Chemistry, 21.01.2021 22:20 stephensandrew4293
When the concentration of A in the reaction A B was changed from 1.20 M to 0.60 M, the half-life increased from 2.0 min to 4.0 min at 25°C. Calculate the order of the reaction and the rate constant.
Answers: 2
![{[A]_0}_A=1.2\ \text{M}](/tpl/images/1053/6371/ba19d.png)
![{[A]_0}_B=0.6\ \text{M}](/tpl/images/1053/6371/61cc0.png)
![t_{1/2}\propto \dfrac{1}{[A]_0^{n-1}}](/tpl/images/1053/6371/3ebb4.png)
![\dfrac{{t_{1/2}}_A}{{t_{1/2}}_B}=\left(\dfrac{{[A]_0}_B}{{[A]_0}_A}\right)^{n-1}\\\Rightarrow \dfrac{2}{4}=\left(\dfrac{0.6}{1.2}\right)^{n-1}\\\Rightarrow \dfrac{1}{2}=\left(\dfrac{1}{2}\right)^{n-1}](/tpl/images/1053/6371/86904.png)
![t_{1/2}=\dfrac{1}{k[A]_0^{n-1}}\\\Rightarrow k=\dfrac{1}{t_{1/2}[A]_0^{n-1}}\\\Rightarrow k=\dfrac{1}{2\times 1.2^{2-1}}\\\Rightarrow k=0.4167\ \text{M}^{-1}\text{min}^{-1}](/tpl/images/1053/6371/f48ea.png)
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When the concentration of A in the reaction A B was changed from 1.20 M to 0.60 M, the half-life in...
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