For a reaction, `I^(-) + OCl^(-) to IO^(-) + Cl^(-)` in an aqueous medium, the rate of reaction is given by `(d[IO^(-)])/(dt) = k ([I^(-)[OCl^(-)])/([OH^(-)]))`. The overall order of reaction is

Options

A. `-1`
B. 0
C. 1
D. 2

Explanation

To determine the overall order of the reaction given by the rate law:

\[ \frac{d[IO^-]}{dt} = k \frac{[I^-][OCl^-]}{[OH^-]} \]

we will follow these steps:

### Step 1: Identify the concentration terms in the rate equation
In the rate equation, we have three concentration terms:
- \([I^-]\)
- \([OCl^-]\)
- \([OH^-]\)

### Step 2: Determine the order with respect to each reactant
The order of the reaction with respect to each reactant is determined by the exponent of each concentration term in the rate law:
- For \([I^-]\), the exponent is 1 (since it is not explicitly raised to any power).
- For \([OCl^-]\), the exponent is also 1.
- For \([OH^-]\), the exponent is -1 (since it is in the denominator).

### Step 3: Calculate the overall order of the reaction
The overall order of the reaction is calculated by summing the orders of each reactant:
\[ \text{Overall order} = \text{Order with respect to } [I^-] + \text{Order with respect to } [OCl^-] - \text{Order with respect to } [OH^-] \]
Substituting the values:
\[ \text{Overall order} = 1 + 1 - 1 = 1 \]

### Conclusion
The overall order of the reaction is 1.