Advertisements
Advertisements
Question
A zero order reaction is 20% complete in 20 minutes. Calculate the value of the rate constant. In what time will the reaction be 80% complete?
Advertisements
Solution
1. A = 100%, x = 20%, Therefore, a – x = 100 – 20 = 80
For the zero order reaction k = `("x"/"t")` ⇒ k = `(20/20)` = 1
Rate constant for a reaction = 1
2. To calculate the time for 80% of completion
k = 1, a = 100, x = 80%, t = ?
Therefore, t = `("x"/"k") = (80/1)` = 80 min
APPEARS IN
RELATED QUESTIONS
Answer the following in brief.
What is a zeroth-order reaction?
Solve
A first-order reaction takes 40 minutes for 30% decomposition. Calculate its half-life.
Rate constant of a reaction is 3.6 × 10–3 s–1. The order of reaction is ______.
In a first order reaction \[\ce{x -> y}\]; if k is the rate constant and the initial concentration of the reactant x is 0.1 M, then, the half life is
Which among the following reaction is an example of a zero order reaction?
In a first order reaction, the concentration of the reactant, decreases from 0.8 mol dm−3 to 0.4 mol dm−3 in 15 minutes. The time taken for the concentration to change from 0.1 mol dm−3 to 0.025 mol dm−3 is ____________.
Reaction given below follows first order kinetics:
\[\ce{2N2O2 -> 4NO2 + O2}\]
Calculate the rate constant of reaction if concentration of N2O2 is 0.05 M and rate of reaction is 1.5 × 10−6 mol L−1 s−1?
A first order reaction is 50% completed in 16 minutes. The percentage of reactant that will react in 32 minutes is ____________.
The integrated rate law is a direct relationship between time and ______
The half-life of first order reaction is 1.7 hour. What is its rate constant?
