Question

If a plot of \(\log C_0\) versus \(t\) gives a straight line for a given reaction, then the reaction is

• A. zero order
• B. first order
• C. second order
• D. third order

Hint:

First order reactions give straight line for \(\log [A]\) vs \(t\); slope = \(-k/2.303\).

Answer 1

The Correct Option is B

Step 1: Recall integrated rate law for first order reaction.
For first order:
\[ \log C = \log C_0 - \frac{kt}{2.303} \]
Step 2: Identify linear form.
This equation is of the form:
\[ y = mx + c \]
Where:
\(y = \log C\), \(x=t\).
Step 3: Interpret graph.
So a straight line graph of \(\log C\) versus \(t\) indicates first order kinetics.
Final Answer:
\[ \boxed{\text{(B) first order}} \]