For a certain reaction, a plot of `([C_(0)-C])/(C )` against time `t`, yields a straight line. `C_(0)` and C are concentrations of reaction at `t=0` and `t=t` respectively. The order of reaction is:

Options

A. `3`
B. Zero
C. `1`
D. `2`

Explanation

To determine the order of the reaction based on the given information, we can follow these steps:

### Step 1: Understand the given information
We are given that a plot of \(\frac{C_0 - C}{C}\) against time \(t\) yields a straight line. Here, \(C_0\) is the initial concentration and \(C\) is the concentration at time \(t\).

### Step 2: Analyze the expression
The expression \(\frac{C_0 - C}{C}\) can be rewritten as:
\[ \frac{C_0 - C}{C} = \frac{C_0}{C} - 1 \]
This implies that if we plot \(\frac{C_0 - C}{C}\) against \(t\), we are essentially looking at a linear relationship.

### Step 3: Relate to reaction order
For a second-order reaction, the integrated rate law is given by:
\[ \frac{1}{C} - \frac{1}{C_0} = kt \]
This can be rearranged to:
\[ \frac{C_0 - C}{C \cdot C_0} = kt \]
This shows that \(\frac{C_0 - C}{C}\) is proportional to \(kt\), which indicates that the plot of \(\frac{C_0 - C}{C}\) against \(t\) will yield a straight line.

### Step 4: Conclusion
Since the plot of \(\frac{C_0 - C}{C}\) against time \(t\) yields a straight line, we can conclude that the reaction is of second order.

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

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