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question_answer1)
In which of the following reaction the value of \[Kp\]will be equal to \[{{K}_{c}}\]?
A)
\[{{H}_{2}}+{{I}_{2}}\rightleftarrows 2HI\] done
clear
B)
\[PC{{l}_{5}}\rightleftarrows PC{{l}_{3}}+C{{l}_{2}}\] done
clear
C)
\[2N{{H}_{3}}\rightleftarrows {{N}_{2}}+3{{H}_{2}}\] done
clear
D)
\[2S{{O}_{2}}+{{O}_{2}}\rightleftarrows 2S{{O}_{3}}\] done
clear
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question_answer2)
The equilibrium constant for the reversible reaction, \[{{N}_{2}}+3{{H}_{2}}\rightleftarrows 2N{{H}_{3}}\]is K and for the reaction \[\frac{1}{2}{{N}_{2}}+\frac{3}{2}{{H}_{2}}\rightleftarrows N{{H}_{3}}\] the equilibrium constant is K'. K and K' will be related as
A)
\[K=K'\] done
clear
B)
\[K'=\sqrt{K}\] done
clear
C)
\[K=\sqrt{K'}\] done
clear
D)
\[K\times K'=1\] done
clear
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question_answer3)
At constant temperature, the equilibrium constant (\[Kp\]) for the decomposition reaction \[{{N}_{2}}{{O}_{4}}\rightleftarrows 2N{{O}_{2}}\] is expressed by \[{{K}_{P}}=\frac{(4{{x}^{2}}p)}{(1-{{x}^{2}})}\], where p=pressure, x=extent of decomposition. Which one of the following statements is true?
A)
\[{{K}_{P}}\]increases with increase of p done
clear
B)
\[{{K}_{P}}\]increases with increase of x done
clear
C)
\[{{K}_{P}}\]increases with decrease of x done
clear
D)
\[{{K}_{P}}\]remains constant with change in p and x done
clear
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question_answer4)
If in the reaction \[{{N}_{2}}{{O}_{4}}=2N{{O}_{2,}}\,a\]is that part of \[{{N}_{2}}{{O}_{4}}\]which dissociates, then the number of moles at equilibrium will be
A)
3 done
clear
B)
1 done
clear
C)
\[{{(1-a)}^{2}}\] done
clear
D)
\[{{(1+a)}^{2}}\] done
clear
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question_answer5)
The dissociation equilibrium of a gas \[A{{B}_{2}}\]can be represented as \[2A{{B}_{2}}(g)\rightleftarrows 2AB(g)+{{B}_{2}}(g)\]The degree of dissociation is x and is small compared to 1. The expression relating the degree of dissociation (x) with equilibrium constant \[{{K}_{P}}\]and total pressure p is
A)
\[{{(2{{K}_{P}}/P)}^{1/3}}\] done
clear
B)
\[{{(2{{K}_{P}}/P)}^{1/2}}\] done
clear
C)
\[({{K}_{P}}/P)\] done
clear
D)
\[(2{{K}_{P}}/P)\] done
clear
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question_answer6)
The reaction which proceeds in the forward direction is
A)
\[F{{e}_{2}}{{O}_{3}}+6HCl\to 2FeC{{l}_{3}}+3{{H}_{2}}O\] done
clear
B)
\[N{{H}_{3}}+{{H}_{2}}O+NaCl\to N{{H}_{4}}Cl+NaOH\] done
clear
C)
\[SnC{{l}_{4}}+HgC{{l}_{2}}\to SnC{{l}_{2}}+2HgC{{l}_{2}}\] done
clear
D)
\[2Cul+{{I}_{2}}+4{{K}^{+}}\to 2C{{u}^{2+}}+4KI\] done
clear
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question_answer7)
Consider following reaction in equilibrium concentration 0.01 M of every species
(I) \[PC{{l}_{5}}(g)\rightleftarrows PC{{l}_{3}}(g)+C{{l}_{2}}(g)\] |
(II) \[2HI(g)\rightleftarrows {{H}_{2}}(g)+{{I}_{2}}(g)\] |
(III) \[{{N}_{2}}(g)+3{{H}_{2}}(g)\rightleftarrows 2N{{H}_{3}}(g)\] |
Extent of the reactions taking place is |
A)
I > II > III done
clear
B)
I < II < III done
clear
C)
II < III < I done
clear
D)
III < I < II done
clear
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question_answer8)
'a' moles of \[PC{{l}_{5}}\], undergoes, thermal dissociation as:\[PC{{l}_{5}}\rightleftarrows PC{{l}_{3}}+C{{l}_{2}}\], the mole fraction of \[PC{{l}_{3}}\]at equilibrium is 0.25 and the total pressure is 2.0 atmosphere. The partial pressure of \[C{{I}_{2}}\]at equilibrium is:
A)
2.5 done
clear
B)
1.0 done
clear
C)
0.5 done
clear
D)
None of these done
clear
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question_answer9)
To an equilibrium mixture of\[2S{{O}_{2}}(g)+{{O}_{2}}(g)\rightleftarrows 2S{{O}_{2}}(g)\] some helium, an inert gas, is added at constant volume. The addition of helium causes the total pressure to double. Which of the following is true?
A)
The concentration of the three gases is unchanged done
clear
B)
The concentration of sulphur trioxide increases done
clear
C)
The number of moles of sulphur trioxide increases done
clear
D)
The concentration of sulphur dioxide increases done
clear
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question_answer10)
\[{{N}_{2}}{{O}_{4}}\]is 10% dissociated at a total pressure \[{{P}_{1}}\]and 20% dissociated at a total pressure \[{{P}_{2}}\]. Then ration \[{{P}_{1}}/{{P}_{2}}\]is
A)
\[\frac{1}{2}\] done
clear
B)
\[\frac{2}{1}\] done
clear
C)
\[\frac{1}{4}\] done
clear
D)
\[\frac{4}{1}\] done
clear
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question_answer11)
For the reaction equilibrium;\[{{N}_{2}}{{O}_{4}}(g)\rightleftarrows 2N{{O}_{2}}(g)\]; the concentration of \[{{N}_{2}}{{O}_{4}}\]and \[N{{O}_{2}}\]at equilibrium are \[4.8\times {{10}^{-2}}\]and \[1.2\times {{10}^{-2}}\]mol/L respectively. The value of \[{{K}_{C}}\] for the reaction is:
A)
\[3\times {{10}^{-3}}M\] done
clear
B)
\[3\times {{10}^{3}}M\] done
clear
C)
\[3.3\times {{10}^{2}}M\] done
clear
D)
\[3\times {{10}^{-1}}M\] done
clear
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question_answer12)
What is the equilibrium constant for the reaction? \[{{P}_{4(s)}}+5{{O}_{2(g)}}\rightleftarrows {{P}_{4}}{{O}_{10(s)}}\]
A)
\[{{K}_{C}}=\frac{1}{{{\left[ {{O}_{2}} \right]}^{5}}}\] done
clear
B)
\[{{K}_{C}}=\frac{\left[ {{P}_{4}}{{O}_{10}} \right]}{5\left[ {{P}_{4}} \right]\left[ {{O}_{2}} \right]}\] done
clear
C)
\[{{K}_{C}}={{\left[ {{O}_{2}} \right]}^{5}}\] done
clear
D)
\[{{K}_{C}}=\frac{\left[ {{P}_{4}}{{O}_{10}} \right]}{5\left[ {{P}_{4}} \right]{{\left[ {{O}_{2}} \right]}^{5}}}\] done
clear
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question_answer13)
The equilibrium constant for the reaction; \[{{N}_{2(g)}}+{{O}_{2(g)}}\rightleftarrows 2N{{O}_{(g)}}\] at temperature T is \[4\times {{10}^{-4.}}\].The value of \[{{K}_{c}}\]for the reaction. \[N{{O}_{(g)}}\rightleftarrows 1/2{{N}_{2(g)}}+1/2{{O}_{2(g)}}\]at the temperature is
A)
0.02 done
clear
B)
50 done
clear
C)
\[4\times {{10}^{-4}}\] done
clear
D)
\[2.5\times {{10}^{-2}}\] done
clear
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question_answer14)
For the following three reactions, 1, 2 and 3, equilibrium constants are given
(1) \[C{{O}_{(g)}}+{{H}_{2}}{{O}_{(g)}}\rightleftarrows C{{O}_{2(g)}}+{{H}_{2(g)}};{{K}_{1}}\] |
(2) \[C{{H}_{4(g)}}\]\[+{{H}_{2}}{{O}_{(g)}}\rightleftarrows \]\[C{{O}_{(g)}}\]\[3{{H}_{2(g)}};{{K}_{2}}\] |
(3) \[C{{H}_{4(g)}}+2{{H}_{2}}{{O}_{(g)}}\rightleftarrows C{{O}_{2(g)}}+4{{H}_{2(g)}};{{K}_{3}}\] |
Which of the following relationship is correct?
A)
\[{{K}_{1}}\sqrt{{{K}_{2}}}={{K}_{3}}\] done
clear
B)
\[{{K}_{2}}{{K}_{3}}={{K}_{1}}\] done
clear
C)
\[{{K}_{3}}={{K}_{1}}{{K}_{2}}\] done
clear
D)
\[{{K}_{3}}.\,{{K}^{3}}_{2}={{K}^{2}}_{1}\] done
clear
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question_answer15)
The standard Gibbs energy change at 300 K for the reaction \[2A\to B+C\]is 2494.2J. At a given time, the composition of the reaction mixture is [A]=\[\frac{1}{2},[B]=2\,and\,(C)=\frac{1}{2}\]. [R=8.314J/Kmol, e=2.718]
A)
forward direction because \[Q>{{K}_{C}}\] done
clear
B)
reverse direction because \[Q>{{K}_{C}}\] done
clear
C)
forward direction because \[Q<{{K}_{C}}\] done
clear
D)
reverse direction because \[Q<{{K}_{C}}\] done
clear
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question_answer16)
For the reaction: \[{{H}_{2}}(g)+{{I}_{2}}(g)\rightleftarrows 2HI(g)\] The equilibrium constant \[Kp\]changes with
A)
total pressure done
clear
B)
catalyst done
clear
C)
the amounts of \[{{H}_{2}}\]and \[{{I}_{2}}\]present done
clear
D)
temperature done
clear
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question_answer17)
One mole of \[{{N}_{2}}{{O}_{4}}(g)\]at 300 K is kept in closed container under one atmosphere. It is heated to 600 K when 20% by mass of \[{{N}_{2}}{{O}_{4}}(g)\]decomposes to \[N{{O}_{2}}(g)\]. The lresultant pressure is
A)
1.2 atm done
clear
B)
2.4 atm done
clear
C)
2.0 atm done
clear
D)
1.0 atm done
clear
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question_answer18)
For the chemical reaction \[3X(g)+Y(g)\rightleftharpoons {{X}_{3}}Y(g)\] The amount of \[{{X}_{3}}Y\]at equilibrium is affected by
A)
temperature and pressure done
clear
B)
temperature only done
clear
C)
pressure only done
clear
D)
temperature, pressure, and catalyst done
clear
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question_answer19)
Consider the following equilibrium in a closed container\[{{N}_{2}}{{O}_{4(g)}}\rightleftharpoons 2N{{O}_{2}}(g)\]At a fixed temperature, the volume of the raction container is halved. For this change, which of the statements holds true regarding the equilibrium constant \[({{K}_{p}})\]and the degree of dissociation \[(\alpha )?\]
A)
Neither \[{{K}_{p}}\]nor a changes done
clear
B)
Both \[{{K}_{p}}\]and a change done
clear
C)
\[{{K}_{p}}\]changes but a does not change done
clear
D)
\[{{K}_{p}}\]does not change but a change done
clear
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question_answer20)
Pure ammonia is placed in a vessel at a temperature where its dissociation constant is appreciable. At equilibrium:
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 hydrogen is less than that of nitrogen done
clear
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question_answer21)
One mole of a compound AB reacts with 1 mole of a compound CD according to the equation \[AB+CD\rightleftharpoons AD+CB\] .When equilibrium had been established it was found that \[\frac{3}{4}\]mole each of reactant AB and CD had been converted to AD and CB. There is no change in Volume. The equilibrium constant for the reaction is.
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question_answer22)
For the reaction \[C(s)+C{{O}_{2}}(g)\rightleftharpoons 2CO(g)\],the partial pressure of \[C{{O}_{2}}\]and CO are 2.0 and 4.0 atm respectively at equilibrium. The \[{{K}_{p}}\]for the reaction is
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question_answer23)
For the reaction \[{{H}_{2}}+{{I}_{2}}\rightleftharpoons 2HI\] at 721 K, the value of equilibrium constant is 50. If 0.5 mol each of \[{{H}_{2}}\]and \[{{I}_{2}}\]is added to the system the value of equilibrium constant will be
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question_answer24)
In the system, \[LaC{{l}_{2}}(s)+{{H}_{2}}O(g)+heat\rightleftharpoons LaClO(s)+2HCl(g)\]. More water vapour is added to reestablish the equilibrium. The pressure of water vapour is doubled. The factor by which pressure of HCl is changed is
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question_answer25)
For the reaction,\[A(g)+B(g)\rightleftharpoons C(g)+D(g)\,\,at298K\], the values of \[\Delta {{H}^{o}}\]and \[\Delta {{S}^{0}}\]are -29.8 kcal and -0.1 kcal \[{{K}^{-1}}\]respectively. The sum of \[\Delta {{G}^{o}}\]and equilibrium constant \[{{K}_{c}}\]is
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