The plote between concentration versus time for a zero order reaction is represented by :

Options

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B.
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D.

Explanation

To determine the plot between concentration versus time for a zero-order reaction, we can follow these steps:

### Step-by-Step Solution:

1. **Understanding Zero-Order Reactions**:
- In a zero-order reaction, the rate of reaction is constant and does not depend on the concentration of the reactant. This can be expressed as:
\[ \text{Rate} = -\frac{d[C]}{dt} = k \]
where \( [C] \) is the concentration of the reactant and \( k \) is the rate constant.

2. **Rearranging the Rate Equation**:
- We can rearrange the equation to express the change in concentration over time:
\[ -d[C] = k \, dt \]

3. **Integrating the Equation**:
- We integrate both sides. The left side will be integrated from the initial concentration \( [C_0] \) to \( [C] \), and the right side from \( 0 \) to \( t \):
\[ \int_{[C_0]}^{[C]} -d[C] = \int_{0}^{t} k \, dt \]

4. **Performing the Integration**:
- The integration results in:
\[ -([C] - [C_0]) = kt \]
- Rearranging gives:
\[ [C] = [C_0] - kt \]

5. **Identifying the Linear Relationship**:
- The equation \( [C] = [C_0] - kt \) represents a linear equation of the form \( y = mx + b \), where:
- \( y = [C] \)
- \( x = t \)
- The slope \( m = -k \) (negative slope)
- The y-intercept \( b = [C_0] \)

6. **Plotting the Graph**:
- When we plot concentration \( [C] \) on the y-axis against time \( t \) on the x-axis, we will obtain a straight line with a negative slope, starting from the initial concentration \( [C_0] \).

### Conclusion:
The plot between concentration versus time for a zero-order reaction is a straight line with a negative slope, where the y-intercept is the initial concentration \( [C_0] \).