question_answer 1)
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_answer 2)
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_answer 3)
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_answer 4)
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_answer 5)
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_answer 6)
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
View Solution play_arrow
question_answer 7)
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
View Solution play_arrow
question_answer 8)
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_answer 9)
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_answer 10)
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_answer 11)
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_answer 12)
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_answer 13)
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_answer 14)
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_answer 15)
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_answer 16)
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
View Solution play_arrow
question_answer 17)
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
View Solution play_arrow
question_answer 18)
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
View Solution play_arrow
question_answer 19)
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
View Solution play_arrow
question_answer 20)
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_answer 21)
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_answer 22)
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_answer 23)
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_answer 24)
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
View Solution play_arrow
question_answer 25)
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_answer 26)
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_answer 27)
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_answer 28)
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_answer 29)
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_answer 30)
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_answer 31)
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
View Solution play_arrow
question_answer 32)
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
View Solution play_arrow
question_answer 33)
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
View Solution play_arrow
question_answer 34)
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
View Solution play_arrow
question_answer 35)
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_answer 36)
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
View Solution play_arrow
question_answer 37)
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
View Solution play_arrow
question_answer 38)
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
View Solution play_arrow
question_answer 39)
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_answer 40)
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_answer 41)
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_answer 42)
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_answer 43)
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_answer 44)
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
View Solution play_arrow
question_answer 45)
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_answer 46)
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_answer 47)
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
View Solution play_arrow
question_answer 48)
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
View Solution play_arrow
question_answer 49)
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
View Solution play_arrow
question_answer 50)
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_answer 51)
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
View Solution play_arrow
question_answer 52)
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_answer 53)
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
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question_answer 54)
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
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question_answer 55)
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
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question_answer 56)
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
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question_answer 57)
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_answer 58)
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
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question_answer 59)
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_answer 60)
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_answer 61)
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
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question_answer 62)
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_answer 63)
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
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question_answer 64)
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_answer 65)
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
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question_answer 66)
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_answer 67)
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
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question_answer 68)
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_answer 69)
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
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question_answer 70)
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_answer 71)
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_answer 72)
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
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question_answer 73)
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_answer 74)
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