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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

Sagot :

Onyebuchinnajiidn

H₂O₂(aq)  has a slow rate at 298K because the activation energy is relatively high.

What is activation energy?

Activation energy is the minimum amount of energy that must be provided for compounds to result in a chemical reaction.

If  the decomposition of H₂O₂(aq) is thermodynamically favorable but H₂O₂(aq) is typically stable for up to a year stored in a dark bottle at 298K, then we can conclude that, H₂O₂(aq)  has a slow rate at 298K because the activation energy is relatively high.

Learn more about activation energy here: https://brainly.com/question/26724488

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