Overall reaction: 2 H2O2(l) → 2 H2O(l) + O2(g)
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
Decomposition reaction: 2 H2O2(l) → 2 H2(g) + 2 O2(g)
Formation equation: 2 H2(g) + 2 O2(g) → 2 H2O(l) + O2(g)
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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