Practicing Success
The rate constant of a first-order reaction at 27°C is 10−3 min−1. The temperature coefficient of the reaction is 2. What is the rate constant at 17°C for this reaction? |
\(10^{−3}\) \(5 × 10^{−4}\) \(2 × 10^{−3}\) \(10^{−2}\) |
\(5 × 10^{−4}\) |
Given, \(T_1 = 17^oC\) \(T_2 = 27^oC\) So, \(\Delta T = T_2 − T_1 = (27 − 17)^oC = 10^oC\) We know, \(\frac{K_{T_2}}{K_{T_1}} = (2)^{\Delta T / 10}\) ⇒ \(\frac{10^{−3}}{K_{T_1}} = (2)^{10 / 10}\) ⇒ \(K_{T_1} = \frac{10^{−3}}{2}\) ⇒ \(K_{T_1} = 0.5 × 10^{−3}\) ∴ \(K_{T_1} = 5 × 10^{−4} min^{−1}\) |