Chemical Kinetics and Nuclear ChemistryHard
Question
The decomposition of H2O2 can be followed by titration with KMnO4 and is found to be a first order reaction. The rate constant is 4.5 × 10−2. In an experiment, the initial titre value was 25 ml. The titre will be 5 ml after
Options
A.4.5 × 10−2 × 5 min
B.$\frac{\ln 5}{4.5 \times 10^{- 2}}\text{min}$
C.$\frac{\ln(5/4)}{4.5 \times 10^{- 2}}\text{min}$
D.4.5 × 1.25 min
Solution
$Kt = \ln\frac{\left\lbrack H_{2}O_{2} \right\rbrack_{0}}{\left\lbrack H_{2}O_{2} \right\rbrack_{t}} = \ln\frac{V_{0}}{V_{t}}$
$\therefore t = \frac{1}{4.5 \times 10^{- 2}\text{ min}}.\ln\frac{25}{2} = \frac{\ln 5}{4.5 \times 10^{- 2}}\text{ min}$
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