The rate constant for zero order reaction is

Options

A. `A. k = (c_(0))/(2t)`
B. `B..k = ((c_(0)-c_(t)))/(t)`
C. `C. k = ln((c_(0)-c_(t))/(2t))`
D. `D. k = (c_(0))/(c_(t))`

Explanation

To determine the rate constant for a zero-order reaction, we can follow these steps:

### Step-by-Step Solution:

1. **Understand the Zero-Order Reaction**:
In a zero-order reaction, the rate of reaction is constant and does not depend on the concentration of the reactants. This means that the rate of reaction can be expressed as:
\[ \text{Rate} = k \]
where \( k \) is the rate constant.

2. **Write the Integrated Rate Law**:
For a zero-order reaction, the integrated rate law can be expressed as:
\[ [C_0] - [C_t] = kt \]
where:
- \( [C_0] \) is the initial concentration of the reactant,
- \( [C_t] \) is the concentration of the reactant at time \( t \),
- \( k \) is the rate constant,
- \( t \) is the time.

3. **Rearranging the Equation**:
We can rearrange the integrated rate law to solve for the rate constant \( k \):
\[ k = \frac{[C_0] - [C_t]}{t} \]

4. **Conclusion**:
Thus, the expression for the rate constant \( k \) for a zero-order reaction is:
\[ k = \frac{[C_0] - [C_t]}{t} \]

### Final Answer:
The rate constant for a zero-order reaction is given by the formula:
\[ k = \frac{[C_0] - [C_t]}{t} \]