Advertisements
Advertisements
प्रश्न
A reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is doubled?
Advertisements
उत्तर
\[\ce{Reactant -> Product}\]
Rate of reaction (R) = k [A]2
If the concentration of the reactant is doubled, i.e., [A] = 2A, then the rate of the reaction would be,
R = k[2A]2
= k 4 A2
= 4 kA2
Change in rate of reaction = `"rate of reaction when concentration is doubled"/"rate of reaction originally"`
= `(4 kA^2)/(kA^2)`
= 4 : 1
When the concentration is doubled, the reaction rate increases by a factor of 4.
APPEARS IN
संबंधित प्रश्न
A → B is a first order reaction with rate 6.6 × 10-5m-s-1. When [A] is 0.6m, rate constant of the reaction is
- 1.1 × 10-5s-1
- 1.1 × 10-4s-1
- 9 × 10-5s-1
- 9 × 10-4s-1
For a reaction A + B ⟶ P, the rate is given by
Rate = k [A] [B]2
What is the overall order of reaction if A is present in large excess?
From the rate expression for the following reaction, determine the order of reaction and the dimension of the rate constant.
\[\ce{H2O2_{( aq)} + 3I^-_{( aq)} + 2H^+ -> 2H2O_{(l)} + I^-_3}\] Rate = k[H2O2][I−]
A reaction is first order in A and second order in B. Write the differential rate equation.
A reaction is first order in A and second order in B. How is the rate affected when the concentrations of both A and B are doubled?
The decomposition of N2O5(g) at 320K according to the following equation follows first order reaction:
`N_2O_(5(g))->2NO_(2(g))+1/2O_(2(g))`
The initial concentration of N2O5(g) is 1.24 x 10-2 mol. L-1 and after 60 minutes 0.20x10-2 molL-1. Calculate the rate constant of the reaction at 320K.
Write the principle behind the following methods of refining:
Hydraulic washing
Which of the following statements is not correct about order of a reaction.
In any unimolecular reaction:
(i) only one reacting species is involved in the rate determining step.
(ii) the order and the molecularity of slowest step are equal to one.
(iii) the molecularity of the reaction is one and order is zero.
(iv) both molecularity and order of the reaction are one.
Why can’t molecularity of any reaction be equal to zero?
Use Molecular Orbital theory to determine the bond order in each of species, [He2j+ and [He2]2+?
A catalyst in a reaction changes which of the following?
The rate constant for the reaction \[\ce{2H2O5 -> 4NO2 + O2}\] is 30 × 10–5 sec–1. if the rate is 204 × 10–5 mol L–1 S–1, then the concentration of N2O5 (in mol–1) is-
For a first order A → B, the reaction rate at reactant concentration of 0.01 m is found to be 2.0 × 10–5. The half-life period of reaction.
The rate of a chemical reaction double for every 10° rise in temperature. If the temperature is raised. by 50°C, the rate of relation by about:-
If the 0.05 molar solution of m+ is replaced by a 0.0025 molar m+ solution, then the magnitude of the cell potential would be
The half-life period of a. substance in a certain enzyme catalysed reaction is 138 s. The time required for the concentration of the substance to fall from 1.28 mol–1 to 0.04 mg L–1 is
The conversion of molecules A to B follow second order kinetics. If concentration of A is increased to three times, how will it affect the rate of formation of B?
Assertion (A): Order of reaction is applicable to elementary as well as complex reactions.
Reason (R): For a complex reaction, molecularity has no meaning.
