मराठी
कर्नाटक बोर्ड पी.यू.सी.पीयूसी विज्ञान 2nd PUC Class 12

For a reaction, A+B⟶Product; the rate law is given by, r=k[A]12[B]2. What is the order of the reaction? - Chemistry

Advertisements
Advertisements

प्रश्न

For a reaction, \[\ce{A + B -> Product}\]; the rate law is given by, `r = k[A]^(1/2)[B]^2`. What is the order of the reaction?

संख्यात्मक

उत्तर

The order of the reaction = `1/2+2`

= `2 1/2`

= 2.5

shaalaa.com
  या प्रश्नात किंवा उत्तरात काही त्रुटी आहे का?
पाठ 4: Chemical Kinetics - Intext Questions [पृष्ठ १०३]

APPEARS IN

एनसीईआरटी Chemistry [English] Class 12
पाठ 4 Chemical Kinetics
Intext Questions | Q 3 | पृष्ठ १०३

संबंधित प्रश्‍न

A reaction is second order in A and first order in B.

(i) Write the differential rate equation.

(ii) How is the rate affected on increasing the concentration of A three times?

(iii) How is the rate affected when the concentrations of both A and B are doubled?

 


For a reaction: 

Rate = k

(i) Write the order and molecularity of this reaction.

(ii) Write the unit of k.


From the rate expression for the following reaction, determine the order of reaction and the dimension of the rate constant.

\[\ce{CH3CHO_{(g)} -> CH4_{(g)} + CO_{(g)}}\] Rate = k [CH3CHO]3/2


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.


Define the following terms:

Pseudo first-order reaction


Consider a first order gas phase decomposition reaction given below :
\[\ce{A(g) -> B(g) + C(g)}\]
The initial pressure of the system before decomposition of A was pi. After lapse of time ‘t’, total pressure of the system increased by x units and became ‘pt’ The rate constant k for the reaction is given as ______.


Compounds ‘A’ and ‘B’ react according to the following chemical equation.
\[\ce{A(g) + 2B(g) -> 2C(g)}\]
Concentration of either ‘A’ or ‘B’ were changed keeping the concentrations of one of the reactants constant and rates were measured as a function of initial concentration. Following results were obtained. Choose the correct option for the rate equations for this reaction.

Experiment Initial
concentration
of [A]/mol L¹
Initial
concentration
of [B]/mol L¹
Initial rate of
formation of
[C]/mol L¹ s¹
1. 0.30 0.30 0.10
2. 0.30 0.60 0.40
3. 0.60 0.30 0.20

For which type of reactions, order and molecularity have the same value?


Why is the probability of reaction with molecularity higher than three very rare?


Match the graph given in Column I with the order of reaction given in Column II. More than one item in Column I may link to the same item of Column II.

  Column I Column II
(i)  
(ii)  (a) 1st order
(iii) (b) Zero-order
(iv)    

A catalyst in a reaction changes which of the following?


The role of a catalyst is to change


For a reaction \[\ce{Cl2l(g) + 2No(g) -> 2NaCl(g)}\] the rate law is expressed as rate= K[Cl2] [No]2 what is the order of the reaction?


The rate constant for the reaction \[\ce{2H2O5 -> 4NO2 + O2}\] is 30 × 10–5 sec–1. if the rate is 204 × 10–5 mol L1 S1, then the concentration of N2O5 (in mol1) is-


For a reaction 1/2 A ⇒ 2B, rate of disappearance of A is related 't o the appearance of B by the expression:


Identify the order of reaction from the following unit for its rate constant:

L mol–1s–1


The following data was obtained for chemical reaction given below at 975 K.

\[\ce{2NO(g) + 2H2(g) -> N2(g) + 2H2O(g)}\]

  [NO] [H2] Rate
  Mol L-1 Mol L-1 Mol L-1 s-1
(1) 8 × 10-5 8 × 10-5 7 × 10-9
(2) 24 × 10-5 8 × 10-5 2.1 × 10-8
(3) 24 × 10-5 32 × 10-5 8.4 × 10-8

The order of the reaction with respect to NO is ______. (Integer answer)


A drop of solution (volume 0.05 ml) contains 3.0 × 10-6 mole of H+. If the rate constant of disappearance of H+ is 1.0 × 107 mole l-1s-1. It would take for H+ in drop to disappear in ______ × 10-9s.


For a chemical reaction starting with some initial concentration of reactant At as a function of time (t) is given by the equation,

`1/("A"_"t"^4) = 2 + 1.5 xx 10^-3` t

The rate of disappearance of [A] is ____ × 10-2 M/sec when [A] = 2 M.

[Given: [At] in M and t in sec.]
[Express your answer in terms of 10-2 M /s]
[Round off your answer if required]


A reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is reduced to half?


Share
Notifications

Englishहिंदीमराठी


      Forgot password?
Use app×