For a hypothetical reaction: `A+B rarr` Products, the rate law is `r = k[A][B]^(0)`. The order of reaction is

Options

A. `0`
B. `1`
C. `2`
D. `3`

Explanation

To determine the order of the reaction for the given rate law \( r = k[A][B]^0 \), we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Rate Law**: The rate law is given as \( r = k[A][B]^0 \). Here, \( k \) is the rate constant, and \( [A] \) and \( [B] \) are the concentrations of the reactants A and B, respectively.

2. **Analyze the Exponents**: In the rate law, the exponent of \( [A] \) is 1 (since it is not written explicitly, it is assumed to be 1), and the exponent of \( [B] \) is 0 (as indicated by \( [B]^0 \)).

3. **Calculate the Order of Reaction**: The order of a reaction is defined as the sum of the powers of the concentrations of the reactants in the rate law. Therefore, we can calculate the order as follows:
\[ \text{Order of Reaction} = \text{Exponent of } [A] + \text{Exponent of } [B] = 1 + 0 = 1 \]

4. **Conclusion**: The total order of the reaction is 1.

### Final Answer:
The order of the reaction is **1**.

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