Given below is an expression for the rate constant of a first-order reaction occurring at a certain temperature, T (K): ln k = 14.34 - (1.25 × 10⁴)/(T)$$\ln k = 14.34 - \frac{1.25 \times 10^4}{T}$$ The energy of activation in kcal mol⁻¹$\text{kcal mol}^{-1}$ for the reaction is: (Given: k in s⁻¹$\text{s}^{-1}$, R = 1.987 cal mol⁻¹ K⁻¹$R = 1.987 \text{ cal mol}^{-1} \text{K}^{-1}$)

Related Formula

Core Logic

Step 1: Conclusion

Matches: A-IV, B-III, C-I, D-II.

Pattern Recognition

Substitute n$n$ into (mol/L)¹⁻ⁿ s⁻¹$(mol/L)^{1-n} s^{-1}$ formula for reaction order.

Chapter Mix

Class 12 Chemistry: Chemical Kinetics

Related Formula

Core Logic

Integrated rate equation for zero order reaction is [R] = [R₀] - kt$[R] = [R_0] - kt$. A plot of [R]$[R]$ vs t$t$ gives a straight line with slope = -k$= -k$ and intercept [R₀]$[R_0]$.

Step 1: Conclusion

Reaction order is 0.

Pattern Recognition

[R]$[R]$ vs t$t$ linear arrow$\rightarrow$ Zero order; ln[R]$\ln[R]$ vs t$t$ linear arrow$\rightarrow$ First order.

Chapter Mix

Class 12 Chemistry: Chemical Kinetics