Consider the following first order reaction:
A → Product
The values of the initial concentration of the reactant A are given below:
(A) 0.2 M
(B) 0.3 M
(C) 0.4 M
(D) 0.5 M
The initial rate of the given reaction in increasing order is
Choose the correct answer from the options given below:
Answer & explanation
Correct answer: option 1
The correct answer is Option (1) → (A), (B), (C), (D).
For a first order reaction, the rate is directly proportional to the concentration of the reactant:
\( \displaystyle \mathrm{Rate}=k[\mathrm{A}] \)
At a given temperature k is constant, so doubling [A] doubles the rate. The higher the initial concentration, the higher the initial rate.
For the given initial concentrations:
\( \displaystyle \text{(A) Rate}=k\times0.2 \)
\( \displaystyle \text{(B) Rate}=k\times0.3 \)
\( \displaystyle \text{(C) Rate}=k\times0.4 \)
\( \displaystyle \text{(D) Rate}=k\times0.5 \)