When rate `= k[A]^(2)[B]`, the reaction is said to be of …………….order in `A` and of………..order in `B`. The order of the overall reaction will be sum of the………..of `A` and `B`.

Answer

To solve the question, we need to analyze the given rate equation and determine the order of the reaction with respect to each reactant and the overall order of the reaction.

### Step-by-Step Solution:

1. **Identify the Rate Expression**:
The rate of the reaction is given by the expression:
\[ \text{Rate} = k[A]^2[B]^1 \]

2. **Determine the Order with Respect to A**:
In the rate expression, the exponent of [A] is 2. The order of the reaction with respect to a reactant is defined by the exponent of that reactant in the rate expression. Therefore, the reaction is:
\[ \text{Second order in } A \]

3. **Determine the Order with Respect to B**:
In the rate expression, the exponent of [B] is 1. Thus, the order of the reaction with respect to B is:
\[ \text{First order in } B \]

4. **Calculate the Overall Order of the Reaction**:
The overall order of the reaction is the sum of the orders with respect to each reactant. Therefore, we add the orders:
\[ \text{Overall order} = \text{Order in } A + \text{Order in } B = 2 + 1 = 3 \]

### Final Answer:
- The reaction is said to be of **second order in A** and **first order in B**.
- The overall order of the reaction will be the sum of the **orders of A and B**, which is **3**.