Question

The concentrations of the reactant A in the reaction \( A \rightarrow B \) at different times are given below Concentration (M) \quad 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 M/min
• B. 0.001 min\(^{-1}\)
• C. 0.001 min/M
• D. 0.001 M\(^{-1}\) 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.