Advertisements
Advertisements
Question

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)
Options
0.125 M
0.215 M
0.25 × 2.303 M
0.05 M
Advertisements
Solution
0.125 M
APPEARS IN
RELATED QUESTIONS
Answer the following in brief.
Derive the integrated rate law for the first-order reaction.
Answer the following in brief.
What is a zeroth-order reaction?
For the reaction 2NOBr → 2NO2 + Br2, the rate law is rate = k[NOBr]2. If the rate of a reaction is 6.5 × 10–6 mol L–1 s–1, when the concentration of NOBr is 2 × 10–3 mol L–1. What would be the rate constant of the reaction?
Explain with the help of a potential energy diagram that the catalyst increases the rate of the reaction.
Write the rate law for the following reaction.
A reaction that is `3/2` order in x and zero order in y.
Give two examples for zero order reaction.
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?
Half-life period of a first order reaction, \[\ce{A -> product}\] is 3.0 hours. What is the value of rate constant?
Which one of the following reactions is a true first-order reaction?
Which is the relation between half life and rate constant for a zero order?
