JEE Main & Advanced Chemistry Chemical Kinetics / रासायनिक बलगतिकी Question Bank

done Mock Test - Chemical Kinetics Total Questions - 25

• question_answer1)
  In the formation of sulphur trioxide by the contact process, \[2S{{O}_{2}}+{{O}_{2}}\rightleftharpoons 2S{{O}_{3}}\], the rate of reaction was measured as  \[\frac{d[{{O}_{2}}]}{dt}=3.0\times {{10}^{-4}}mol\,{{L}^{-1}}{{s}^{-1}}\]. The rate of reaction expressed in terms of \[S{{O}_{3}}\] will be
  A)
  \[3.0\times {{10}^{-4}}mol\,{{L}^{-1}}{{s}^{-1}}\] done clear
  B)
  \[6.0\times {{10}^{-4}}mol\,{{L}^{-1}}{{s}^{-1}}\] done clear
  C)
  \[1.5\times {{10}^{-4}}mol\,{{L}^{-1}}{{s}^{-1}}\] done clear
  D)
  \[4.5\times {{10}^{-4}}mol\,{{L}^{-1}}{{s}^{-1}}\]   done clear
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• question_answer2)
  Which one of the following is wrongly matched?
  A)
  Saponification of \[C{{H}_{3}}COOC{{H}_{5}}\]- Second order reaction done clear
  B)
  Hydrolysis of \[C{{H}_{3}}COOC{{H}_{3}}\]- Pseudo unimolecular reaction done clear
  C)
  Decomposition of \[{{H}_{2}}{{O}_{2}}\]- First order reaction done clear
  D)
  Combination of \[{{H}_{2}}\] and \[{{B}_{2}}\] to give HBr -Zero order reaction done clear
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• question_answer3)

  The reaction, \[X+2Y+Z\to N\] occurs by the following mechanism

  (i) \[X+Y\rightleftharpoons M\] (very rapid equilibrium)

  (ii) \[M+Z\to O\](slow)

  (iii) \[O+Y~\to N\](very fast)

  What is the rate law for this reaction?

  A)
  Rate = k[Z]        done clear
  B)
  Rate = k[X] \[{{[Y]}^{2}}\] [Z] done clear
  C)
  Rate = k[N]       done clear
  D)
  Rate = k[X] [Y] [Z] done clear
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• question_answer4)
  The rate of the reaction, \[3A+2B\to \] Products is given by the rate expression: Rate k = [A]\[{{[B]}^{2}}\]. If A is taken in excess, the order of the reaction would be
  A)
  3          done clear
  B)
  2 done clear
  C)
  1                      done clear
  D)
  5 done clear
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• question_answer5)
  In a first-order reaction, the concentration of the reactant decreases from 0.8 M to 0.4 M in 15 minutes. The time taken for the concentration to change from 0.1 M to 0.025 M is
  A)
  60 minutes         done clear
  B)
  15 minutes done clear
  C)
  7.5 minutes        done clear
  D)
  30 minutes done clear
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• question_answer6)
  The rate for a first order reaction is \[0.6932\text{ }\times {{10}^{-2}}mol\,{{L}^{-1}}\] and the initial concentration of the reactants is 1 M, \[{{T}_{1/2}}\] is equal to
  A)
  6.932 mm          done clear
  B)
  100 min done clear
  C)
  \[0.6932\text{ }\times {{10}^{-3}}\min \] done clear
  D)
  \[0.6932\text{ }\times {{10}^{-2}}\min \] done clear
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• question_answer7)
  \[2A\to B+C\]. It would be a zero-order reaction when
  A)
  the rate of reaction is proportional to square of conc. of A done clear
  B)
  the rate of reaction remains same at any conc. of A done clear
  C)
  the rate remains unchanged at any conc. of B and done clear
  D)
  the rate of reaction doubles if conc. of B is increase to double. done clear
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• question_answer8)
  A gaseous compound A reacts by three independent first order processes (as shown in figure) with rate constant \[2\text{ }\times {{10}^{-3}}\], \[3\text{ }\times {{10}^{-3}}\] and \[1.93\text{ }\times {{10}^{-3}}\]\[{{\sec }^{-1}}\] for products B, and D respectively. If initially pure A was taken in a cloy container with P = 8 atm, then the partial pressure of B (in atm) after 100 sec from start of experiment
  A)
  0.288    done clear
  B)
  0.577 done clear
  C)
  1.154    done clear
  D)
  none of these done clear
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• question_answer9)
  A chemical reaction is said to take place through the various stages with \[\Delta G{}^\circ \] values indicated by the graph: Progress Stages I and II represent respectively
  A)

  I	II
  reaction intermediate	activated complex

  done clear
  B)

  activated complex

  activated complex

  done clear
  C)

  reaction intermediate

  reaction intermediate

  done clear
  D)

  activated complex

  reaction intermediate

  done clear
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• question_answer10)
        The specific rate constant of the decomposition of \[{{N}_{2}}{{O}_{5}}\] is 0.008\[{{\min }^{-1}}\]. The volume of \[{{O}_{2}}\]collected after 20 minutes is 16 mL. find the volume that would be collected at the end of reaction. \[N{{O}_{2}}\]formed is dissolved in \[CC{{l}_{4}}\]
  A)
  17.49 mL          done clear
  B)
  27.49 mL done clear
  C)
  37.49 mL          done clear
  D)
  47.49 mL done clear
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• question_answer11)
  A hydrogenation reaction is carried out at 500 K. \[C{{H}_{2}}=C{{H}_{2}}+{{H}_{2}}\xrightarrow[no\,catalyst]{500k}C{{H}_{3}}-C{{H}_{3}}\] Activation energy \[-\,{{E}_{a}}\,KJ\,mo{{l}^{-1}}\] \[C{{H}_{2}}=C{{H}_{2}}+{{H}_{2}}\xrightarrow{pd,400k}C{{H}_{3}}-C{{H}_{3}}\] Activation energy = (\[{{E}_{a}}-20\]) KJ \[mo{{l}^{-1}}\] If rate remains constant, then \[{{E}_{a}}\] is
  A)
  \[120\text{ }kJmo{{l}^{-1}}\]   done clear
  B)
  \[100\text{ }kJmo{{l}^{-1}}\] done clear
  C)
  \[20kJmo{{l}^{-1}}\]    done clear
  D)
  \[80\text{ }kJmo{{l}^{-1}}\] done clear
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• question_answer12)
  The rate constant of a certain reaction is given by log\[K\text{ }=A-\frac{B}{T}+C\,\log \,T\]. Then activation energy of reaction at 300 K is:
  A)
  \[\frac{B}{T}+C\,\log \,T\]          done clear
  B)
  \[[2.303\,B+CT]R\] done clear
  C)
  C log T  done clear
  D)
  B + CTR done clear
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• question_answer13)
  For the reaction, \[P\text{ }+\text{ }Q+\text{ }R\to S\] Experimental data for the measured initial rates in given below.

  Expt.	(P)	(Q)	(R)	Initial rate (in \[m{{s}^{-1}}\])
  1.	0.2M	0.5M	0.4M	\[8.0\times {{10}^{-5}}\]
  2.	0.4M	0.5M	0.4M	\[3.2\times {{10}^{-4}}\]
  3.	0.4M	2.0M	0.4M	\[1.28\times {{10}^{-3}}\]
  4.	0.1M	0.2M	1.6M	\[4.0\times {{10}^{-8}}\]

  The order of the reaction with respect of P, Q and R respectively is
  A)
  4, 1, 3   done clear
  B)
  2, 2, 1 done clear
  C)
  1, 2, 1   done clear
  D)
  2, 1, 1 done clear
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• question_answer14)
  The dissociation of nitrogen pentaoxide is a first order reaction. In first 12 min, 75% of nitrogen pentaoxide is dissociated. What amount of nitrogen pentaoxide will be left behind after one hour of the start of reaction?
  A)
  3.01%   done clear
  B)
  0.21% done clear
  C)
  0.098% done clear
  D)
  None of these done clear
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• question_answer15)
  Which of the following plot(s) is/are correct for the first order reaction?          
  A)
  I, II                   done clear
  B)
  II, III done clear
  C)
  I, II, III  done clear
  D)
  I, III done clear
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• question_answer16)
  The rate of a first order reaction is \[0.04\text{ }mol{{L}^{-1}}{{S}^{-1}}\] at 30 min and \[0.03\text{ }mol{{L}^{-1}}{{S}^{-1}}\] at 40 min. Thus, half-life of the reaction is
  A)
  32.4 mm           done clear
  B)
  51.2 mm done clear
  C)
  46.8 mm           done clear
  D)
  24.1 min done clear
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• question_answer17)
  Consider a first order decomposition process \[{{A}_{3}}\to \frac{3}{2}{{A}_{2}}\] A plot of concentration of \[{{A}_{3}}\] and \[{{A}_{2}}\] versus time is shown below. At time \[{{t}_{A}}\] percentage of reactant decomposed is
  A)
  75%                  done clear
  B)
  50% done clear
  C)
  40%                  done clear
  D)
  30% done clear
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• question_answer18)
  The rate law of a reaction \[A\text{ }+\text{ }B\text{ }\to \]Product is rate =\[k{{[A]}^{n}}\]\[{{[B]}^{n}}\] On doubling the concentration of A and halving the concentration of B, the ratio of new rate to the earlier rate of reaction will be
  A)
  \[n-m\]   done clear
  B)
  \[{{2}^{n-m}}\] done clear
  C)
  \[\frac{1}{{{2}^{m+n}}}\]      done clear
  D)
  \[m+n\] done clear
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• question_answer19)
  The energy of activations for forward and backward change for an endothermic reaction; X \[\to \] Y are \[{{E}_{F}}\] and \[{{E}_{b}}\] respectively. Which is correct?
  A)
   \[{{E}_{b}}<{{E}_{F}}\] done clear
  B)
   \[{{E}_{b}}>{{E}_{F}}\] done clear
  C)
   \[{{E}_{b}}={{E}_{F}}\] done clear
  D)
  No relation between them done clear
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• question_answer20)
  \[{{t}_{1/4}}\] can be taken as the time taken for concentration of reactant to drop to 3/4 of its initial value. If the rate constant for a first order reaction is k, then \[{{t}_{1/4}}\] can be written as
  A)
  0.10/K   done clear
  B)
  0.29/K done clear
  C)
  0.69/K   done clear
  D)
  0.15/K done clear
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• question_answer21)
  An organic compound undergoes first-order decomposition. The time taken for its decomposition to 1/8 and 1/10 of its initial concentration are \[{{t}_{1/8}}\] and \[{{t}_{1/10}}\] respectively. What is the value of\[\left[ \frac{{{t}_{1/8}}}{{{t}_{1/10}}} \right]\times 10\]? \[(lo{{g}_{10}}2=0.3)\,k=\frac{2.303}{t}\log \frac{[{{A}_{0}}]}{[A]}\]
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• question_answer22)
  A drop of solution of volume 0.05 ml contains \[3\times {{10}^{-6}}\] mole of \[{{H}^{+}}\] If the rate constant for the disappearance of \[{{H}^{+}}\] is \[{{10}^{7}}\] mol \[{{L}^{-1}}{{s}^{-1}}\]. How many nanoseconds it required for \[{{H}^{+}}\] in drop to disappear?
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• question_answer23)
  For the reaction,  \[A\left( g \right)\text{ }+\text{ }2B\left( g \right)\to C\left( g \right)\text{ }+\text{ }D\left( g \right)\] \[\frac{dx}{dt}=K[A]{{[B]}^{2}}\] Initial pressure of A and B are respectively 0.60 atm an 0.80 atm. At a time when pressure of C is 0.20 atm, ratio of initial rate and final rate is y. What is the value of y?
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• question_answer24)
  In the following first order competing reactions; A + Reagent \[\xrightarrow{{{k}_{1}}}\] Product B + Reagent \[\xrightarrow{{{k}_{2}}}\] Product The ratio of \[{{k}_{1}}/{{k}_{2}}\]if only 50% of B will have been react when 94% of A has been reacted is
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• question_answer25)
  If the rate of reaction is \[2.6\text{ }\times {{10}^{-3}}\] \[mol\,{{L}^{-1}}{{s}^{-1}}\] at \[50{}^\circ C\] and \[7.02\text{ }\times {{10}^{-2}}\] \[mol\,{{L}^{-1}}{{s}^{-1}}\] at\[80{}^\circ C\], then what will be 1 temperature coefficient of the reaction?
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