For a reaction, `A+2B to C,` rate is given by `+(d[C])/(dt)=k[A][B],` hence, the order of the reaction is

Options

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

Explanation

To determine the order of the reaction given by the equation \( A + 2B \rightarrow C \) with the rate expression \( \frac{d[C]}{dt} = k[A][B] \), we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Rate Law Expression**:
The rate of the reaction is given as:
\[ \frac{d[C]}{dt} = k[A][B] \]
Here, \( k \) is the rate constant, and \( [A] \) and \( [B] \) are the concentrations of the reactants.

2. **Determine the Exponents in the Rate Law**:
In the rate law expression, the concentration of each reactant is raised to a power. In this case:
- The concentration of \( A \) is raised to the power of 1.
- The concentration of \( B \) is also raised to the power of 1.

3. **Sum the Exponents**:
The order of the reaction is defined as the sum of the powers of the concentrations of the reactants in the rate law expression. Thus, we calculate:
\[ \text{Order} = 1 \, (\text{from } [A]) + 1 \, (\text{from } [B]) = 2 \]

4. **Conclusion**:
Therefore, the order of the reaction \( A + 2B \rightarrow C \) is 2, which means it is a second-order reaction.

### Final Answer:
The order of the reaction is **2** (second order).

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