Advertisements
Advertisements
प्रश्न
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
विकल्प
`"k" = (2.303/"t") log ((2"P"_0)/(3"P"_0 - "P"))`
`"k" = (2.303/"t") log ((2"P"_0)/("P"_0 - "P"))`
`"k" = (2.303/"t") log ((3"P"_0 - "P")/(2"P"_0))`
`"k" = (2.303/"t") log ((2"P"_0)/(3"P"_0 - 2"P"))`
Advertisements
उत्तर
`"k" = (2.303/"t") log ((2"P"_0)/(3"P"_0 - "P"))`
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)
The correct difference between first and second order reactions is that
Explain the effect of catalyst on reaction rate with an example.
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.
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 concentrations of the reactant influence the rate of reaction?
How do nature of the reactant influence rate of reaction?
