Advertisements
Advertisements
प्रश्न
The rate constant of the first order reaction is 1.386 min–1. Calculate the time required for 80% reactant to decompose?
उत्तर
Given: [A]0 = 100%, k = 1.386 min–1
To find: Time required for 80% reactant to decompose
Formula: t = `2.303/"k" log_10 ["A"]_"o"/["A"]_"t"`
Calculations: The reactant is 80% decomposed. Hence, [A]t = 20%.
t = `2.303/"k" log_10 ["A"]_"o"/["A"]_"t"`
Substituting the values,
t = `2.303/(1.386 "min"^-1) log_10 100/20`
= `2.303/(1.386 "min"^-1) xx 0.69897`
= 1.16 min × `(60 "s")/(1 "min")`
= 69.6 s
Time required for reducing concentration of reactant to 20 % is 1.16 min or 69.6 s.
APPEARS IN
संबंधित प्रश्न
Answer the following in one or two sentences.
Write the relationships between rate constant and half-life of the first order and zeroth-order reactions.
Answer the following in one or two sentences.
How do the half-lives of the first order and zero-order reactions change with the initial concentration of reactants?
Answer the following in brief.
How will you represent the zeroth-order reaction graphically?
Answer the following in brief.
Derive the integrated rate law for the first-order reaction.
Answer the following in brief.
What are the units of the rate constant?
Rate constant of a reaction is 3.6 × 10–3 s–1. The order of reaction is ______.
Give one example of pseudo first-order reaction.
Explain with the help of a potential energy diagram that the catalyst increases the rate of the reaction.
Derive an integrated rate law expression for first order reaction: A → B + C
Derive an expression for the relation between half-life and rate constant for first-order reaction.
The rate constant of a reaction is 5.8 × 10−2 s−1. The order of the reaction is ____________.
Identify the order for the following reaction.
Radioactive disintegration of 92U238
If [A] is the concentration of A at any time t and [A]0 is the concentration at t = 0, then for the 1st order reaction, the rate equation can be written as ____________.
If [A]0 is the initial concentration, then the half life of zero order reaction is ____________.
The order of the reaction for which the unit of rate constant is s−1 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?
The slope of a graph, log [A]t versus 't' for a first order reaction is −2.5 × 10−3 s−1. The rate constant for the reaction is ____________.
The half-life of a first order reaction is 6.0 hour. How long will it take for the concentration of reactant to decrease from 0.4 M to 0.12 M?
Which among the following is an example of zero order reaction?
A first order reaction is 50% completed in 16 minutes. The percentage of reactant that will react in 32 minutes is ____________.
What is the unit of rate constant for the zero order reaction?
Half-life of first-order reaction \[\ce{X -> Y + Z}\] is 3 minutes. What is the time required to reduce the concentration of 'X' by 90 % of it's initial concentration?
The expression to calculate time required for completion of zero order reaction is ______.
Which of the following reactions is not of the first order?
Which of the following is correct for a first-order reaction?
Half-life of a first order reaction is 30 minutes and initial concentration of reactant is 0.1 M.
What is half-life of the reaction if initial concentration of reactant is doubled?
