Advertisements
Advertisements
प्रश्न
The rate law for a reaction of A, B and C has been found to be rate = `"k" ["A"]^2["B"] ["L"]^(3/2)`. How would the rate of reaction change when
- Concentration of [L] is quadrupled
- Concentration of both [A] and [B] are doubled
- Concentration of [A] is halved
- Concentration of [A] is reduced to `(1/3)` and concentration of [L] is quadrupled.
Advertisements
उत्तर
Rate = `"k" ["A"]^2["B"] ["L"]^(3/2)` ..........(1)
i. when [L] = [4L]
Rate = `"k" ["A"]^2["B"] [4"L"]^(3/2)`
Rate = `8 ("k" ["A"]^2["B"] ["L"]^(3/2))` ........(2)
Comparing (1) and (2); rate is increased by 8 times.
ii. when [A] = [2A] and [B] = [2B]
Rate = `"k" [2"A"]^2 [2"B"] ["L"]^(3/2)`
Rate = `8 ("k" ["A"]^2["B"] ["L"]^(3/2))` ........(3)
Comparing (1) and (3); rate is increased by 8 times.
iii. when [A] = `["A"/2]`
Rate = `"k" ["A"/2]^2 ["B"] ["L"]^(3/2)`
Rate = `(1/4) ("k" ["A"]^2["B"] ["L"]^(3/2))` .........(4)
Comparing (1) and (4); rate is reduced to `1/4` times.
iv. when [A] = `["A"/3]` and [L] = [4L]
Rate = `"k" ["A"/3]^2 ["B"] [4"L"]^(3/2)`
Rate = `(8/9) ("k" ["A"]^2["B"] ["L"]^(3/2))` ........(5)
Comparing (1) and (5); rate is reduced to `8/9` times.
APPEARS IN
संबंधित प्रश्न
The addition of a catalyst during a chemical reaction alters which of the following quantities?
In a reversible reaction, the enthalpy change and the activation energy in the forward direction are respectively −x kJ mol−1 and y kJ mol−1. Therefore , the energy of activation in the backward direction is
What is the activation energy for a reaction if its rate doubles when the temperature is raised from 200 K to 400 K? (R = 8.314 JK−1mol−1)
If the initial concentration of the reactant is doubled, the time for half reaction is also doubled. Then the order of the reaction is ____________.
In a homogeneous reaction \[\ce{A -> B + C + D}\], the initial pressure was P0 and after time t it was P. Expression for rate constant in terms of P0, P and t will be
The correct difference between first and second order reactions is that
Explain the effect of catalyst on reaction rate with an example.
The rate of formation of a dimer in a second order reaction is 7.5 × 10−3 mol L−1s−1 at 0.05 mol L−1 monomer concentration. Calculate the rate constant.
For a reaction \[\ce{x + y + z -> products}\] the rate law is given by rate = `"k" ["x"]^(3/2) ["y"]^(1/2)` what is the overall order of the reaction and what is the order of the reaction with respect to z.
How do nature of the reactant influence rate of reaction?
