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?
Advertisements
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
What are pseudo-first-order reactions?
Solve
A first-order reaction takes 40 minutes for 30% decomposition. Calculate its half-life.
Derive the integrated rate law for the zeroth order reaction.
Write order of the following reaction:
\[\ce{2NH_{3(g)} -> N_{2(g)} + 3H_{2(g)}}\]
Explain pseudo first order reaction with a suitable example.
Write units of rate constants for:
- First-order reaction
- Zero-order reaction
Derive an expression for the relation between half-life and rate constant for first-order reaction.
For a first-order reaction \[\ce{A -> B}\] the rate constant is x min−1. If the initial concentration of A is 0.01 M, the concentration of A after one hour is given by the expression.
How long would it take to electroplate a spoon with 0.1 mol of silver (108 g/mol) at a constant current of 2.0 A using AgNO3?
A first order reaction is 25% completed in 40 minutes. What is the rate constant k tor the reaction?
The time of completion of 90% of a first order reaction is approximately ____________.
The rate constant of a reaction has same units as the rate of reaction. The reaction is of ____________.
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 ____________.
The rate constant of a first order reaction is 3 × 10−6 per s. If the initial concentration is 0.10 mol dm−3, the initial rate of reaction is ____________.
Which of the following represents the expression for `(3/4)^"th"` life of 1st order reaction?
The order of the reaction for which the unit of rate constant is s−1 is ____________.
Half-life period of a first order reaction, \[\ce{A -> product}\] is 3.0 hours. What is the value of rate constant?
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 takes 40 minutes for 30% decomposition. What is the half-life of reaction?
In a reaction \[\ce{N2_{(g)} + 3H2_{(g)} -> 2NH3_{(g)}}\], if the rate of disappearance of N2(g) is 2.6 × 10−4 M/s, the rate of disappearance of H2(g) in M/s is ____________.
0.0210 M solution of N2O5 is allowed to decompose at 43°C. How long will it take to reduce to 0.0150 M?
(Given k = 6.0 × 10−4 sec−1)
For the first order reaction A → B, the rate constant is 0.25 s-1, if the concentration of A is reduced to half, the value of rate constant will be ________.
A certain zero order reaction has rate constant 0.025 M s-1. What will be the concentration of reactant 'A' after 15 seconds, if initial concentration is 0.50 M?
Half-life of first order reaction is 20 minutes. What is the time taken to reduce the initial concentration of the reactant to `1/10`th?
Rate constant for zero order reaction is 2 × 10-2 mol L-1 s-1. If the concentration of the reactant after 25 sec. is 0.5 M, what is the initial concentration of reactant?
The integrated rate equation is Rt = log C0 – log Ct, then the straight-line graph is obtained by plotting.
Which of the following reactions is not of the first order?
What are integrated rate laws?
The plot that represents the zero order reaction is:
