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

The rate law for a zero-order reaction is given by: \[ \frac{d[A]}{dt} = -k \] Upon integration, the equation becomes: \[ [A] = [A]_0 - kt \] This equation follows the form \( y = mx + c \), indicating a linear relationship when \([A]\) is plotted against \(t\). The plot will exhibit a straight line with a negative slope. Therefore, a plot of \([A]\) versus \(t\) results in a straight line.