Advertisements
Advertisements
Question
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.
Options
0.01 e−x
1 × 10−2 (1 − e−60x)
(1 × 10−2) e−60x
none of these
Advertisements
Solution
(1 × 10−2) e−60x
APPEARS IN
RELATED QUESTIONS
Answer the following in brief.
Derive the integrated rate law for the first-order reaction,
\[\ce{A_{(g)} -> B_{(g)} + C_{(g)}}\] in terms of pressure.
In a first-order reaction, the concentration of the reactant decreases from 20 mmol dm−3 to 8 mmol dm−3 in 38 minutes. What is the half-life of reaction?
Solve
The half-life of a first-order reaction is 1.7 hours. How long will it take for 20% of the reactant to react?
What is half life of first order reaction if time required to decrease concentration of reactants from 0.8 M to 0.2 M is 12 hours?
A zero-order reaction \[\ce{X -> Product}\], with an initial concentration 0.02 M has a half-life of 10 min. if one starts with concentration 0.04 M, then the half-life is
This reaction follows first-order kinetics. The rate constant at particular temperature is 2.303 × 10−2 hour−1. The initial concentration of cyclopropane is 0.25 M. What will be the concentration of cyclopropane after 1806 minutes? (log 2 = 0.3010)
For a first-order reaction, the rate constant is 6.909 min−1 the time taken for 75% conversion in minutes is
The time for half change in a first order decomposition of a substance A is 60 seconds. Calculate the rate constant. How much of A will be left after 180 seconds?
A first order reaction takes 40 minutes for 30% decomposition. What is the half-life of reaction?
Consider the following reaction.
\[\ce{SO2(g) + 1/2 O2(g) <=>[K1] SO3(g)}\]
\[\ce{2SO3(g)<=>[K2] 2SO2(g) + O2(g)}\]
What is the relation between K1 and K2?
