Problem: Consider the decomposition of liquid hydrogen peroxide (H2O2) to form water and oxygen.Draw a scale diagram of this reaction (1 cm = 100 kJ) that shows the relative energies of reactants (on the left), products (on the right), and the elements in their most stable states (in the middle). Label all the energies you know. What is the heat of reaction for the process?

FREE Expert Solution

Overall reaction: 2 H2O2(l) → 2 H2O(l) + O2(g)

Formation equations:

H2(g) + O2(g) → H2O2(l)            ΔH°f = -187.8 kJ/mol

H2(g) + 1/2 O2(g) → H2O(l)        ΔH°f = -285.8 kJ/mol

O2(g) → standard state →       ΔH°f = 0

Energy Diagram:

Decomposition reaction:  2 H2O2(l) → 2 H2(g) + 2 O2(g) 

Formation equation: 2 H2(g) + 2 O2(g) → 2 H2O(l) + O2(g) 

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Problem Details

Consider the decomposition of liquid hydrogen peroxide (H2O2) to form water and oxygen.

Draw a scale diagram of this reaction (1 cm = 100 kJ) that shows the relative energies of reactants (on the left), products (on the right), and the elements in their most stable states (in the middle). Label all the energies you know. What is the heat of reaction for the process?

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