Chemical Kinetics and Nuclear ChemistryHard
Question
For a first order reaction, (A) → products, theconcentration of A changes from 0.1 M to0.025 M in 40 minutes. The rate of reactionwhen the concentration of A is 0.01 M is :-
Options
A.1.73 × 10-4 M/min
B.1.73 × 10-5 M/min
C.3.74 × 10-4 M/min
D.3.74 × 10-5 M/min
Solution
For first order reaction
Given [A]0 = 0.1 M, [A]t = 0.025 M
∴
Rate = K [A]1
0.01 = 0.0003465 M/min
= 3.47 × 10-4 M/min
Given [A]0 = 0.1 M, [A]t = 0.025 M
∴
Rate = K [A]1
0.01 = 0.0003465 M/min= 3.47 × 10-4 M/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
Which of the following statement is incorrect?...A reaction takes place in three steps having rate constants K1, K2, K3 respectively. The overall rate constant K = . If ...Inversion of sucrose (C12H22O11) is first-order reaction and is studied by measuring angle of rotation at different inst...t1/2 of a reaction: A → Products $\left( \text{Order = }\frac{3}{2} \right)$ is represented by $t_{1/2}\alpha\frac{1}{\l...Half life is independent of the concentration of A. After 10 min volume of N2 gas is 10 L and after complete reaction is...