The unit of rate constant for a zero order reaction is `s^(-1)`.

Answer

To determine the unit of the rate constant (k) for a zero-order reaction, we can follow these steps:

### Step 1: Understand the Rate Expression
For a zero-order reaction, the rate of the reaction is independent of the concentration of the reactant. The general rate expression for a reaction can be written as:
\[ \text{Rate} = k [A]^n \]
where \( n \) is the order of the reaction with respect to reactant A.

### Step 2: Set the Order of the Reaction
Since we are dealing with a zero-order reaction, we set \( n = 0 \). Therefore, the rate expression simplifies to:
\[ \text{Rate} = k [A]^0 \]
Since any quantity raised to the power of 0 is 1, this simplifies further to:
\[ \text{Rate} = k \]

### Step 3: Define the Rate
The rate of a reaction is defined as the change in concentration of a reactant or product per unit time. The unit of rate can be expressed as:
\[ \text{Rate} = \frac{\Delta [A]}{\Delta t} \]
where \( \Delta [A] \) is the change in concentration (in moles per liter, or mol/L) and \( \Delta t \) is the change in time (in seconds).

### Step 4: Determine the Unit of Rate
Thus, the unit of rate can be expressed as:
\[ \text{Unit of Rate} = \frac{\text{mol/L}}{\text{s}} = \text{mol L}^{-1} \text{s}^{-1} \]

### Step 5: Relate the Unit of Rate to the Unit of Rate Constant
Since we established that for a zero-order reaction, the rate is equal to the rate constant (k), we can conclude:
\[ k = \text{Rate} \]
Thus, the unit of the rate constant (k) for a zero-order reaction is the same as the unit of rate:
\[ \text{Unit of } k = \text{mol L}^{-1} \text{s}^{-1} \]

### Conclusion
Therefore, the statement that "the unit of rate constant for a zero-order reaction is \( s^{-1} \)" is false. The correct unit is \( \text{mol L}^{-1} \text{s}^{-1} \).

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