For a first order reaction, (A) product the concentration of A changes from 0.1 M to…
Chemistry · JEE Main · NTA Exams — Chemical Kinetics
For a first order reaction, (A) 
product the concentration of A changes from 0.1 M to 0.025 M in 40 min. The rate of reaction when the concentration of A is 0.01 M is
product the concentration of A changes from 0.1 M to 0.025 M in 40 min. The rate of reaction when the concentration of A is 0.01 M is- 1.73 × 10–5 M/min
- 3.47 × 10–4 M/min
- 3.47 × 10–5 M/min
- 1.73 × 10–4 M/min
Answer
(B) 3.47 × 10 –4 M/min
Sign up free on Edukali to view the step-by-step worked solution and practice thousands of similar questions.
Related practice questions
- For a first order reaction; which of the following statement is correct:
- Given below are two statements. One is labelled as Assertion and the other is labelled as Reason. Assertion…
- Consider the reaction: Cl _ 2 ( aq )+ H _ 2 5( aq ) 5(5)+2 H ^ + ( aq )+2 Cl ^ - ( aq ) The rate equation for…
- For the two gaseous reactions, following data are given A ~B ; k _ 1 =10^ 10 e ^ -20,000 / T C D ; k _ 2 =10^…
- Iron(III) catalyses the reaction between iodide and persulphate ions, in which (A) Fe 3+ oxidises the iodide…
- The rate equation for the reaction, 2A + B → C is found to be : rate = k [A] [B]. The correct statement in…
- The rate of reaction A + B + C → Products is given by Rate = k [A] 1/2 [B] 1/3 [C] The order of the reaction…
- The following results were obtained during kinetic studies of the reaction: 2A + B → Products Experiment [A]…
More Chemical Kinetics questions · Browse all practice questions