Solved papers for NEET Chemistry NEET PYQ-Chemical Kinetics

done NEET PYQ-Chemical Kinetics Total Questions - 49

• question_answer1) Activation energy of a chemical reaction can be determined by:                               [AIPMT 1998]
  A)
  evaluating rate constant at standard temperature
  done clear
  B)
  evaluating velocities of reaction at two different temperatures
  done clear
  C)
  evaluating rate constants at two different temperatures
  done clear
  D)
  changing concentration of reactants
  done clear
  View Answer play_arrow

• question_answer2) For a first-order reaction, the half-life period is independent of:                                 [AIPMT 1999]
  A)
  initial concentration                    
  done clear
  B)
  cube root of initial concentration
  done clear
  C)
  first power of final concentration  
  done clear
  D)
  square root of final concentration
  done clear
  View Answer play_arrow

• question_answer3) 

  In the following reaction, how is the rate of appearance of the underlined product related to the rate of disappearance of the underlined reactant?                               [AIPMT 2000]

  \[BrO_{3}^{-}(aq)+\underline{5B{{r}^{-}}(aq)}+6{{H}^{+}}(aq)\xrightarrow{{}}\]\[\underline{3B{{r}_{2}}(l)}+3{{H}_{2}}O(l)\]

  A)
        \[\frac{d[B{{r}_{2}}]}{dt}=-\frac{5}{3}\frac{d[B{{r}^{-}}]}{dt}\]
  done clear
  B)
  \[\frac{d[B{{r}_{2}}]}{dt}=-\frac{d[B{{r}^{-}}]}{dt}\]
  done clear
  C)
  \[\frac{d[B{{r}_{2}}]}{dt}=\frac{3}{5}\frac{d[B{{r}^{-}}]}{dt}\]         
  done clear
  D)
  \[\frac{d[B{{r}_{2}}]}{dt}=-\frac{3}{5}\frac{d[B{{r}^{-}}]}{dt}\]
  done clear
  View Answer play_arrow

• question_answer4) For the reactions \[2{{N}_{2}}{{O}_{5}}\to 4N{{O}_{2}}+{{O}_{2}}\] rate and rate constant are \[1.02\times {{10}^{-4}}\] and \[3.4\times {{10}^{-5}}\,{{s}^{-1}}\] respectively, then cone, of \[{{N}_{2}}{{O}_{5}}\] at that time will be:                                               [AIPMT 2001]
  A)
  1.732
  done clear
  B)
  3
  done clear
  C)
  \[1.02\times {{10}^{-4}}\]
  done clear
  D)
  \[3.4\times {{10}^{5}}\]
  done clear
  View Answer play_arrow

• question_answer5) When a biochemical reaction is carried out in laboratory from out-side of human body in the absence of enzyme then of reaction Obtained is \[{{10}^{-6}}\] times, then activation energy of reaction in the presence of enzyme is:         [AIPMT 2001]
  A)
  \[\frac{6}{RT}\]            
  done clear
  B)
                   P it required                  
  done clear
  C)
  Different from \[{{E}_{a}}\] obtained in laboratory
  done clear
  D)
  Cannot say any things
  done clear
  View Answer play_arrow

• question_answer6) \[3A\xrightarrow{{}}2B,\] rate of reaction \[+\frac{d[B]}{dt}\] is equal to: [AIPMT 2002]
  A)
  \[-\frac{3}{2}\frac{d[A]}{dt}\]
  done clear
  B)
  \[-\frac{2}{3}\frac{d[A]}{dt}\]
  done clear
  C)
  \[-\frac{1}{3}\frac{d[A]}{dt}\]
  done clear
  D)
  \[+2\frac{d\,[A]}{dt}\]
  done clear
  View Answer play_arrow

• question_answer7) \[3A\xrightarrow[{}]{{}}B+C\] It would be a zero order reaction when:                                            [AIPMT 2002]
  A)
  the rate of reaction is proportional to square of concentration of A
  done clear
  B)
  the rate of reaction remains same at any concentration of A
  done clear
  C)
  the rate remains unchanged at any concentration of B and C
  done clear
  D)
  the rate of reaction doubles if concentration of B is increased to double
  done clear
  View Answer play_arrow

• question_answer8) 

  The reaction \[A\to B\] follows first order kinetics. The time taken for 0.8 mole of A to produce 0.6 mole of B is 1 hour.

  What is the time taken for conversion of 0.9 mole of A to produce 0.675 mole of B?   [AIPMT 2003]

  A)
  0.25 h
  done clear
  B)
  2 h
  done clear
  C)
  1 h
  done clear
  D)
  0.5 h
  done clear
  View Answer play_arrow

• question_answer9) 

  The emf of a Daniell cell at 298 K is\[{{E}_{1}}\] [AIPMT 2003]

  \[ZN\,\left| \begin{align}   & ZnS{{O}_{4}} \\  & (0.01\,M) \\ \end{align} \right|\,\left| \begin{align}   & CuS{{O}_{4}} \\  & (1.0\,M) \\ \end{align} \right|Cu\]

  When the concentration of \[ZnS{{O}_{4}}\] is 1.0 M and that of \[CuS{{O}_{4}}\] is 0.01 M, the emf changed to \[{{E}_{2}}.\]What is the relationship between \[{{E}_{1}}\] and \[{{E}_{2}}\]?

  A)
  \[{{E}_{1}}={{E}_{2}}\]
  done clear
  B)
  \[{{E}_{2}}=0\,\ne {{E}_{1}}\]
  done clear
  C)
  \[{{E}_{1}}>E{{ & }_{2}}\]
  done clear
  D)
  \[{{E}_{1}}<{{E}_{2}}\]
  done clear
  View Answer play_arrow

• question_answer10) The temperature dependence of rate constant (k) of a chemical reaction is written in terms of Arrhenius equation, \[k=A{{e}^{-E*/RT}}\]. Activation energy \[(E*)\] of the reaction can be calculated by ploting: [AIPMT 2003]
  A)
  \[\log \,k\,vs\frac{1}{T}\]
  done clear
  B)
  \[\log \,k\,vs\,\frac{1}{\log \,T}\]
  done clear
  C)
  \[k\,vs\,T\]
  done clear
  D)
  \[k\,vs\frac{1}{\log \,T}\]
  done clear
  View Answer play_arrow

• question_answer11) If the rate of the reaction is equal to the rate constant, the order of the reaction is:       [AIPMT 2003]
  A)
  2
  done clear
  B)
  3
  done clear
  C)
  0
  done clear
  D)
  1
  done clear
  View Answer play_arrow

• question_answer12) The activation energy for a simple chemical reaction \[A\to B\] is \[{{E}_{a}}\] in forward direction. The activation energy for reverse reaction:                                                 [AIPMT 2003]
  A)
  can be less than or more than \[{{E}_{a}}\]                   
  done clear
  B)
  is always double of \[{{E}_{a}}\]
  done clear
  C)
  is negative of \[{{E}_{a}}\]                 
  done clear
  D)
  is always less than \[{{E}_{a}}\]
  done clear
  View Answer play_arrow

• question_answer13) The rate of first order reaction is \[1.5\times {{10}^{-2}}\,mo{{l}^{-1}}\,{{\min }^{-1}}\] at 0.5 M concentration of the reactant. The half-life of the reaction is: [AIPMT (S) 2004]
  A)
  0.383 mm
  done clear
  B)
  23.1 mm
  done clear
  C)
  8.73 mm
  done clear
  D)
  7.53 mm
  done clear
  View Answer play_arrow

• question_answer14) For a first order reaction \[A\xrightarrow[{}]{{}}B\,,\] the reaction rate at reactant concentration of 0.01 M is found to be \[2.0\times {{10}^{-5}}\,mol\,{{L}^{-1}}\,{{s}^{-1}}\]. The half-life period of the reaction is:                       [AIPMT (S) 2005]
  A)
  220 s
  done clear
  B)
  30 s 
  done clear
  C)
  300 s
  done clear
  D)
  347 s
  done clear
  View Answer play_arrow

• question_answer15) The rate of reaction between two reactants A and B decreases by a factor of 4, if die concentration of reactant B is doubled. The order of this reaction with respect to reactant B is: [AIPMT (S) 2005]
  A)
  - 1
  done clear
  B)
  - 2
  done clear
  C)
  1
  done clear
  D)
  2
  done clear
  View Answer play_arrow

• question_answer16) For the reaction \[2A+B~\to 3C+D\]which of the following does not express the reaction rate?  [AIPMT (S) 2006]
  A)
  \[-\frac{d\,[C]}{3\,dt}\]
  done clear
  B)
  \[-\frac{d\,[B]}{dt}\]      
  done clear
  C)
  \[\frac{d\,[D]}{dt}\]
  done clear
  D)
   \[-\frac{d\,[A]}{2\,dt}\]
  done clear
  View Answer play_arrow

• question_answer17) 

  Consider the reaction \[{{N}_{2}}(g)+3{{H}_{2}}(g)\xrightarrow{{}}2N{{H}_{3}}(g)\]

  The equality relationship between \[\frac{d[N{{H}_{3}}]}{dt}\] and \[-\frac{d[{{H}_{2}}]}{dt}\] is:                  [AIPMT (S) 2006]

  A)
  \[\frac{d\,[N{{H}_{3}}]}{dt}=-\frac{1}{3}\,\frac{d\,[{{H}_{2}}]}{dt}\]
  done clear
  B)
  \[+\frac{d\,[N{{H}_{3}}]}{dt}=-\frac{2}{3}\,\frac{d\,[{{H}_{2}}]}{dt}\]           
  done clear
  C)
  \[+\frac{d\,[N{{H}_{3}}]}{dt}=-\frac{3}{2}\,\frac{d\,[{{H}_{2}}]}{dt}\]
  done clear
  D)
  \[\frac{d\,[N{{H}_{3}}]}{dt}=-\,\frac{d\,[{{H}_{2}}]}{dt}\]
  done clear
  View Answer play_arrow

• question_answer18) 

  The reaction of hydrogen and iodine monochloride is given as:      [AIPMT (S) 2007]

  \[{{H}_{2}}(g)+2ICl(g)\xrightarrow{{}}2HCl(g)+{{I}_{2}}(g)\]

  This reaction is of first order with respect to \[{{H}_{2}}(g)\] and \[ICl(g),\] following mechanisms were proposed:

  Mechanism A:    \[{{H}_{2}}(g)+2ICl(g)\xrightarrow{{}}2HCl(g)+{{I}_{2}}(g)\]

  Mechanism B: \[{{H}_{2}}(g)+ICl(g)\xrightarrow{{}}HCl(g)+HI(g)\]; show

  \[HI(g)+ICl(g)\xrightarrow{{}}HCl(g)+{{I}_{2}}(g)\]; fast

  Which of the above mechanism (s) can be consistent with the given information about the reaction?

  A)
  B only
  done clear
  B)
  A and B both
  done clear
  C)
  Neither A nor B
  done clear
  D)
  A only
  done clear
  View Answer play_arrow

• question_answer19) In a first order reaction \[A\xrightarrow[{}]{{}}B,\] if k is rate constant and  initial  concentration  of the reactant A is 0.5 M then the half-life is :                                                               [AIPMT (S) 2007]
  A)
                              \[\frac{0.693}{0.5\,k}\]
  done clear
  B)
  \[\frac{\log \,2}{k}\]
  done clear
  C)
        \[\frac{\log \,2}{k\sqrt{0.5}}\]
  done clear
  D)
        \[\frac{\ln \,2}{k}\]
  done clear
  View Answer play_arrow

• question_answer20) 

  If 60% of a first order reaction was completed in 60 min 50% of the same reaction would be completed in approximately: [AIPMT (S) 2007]

  (log 4 = 0.60 log 5 = 0.69)

  A)
  50 min
  done clear
  B)
  45 min
  done clear
  C)
  60 min
  done clear
  D)
  40 min
  done clear
  View Answer play_arrow

• question_answer21) The rate constants \[{{k}_{1}}\] and \[{{k}_{2}}\] for two different reactions are \[{{10}^{16}}.{{e}^{-2000/T}}\] and \[{{10}^{15}}.{{e}^{-1000/T}},\] respectively. The temperature at which \[{{k}_{1}}={{k}_{2}}\] is [AIPMT (S) 2008]
  A)
  1000 K
  done clear
  B)
  \[\frac{2000}{2.303}K\]
  done clear
  C)
  2000K
  done clear
  D)
  \[\frac{1000}{2.303}K\]
  done clear
  View Answer play_arrow

• question_answer22) 

  The bromination of acetone that occurs in acid solution is represented by this equation. [AIPMT (S) 2008]

  \[C{{H}_{3}}COC{{H}_{3}}(aq)+B{{r}_{2}}(aq)\xrightarrow[{}]{{}}\]\[C{{H}_{3}}COC{{H}_{2}}Br(aq)+{{H}^{+}}(aq)+B{{r}^{-}}(aq)\]

  These kinetic data were obtained for given reaction concentrations.

  Initial concentrations, M

  \[[C{{H}_{3}}COC{{H}_{3}}]\]            \[[B{{r}_{2}}]\]             \[[{{H}^{+}}]\]

  0.30                  0.05                  0.05

  0.30                  0.10                  0.05

  0.30                  0.10                  0.10

  0.40                  0.05                  0.20

  Initial rate, disappearance of \[B{{r}_{2}},M{{s}^{-1}}\]

  \[5.7\times {{10}^{-5}}\]

  \[5.7\times {{10}^{-5}}\]

  \[1.2\times {{10}^{-4}}\]

  \[3.1\times {{10}^{-4}}\]

  Based on these data, the rate equation is

  A)
  Rate \[=k[C{{H}_{3}}COC{{H}_{3}}][{{H}^{+}}]\]
  done clear
  B)
  Rate \[=k[CH=COC{{H}_{3}}][B{{r}_{2}}]\]
  done clear
  C)
  Rate \[=k[C{{H}_{3}}COC{{H}_{3}}][B{{r}_{2}}]{{[{{H}^{+}}]}^{2}}\]
  done clear
  D)
  Rate \[=k[C{{H}_{3}}COC{{H}_{3}}][B{{r}_{2}}]{{[{{H}^{+}}]}^{2}}\]
  done clear
  View Answer play_arrow

• question_answer23) Half-life period of a first order reaction is 1386s. The specific rate constant of the reaction is [AIPMT (S) 2009]
  A)
  \[{{(C{{H}_{3}})}_{2}}P\]
  done clear
  B)
  \[{{(C{{H}_{3}})}_{3}}N\]
  done clear
  C)
  \[0.5\times {{10}^{-3}}\,{{s}^{-1}}\]
  done clear
  D)
  \[0.0\times {{10}^{-2}}\,{{s}^{-1}}\]
  done clear
  View Answer play_arrow

• question_answer24) For the reaction, \[(At.no.Zn=30,Sc=21,Ti=22,Cr=24)\]if \[{{[Sc{{({{H}_{2}}O)}_{3}}{{(N{{H}_{3}})}_{3}}]}^{3+}}\] mol \[{{[Ti{{(en)}_{2}}{{(N{{H}_{3}})}_{2}}]}^{4+}}\]the value of \[{{[Cr{{(N{{H}_{3}})}_{6}}]}^{2+}}\]would be                [AIPMT (S) 2009]
  A)
  \[{{[Zn{{(N{{H}_{3}})}_{6}}]}^{2+}}\]
  done clear
  B)
  \[5.0\times {{10}^{-3}}{{s}^{-1}}\]
  done clear
  C)
  \[0.5\times {{10}^{-2}}{{s}^{-1}}\]
  done clear
  D)
  \[0.5\times {{10}^{-3}}{{s}^{-1}}\]
  done clear
  View Answer play_arrow

• question_answer25) 

  In the reaction,                  [AIPMT (S) 2009]

  \[\frac{-d[{{H}_{2}}]}{dt}\]

  \[3\times {{10}^{4}}\,mol\,{{L}^{-1}}\,{{s}^{-1}}\]

  The rate of appearance of bromine \[4\times {{10}^{4}}\,mol\,{{L}^{-1}}\,{{s}^{-1}}\]) is related to rate of disappearance of bromide ions as following

  A)
  \[6\times {{10}^{4}}\,mol\,{{L}^{-1}}\,{{s}^{-1}}\]
  done clear
  B)
  \[1\times {{10}^{4}}\,mol\,{{L}^{-1}}\,{{s}^{-1}}\]
  done clear
  C)
  \[[O{{H}^{-}}]\]
  done clear
  D)
  \[\text{Ba(OH}{{\text{)}}_{\text{2}}}\]
  done clear
  View Answer play_arrow

• question_answer26) For the reaction, \[{{N}_{2}}{{O}_{5}}(g)\xrightarrow[{}]{{}}2N{{O}_{2}}(g)+\frac{1}{2}{{O}_{2}}(g)\]the value of rate of disappearance of \[{{\text{N}}_{\text{2}}}{{\text{O}}_{\text{5}}}\] is given as \[6.25\times {{10}^{-3}}\]\[\text{mol}\,{{\text{L}}^{\text{-1}}}{{\text{s}}^{\text{-1}}}\]. The rate of formation of \[N{{O}_{2}}\] and \[{{O}_{2}}\] is given respectively as            [AIPMT (S) 2010]
  A)
  \[6.25\times {{10}^{-3}}mol\,{{L}^{-1}}{{s}^{-1}}\]and \[6.25\times {{10}^{-3}}mol\,{{L}^{-1}}{{s}^{-1}}\]
  done clear
  B)
  \[1.25\times {{10}^{-2}}mol\,{{L}^{-1}}{{s}^{-1}}\]and\[3.125\times {{10}^{-3}}mol\,{{L}^{-1}}{{s}^{-1}}\]
  done clear
  C)
  \[6.25\times {{10}^{-3}}mol\,{{L}^{-1}}{{s}^{-1}}\]and \[3.125\times {{10}^{-3}}mol\,{{L}^{-1}}{{s}^{-1}}\]
  done clear
  D)
  \[1.25\times {{10}^{-3}}mol\,{{L}^{-1}}{{s}^{-1}}\]and \[6.25\times {{10}^{-3}}mol\,{{L}^{-1}}{{s}^{-1}}\]
  done clear
  View Answer play_arrow

• question_answer27) 

  During the kinetic study of the reaction, \[2A+B\to C+D,\] following results were obtained        [AIPMT (S) 2010]

  \[Ru\,[A]/mol\,{{L}^{-1}}[B]/mol\,{{L}^{-1}}\]Initial rate of formation of \[D/mol\,{{L}^{-1}}{{\min }^{-1}}\]

  I           0.1        0.1        \[6.0\times {{10}^{-3}}\]

  II          0.3        0.2        \[7.2\times {{10}^{-2}}\]

  III         0.3        0.4        \[2.88\times {{10}^{-1}}\]

  IV         0.4        0.1        \[2.40\times {{10}^{-2}}\]

  Based on the above data which one of the following is correct ?

  A)
  \[rate=k{{[A]}^{2}}[B]\]
  done clear
  B)
  \[rate=k[A][B]\]
  done clear
  C)
  \[rate=k{{[A]}^{2}}{{[B]}^{2}}\]
  done clear
  D)
  \[rate=k[A]{{[B]}^{2}}\]
  done clear
  View Answer play_arrow

• question_answer28) The rate of the reaction,\[2NO+C{{l}_{2}}\xrightarrow[{}]{{}}2NOCl\]is given by the rate equation, rate\[=k{{[NO]}^{2}}[C{{l}_{2}}]\]The value of the rate constant can be increased by [AIPMT (M) 2010]
  A)
  increasing the temperature
  done clear
  B)
  increasing the concentration of NO
  done clear
  C)
  increasing the concentration of the Cl2 doing
  done clear
  D)
  all of the above
  done clear
  View Answer play_arrow

• question_answer29) Which one of the following statements for the order of a reaction is incorrect? [AIPMT (S) 2011]
  A)
  Order is not influenced by stoichiometric coefficient of the reactants
  done clear
  B)
  Order of reaction is sum of power to the concentration terms of reactants to express the rate of reaction
  done clear
  C)
  Order of reaction is always whole number
  done clear
  D)
  Order   can   be   determined   only experimentally
  done clear
  View Answer play_arrow

• question_answer30) The half-life of a substance in a certain enzyme-catalyses reaction is 138 s. The time required for the concentration of the substance to fall from 1.28 mg \[{{\text{L}}^{\text{-1}}}\] to 0.04 mg \[{{\text{L}}^{\text{-1}}}\] is [AIPMT (M) 2011]
  A)
  414 s
  done clear
  B)
  552 s
  done clear
  C)
  690 s
  done clear
  D)
  276 s
  done clear
  View Answer play_arrow

• question_answer31) 

  The rate of reaction \[2{{N}_{2}}{{O}_{5}}\xrightarrow[{}]{{}}4N{{O}_{2}}+{{O}_{2}}\]can be written in three ways

  \[\frac{-d[{{N}_{2}}{{O}_{5}}]}{dt}=k[{{N}_{2}}{{O}_{5}}]\]            \[\frac{d[NO_{7}^{2}]}{dt}=k'[{{N}_{2}}{{O}_{5}}]\]

  \[\frac{d[O_{2}^{{}}]}{dt}=k''[{{N}_{2}}{{O}_{5}}]\]    [AIPMT (M) 2011]

  The relationship between k and k' and between k’’ and k'' are

  A)
  k’ = 2 k; k’ = k
  done clear
  B)
  k’ = 2k; k’’=k/2
  done clear
  C)
  k’ = 2k; k’’ = 2k
  done clear
  D)
  k’ = k; k’’ = k
  done clear
  View Answer play_arrow

• question_answer32) The unit of rate constant for- a zero order reaction is                                        [AIPMT (M) 2011]
  A)
  \[\text{mol}\,{{\text{L}}^{\text{-1}}}\,{{\text{s}}^{\text{-1}}}\]
  done clear
  B)
  \[\text{L}\,\text{mo}{{\text{l}}^{\text{-1}}}\,{{\text{s}}^{\text{-1}}}\]
  done clear
  C)
  \[{{\text{L}}^{\text{2}}}\,\text{mo}{{\text{l}}^{\text{-2}}}\,{{\text{s}}^{\text{-1}}}\]
  done clear
  D)
  \[\,{{\text{s}}^{\text{-1}}}\]
  done clear
  View Answer play_arrow

• question_answer33) In a reaction, \[\text{A}\,\text{+}\,\text{B}\to \] Product, rate is doubled when the concentration of B is doubled, and rate increases by a factor of 8 when the concentrations of both the reactants (A and B) are doubled. Rate law for the reaction can be written a [AIPMT (S) 2012]
  A)
  \[\text{Rate}\,\text{=}\,\text{k}\,\text{ }\!\![\!\!\text{ A }\!\!]\!\!\text{ }\,{{\text{ }\!\![\!\!\text{ B }\!\!]\!\!\text{ }}^{\text{2}}}\]
  done clear
  B)
  \[\text{Rate}\,\text{=}\,\text{k}\,{{\text{ }\!\![\!\!\text{ A }\!\!]\!\!\text{ }}^{\text{2}}}\,{{\text{ }\!\![\!\!\text{ B }\!\!]\!\!\text{ }}^{\text{2}}}\]
  done clear
  C)
  \[\text{Rate}\,\text{=}\,\text{k}\,\text{ }\!\![\!\!\text{ A }\!\!]\!\!\text{ }\,\text{ }\!\![\!\!\text{ B }\!\!]\!\!\text{ }\]
  done clear
  D)
  \[\text{Rate}\,\text{=}\,\text{k }\!\![\!\!\text{ A}{{\text{ }\!\!]\!\!\text{ }}^{\text{2}}}\text{ }\!\![\!\!\text{ B }\!\!]\!\!\text{ }\]
  done clear
  View Answer play_arrow

• question_answer34) In a zero order reaction for every 10° rise of temperature, the rate is doubled. If the temperature is increased from 10°C to 100°C, the rate of the reaction will become [AIPMT (S) 2012]
  A)
  256 times
  done clear
  B)
  512 times
  done clear
  C)
  64 times
  done clear
  D)
  128 times
  done clear
  View Answer play_arrow

• question_answer35) Activation energy (Ea) and rate constants (k1 and k2) of a chemical reaction at two different temperatures T1 and T2) are related by  [AIPMT (M) 2012]
  A)
  \[\ln \frac{{{k}_{2}}}{{{k}_{1}}}=-\frac{{{E}_{a}}}{R}\left( \frac{1}{{{T}_{1}}}-\frac{1}{{{T}_{2}}} \right)\]
  done clear
  B)
  \[\ln \frac{{{k}_{2}}}{{{k}_{1}}}=-\frac{{{E}_{a}}}{R}\left( \frac{1}{{{T}_{2}}}-\frac{1}{{{T}_{1}}} \right)\]
  done clear
  C)
  \[\ln \frac{{{k}_{2}}}{{{k}_{1}}}=-\frac{{{E}_{a}}}{R}\left( \frac{1}{{{T}_{2}}}+\frac{1}{{{T}_{1}}} \right)\]
  done clear
  D)
  \[\ln \frac{{{k}_{2}}}{{{k}_{1}}}=\frac{{{E}_{a}}}{R}\left( \frac{1}{{{T}_{1}}}-\frac{1}{{{T}_{2}}} \right)\]
  done clear
  View Answer play_arrow

• question_answer36) 

  What is the activation energy for a reaction if its rate doubles when the temperature is raised from 20°C to 35°C?

  (\[\text{R=}\,\text{8}\text{.314}\,\text{J}\,\text{mo}{{\text{l}}^{\text{-1}}}\,{{\text{K}}^{\text{-1}}}\])[NEET 2013]

  A)
  \[\text{342}\,\text{kJ}\,\text{mo}{{\text{l}}^{\text{-1}}}\]
  done clear
  B)
  \[269\,\text{kJ}\,\text{mo}{{\text{l}}^{\text{-1}}}\]
  done clear
  C)
  \[34.7\,\text{kJ}\,\text{mo}{{\text{l}}^{\text{-1}}}\]
  done clear
  D)
  \[15.1\,\text{kJ}\,\text{mo}{{\text{l}}^{\text{-1}}}\]
  done clear
  View Answer play_arrow

• question_answer37) A reaction having equal energies of activation for forward and reverse reactions has [NEET 2013]
  A)
  \[\Delta S=0\]
  done clear
  B)
  \[\Delta G=0\]
  done clear
  C)
  \[\Delta H=0\]
  done clear
  D)
  \[\Delta H=\Delta G=\Delta S=0\]
  done clear
  View Answer play_arrow

• question_answer38) The activation energy of a reaction can be determined from the slope of which of the following graphs?         [NEET 2015 ]
  A)
  In \[K\,vsT\]
  done clear
  B)
  \[\frac{\text{ln}K}{T}vsT\]
  done clear
  C)
  In \[Kvs\frac{l}{T}\]
  done clear
  D)
  \[\frac{T}{\ln \,k}vs\frac{l}{T}\]
  done clear
  View Answer play_arrow

• question_answer39) When initial concentration of a reactant is doubled in a reaction, its half-life period is not affected. The order of the reaction is [NEET 2015 ]
  A)
  zero
  done clear
  B)
  first
  done clear
  C)
  second
  done clear
  D)
  more than zero but less than first
  done clear
  View Answer play_arrow

• question_answer40) The rate constant of the reaction A ® B is \[0.6\times {{10}^{-3}}\] mole per second. If the concentration of A is 5 M then concentration of B after 20 min is                             [NEET 2015 (Re)]
  A)
  1.08 M
  done clear
  B)
  3.60 M
  done clear
  C)
  0.36 M
  done clear
  D)
  0.72 M
  done clear
  View Answer play_arrow

• question_answer41) The rat e of a first -order react ion is \[\text{0}\text{.04}\,\text{mol}\,{{\ell }^{-1}}{{s}^{-1}}\]at 10 seconds and \[0.03\,\text{mol }{{\ell }^{-1}}{{s}^{-1}}\]at 20 seconds after initiation of the reaction. The half-life period of the reaction is:                                           [NEET - 2016]
  A)
  24.1 s
  done clear
  B)
  34.1 s
  done clear
  C)
  44.1 s
  done clear
  D)
  54.1 s
  done clear
  View Answer play_arrow

• question_answer42) 

  Mechanism of a hypothetical reaction\[{{X}_{2}}+{{Y}_{2}}\to 2XY\] is given below:            [NEET-2017]

  (i) \[{{X}_{2}}\to X+X(fast)\]

  (ii) \[X+{{Y}_{2}}XY+Y(slow)\]

  (iii)\[X+Y\to XY(fast)\]

  The overall order of the reaction will be

  A)
              1.5
  done clear
  B)
  1
  done clear
  C)
              2
  done clear
  D)
  0
  done clear
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• question_answer43) A first order reaction has a specific reaction rate of\[{{10}^{-2}}{{s}^{-1}}.\] How much time will it take for 20 g of the reactant to reduce to 5 g?       [NEET-2017]
  A)
  693.0 second
  done clear
  B)
  238.6 second
  done clear
  C)
  138.6 second
  done clear
  D)
  346.5 second
  done clear
  View Answer play_arrow

• question_answer44) The correct difference between first and second order reactions is that  [NEET-2018]
  A)
  A first-order reaction can catalyzed; a second-order reaction cannot be catalyzed
  done clear
  B)
  The half-life of a first-order reaction does not depend on \[{{\text{ }\!\![\!\!\text{ A }\!\!]\!\!\text{ }}_{0}}\]; the half-life of a second-order reaction does depend on \[{{\text{ }\!\![\!\!\text{ A }\!\!]\!\!\text{ }}_{0}}\]
  done clear
  C)
  The rate of a first-order reaction does not depend on reactant concentrations; the rate of a second-order reaction does depend on reactant concentrations
  done clear
  D)
  The rate of a first-order reaction does depend on reactant concentrations; the rate of a second-order reaction does not depend on reactant concentrations.
  done clear
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• question_answer45) When initial concentration of the reactant is doubled, the half-life period of a zero order reaction                          [NEET - 2018]
  A)
  Is tripled          
  done clear
  B)
  Is doubled
  done clear
  C)
  Is halved                     
  done clear
  D)
  Remains unchanged
  done clear
  View Answer play_arrow

• question_answer46) For the chemical reaction \[{{N}_{2}}\text{(g)}+3{{H}_{2}}(g)\rightleftharpoons 2N{{H}_{3}}\left( g \right)\]  [NEET 2019]
  A)
  \[-\frac{d[{{N}_{2}}]}{dt}=\frac{1}{2}\frac{d[N{{H}_{3}}]}{dt}\]
  done clear
  B)
  \[3\frac{d[{{H}_{2}}]}{dt}=2\frac{d[N{{H}_{3}}]}{dt}\]
  done clear
  C)
  \[-\frac{1}{3}\frac{d[{{H}_{2}}]}{dt}=-\frac{1}{2}\frac{d[N{{H}_{3}}]}{dt}\]
  done clear
  D)
  \[-\frac{d[{{N}_{2}}]}{dt}=2\frac{d[N{{H}_{3}}]}{dt}\]
  done clear
  View Answer play_arrow

• question_answer47) If the rate constant for a first order reaction is k, the time (t) required for the completion of 99 % of the reaction is given by-           [NEET 2019]
  A)
  t = 4.606/k
  done clear
  B)
  t = 2.303/k
  done clear
  C)
  t = 0.693/k
  done clear
  D)
  t = 6.909/k
  done clear
  View Answer play_arrow

• question_answer48) The rate constant for a first order reaction is\[4.606\times {{10}^{3}}{{s}^{1}}\]. The time required to reduce 2.0 g of the reactant to 0.2 g is:         [NEET 2020]
  A)
  200 s
  done clear
  B)
  500 s
  done clear
  C)
  1000 s
  done clear
  D)
  100 s
  done clear
  View Answer play_arrow

• question_answer49) An increase in the concentration of the reactants of a reaction leads to change in         [NEET 2020]
  A)
  heat of reaction
  done clear
  B)
  threshold energy
  done clear
  C)
  collision frequency
  done clear
  D)
  activation energy
  done clear
  View Answer play_arrow