Question

The decomposition of hydrogen peroxide, H₂O₂, has been used to provide thrust in the control jets of various space vehicles. Using the data in Appendix G, determine how much heat is produced by the decomposition of exactly 1 mole of H₂O₂ under standard conditions.

2H₂O₂(l)⟶2H₂O(g)+O₂(g)

Answer 1

To determine the heat produced during the decomposition of 1 mole of hydrogen peroxide, one uses standard enthalpy of formation values (ΔH°f) from an appendix and applies Hess's law. The specific numerical answer requires data from Appendix G, which is not provided.

Step-by-step explanation:

The question asks to determine how much heat is produced by the decomposition of hydrogen peroxide (H2O2) under standard conditions. The balanced chemical equation given is 2H2O2(l) → 2H2O(g) + O2(g).

To find the heat produced, we look up the standard enthalpy of formation (ΔH°f) values for the reactants and products in Appendix G. The enthalpy change for the reaction (ΔH°rxn) is calculated using Hess's law:

ΔH°rxn = ∑ΔH°f(products) - ∑ΔH°f(reactants)

Without the actual values from Appendix G, we cannot provide a numerical answer.

However, with the data at hand, we would substitute the ΔH°f values for each compound into the equation, remembering to take into account the stoichiometry of the reaction.

Given that the decomposition of 1 mole of H2O2 is needed, the calculated ΔH°rxn would represent the heat produced for the decomposition of exactly 1 mole of H2O2.