The rate equation for the overall equation is:
`H_(3)AsO_(4) (aq)+2H^(o+) + 3I^(Θ)(aq) underset(k_(r ))overset(k_(f))hArr H_(3)AsO_(3)(aq)+I_(3)^(Θ)(eq)+H_(2)O(l)`
`(d[I_(3)^(ɵ)])/(dt)=k_(f)[H_(3)AsO_(4)][I^(ɵ)][H^(o+)]-k_(f)([H_(3)AsO_(3)][I^(ɵ)3])/{[I^(ɵ)]^(2)[H^(o+)])`
where `k_(f)= 4.7xx10^(-4)L^(2)mol^(-2)mi n^(-1)` and
`k_(r )= 3xx10^(-3)mol^(2)L^(-2)min^(-1)`
Determine the equilibrium constant for this reaction form the rate constants.

Explanation

To determine the equilibrium constant \( K_{eq} \) for the given reaction from the rate constants \( k_f \) (forward rate constant) and \( k_r \) (reverse rate constant), we can use the relationship between these constants.

### Step-by-step solution:

1. **Identify the Reaction**:
The reaction is given as:
\[
H_3AsO_4 (aq) + 2H^+ + 3I^- \rightleftharpoons H_3AsO_3 (aq) + I_3^- + H_2O (l)
...