JEE Main & Advanced Chemistry Equilibrium / साम्यावस्था Question Bank

done Law of equilibrium and Equilibrium constant Total Questions - 74

• question_answer1)
  For the system \[3A+2B\] ⇌ \[C\], the expression for equilibrium constant is [NCERT 1981; CPMT 1989; MP PMT 1990; RPMT 1999; Pb. PMT 2002; Pb. CET 2002]
  A)
                  \[\frac{[3A][2B]}{C}\]     done clear
  B)
                  \[\frac{[C]}{[3A][2B]}\] done clear
  C)
                  \[\frac{{{[A]}^{3}}{{[B]}^{2}}}{[C]}\]        done clear
  D)
                  \[\frac{[C]}{{{[A]}^{3}}{{[B]}^{2}}}\] done clear
  View Solution play_arrow

• question_answer2)
  In the reversible reaction \[A+B\]⇌ \[C+D\], the concentration of each C and D at equilibrium was 0.8 mole/liter, then the equilibrium constant \[{{K}_{c}}\] will be               [MP PET 1986]
  A)
                  6.4          done clear
  B)
                  0.64 done clear
  C)
                  1.6          done clear
  D)
                  16.0 done clear
  View Solution play_arrow

• question_answer3)
  4 moles of A are mixed with 4 moles of B. At equilibrium for the reaction \[A+B\]⇌\[C+D\], 2 moles of C and D are formed. The equilibrium constant for the reaction will be             [CPMT 1992]
  A)
                  \[\frac{1}{4}\]    done clear
  B)
                  \[\frac{1}{2}\] done clear
  C)
                  1              done clear
  D)
                  4 done clear
  View Solution play_arrow

• question_answer4)
  On a given condition, the equilibrium concentration of \[HI,\,{{H}_{2}}\] and \[{{I}_{2}}\] are 0.80, 0.10 and 0.10 mole/litre. The equilibrium constant for the reaction \[{{H}_{2}}+{{I}_{2}}\] ⇌ \[2HI\]  will be            [MP PET 1986]
  A)
                  64           done clear
  B)
                  12 done clear
  C)
                  8              done clear
  D)
                  0.8 done clear
  View Solution play_arrow

• question_answer5)
  In which of the following, the reaction proceeds towards completion                                     [MNR 1990]
  A)
                  \[K={{10}^{3}}\]                done clear
  B)
                  \[K={{10}^{-2}}\] done clear
  C)
                  \[K=10\]               done clear
  D)
                  \[K=1\] done clear
  View Solution play_arrow

• question_answer6)
  A reversible chemical reaction having two reactants in equilibrium. If the concentrations of the reactants are doubled, then the equilibrium constant will [CPMT 1982, 90; MP PMT 1990,2004; MNR 1992; UPSEAT 2002; KCET 1999; Pb. CET 2004]
  A)
                  Also be doubled               done clear
  B)
                  Be halved done clear
  C)
                  Become one-fourth        done clear
  D)
                  Remain the same done clear
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• question_answer7)
  The equilibrium constant in a reversible reaction at a given temperature                                               [AIIMS 1982]
  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)
  Pure ammonia is placed in a vessel at temperature where its dissociation constant (\[\alpha \]) is appreciable. At equilibrium [IIT 1984; Kurukshetra CEE 1998]
  A)
                  \[{{K}_{p}}\] does not change significantly with pressure done clear
  B)
                  \[\alpha \] does not change with pressure done clear
  C)
                  Concentration of \[N{{H}_{3}}\] does not change with pressure done clear
  D)
                  Concentration of \[{{H}_{2}}\] is less than that of \[{{N}_{2}}\] done clear
  View Solution play_arrow

• question_answer9)
  For the system \[A(g)+2B(g)\]⇌\[C(g)\], the equilibrium concentrations are  0.06 mole/litre  0.12 mole/litre  0.216 mole/litre. The \[{{K}_{eq}}\] for the reaction is [CPMT 1983]
  A)
                  250         done clear
  B)
                  416 done clear
  C)
                  \[4\times {{10}^{-3}}\]   done clear
  D)
                  125 done clear
  View Solution play_arrow

• question_answer10)
  The equilibrium constant for the given reaction  \[{{H}_{2}}+{{I}_{2}}\]⇌\[2HI\] is correctly given by expression [CPMT 1984]
  A)
                  \[{{K}_{c}}=\frac{[{{H}_{2}}][{{I}_{2}}]}{[HI]}\]    done clear
  B)
                  \[{{K}_{c}}=\frac{[{{H}_{2}}][{{I}_{2}}]}{[2HI]}\] done clear
  C)
                  \[{{K}_{c}}=\frac{[{{H}_{2}}][{{I}_{2}}]}{{{[HI]}^{2}}}\] done clear
  D)
                  \[{{K}_{c}}=\frac{{{[HI]}^{2}}}{[{{H}_{2}}][{{I}_{2}}]}\] done clear
  View Solution play_arrow

• question_answer11)
  Partial pressures of A, B, C and D on the basis of gaseous system \[A+2B\] ⇌ \[C+3D\] are A = 0.20; B = 0.10; C = 0.30 and D = 0.50 atm. The numerical value of equilibrium constant is                                            [CPMT 1987]
  A)
                  11.25     done clear
  B)
                  18.75 done clear
  C)
                  5              done clear
  D)
                  3.75 done clear
  View Solution play_arrow

• question_answer12)
  For the reaction \[A+2B\] ⇌ \[C\], the expression for equilibrium constant is [MNR 1987; MP PMT 1999; UPSEAT 2002]
  A)
                  \[\frac{[A]{{[B]}^{2}}}{[C]}\]       done clear
  B)
                  \[\frac{[A][B]}{[C]}\] done clear
  C)
                  \[\frac{[C]}{[A]{{[B]}^{2}}}\]       done clear
  D)
                  \[\frac{[C]}{2[B][A]}\] done clear
  View Solution play_arrow

• question_answer13)
  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 [MP PMT 1989; RPMT 2000; UPSEAT 2004; Kerala CET 2005]
  A)
                  0.266     done clear
  B)
                  0.53 done clear
  C)
                  2.66        done clear
  D)
                  5.3 done clear
  View Solution play_arrow

• question_answer14)
  For which of the following reactions does the equilibrium  constant depend on the units of concentration [AIIMS 1983]
  A)
                  \[N{{O}_{(g)}}\] ⇌ \[\frac{1}{2}{{N}_{2(g)}}+\frac{1}{2}{{O}_{2(g)}}\] done clear
  B)
                  \[Z{{n}_{(s)}}+Cu_{(aq)}^{2+}\] ⇌ \[C{{u}_{(s)}}+Zn_{(aq)}^{2+}\] done clear
  C)
   \[{{C}_{2}}{{H}_{5}}O{{H}_{(l)}}+C{{H}_{3}}COO{{H}_{(l)}}\]⇌\[C{{H}_{3}}COO{{C}_{2}}{{H}_{5(l)}}+{{H}_{2}}{{O}_{(l)}}\] (Reaction carried in an inert solvent) done clear
  D)
                  \[COC{{l}_{2(g)}}\] ⇌ \[C{{O}_{(g)}}+C{{l}_{2\,(g)}}\] done clear
  View Solution play_arrow

• question_answer15)
  Unit of equilibrium constant for the reversible reaction \[{{H}_{2}}+{{I}_{2}}\] ⇌ \[2HI\] is                                           [DPMT 1984]
  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
  View Solution play_arrow

• question_answer16)
  The decomposition of \[{{N}_{2}}{{O}_{4}}\] to \[N{{O}_{2}}\] is carried out at \[280K\] in chloroform. When equilibrium has been established, 0.2 mol of \[{{N}_{2}}{{O}_{4}}\] and \[2\times {{10}^{-3}}\] mol of \[N{{O}_{2}}\]  are present in 2 litre solution. The equilibrium constant for reaction \[{{N}_{2}}{{O}_{4}}\] ⇌ \[2N{{O}_{2}}\] is                                  [AIIMS 1984]
  A)
                  \[1\times {{10}^{-2}}\]   done clear
  B)
                  \[2\times {{10}^{-3}}\] done clear
  C)
                  \[1\times {{10}^{-5}}\]   done clear
  D)
                  \[2\times {{10}^{-5}}\] done clear
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• question_answer17)
  Concentration of a gas is expressed in the following terms in the calculation of equilibrium constant        [EAMCET 1982]
  A)
                  No. of molecules per litre done clear
  B)
                  No. of grams per litre done clear
  C)
                  No. of gram equivalent per litre done clear
  D)
                  No. of molecules equivalent per litre done clear
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• question_answer18)
  The unit of equilibrium constant K for the reaction \[A+B\]⇌ \[C\]  would be      [CPMT 1987]
  A)
                  \[mol\,\,litr{{e}^{-1}}\] done clear
  B)
                  \[litre\,\,mo{{l}^{-1}}\] done clear
  C)
                  \[mol\,\,litre\] done clear
  D)
                  Dimensionless done clear
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• question_answer19)
  In a reaction \[A+B\]⇌ \[C+D\], the concentrations of A, B, C and D (in moles/litre) are 0.5, 0.8, 0.4 and 1.0 respectively. The equilibrium constant is          [BHU 1981]
  A)
                  0.1          done clear
  B)
                  1.0 done clear
  C)
                  10           done clear
  D)
                  \[\infty \] done clear
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• question_answer20)
  In a chemical equilibrium  \[A+B\] ⇌ \[C+D\], when one mole each of the two reactants are mixed, 0.6 mole each of the products are formed. The equilibrium constant calculated is [CBSE PMT 1989]
  A)
                  1              done clear
  B)
                  0.36 done clear
  C)
                  2.25        done clear
  D)
                  4/9 done clear
  View Solution play_arrow

• question_answer21)
  For the reaction \[{{N}_{2(g)}}+3{{H}_{2(g)}}\] ⇌ \[2N{{H}_{3(g)}}\], the correct expression of equilibrium constant  K is [CPMT 1984, 2000]
  A)
                  \[K=\frac{{{[N{{H}_{3}}]}^{2}}}{[{{N}_{2}}]{{[{{H}_{2}}]}^{3}}}\]                 done clear
  B)
                  \[K=\frac{[{{N}_{2}}]{{[{{H}_{2}}]}^{3}}}{{{[N{{H}_{3}}]}^{2}}}\] done clear
  C)
                  \[K=\frac{2[N{{H}_{3}}]}{[{{N}_{2}}]\times 3[{{H}_{2}}]}\]            done clear
  D)
                  \[K=\frac{[{{N}_{2}}]\times 3[{{H}_{2}}]}{2[N{{H}_{3}}]}\] done clear
  View Solution play_arrow

• question_answer22)
  The suitable expression for the equilibrium constant of the reaction \[2N{{O}_{(g)}}+C{{l}_{2(g)}}\] ⇌ \[2NOC{{l}_{(g)}}\]  is [CPMT 1983, 87]
  A)
                  \[{{K}_{c}}=\frac{[2NOCl]}{[2NO]\,[C{{l}_{2}}]}\]               done clear
  B)
                  \[{{K}_{c}}=\frac{{{[NOCl]}^{2}}}{{{[NO]}^{2}}[C{{l}_{2}}]}\]  done clear
  C)
                  \[{{K}_{c}}=\frac{{{[NOCl]}^{2}}}{[NO]{{[C{{l}_{2}}]}^{2}}}\]         done clear
  D)
                  \[{{K}_{c}}=\frac{{{[NOCl]}^{2}}}{{{[NO]}^{2}}{{[C{{l}_{2}}]}^{2}}}\] done clear
  View Solution play_arrow

• question_answer23)
  A + B ⇌ C + D. If finally the concentration of A and B are both equal but at equilibrium concentration of D will be twice of that of A then what will be the equilibrium constant of reaction. [BHU 2005]
  A)
                  4 / 9       done clear
  B)
                  9 / 4 done clear
  C)
                  1 / 9       done clear
  D)
                  4 done clear
  View Solution play_arrow

• question_answer24)
  If in the reaction \[{{N}_{2}}{{O}_{4}}=2N{{O}_{2}},\,\alpha \] is that part of \[{{N}_{2}}{{O}_{4}}\] which dissociates, then the number of moles at equilibrium will be          [MP PET 1990; MH CET 2001; KCET 2005]
  A)
                  3              done clear
  B)
                  1 done clear
  C)
                  \[{{(1-\alpha )}^{2}}\]    done clear
  D)
                  \[(1+\alpha )\] done clear
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• question_answer25)
  In the gas phase reaction, \[{{C}_{2}}{{H}_{4}}+{{H}_{2}}\]⇌ \[{{C}_{2}}{{H}_{6}}\], the equilibrium constant can be expressed in units of [CBSE PMT 1992; Pb. PMT 1999]
  A)
                  \[litr{{e}^{-1}}\,mol{{e}^{-1}}\]  done clear
  B)
                  \[litre\,mol{{e}^{-1}}\] done clear
  C)
                  \[mol{{e}^{2}}\,litr{{e}^{-2}}\] done clear
  D)
                  \[mole\,litr{{e}^{-1}}\] done clear
  View Solution play_arrow

• question_answer26)
  For the reaction \[2S{{O}_{2}}+{{O}_{2}}\] ⇌ \[2S{{O}_{3}}\], the units of \[{{K}_{c}}\] are [CPMT 1990]
  A)
                  \[litre\,mol{{e}^{-1}}\] done clear
  B)
                  \[mol\,\,litr{{e}^{-1}}\] done clear
  C)
                  \[{{(mol\,\,litr{{e}^{-1}})}^{2}}\]               done clear
  D)
                  \[{{(litre\,\,mol{{e}^{-1}})}^{2}}\] done clear
  View Solution play_arrow

• question_answer27)
  A quantity of \[PC{{l}_{5}}\] was heated in a 10 litre vessel at \[{{250}^{o}}C\]; \[PC{{l}_{5}}(g)\]⇌ \[PC{{l}_{3}}(g)+C{{l}_{2}}(g)\]. At equilibrium the vessel contains 0.1 mole of \[PC{{l}_{5}}\,0.20\]  mole of \[PC{{l}_{3}}\] and 0.2 mole of \[C{{l}_{2}}\]. The equilibrium constant of the reaction is [KCET 1993, 2001; MP PMT 2003]
  A)
                  0.02        done clear
  B)
                  0.05 done clear
  C)
                  0.04        done clear
  D)
                  0.025 done clear
  View Solution play_arrow

• question_answer28)
  A mixture of 0.3 mole of \[{{H}_{2}}\] and 0.3 mole of \[{{I}_{2}}\] is allowed to react in a 10 litre  evacuated flask at \[{{500}^{o}}C\]. The reaction is \[{{H}_{2}}+{{I}_{2}}\]⇌ \[2HI\], the \[K\] is found to be 64. The amount of unreacted \[{{I}_{2}}\] at equilibrium is       [KCET 1990]
  A)
                  0.15 mole            done clear
  B)
                  0.06 mole done clear
  C)
                  0.03 mole            done clear
  D)
                  0.2 mole done clear
  View Solution play_arrow

• question_answer29)
  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    [KCET 1989]
  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
  View Solution play_arrow

• question_answer30)
  28 g  of \[{{N}_{2}}\] and 6 g  of \[{{H}_{2}}\] were kept at \[{{400}^{o}}C\] in 1 litre vessel, the equilibrium mixture contained  \[27.54g\] of \[N{{H}_{3}}\]. The approximate  value of \[{{K}_{c}}\] for the  above reaction can be (in \[mol{{e}^{-2}}\,\,litr{{e}^{2}}\])              [CBSE PMT 1990]
  A)
                  75           done clear
  B)
                  50 done clear
  C)
                  25           done clear
  D)
                  100 done clear
  View Solution play_arrow

• question_answer31)
  The equilibrium concentration of \[X,\,Y\] and \[Y{{X}_{2}}\] are 4, 2 and 2 moles respectively for the equilibrium \[2X+Y\]⇌\[Y{{X}_{2}}\]. The value of \[{{K}_{c}}\] is [EAMCET 1990]
  A)
                  0.625     done clear
  B)
                  0.0625 done clear
  C)
                  6.25        done clear
  D)
                  0.00625 done clear
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• question_answer32)
  An amount of solid \[N{{H}_{4}}HS\] is placed in a flask already containing ammonia gas at a certain temperature and 0.50 atm. pressure. Ammonium hydrogen sulphide decomposes to yield \[N{{H}_{3}}\] and \[{{H}_{2}}S\] gases in the flask. When the decomposition reaction reaches equilibrium, the total pressure in the flask rises to 0.84 atm. The equilibrium constant for \[N{{H}_{4}}HS\] decomposition at this temperature is [AIEEE 2005]
  A)
                  0.30        done clear
  B)
                  0.18 done clear
  C)
                  0.17        done clear
  D)
                  0.11 done clear
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• question_answer33)
  In the reaction \[A+2B\]⇌\[2C\], if 2 moles of \[A,\,\,3.0\] moles of \[B\] and 2.0 moles of \[C\] are placed in a \[2.0\,\,l\] flask and the equilibrium concentration of \[C\] is 0.5 mole/\[l\]. The equilibrium constant \[({{K}_{c}})\] for the reaction is                [KCET 1996]
  A)
                  0.073     done clear
  B)
                  0.147 done clear
  C)
                  0.05        done clear
  D)
                  0.026 done clear
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• question_answer34)
  In a \[500ml\] capacity vessel \[CO\] and \[C{{l}_{2}}\] are mixed to form \[COC{{l}_{2}}\]. At equilibrium, it contains 0.2 moles of \[COC{{l}_{2}}\] and 0.1 mole of each of \[CO\] and \[C{{O}_{2}}\]. The equilibrium constant \[{{K}_{c}}\] for the reaction \[CO+C{{l}_{2}}\] ⇌\[COC{{l}_{2}}\] is [CBSE PMT 1998]
  A)
                  5              done clear
  B)
                  10 done clear
  C)
                  15           done clear
  D)
                  20 done clear
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• question_answer35)
  A reaction is \[A+B\to C+D\]. Initially we start with equal concentration of \[A\] and \[B\]. At equilibrium we find the moles of \[C\] is two times of \[A\]. What is the equilibrium constant of the reaction    [BHU 1998; KCET 2000]
  A)
                  4              done clear
  B)
                  2 done clear
  C)
                  \[1/4\] done clear
  D)
                  \[1/2\] done clear
  View Solution play_arrow

• question_answer36)
  4.5 moles each of hydrogen and iodine heated in a sealed ten litre vessel. At equilibrium, 3 moles of \[HI\] were found. The equilibrium constant for               \[{{H}_{2}}(g)+{{I}_{2}}(g)\]⇌\[2HI(g)\] is [EAMCET 1998]
  A)
                  1              done clear
  B)
                  10 done clear
  C)
                  5              done clear
  D)
                  0.33 done clear
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• question_answer37)
  An equilibrium mixture of the reaction \[2{{H}_{2}}S(g)\]⇌\[2{{H}_{2}}(g)+{{S}_{2}}(g)\] had 0.5 mole \[{{H}_{2}}S\], 0.10 mole \[{{H}_{2}}\] and 0.4 mole \[{{S}_{2}}\] in one litre vessel. The value of equilibrium constant \[(K)\] in mole litre-1 is [AIIMS 1998; IIT 1992; AFMC 1999; UPSEAT 2001]
  A)
                  0.004     done clear
  B)
                  0.008 done clear
  C)
                  0.016     done clear
  D)
                  0.160 done clear
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• question_answer38)
  At 3000 K the equilibrium pressures of CO2, CO and O2 are 0.6,0.4 and 0.2 atmospheres respectively. \[{{K}_{p}}\]for the reaction, \[2C{{O}_{2}}\]⇌\[2CO+{{O}_{2}}\] is          [JIPMER 1999]
  A)
                  0.089     done clear
  B)
                  0.0533 done clear
  C)
                  0.133     done clear
  D)
                  0.177 done clear
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• question_answer39)
  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 \[C{{H}_{3}}COO{{C}_{2}}{{H}_{5}}+{{H}_{2}}O\]⇌\[C{{H}_{3}}COOH\]\[+{{C}_{2}}{{H}_{5}}OH\] [AIIMS 1999]
  A)
                  4.33        done clear
  B)
                  5.33 done clear
  C)
                  6.33        done clear
  D)
                  7.33 done clear
  View Solution play_arrow

• question_answer40)
  At a certain temp. 2HI ⇌ H2 + I2 Only 50% HI is dissociated at equilibrium. The equilibrium constant is [DCE 1999]
  A)
                  0.25        done clear
  B)
                  1.0 done clear
  C)
                  3.0          done clear
  D)
                  0.50 done clear
  View Solution play_arrow

• question_answer41)
  When 3 mole of A and 1 mole of B are mixed in 1 litre vessel the following reaction takes place \[{{A}_{(g)}}+{{B}_{(g)}}\]⇌\[2{{C}_{(g)}}\]. 1.5 moles of C are formed. The equilibrium constant for the reaction is     [MP PMT 2000]
  A)
                  0.12        done clear
  B)
                  0.25 done clear
  C)
                  0.50        done clear
  D)
                  4.0 done clear
  View Solution play_arrow

• question_answer42)
  A 1 M solution of glucose reaches dissociation equilibrium according to equation given below \[6HCHO\]⇌\[{{C}_{6}}{{H}_{12}}{{O}_{6}}\]. What is the concentration of HCHO at equilibrium if equilibrium constant is \[6\times {{10}^{22}}\] [MP PMT 2000]
  A)
                  \[1.6\times {{10}^{-8}}M\]           done clear
  B)
                  \[3.2\times {{10}^{-6}}M\] done clear
  C)
                  \[3.2\times {{10}^{-4}}M\]           done clear
  D)
                  \[1.6\times {{10}^{-4}}M\] done clear
  View Solution play_arrow

• question_answer43)
  Equilibrium concentration of \[HI,\,{{I}_{2}}\] and \[{{H}_{2}}\] is \[0.7,\,0.1\] and \[0.1\,M\] respectively. The equilibrium constant for the reaction \[{{I}_{2}}+{{H}_{2}}\]⇌\[2HI\] is                                       [JIPMER 2000]
  A)
                  36           done clear
  B)
                  49 done clear
  C)
                  0.49        done clear
  D)
                  0.36 done clear
  View Solution play_arrow

• question_answer44)
  For the equilibrium \[{{N}_{2}}+3{{H}_{2}}\]⇌\[2N{{H}_{3}},{{K}_{c}}\] at 1000K is \[2.37\times {{10}^{-3}}\]. If at equilibrium \[[{{N}_{2}}]=2M,\,[{{H}_{2}}]=3M\], the concentration of \[N{{H}_{3}}\] is                 [JIPMER 2000]
  A)
                  0.00358 M           done clear
  B)
                  0.0358 M done clear
  C)
                  0.358 M                done clear
  D)
                  3.58 M done clear
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• question_answer45)
  In the reaction, \[A+B\]⇌\[2C\], at equilibrium, the concentration of A and B is \[0.20\,\,mol\,\,{{l}^{-1}}\] each and that of C was found to be \[0.60\,\,mol\,\,{{l}^{-1}}\]. The equilibrium constant of the reaction is                                                          [MH CET 2000]
  A)
                  2.4          done clear
  B)
                  18 done clear
  C)
                  4.8          done clear
  D)
                  9 done clear
  View Solution play_arrow

• question_answer46)
  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  [KCET 2005]
  A)
                  50           done clear
  B)
                  15 done clear
  C)
                  100         done clear
  D)
                  25 done clear
  View Solution play_arrow

• question_answer47)
  In a chemical reaction equilibrium is established when [MP PET 2001]
  A)
                  Opposing reaction ceases            done clear
  B)
                          Concentration of reactants and products are equal done clear
  C)
                  Velocity of opposing reaction is the same as that of forward reaction done clear
  D)
                  Reaction ceases to generate heat done clear
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• question_answer48)
  For the reaction\[{{H}_{2}}+{{I}_{2}}=2HI\],the equilibrium concentration of \[{{H}_{2\,}},\,{{I}_{2}}\] and \[HI\] are 8.0, 3.0 and 28.0 mol per litre respectively, the equilibrium constant of the reaction is [BHU 2000; CBSE PMT 2001]
  A)
                  30.66     done clear
  B)
                          32.66 done clear
  C)
                  34.66     done clear
  D)
                  36.66 done clear
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• question_answer49)
  Change in volume of the system does not alter the number of moles in which of the following equilibrium [AIEEE 2002]
  A)
                  \[{{N}_{2(g)}}+{{O}_{2(g)}}\]⇌ \[2N{{O}_{(g)}}\]               done clear
  B)
                  \[PC{{l}_{5(g)}}\]⇌\[PC{{l}_{3(g)}}+C{{l}_{2(g)}}\]      done clear
  C)
                  \[{{N}_{2(g)}}+3{{H}_{2}}_{(g)}\]⇌\[2N{{H}_{3(g)}}\] done clear
  D)
                  \[S{{O}_{2}}C{{l}_{2(g)}}\]⇌ \[S{{O}_{2(g)}}+C{{l}_{2(g)}}\] done clear
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• question_answer50)
  The rate of forward reaction is two times that of reverse reaction at a given temperature and identical concentration. Kequilibrium is          [KCET 2002]
  A)
                  2.5          done clear
  B)
                          2.0 done clear
  C)
                  0.5          done clear
  D)
                  1.5 done clear
  View Solution play_arrow

• question_answer51)
  Write the equilibrium constant K for \[C{{H}_{3}}COOH+{{H}_{2}}O={{H}_{3}}{{O}^{+}}+C{{H}_{3}}CO{{O}^{-}}\] [Kerala (Med.) 2002]
  A)
                  \[K=\frac{[{{H}_{3}}{{O}^{+}}][{{H}_{2}}O]}{[C{{H}_{3}}CO{{O}^{-}}][C{{H}_{3}}COOH]}\] done clear
  B)
                  \[K=\frac{[{{H}_{3}}{{O}^{+}}][C{{H}_{3}}CO{{O}^{-}}]}{[{{H}_{2}}O][C{{H}_{3}}COOH]}\] done clear
  C)
                  \[K=\frac{[{{H}_{3}}{{O}^{+}}][{{H}_{2}}O]}{[C{{H}_{3}}COOH][C{{H}_{3}}CO{{O}^{-}}]}\] done clear
  D)
                  \[K=\frac{[{{H}_{2}}O][C{{H}_{3}}CO{{O}^{-}}]}{[{{H}_{2}}O][C{{H}_{3}}COOH]}\] done clear
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• question_answer52)
  The equilibrium constant (Kc) for the reaction \[\text{HA}+\text{B}\]⇌\[\text{B}{{\text{H}}^{+}}+{{\text{A}}^{-}}\] is 100. If the rate constant for the forward reaction is 105, then rate constant for the backward reaction is              [CBSE PMT 2002]
  A)
                  \[{{10}^{7}}\]     done clear
  B)
                  \[{{10}^{3}}\] done clear
  C)
                  \[{{10}^{-3}}\]   done clear
  D)
                  \[{{10}^{-5}}\] done clear
  View Solution play_arrow

• question_answer53)
  9.2 grams of \[{{N}_{2}}{{O}_{4(g)}}\] is taken in a closed one litre vessel and heated till the following equilibrium is reached \[{{N}_{2}}{{O}_{4(g)}}\]⇌ \[2N{{O}_{2(g)}}\]. At equilibrium, 50% \[{{N}_{2}}{{O}_{4(g)}}\] is dissociated. What is the equilibrium constant (in mol litre?1) (Molecular weight of \[{{N}_{2}}{{O}_{4}}=92)\]       [MP PET 2003]
  A)
                  0.1          done clear
  B)
                          0.4 done clear
  C)
                  0.2          done clear
  D)
                  2 done clear
  View Solution play_arrow

• question_answer54)
  Two moles of \[N{{H}_{3}}\] when put into a previously evacuated vessel (one litre), partially dissociate into \[{{N}_{2}}\] and \[{{H}_{2}}\]. If at equilibrium one mole of NH3 is present, the equilibrium constant is                                            [MP PET 2003]
  A)
                  3/4 \[mo{{l}^{2}}\,litr{{e}^{-2}}\]              done clear
  B)
                  27/64 \[mo{{l}^{2}}\,litr{{e}^{-2}}\] done clear
  C)
                  27/32 \[mo{{l}^{2}}\,litr{{e}^{-2}}\]          done clear
  D)
                  27/1 \[mo{{l}^{2}}\,litr{{e}^{-2}}\] done clear
  View Solution play_arrow

• question_answer55)
  In a reaction, reactant ?A? decomposes 10% in 1 hour, 20% on 2 hour and 30% in 3 hour. The unit of rate constant of this reaction is                                           [MP PET 2003]
  A)
                  \[se{{c}^{-1}}\] done clear
  B)
                  \[mol\,\,litr{{e}^{-1}}\,se{{c}^{-1}}\] done clear
  C)
                  \[litre\,\,mo{{l}^{-1}}\,se{{c}^{-1}}\]       done clear
  D)
   \[litr{{e}^{2}}\,mo{{l}^{-2}}\,se{{c}^{-1}}\] done clear
  View Solution play_arrow

• question_answer56)
  In the reaction \[PC{{l}_{5(g)}}\]⇌ \[PC{{l}_{3(g)}}\]\[+C{{l}_{2(g)}}.\] 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             [EAMCET 2003]
  A)
                  2.0          done clear
  B)
                  1.5 done clear
  C)
                  1.0          done clear
  D)
                  0.5 done clear
  View Solution play_arrow

• question_answer57)
  In Haber process 30 litres of dihydrogen and 30 litres of dinitrogen were taken for reaction which yielded only 50% of the expected product. What will be the composition of gaseous mixture under the aforesaid condition in the end [CBSE PMT 2003]
  A)
                  20 litres ammonia, 25 litres nitrogen, 15 litres hydrogen  done clear
  B)
                          20 litres ammonia, 20 litres nitrogen, 20 litres hydrogen done clear
  C)
                  10 litres ammonia, 25 litres nitrogen, 15 litres hydrogen done clear
  D)
                  20 litres ammonia, 10 litres nitrogen, 30 litres hydrogen done clear
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• question_answer58)
  For the reaction equilibrium \[{{N}_{2}}{{O}_{4}}\]⇌\[2N{{O}_{2(g)}}\], the concentrations of \[{{N}_{2}}{{O}_{4}}\] and \[N{{O}_{2}}\] at equilibrium are \[4.8\times {{10}^{-2}}\]and \[1.2\times {{10}^{-2}}\,mol\,litr{{e}^{-1}}\] respectively. The value of \[{{K}_{c}}\] for the reaction is [AIEEE 2003]
  A)
                  \[3.3\times {{10}^{2}}\]\[mol\,\,litr{{e}^{-1}}\]  done clear
  B)
                          \[3\times {{10}^{-1}}\]\[mol\,\,litr{{e}^{-1}}\] done clear
  C)
                  \[3\times {{10}^{-3}}\]\[mol\,\,litr{{e}^{-1}}\]    done clear
  D)
                  \[3\times {{10}^{3}}\]\[mol\,\,litr{{e}^{-1}}\] done clear
  View Solution play_arrow

• question_answer59)
  3.2 moles of hydrogen iodide were heated in a sealed bulb at \[{{444}^{o}}C\] till the equilibrium state was reached. Its degree of dissociation at this temperature was found to be 22%. The number of moles of hydrogen iodide present at equilibrium are                 [BHU 1982]
  A)
                  2.496     done clear
  B)
                          1.87 done clear
  C)
                  2              done clear
  D)
                  4 done clear
  View Solution play_arrow

• question_answer60)
  56 g of nitrogen and 8 g hydrogen gas are heated in a closed vessel. At equilibrium 34 g of ammonia are present. The equilibrium number of moles of nitrogen, hydrogen and ammonia are respectively                                                [KCET 2004]
  A)
                  1,2,2      done clear
  B)
                          2,2,1 done clear
  C)
                  1,1,2      done clear
  D)
                  2,1,2 done clear
  View Solution play_arrow

• question_answer61)
  The reaction, \[2S{{O}_{2(g)}}+{{O}_{2(g)}}\]⇌ \[2S{{O}_{3(g)}}\] 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                   [KCET 2004]
  A)
                  \[1:8\]   done clear
  B)
                          \[1:4\] done clear
  C)
                  \[4:1\]   done clear
  D)
                  \[8:1\] done clear
  View Solution play_arrow

• question_answer62)
  The compound A and B are mixed in equimolar proportion to form the products, \[A+B\] ⇌ \[C+D\]. At equilibrium, one third of A and B are consumed. The equilibrium constant for the reaction is             [KCET 2004]
  A)
                  0.5          done clear
  B)
                          4.0 done clear
  C)
                  2.5          done clear
  D)
                  0.25 done clear
  View Solution play_arrow

• question_answer63)
  Calculate the partial pressure of carbon monoxide from the following    \[CaC{{O}_{3(s)}}\xrightarrow{\Delta }Ca{{O}_{(s)}}+C{{O}_{2}}\uparrow \]; \[{{K}_{p}}=8\times {{10}^{-2}}\] \[C{{O}_{2(g)}}+{{C}_{(s)}}\to 2C{{O}_{(g)}}\] ; \[{{K}_{p}}=2\]\[\]            [Orissa JEE 2004]
  A)
                  0.2          done clear
  B)
                          0.4 done clear
  C)
                  1.6          done clear
  D)
                  4 done clear
  View Solution play_arrow

• question_answer64)
  The equilibrium constant for the reaction \[{{N}_{2(g)}}+{{O}_{2(g)}}\]⇌ \[2N{{O}_{(g)}}\] at temperature T is \[4\times {{10}^{-4}}\]. The value of \[{{K}_{c}}\]for the reaction \[N{{O}_{(g)}}\]⇌\[\frac{1}{2}{{N}_{2(g)}}+\frac{1}{2}{{O}_{2(g)}}\] at the same temperature is                                                        [AIEEE 2004]
  A)
                  \[4\times {{10}^{-4}}\]   done clear
  B)
                          \[50\] done clear
  C)
                  \[2.5\times {{10}^{2}}\] done clear
  D)
                  0.02 done clear
  View Solution play_arrow

• question_answer65)
  What is the equilibrium expression for the reaction \[{{P}_{4(s)}}+5{{O}_{2(g)}}\]⇌ \[{{P}_{4}}{{O}_{10(s)}}\]                                                          [AIEEE 2004]
  A)
                  \[{{K}_{c}}={{[{{O}_{2}}]}^{5}}\]                done clear
  B)
                          \[{{K}_{c}}=[{{P}_{4}}{{O}_{10}}]/5[{{P}_{4}}][{{O}_{2}}]\] done clear
  C)
                  \[{{K}_{c}}=[{{P}_{4}}{{O}_{10}}]/[{{P}_{4}}]{{[{{O}_{2}}]}^{5}}\]               done clear
  D)
                  \[{{K}_{c}}=1/{{[{{O}_{2}}]}^{5}}\] done clear
  View Solution play_arrow

• question_answer66)
  In the reaction, \[{{H}_{2}}+{{I}_{2}}\]⇌\[2HI\]. 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, \[{{K}_{c}}\]             [CPMT 2004]
  A)
                  20.2        done clear
  B)
                          25.4 done clear
  C)
                  0.284     done clear
  D)
                  11.1 done clear
  View Solution play_arrow

• question_answer67)
  Ammonia carbonate when heated to 200°C gives a mixture of \[N{{H}_{3}}\] and \[C{{O}_{2}}\]vapour with a density of 13.0. What is the degree of dissociation of ammonium carbonate [Kerala PMT 2004]
  A)
                  \[3/2\]  done clear
  B)
                          \[1/2\] done clear
  C)
                  2              done clear
  D)
                  1 done clear
  E)
                  \[5/2\] done clear
  View Solution play_arrow

• question_answer68)
  2 mol of \[{{N}_{2}}\] is mixed with 6 mol of \[{{H}_{2}}\]in a closed vessel of one litre capacity. If 50% of \[{{N}_{2}}\]is converted into \[N{{H}_{3}}\]at equilibrium, the value of \[{{K}_{c}}\]for the reaction \[{{N}_{2(g)}}+3{{H}_{2(g)}}\] ⇌\[2N{{H}_{3(g)}}\]is              [Kerala PMT 2004]
  A)
                  \[4/27\]                done clear
  B)
                          \[27/4\] done clear
  C)
                  \[1/27\]                done clear
  D)
                  24 done clear
  E)
                  9 done clear
  View Solution play_arrow

• question_answer69)
  For a reaction \[{{H}_{2}}+{{I}_{2}}\]⇌\[2HI\]at 721K, the value of equilibrium constant is 50. If 0.5 mols each of \[{{H}_{2}}\]and \[{{I}_{2}}\]is added to the system the value of equilibrium constant will be [DCE 2004]
  A)
                  40           done clear
  B)
                          60 done clear
  C)
                  50           done clear
  D)
                  30 done clear
  View Solution play_arrow

• question_answer70)
  What is the effect of halving the pressure by doubling the volume on the following system at 500°C                         \[{{H}_{2(g)}}+{{I}_{2(g)}}\]⇌ \[2H{{I}_{(g)}}\]                                                 [UPSEAT 2004]
  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
  View Solution play_arrow

• question_answer71)
  When \[NaN{{O}_{3}}\] is heated in a closed vessel, \[{{O}_{2}}\] is liberated and \[NaN{{O}_{2}}\] is left behind. At equilibrium [IIT 1986; Roorkee 1995]
  A)
                  Addition of \[NaN{{O}_{3}}\] favours forward reaction done clear
  B)
                  Addition of \[NaN{{O}_{2}}\] favours reverse reaction done clear
  C)
                  Increasing pressure favours reverse reaction done clear
  D)
                  Increasing temperature favours forward reaction done clear
  View Solution play_arrow

• question_answer72)
  For the reaction : \[{{H}_{2(g)}}+C{{O}_{2(g)}}\]  ⇌\[C{{O}_{(g)}}+{{H}_{2}}{{O}_{(g)}}\], if the initial concentration of \[[{{H}_{2}}]=[C{{O}_{2}}]\] and \[x\] moles/litre of hydrogen is consumed at equilibrium, the correct expression of \[{{K}_{p}}\] is   [Orissa JEE  2005]
  A)
                  \[\frac{{{x}^{2}}}{{{(1-x)}^{2}}}\]              done clear
  B)
                  \[\frac{{{(1+x)}^{2}}}{{{(1-x)}^{2}}}\] done clear
  C)
                  \[\frac{{{x}^{2}}}{{{(2+x)}^{2}}}\]             done clear
  D)
                  \[\frac{{{x}^{2}}}{1-{{x}^{2}}}\] done clear
  View Solution play_arrow

• question_answer73)
  0.6 mole of NH3 in a reaction vessel of 2dm3 capacity was brought to equilibrium. The vessel was then found to contain 0.15 mole of H2 formed by the reaction                 \[2N{{H}_{3(g)}}={{N}_{2(g)}}+3{{H}_{2(g)}}\]                 Which of the following statements is true            [KCET 1999]
  A)
                  0.15 mole of the original NH3 had dissociated at equilibrium done clear
  B)
                  0.55 mole of ammonia is left in the vessel done clear
  C)
                  At equilibrium the vessel contained 0.45 mole of \[{{N}_{2}}\] done clear
  D)
                  The concentration of NH3 at equilibrium is 0.25 mole per dm3 done clear
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• question_answer74)
  5 moles of SO2 and 5 moles of O2 are allowed to react to form SO3 in a closed vessel. At the equilibrium stage 60% of SO2 is used up. The total number of moles of SO2, O2 and SO3 in the vessel now is         [KCET 2001]
  A)
                  10.0        done clear
  B)
                  8.5 done clear
  C)
                  10.5        done clear
  D)
                  3.9 done clear
  View Solution play_arrow