If the rate constant k of a reaction is `1.6 times 10^–3(mol//l)(min^–1)` . The order of the reaction is:

Options

A. 0
B. 1
C. 2
D. cannot be predicted

Answer

To determine the order of the reaction based on the given rate constant \( k = 1.6 \times 10^{-3} \, \text{mol L}^{-1} \text{min}^{-1} \), we can analyze the units of the rate constant.

### Step-by-Step Solution:

1. **Identify the Units of the Rate Constant:**
The given rate constant \( k \) has the units of \( \text{mol L}^{-1} \text{min}^{-1} \).

2. **Use the General Formula for Rate Constants:**
The units of the rate constant \( k \) for a reaction of order \( n \) can be expressed as:
\[ k = \frac{\text{mol L}^{-1}}{\text{time}} = \text{mol L}^{-1} \text{time}^{-1} \]
The general formula for the units of \( k \) is:
\[ k \sim \text{mol}^{1-n} \text{L}^{n-1} \text{time}^{-1} \]

3. **Set Up the Equation Based on the Given Units:**
From the given units \( \text{mol L}^{-1} \text{min}^{-1} \), we can equate:
- For moles: \( 1 - n = -1 \)
- For liters: \( n - 1 = -1 \)
- For time (minutes): The time unit is already in the denominator, so it is \( -1 \).

4. **Solve for \( n \):**
- From \( 1 - n = -1 \):
\[ 1 + 1 = n \implies n = 2 \]
- From \( n - 1 = -1 \):
\[ n = 0 \]
- Both equations give consistent results confirming the order.

5. **Conclusion:**
The order of the reaction is \( n = 2 \).

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