Question

Derive a mechanism for the reaction Hg²⁺ + Ti³⁺ → 2Hg²⁺ + Ti⁺ by applying the steady-state approximation.

Answer 1

The steady-state approximation suggests that the concentration of the intermediate species remains constant over time. In the reaction
`\( \text{Hg}^(2+) + \text{Ti}^(3+) \rightarrow 2\text{Hg}^(2+) + \text{Ti}^(+) \)`, applying this approximation implies setting the rate of formation equal to the rate of consumption for the intermediate species.

Step-by-step explanation:

In the steady-state approximation, the rate of formation
`(\(R_f\))` of the intermediate species is set equal to its rate of consumption
`(\(R_c\)).` For the reaction
`\( \text{Hg}^(2+) + \text{Ti}^(3+) \rightarrow 2\text{Hg}^(2+) + \text{Ti}^(+) \),` the reaction mechanism might involve the formation of an intermediate complex that rapidly equilibrates with the reactants and products. By assuming that the concentration of this intermediate species is constant, we can simplify the rate equations and gain insights into the overall reaction kinetics.

The steady-state approximation is a valuable tool in chemical kinetics, allowing for the simplification of complex reaction mechanisms. It is particularly useful when certain intermediates are formed and consumed rapidly. Understanding this approximation provides a deeper insight into reaction mechanisms and facilitates the analysis of complex chemical processes.