JEE Main & Advanced Chemistry Equilibrium / साम्यावस्था Question Bank

done Topic Test - Chemical Equilibrium (6-5-21) Total Questions - 40

• question_answer1)
  The reaction \[CaC{{O}_{3}}\] \[\rightleftharpoons \] \[CaO+C{{O}_{2}}(g)\] goes to completion in lime kiln because
  A)
  Of the high temperature done clear
  B)
  \[CaO\] is more stable than \[CaC{{O}_{3}}\] done clear
  C)
  \[CaO\] is not dissociated done clear
  D)
  \[C{{O}_{2}}\] escapes continuously done clear
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• question_answer2)
  All reactions which have chemical disintegration
  A)
  Is reversible done clear
  B)
  Is reversible and endothermic done clear
  C)
  Is exothermic done clear
  D)
  Is reversible or irreversible and endothermic or exothermic done clear
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• question_answer3)
  Which of the following conditions represents an equilibrium
  A)
  Freezing of ice in a open vessel, temperature of ice is constant done clear
  B)
  Few drops of water is present along with air in a balloon, temperature of balloon is constant done clear
  C)
  Water is boiling in an open vessel over stove, temperature of water is constant done clear
  D)
  All the statements [a], [b] and [c] are correct for the equilibrium done clear
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• question_answer4)
  If a system is at equilibrium the rate of forward to the reverse reaction is                    
  A)
  Less      done clear
  B)
  Equal done clear
  C)
  High done clear
  D)
  At equilibrium done clear
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• question_answer5)
  In a reaction the rate of reaction is proportional to its active mass, this statement is known as  
  A)
  Law of mass action done clear
  B)
  Le-chatelier principle done clear
  C)
  Faraday law of electrolysis done clear
  D)
  Law of constant proportion done clear
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• question_answer6)
  In the thermal decomposition of potassium chlorate given as \[2K\,Cl{{O}_{3}}\xrightarrow{{}}2KCl+3{{O}_{2}}\], law of mass action
  A)
  Cannot be applied done clear
  B)
  Can be applied done clear
  C)
  Can be applied at low temperature done clear
  D)
  Can be applied at high temp and pressure done clear
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• question_answer7)
  The equilibrium constant in a reversible reaction at a given temperature                     
  A)
  Depends on the initial concentration of the reactants done clear
  B)
  Depends on the concentration of the products at equilibrium done clear
  C)
  Does not depend on the initial concentrations done clear
  D)
  It is not characteristic of the reaction done clear
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• question_answer8)
  Unit of equilibrium constant for the reversible reaction \[{{H}_{2}}+{{I}_{2}}\]sss. \[2HI\] is            
  A)
  \[mo{{l}^{-1}}\,litre\] done clear
  B)
  \[mo{{l}^{-2}}\,litre\] done clear
  C)
  \[mol\,\,litr{{e}^{-1}}\] done clear
  D)
  None of these done clear
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• question_answer9)
  In a chemical equilibrium, the rate constant of the backward reaction is \[7.5\times {{10}^{-4}}\] and the equilibrium constant is 1.5. So the rate constant of the forward reaction is          
  A)
  \[5\times {{10}^{-4}}\] done clear
  B)
  \[2\times {{10}^{-3}}\] done clear
  C)
  \[1.125\times {{10}^{-3}}\] done clear
  D)
  \[9.0\times {{10}^{-4}}\] done clear
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• question_answer10)
  15 moles of \[{{H}_{2}}\] and 5.2 moles of \[{{I}_{2}}\] are mixed and allowed to attain equilibrium at \[{{500}^{o}}C\]. At equilibrium, the concentration of \[HI\] is found to be 10 moles. The equilbrium constant for the formation of \[HI\] is 
  A)
  50 done clear
  B)
  15 done clear
  C)
  100 done clear
  D)
  25 done clear
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• question_answer11)
  The reaction, \[2S{{O}_{2(g)}}+{{O}_{2(g)}}\]\[\rightleftharpoons \] \[2S{{O}_{3(g)}}\] is carried out in a 1\[d{{m}^{3}}\]vessel and \[2\ d{{m}^{3}}\]vessel separately. The ratio of the reaction velocities will be     
  A)
  \[1:8\]    done clear
  B)
  \[1:4\] done clear
  C)
  \[4:1\] done clear
  D)
  \[8:1\] done clear
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• question_answer12)
  5 moles of \[S{{O}_{2}}\] and 5 moles of \[{{O}_{2}}\] are allowed to react to form \[S{{O}_{3}}\] in a closed vessel. At the equilibrium stage 60% of \[S{{O}_{2}}\] is used up. The total number of moles of \[S{{O}_{2}}\], \[{{O}_{2}}\] and \[S{{O}_{3}}\] in the vessel now is
  A)
  10.0 done clear
  B)
  8.5 done clear
  C)
  10.5 done clear
  D)
  3.9 done clear
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• question_answer13)
  The relation between equilibrium constant \[{{K}_{p}}\] and \[{{K}_{c}}\] is          
  A)
  \[{{K}_{c}}={{K}_{p}}\,{{(RT)}^{\Delta n}}\] done clear
  B)
  \[{{K}_{p}}={{K}_{c}}{{(RT)}^{\Delta n}}\] done clear
  C)
  \[{{K}_{p}}={{\left( \frac{{{K}_{c}}}{RT} \right)}^{\Delta n}}\] done clear
  D)
  \[{{K}_{p}}-{{K}_{c}}={{(RT)}^{\Delta n}}\] done clear
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• question_answer14)
  \[{{H}_{2}}+{{I}_{2}}\]\[\rightleftharpoons \]\[2HI\] In the above equilibrium system if the concentration of the reactants at \[{{25}^{o}}C\] is increased, the value of \[{{K}_{c}}\] will
  A)
        Increase done clear
  B)
  Decrease done clear
  C)
  Remains the same done clear
  D)
  Depends on the nature of the reactants done clear
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• question_answer15)
  The equilibrium constant \[({{K}_{p}})\] for the reaction \[PC{{l}_{5}}(g)\to PC{{l}_{3}}(g)+C{{l}_{2}}(g)\] is 16. If the volume of the container is reduced to one half its original volume, the value of \[{{K}_{p}}\] for the reaction at the same temperature will be
  A)
  32 done clear
  B)
  64 done clear
  C)
  16 done clear
  D)
  4 done clear
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• question_answer16)
  \[CaC{{O}_{3(s)}}\]\[\rightleftharpoons \]\[Ca{{O}_{(s)}}+C{{O}_{2(g)}}\] which of the following expression is correct                            
  A)
  \[{{K}_{P}}=({{P}_{CaO}}+{{P}_{C{{O}_{2}}}}/{{P}_{CaC{{O}_{3}}}})\] done clear
  B)
  \[{{K}_{P}}={{P}_{C{{O}_{2}}}}\]    done clear
  C)
  \[{{K}_{P}}\times ({{P}_{CaO}}\times {{P}_{C{{O}_{2}}}}).{{P}_{CaC{{O}_{3}}}}\] done clear
  D)
  \[\frac{{{K}_{p}}[CaO][C{{O}_{2}}]}{[CaC{{O}_{3}}]}\] done clear
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• question_answer17)
  In which of the following reactions, increase in the volume at constant temperature don’t affect the number of moles at equilibrium.                       
  A)
  \[2N{{H}_{3}}\]\[\rightleftharpoons \] \[{{N}_{2}}+3{{H}_{2}}\] done clear
  B)
  \[{{C}_{(g)}}\]\[+\ \frac{1}{2}\] \[{{O}_{2(g)}}\]\[\to \]\[C{{O}_{(g)}}\]     done clear
  C)
  \[{{H}_{2(g)}}\]+ \[{{O}_{2(g)}}\] \[\to \]\[{{H}_{2}}{{O}_{2(g)}}\] done clear
  D)
  None of these done clear
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• question_answer18)
  What is the effect of increasing pressure on the dissociation of \[PC{{l}_{5}}\] according to the equation \[PC{{l}_{5(g)}}\]\[\rightleftharpoons \] \[PC{{l}_{3(g)}}+C{{l}_{2(g)}}-x\ cal\]   
  A)
        Dissociation decreases done clear
  B)
  Dissociation increases done clear
  C)
  Dissociation does not change done clear
  D)
  None of these done clear
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• question_answer19)
  The vapour density of completely dissociated \[N{{H}_{4}}Cl\] would be                
  A)
  Slight less than half that of \[N{{H}_{4}}Cl\] done clear
  B)
  Half  that of \[N{{H}_{4}}Cl\] done clear
  C)
  Double that of \[N{{H}_{4}}Cl\] done clear
  D)
  Determined by the amount of solid \[N{{H}_{4}}Cl\] in the experiment done clear
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• question_answer20)
  \[\Delta {{G}^{0}}(HI,\,g)\cong +1.7\,kJ\]. What is the equilibrium constant  at \[{{25}^{o}}C\] for \[2HI(g)\] D \[{{H}_{2}}(g)+{{I}_{2}}(g)\]
  A)
  24.0      done clear
  B)
  3.9 done clear
  C)
  2.0 done clear
  D)
  0.5 done clear
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• question_answer21)
  Calculate \[\Delta G{}^\circ \]for conversion of oxygen to ozone \[3/2\ {{O}_{2}}(g)\to {{O}_{3}}(g)\]at 298 K, if \[{{K}_{p}}\]for this conversion is \[2.47\times {{10}^{-29}}\]
  A)
  \[163\ kJ\ mo{{l}^{-1}}\]          done clear
  B)
  \[2.4\times {{10}^{2}}\ kJ\ mo{{l}^{-1}}\] done clear
  C)
  \[1.63\ kJ\ mo{{l}^{-1}}\]         done clear
  D)
  \[2.38\times {{10}^{6}}\ kJ\ mo{{l}^{-1}}\] done clear
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• question_answer22)
  Le-chatelier principle is applicable
  A)
  Both for physical and chemical equilibrium done clear
  B)
  Only for chemical equilibrium done clear
  C)
  Only for physical equilibrium done clear
  D)
  Neither for [b] nor for [c] done clear
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• question_answer23)
  Following gaseous reaction is undergoing in a vessel \[{{C}_{2}}{{H}_{4}}+{{H}_{2}}\]\[\rightleftharpoons \] \[{{C}_{2}}{{H}_{6}}\]; \[\Delta H=-32.7\,Kcal\] Which will increase the equilibrium concentration of \[{{C}_{2}}{{H}_{6}}\]
  A)
  Increase of temperature done clear
  B)
  By reducing temperature done clear
  C)
  By removing some hydrogen done clear
  D)
  By adding some \[{{C}_{2}}{{H}_{6}}\] done clear
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• question_answer24)
  The equilibrium which remains uneffected by change in pressure of the reactants is
  A)
  \[{{N}_{2(g)}}+{{O}_{2(g)}}\] \[\rightleftharpoons \] \[2N{{O}_{(g)}}\] done clear
  B)
  \[2S{{O}_{2(g)}}+{{O}_{2(g)}}\] \[\rightleftharpoons \] \[2S{{O}_{3(g)}}\] done clear
  C)
  \[2{{O}_{3(g)}}\]\[\rightleftharpoons \] \[3{{O}_{2(g)}}\] done clear
  D)
  \[2N{{O}_{2(g)}}\] \[\rightleftharpoons \] \[{{N}_{2}}{{O}_{4(g)}}\] done clear
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• question_answer25)
  For the reaction \[PC{{l}_{5}}(g)\]\[\rightleftharpoons \] \[PC{{l}_{3}}(g)+C{{l}_{2}}(g)\], the forward reaction at constant temperature is favoured by
  A)
  Introducing an inert gas at constant volume done clear
  B)
  Introducing chlorine gas at constant volume done clear
  C)
  Introducing an inert  gas at constant pressure done clear
  D)
  Decreasing the volume of the container done clear
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• question_answer26)
  The equilibrium \[2S{{O}_{2(g)}}+{{O}_{2(g)}}\]\[\rightleftharpoons \]\[2S{{O}_{3(g)}}\] shifts forward, if
  A)
  A catalyst is used done clear
  B)
  An adsorbent is used to remove \[S{{O}_{3}}\] as soon as it is formed done clear
  C)
  Low pressure done clear
  D)
  Small amounts of reactants are used done clear
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• question_answer27)
  Le-Chatelier principle is not applicable to   
  A)
  \[{{H}_{2(g)}}+{{I}_{2(g)}}\] \[\rightleftharpoons \]\[2H{{I}_{(g)}}\] done clear
  B)
  \[F{{e}_{(S)}}+{{S}_{(S)}}\] \[\rightleftharpoons \]\[Fe{{S}_{(S)}}\] done clear
  C)
  \[{{N}_{2(g)}}+3{{H}_{2(g)}}\]\[\rightleftharpoons \]\[2N{{H}_{3(g)}}\] done clear
  D)
   \[{{N}_{2(g)}}+{{O}_{2(g)}}\]\[\rightleftharpoons \]\[2N{{O}_{(g)}}\] done clear
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• question_answer28)
  The reaction \[2S{{O}_{2}}+{{O}_{2}}\]\[\rightleftharpoons \]\[2S{{O}_{3}}\]; \[\Delta H\] = – ve is favoured by   
  A)
  Low temperature, low pressure done clear
  B)
  Low temperature, high pressure done clear
  C)
  High temperature, high pressure done clear
  D)
  High temperature, low pressure done clear
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• question_answer29)
  Consider the reaction equilibrium, \[2S{{O}_{2(g)}}\]+\[{{O}_{2(g)}}\]\[\rightleftharpoons \]\[2S{{O}_{3(g)}}\]; \[\Delta H{}^\circ \]= –198kJ. On the basis of Le-Chatelier’s principle, the condition favourable for the forward reaction is                    
  A)
  Lowering of temperature as well as pressure done clear
  B)
  Increasing temperature as well as pressure done clear
  C)
  Lowering the temperature and increasing the pressure           done clear
  D)
  Any value of temperature and pressure done clear
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• question_answer30)
  A chemical reaction is at equilibrium when
  A)
  Reactants are completely transformed into products done clear
  B)
  The rates of forward and backward reactions are equal done clear
  C)
  Formation of products is minimised done clear
  D)
  Equal amounts of reactants and products are present done clear
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• question_answer31)
  Which is false
  A)
  The greater the concentration of the substances involved in a reaction, the lower the speed of the reaction done clear
  B)
  The point of dynamic equilibrium is reached when the reaction rate in one direction just balances the reaction rate in the opposite direction done clear
  C)
  The dissociation of weak electrolyte is a reversible reaction done clear
  D)
  The presence of free ions facilitates chemical changes done clear
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• question_answer32)
  2 moles of \[PC{{l}_{5}}\] were heated in a closed vessel of 2 litre capacity. At equilibrium, 40% of \[PC{{l}_{5}}\] is dissociated into \[PC{{l}_{3}}\] and \[C{{l}_{2}}\]. The value of equilibrium constant is
  A)
  0.266 done clear
  B)
  0.53 done clear
  C)
  2.66 done clear
  D)
  5.3 done clear
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• question_answer33)

  The rate constant for forward and backward reactions of hydrolysis of ester are \[1.1\times {{10}^{-2}}\] and \[1.5\times {{10}^{-3}}\] per minute respectively. Equilibrium constant for the reaction is

  \[C{{H}_{3}}COO{{C}_{2}}{{H}_{5}}+{{H}_{2}}O\]\[\rightleftharpoons \]\[C{{H}_{3}}COOH\]\[+{{C}_{2}}{{H}_{5}}OH\]

  A)
        4.33      done clear
  B)
  5.33 done clear
  C)
  6.33 done clear
  D)
  7.33 done clear
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• question_answer34)

  In the reaction \[PC{{l}_{5(g)}}\]\[\rightleftharpoons \] \[PC{{l}_{3(g)}}\]\[+C{{l}_{2(g)}}.\]

  The equilibrium concentrations of \[PC{{l}_{5}}\] and \[PC{{l}_{3}}\] are 0.4 and 0.2 mole/litre respectively. If the value of \[{{K}_{c}}\]is 0.5 what is the concentration of \[C{{l}_{2}}\] in moles/litre

  A)
  2.0 done clear
  B)
  1.5 done clear
  C)
  1.0 done clear
  D)
  0.5 done clear
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• question_answer35)
  In the reaction, \[{{H}_{2}}+{{I}_{2}}\]\[\rightleftharpoons \]\[2HI\]. In a 2 litre flask 0.4 moles of each \[{{H}_{2}}\] and \[{{I}_{2}}\] are taken. At equilibrium 0.5 moles of \[HI\] are formed. What will be the value of equilibrium constant, \[{{K}_{c}}\]   
  A)
  20.2      done clear
  B)
  25.4      done clear
  C)
  0.284 done clear
  D)
  11.1 done clear
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• question_answer36)
  What is the effect of halving the pressure by doubling the volume on the following system at 500°C   \[{{H}_{2(g)}}+{{I}_{2(g)}}\]\[\rightleftharpoons \] \[2H{{I}_{(g)}}\]
  A)
  Shift to product side        done clear
  B)
  Shift to product formation done clear
  C)
  Liquefaction of HI done clear
  D)
  No effect done clear
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• question_answer37)
  Equilibrium constants \[{{K}_{1}}\]and \[{{K}_{2}}\]for the following equilibria       \[NO(g)+\frac{1}{2}{{O}_{2}}\]            \[N{{O}_{2}}(g)\]             and \[2N{{O}_{2}}(g)\]           \[2NO(g)+{{O}_{2}}(g)\] are related as 
  A)
  \[{{K}_{2}}=\frac{1}{{{K}_{1}}}\] done clear
  B)
  \[{{K}_{2}}=K_{1}^{2}\] done clear
  C)
  \[{{K}_{2}}=\frac{{{K}_{1}}}{2}\] done clear
  D)
  \[{{K}_{2}}=\frac{1}{K_{1}^{2}}\] done clear
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• question_answer38)
  \[K\] for the synthesis of \[HI\] is 50. \[K\] for dissociation of \[HI\] is 
  A)
  50 done clear
  B)
  5 done clear
  C)
  0.2 done clear
  D)
  0.02 done clear
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• question_answer39)
  The reaction between \[{{N}_{2}}\] and \[{{H}_{2}}\] to form ammonia has \[{{K}_{c}}=6\times {{10}^{-2}}\] at the temperature 500°C. The numerical value of \[{{K}_{p}}\] for this reaction is 
  A)
  \[1.5\times {{10}^{-5}}\] done clear
  B)
  \[1.5\times {{10}^{5}}\]\[\] done clear
  C)
  \[1.5\times {{10}^{-6}}\] done clear
  D)
  \[1.5\times {{10}^{6}}\] done clear
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• question_answer40)
  A tenfold increase in pressure on the reaction \[{{N}_{2(g)}}\]\[+3{{H}_{2(g)}}\]\[\rightleftharpoons \]\[2N{{H}_{3(g)}}\] at equilibrium, makes \[{{K}_{p}}\]
  A)
  Unchanged done clear
  B)
  Two times done clear
  C)
  Four times done clear
  D)
  Ten times done clear
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