Solved papers for NEET Chemistry Equilibrium / साम्यावस्था NEET PYQ-Chemical Equilibrium

done NEET PYQ-Chemical Equilibrium Total Questions - 21

• question_answer1) 

  If \[{{K}_{1}}\] and \[{{K}_{2}}\] are the respective equilibrium constants for the two reactions:  [AIPMT 1998]

  \[Xe{{F}_{6}}(g)+{{H}_{2}}O(g)~XeO{{F}_{4}}(g)+2HF(g)\]

  \[Xe{{O}_{4}}(g)+Xe{{F}_{6}}(g)~XeO{{F}_{4}}(g)+Xe{{O}_{3}}{{F}_{2}}(g)\]

  the equilibrium constant of the reaction

  \[Xe{{O}_{4}}(g)+2HF(g)~Xe{{O}_{3}}{{F}_{2}}(g)+{{H}_{2}}O(g)\]will be :

  A)
         \[{{K}_{2}}/{{({{K}_{2}})}^{2}}\]
  done clear
  B)
                    \[{{K}_{1}}\,.\,{{K}_{2}}\]     
  done clear
  C)
   \[{{K}_{1}}/{{K}_{2}}\]
  done clear
  D)
                    \[{{K}_{2}}/{{K}_{1}}\]
  done clear
  View Answer play_arrow

• question_answer2) For a reversible reaction, if the concentrations of the reactants are doubled, the equilibrium constant will be: [AIPMT 2000]
  A)
   one-fourth                    
  done clear
  B)
   halved
  done clear
  C)
   doubled                       
  done clear
  D)
   the same
  done clear
  View Answer play_arrow

• question_answer3) 

  For the equilibrium

  \[MgC{{O}_{3}}MgO(s)+C{{O}_{2}}(g)\]

  Which of the following expressions is correct?                                                             [AIPMT 2000]

  A)
   \[{{K}_{p}}={{P}_{C{{O}_{2}}}}\]  
  done clear
  B)
        \[{{K}_{p}}=\frac{[MgO]\,[C{{O}_{2}}]}{[MgC{{O}_{3}}]}\]
  done clear
  C)
  \[{{K}_{p}}=\frac{{{P}_{MgO}}+{{P}_{C{{O}_{2}}}}}{{{P}_{MgC{{O}_{3}}}}}\]
  done clear
  D)
        \[{{K}_{p}}=\frac{{{P}_{MgO}}+{{P}_{C{{O}_{2}}}}}{{{P}_{MgC{{O}_{3}}}}}\]
  done clear
  View Answer play_arrow

• question_answer4) 

  Reaction \[Ba{{O}_{2}}(s)~BaO(s)+{{O}_{2}}(g),~\]

  \[\Delta H=+ve\]. In equilibrium condition, Pressure of \[{{O}_{2}}\] depends on:              [AIPMT 2002]

  A)
   increased mass of \[Ba{{O}_{2}}\]                 
  done clear
  B)
              increased mass of BaO
  done clear
  C)
  increased temperature of equilibrium.
  done clear
  D)
        increased mass of \[Ba{{O}_{2}}\] and BaO both
  done clear
  View Answer play_arrow

• question_answer5) The reaction quotient (Q) for the reaction \[{{N}_{2}}(g)+3{{H}_{2}}(g)~2N{{H}_{3}}(g)\] is given by \[Q=\frac{{{[N{{H}_{3}}]}^{2}}}{[{{N}_{2}}]\,{{[{{H}_{2}}]}^{3}}}\]. The reaction will proceed towards right side if:                                                                                                                                       [AIPMT 2003]
  A)
   \[Q>{{K}_{c}}\]
  done clear
  B)
                    \[Q=0\]
  done clear
  C)
   \[Q={{K}_{c}}\]
  done clear
  D)
                    \[Q<{{K}_{c}}\]
  done clear
  View Answer play_arrow

• question_answer6) 

  The following equilibria are given:                                                 [AIPMT 2003]

  \[\begin{matrix}    {{N}_{2}}+3{{H}_{2}}2N{{H}_{3}} & {{K}_{1}}  \\ \end{matrix}\]

  \[\begin{matrix}    {{N}_{2}}+{{O}_{2}}2NO & {{K}_{2}}  \\ \end{matrix}\]

  \[\begin{matrix}    {{H}_{2}}+\frac{1}{2}{{O}_{2}}{{H}_{2}}O & {{K}_{3}}  \\ \end{matrix}\]

  The equilibrium constant of the reaction \[2N{{H}_{3}}+\frac{5}{2}{{O}_{2}}\rightleftharpoons 2NO+3{{H}_{2}}O\] in terms of \[{{K}_{1}},\text{ }{{K}_{2}}\] and \[{{K}_{3}}\] is:

  A)
   \[\frac{{{K}_{1}}K_{3}^{2}}{{{K}_{2}}}\]
  done clear
  B)
                    \[\frac{{{K}_{2}}\,K_{3}^{3}}{{{K}_{1}}}\]
  done clear
  C)
   \[{{K}_{1}}\,{{K}_{2}}\,{{K}_{3}}\]              
  done clear
  D)
   \[\frac{{{K}_{1}}\,{{K}_{2}}}{{{K}_{3}}}\]
  done clear
  View Answer play_arrow

• question_answer7) In which of the following equilibrium \[{{K}_{c}}\] and \[{{K}_{p}}\] are not equal?                [AIPMT (S) 2010]
  A)
   \[2NO(g){{N}_{2}}(g)+{{O}_{2}}(g)\]
  done clear
  B)
   \[S{{O}_{2}}(g)+N{{O}_{2}}(g)S{{O}_{3}}(g)+NO(g)\]
  done clear
  C)
   \[{{H}_{2}}(g)+{{I}_{2}}(g)2HI(g)\]
  done clear
  D)
   \[2C(s)+{{O}_{2}}(g)2C{{O}_{2}}(g)\]
  done clear
  View Answer play_arrow

• question_answer8)  

  The reaction,                                                                                                                 [AIPMT (M) 2010]

  \[2A(g)+B(g)3C(g)+D(g)\]

  is begun with the concentrations of A and B both at an initial value of 1.00 M. When equilibrium is reached, the concentration of D is measured and found to be 0.25 M. The value for the equilibrium constant for this reaction is given by the expression

  A)
   \[[{{(0.75)}^{3}}(0.25)]\div [{{(1.00)}^{2}}(1.00)]\]
  done clear
  B)
   \[[{{(0.75)}^{3}}(0.25)]\div [{{(0.50)}^{2}}(0.75)]\]
  done clear
  C)
   \[[{{(0.75)}^{3}}(0.25)]\div [{{(0.50)}^{2}}(0.25)]\]
  done clear
  D)
   \[[{{(0.75)}^{3}}(0.25)]\div [{{(0.75)}^{2}}(0.25)]\]
  done clear
  View Answer play_arrow

• question_answer9)   The value of \[\Delta H\] for the reaction\[{{X}_{2}}(g)+4{{Y}_{2}}(g)2X{{Y}_{4}}(g)\] is less than zero. Formation of \[X{{Y}_{4}}(g)\] will be favored at                                                                     [AIPMT (S) 2011]
  A)
   low pressure and low temperature
  done clear
  B)
   high temperature and low pressure
  done clear
  C)
   high pressure and low temperature
  done clear
  D)
   high temperature and high pressure
  done clear
  View Answer play_arrow

• question_answer10)              For the reaction \[{{N}_{2}}(g)+{{O}_{2}}(g)2\] \[NO(g),\] the equilibrium constant is \[{{K}_{1}}\]. The equilibrium constant is \[{{K}_{2}}\] for   the   reaction \[2NO(g)+{{O}_{2}}(g)2N{{O}_{2}}(g)\] What is K for the reaction \[N{{O}_{2}}(g)\frac{1}{2}{{N}_{2}}(g)+{{O}_{2}}(g)\]?                                 [AIPMT (S) 2011]
  A)
   \[1/(4{{K}_{1}}{{K}_{2}})\]    
  done clear
  B)
        \[{{[1/{{K}_{1}}{{K}_{2}}]}^{1/2}}\]
  done clear
  C)
   \[1/({{K}_{1}}{{K}_{2}})\]     
  done clear
  D)
        \[1/(2{{K}_{1}}{{K}_{2}})\]
  done clear
  View Answer play_arrow

• question_answer11)  Given that the equilibrium constant for the reaction, \[2S{{O}_{2}}(g)+{{O}_{2}}(g)2S{{O}_{3}}(g)\] has a value of 278 at a particular temperature. What is the value of the equilibrium constant for the following reaction at the same temperature?\[S{{O}_{3}}(g)S{{O}_{2}}(g)+\frac{1}{2}{{O}_{2}}(g)\].                                [AIPMT (M) 2012]
  A)
   \[1.8\times {{10}^{-3}}\]        
  done clear
  B)
        \[3.6\times {{10}^{-3}}\]        
  done clear
  C)
   \[6.0\times {{10}^{-2}}\]        
  done clear
  D)
        \[1.3\times {{10}^{-5}}\]
  done clear
  View Answer play_arrow

• question_answer12) 

  Given the reaction between two gases represented by \[{{A}_{2}}\] and \[{{B}_{2}}\] to give the compound \[AB.(g).\]\[{{A}_{2}}(g)+{{B}_{2}}(g)2AB(g)\]

  At equilibrium, the concentration of \[{{A}_{2}}=3.0\times {{10}^{-3}}M\] of \[{{B}_{2}}=4.2\times {{10}^{-3}}M\] of \[AB=2.8\times {{10}^{-3}}M\]. If the reaction takes place in a sealed vessel at \[527{}^\circ C,\] then the value of K, will be                                                                                                 [AIPMT (M) 2012]

  A)
   2.0              
  done clear
  B)
   1.9                  
  done clear
  C)
   0.62                
  done clear
  D)
        4.5
  done clear
  View Answer play_arrow

• question_answer13) For the reversible reaction,                        \[{{N}_{2}}(g)+3{{H}_{2}}(g)\rightleftharpoons 2N{{H}_{3}}(g)+Heat\] the equilibrium shifts in forward direction                                                                                 [AIPMT 2014]
  A)
   by increasing the concentration of \[N{{H}_{3}}(g)\]
  done clear
  B)
   by decreasing the pressure
  done clear
  C)
   by decreasing the concentrations of \[{{N}_{2}}(g)\] and \[{{H}_{2}}(g)\]
  done clear
  D)
   by increasing  pressure  and  decreasing temperature
  done clear
  View Answer play_arrow

• question_answer14) For a given exothermic reaction, \[{{K}_{p}}\] and \[K_{p}^{'}\] are the equilibrium constants at temperatures  \[{{T}_{1}}\] and\[{{T}_{2}},\] respectively. Assuming that heat of reaction is constant in 'temperature range between \[{{T}_{1}}\] and\[{{T}_{2}},\] it is readily observed that                                                          [AIPMT 2014]
  A)
  done clear
  B)
   \[{{K}_{p}}<K_{p}^{'}\]       
  done clear
  C)
   \[{{K}_{p}}=K_{p}^{'}\]       
  done clear
  D)
        \[{{K}_{p}}=\frac{1}{K_{p}^{'}}\]
  done clear
  View Answer play_arrow

• question_answer15) If the value of an equilibrium constant for a particular reaction is \[1.6\times {{10}^{12}},\] then at equilibrium the system will contain                                                                                                                          [NEET 2015 ]
  A)
   all reactants     
  done clear
  B)
        mostly reactants
  done clear
  C)
   mostly products
  done clear
  D)
        similar amounts of reactants and products
  done clear
  View Answer play_arrow

• question_answer16) If the equilibrium constant for \[{{N}_{2}}(g)+{{O}_{2}}(g)\rightleftharpoons 2NO(g)\] is K, the equilibrium constant for                                                                                                                                                     [NEET 2015 (Re)] \[\frac{1}{2}{{N}_{2}}(g)+\frac{1}{2}{{O}_{2}}(g)NO(g)\] will the
  A)
   \[{{K}^{1/2}}\]            
  done clear
  B)
                    \[\frac{1}{2}K\]
  done clear
  C)
   K                                
  done clear
  D)
   \[{{K}_{2}}\]
  done clear
  View Answer play_arrow

• question_answer17) 

  The equilibrium constants of the following are.                                                             [NEET-2017]

  \[{{N}_{2}}+3{{H}_{2}}\rightleftharpoons 2N{{H}_{3}}\,{{K}_{4}}\]

  \[{{N}_{2}}+{{O}_{2}}\rightleftharpoons 2NO\,{{K}_{2}}\]

  \[{{H}_{2}}+\frac{1}{2}{{O}_{2}}\xrightarrow{{}}{{H}_{2}}O\,{{K}_{3}}\]

  The equilibrium constant (K) of the reaction \[2N{{H}_{3}}+\frac{5}{2}{{O}_{2}}\xrightarrow{k}2NO+3{{H}_{2}}O,\] will be

  A)
   \[K_{2}^{3}{{K}_{3}}/{{K}_{1}}\]    
  done clear
  B)
        \[{{K}_{1}}K_{3}^{3}/{{K}_{2}}\]
  done clear
  C)
   \[{{K}_{2}}K_{3}^{3}/{{K}_{1}}\]    
  done clear
  D)
        \[{{K}_{2}}{{K}_{3}}/{{K}_{1}}\]
  done clear
  View Answer play_arrow

• question_answer18) A 20 litre container at 400 K contains \[C{{O}_{2}}(g)\] pressure 0.4 atm and an excess of SrO (neglect the volume of solid SrO). The volume of the containers is now decreased by moving the movable piston fitted in the container. The maximum volume of the container, when pressure of \[C{{O}_{2}}\] attains its maximum value, will be  (Given that: \[SrC{{O}_{3}}(s)=SrO(s)+C{{O}_{2}}(g).\]\[{{K}_{p}}=1.6\,atm)\]                                                [NEET-2017]
  A)
   2 litre
  done clear
  B)
                    5 litre
  done clear
  C)
   10 litre
  done clear
  D)
        4 litre
  done clear
  View Answer play_arrow

• question_answer19) Which one of the following conditions will favour maximum formation of the product in the react\[{{A}_{2}}(g)+{{B}_{2}}(g){{X}_{2}}(g){{\Delta }_{r}}H=-X\,\,kJ?\]    [NEET - 2018]
  A)
   High temperature and high pressure
  done clear
  B)
   Low temperature and low pressure
  done clear
  C)
   Low temperature and high pressure
  done clear
  D)
   High temperature and low pressure
  done clear
  View Answer play_arrow

• question_answer20) 

  A mixture of \[{{N}_{2}}\] and Ar gases in a cylinder contains 7 g of \[{{N}_{2}}\] and 8 g of Ar. If the total pressure of the mixture of the gases in the cylinder is 27 bar, the partial pressure of \[{{N}_{2}}\] is:

  [Use atomic masses \[(in\text{ }g\text{ }mo{{l}^{1}}):N=14,\,\,Ar=40]\]                                   [NEET 2020]

  A)
   12 bar
  done clear
  B)
                    15 bar
  done clear
  C)
   18 bar
  done clear
  D)
        9 bar
  done clear
  View Answer play_arrow

• question_answer21) 

  Hydrolysis of sucrose is given by the following reaction.                                                     [NEET 2020]

  \[\text{Sucrose+}{{\text{H}}_{\text{2}}}\text{O}\text{Glucose+Fructose}\]

  If the equilibrium constant \[({{K}_{C}})\] is \[2\times {{10}^{13}}\] at 300 K, the value of \[{{\Delta }_{r}}{{G}^{O-}}\] at the same temperature will be:

  A)
   \[8.314\text{ }J\text{ }mo{{l}^{1}}{{K}^{1}}\times 300\text{ }K\times ln\,\text{(}2\times {{10}^{13}})\]
  done clear
  B)
   \[8.314\text{ }J\text{ }mo{{l}^{1}}{{K}^{1}}\times 300\text{ }K\times ln\,(3\times {{10}^{13}})\]
  done clear
  C)
   \[8.314\text{ }J\text{ }mo{{l}^{1}}{{K}^{1}}\times 300\text{ }K\times ln\text{ (}4\times {{10}^{13}})\]
  done clear
  D)
   \[8.314\text{ }J\text{ }mo{{l}^{1}}{{K}^{1}}\times 300\text{ }K\times ln\,(2\times {{10}^{13}})\]
  done clear
  View Answer play_arrow