2H2O2(aq)→2H2O(l)+O2(g)ΔG°=−234kJ/molrxn

The value of ΔG° for the reaction represented above implies that the decomposition of H2O2(aq) is thermodynamically favorable. However, H2O2(aq) is typically stable for up to a year stored in a dark bottle at 298K. The best explanation for this observation is that the decomposition reaction

a-is only thermodynamically favorable in the presence of a catalyst
b-occurs with an increase in entropy because O2(g) is a product
c- is reversible and H2O2(aq) is produced almost as fast as it decomposes
d-has a slow rate at 298K because the activation energy is relatively high