Chemical Kinetics and Nuclear ChemistryMedium
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
$Kt = \ln\frac{\left\lbrack H_{2}O_{2} \right\rbrack_{0}}{\left\lbrack H_{2}O_{2} \right\rbrack_{t}} = \ln\frac{V_{0}}{V_{t}}$
$\therefore t = \frac{1}{4.5 \times 10^{- 2}\text{ min}}.\ln\frac{25}{2} = \frac{\ln 5}{4.5 \times 10^{- 2}}\text{ min}$
Create a free account to view solution
View Solution FreeTopic: Chemical Kinetics and Nuclear Chemistry·Practice all Chemical Kinetics and Nuclear Chemistry questions
More Chemical Kinetics and Nuclear Chemistry Questions
Consider the reaction : Cl2(aq) + H2S(aq) → S(s) + 2H+(aq) + 2Cl- (aq) The rate equation for this reaction is rate...For the first-order parallel reactions, starting with 1 M of A, which of the following statement(s) is/are correct? $A\o...For the second-order reaction A + B → Products, the rate constant k, is given as$k = \frac{2.303}{(a - b)t}\log\frac{b(a...The rate expression for the reaction A(g) + B(g) → C(g) is rate = K·CA2 ·CB1/2. What changes in the initial concentratio...The rate constant (K) for the reaction 2A + B → Products was found to be 2.58 × 10−5 L mol−1 s−1 after 15 s,2.59 × 10−5 ...