(H_2O_2\) decompose.
Performing these calculations will give you the heat produced in kJ when 1.25 moles of \(H_2O_2\) decompose under standard conditions. If you encounter any specific values from the data that need further explanation or calculation, please provide them, and I can assist further.