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 \( k = 1.6 \times 10^{-3} \, \text{mol/L/min} \), we can analyze the units of the rate constant and compare them with the known units for different reaction orders.

### Step-by-Step Solution:

1. **Identify the given rate constant**:
\[ k = 1.6 \times 10^{-3} \, \text{mol/L/min} \]

2. **Recall the units of the rate constant for different reaction orders**:
- **Zero-order reaction**:
\[ \text{Units of } k = \text{mol/L/min} \]
- **First-order reaction**:
\[ \text{Units of } k = \text{1/min} \]
- **Second-order reaction**:
\[ \text{Units of } k = \text{L/(mol·min)} \]

3. **Compare the given units of \( k \)**:
- The given unit of \( k \) is \( \text{mol/L/min} \).
- This matches the unit for a zero-order reaction.

4. **Conclusion**:
- Since the unit of the rate constant \( k \) corresponds to that of a zero-order reaction, we conclude that the order of the reaction is **zero**.

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

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