Question

The rate constant of the reaction \( A \rightarrow B \) at different times are given below: \[ \text{Concentration (M)} \quad \text{Time (Minutes)}
0.069 \quad 0 \quad 0.052 \quad 17 \quad 0.035 \quad 34 \quad 0.018 \quad 51 \] The rate constant of the reaction according to the correct order of reaction is

• A. \( 0.001 \, \text{M/min} \)
• B. \( 0.001 \, \text{min}^{-1} \)
• C. \( 0.001 \, \text{min/M} \)
• D. \( 0.001 \, \text{M}^{-1} \, \text{min}^{-1} \)

Hint:

For a first-order reaction, the rate constant is obtained from the slope of the \( \ln[A] \) vs time plot.

Answer 1

The Correct Option is B

The rate constant is determined from the concentration-time data and assuming the reaction is of first-order. By plotting \( \ln[A] \) vs time, the rate constant is calculated from the slope of the graph.