Question

Which of the following plots gives a straight line for a zero-order reaction?

• A. \([A] \, \text{vs} \, t\)
• B. \(\log[A] \, \text{vs} \, t\)
• C. \(1/[A] \, \text{vs} \, t\)
• D. \(\ln[A] \, \text{vs} \, t\)

Hint:

For zero-order reactions, concentration decreases linearly with time. Always remember: \([A]\) vs \(t\) gives a straight line with slope \(-k\).

Answer 1

The Correct Option is A

For a zero-order reaction, the rate law is: \[ \frac{d[A]}{dt} = -k \] Integrating, we get: \[ [A] = [A]_0 - kt \] This equation is of the form \( y = mx + c \), which represents a straight line with a negative slope when \([A]\) is plotted against \(t\). Hence, the plot of \([A]\) vs \(t\) gives a straight line.