Explain why the disproportionation of bromine

Explain why the disproportionation of bromine in water is not thermodynamically feasible under standard conditions.

The disproportionation of bromine in water is not thermodynamically feasible under standard conditions due to the unfavourable change in Gibbs free energy. This process involves the conversion of bromine molecules into bromide ions and bromate ions, and it is characterised by a positive change in Gibbs free energy. According to thermodynamics, a positive change in Gibbs free energy indicates that the reaction is not spontaneous and will not occur under standard conditions. In the case of bromine disproportionation, the positive change in Gibbs free energy indicates that the reaction is not thermodynamically favourable.

Furthermore, the disproportionation of bromine in water is not thermodynamically feasible under standard conditions because it violates the second law of thermodynamics. The second law of thermodynamics states that in a closed system, the entropy of the system tends to increase over time. In the case of bromine disproportionation, the formation of bromide ions and bromate ions from bromine molecules results in a decrease in entropy, as the number of particles decreases. This decrease in entropy further contributes to the unfavourable change in Gibbs free energy, making the disproportionation of bromine in water thermodynamically unfeasible under standard conditions.

Moreover, the disproportionation of bromine in water is not thermodynamically feasible under standard conditions because it requires an input of energy to overcome the unfavourable change in Gibbs free energy. In order for the disproportionation of bromine to occur, energy must be supplied to drive the reaction towards the formation of bromide ions and bromate ions. This additional energy input makes the reaction non-spontaneous and not thermodynamically favourable under standard conditions. Therefore, the disproportionation of bromine in water is not feasible from a thermodynamic standpoint due to the unfavourable change in Gibbs free energy, violation of the second law of thermodynamics, and the requirement of additional energy input.

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