In a first order reaction x → y, 40% of the given sample of compound remains unreacted in 45 minutes. Calculate rate constant of the reaction.
For a reaction A + B ⟶ P, the rate is given by
Rate = k [A] [B]2
How is the rate of reaction affected if the concentration of B is doubled?
The following results have been obtained during the kinetic studies of the reaction:
2A + B → C + D
|Experiment||A/ mol L−1||B/ mol L−1||Initial rate of formation of D/mol L−1 min−1|
|I||0.1||0.1||6.0 × 10−3|
|II||0.3||0.2||7.2 × 10−2|
|III||0.3||0.4||2.40 × 10−2|
Determine the rate law and the rate constant for the reaction.
For a reaction, A + B → Product; the rate law is given by, `r = k[A]^(1/2)[B]^2` . What is the order of the reaction?