Q.1
In the reaction N2(g) + O2(g) ↔ 2NO(g) -180.7 kJ, on increasing the temperature, the production of NO [ Chandhigarh CET 2000]
  • a) increases
  • b) decreases
  • c)remains same
  • d)cannot be predicted
Q.2
A 1M solution of glucose reaches dissociation equilibrium according to the equation given below:6HCHO ↔ C6H12O6What is the concentration of HCHO at equilibrium if equilibrium constant is 6×1022 ..[MP PMT 2000]
  • a) 1.6×10⁻⁸M
  • b)3.2×10⁻⁶M
  • c)3.2×10⁻⁴M
  • d)1.6×10⁻⁴M
Q.3
Kc for reactionN2(g) +O2(g) ↔ 2NO(g) at 300K is 4.0×10-Kp for above reaction will be (R=2 cal mol- K-1) ..[CBSE PMT 1994]
  • b) 4 ×10⁻⁶
  • a) 2.4 ×10⁻³
  • c) 4 ×10⁻⁶(RT)2
  • d) 16 × 10⁻¹²
Q.4
The reaction, SO2 + Cl2 → SO2Cl2 is exothermic and reversible. A mixture of SO2(g), Cl2(g) and SO2Cl2(l) is at equilibrium in a closed container. Now a certain quantity of extra SO2 is introduced into the container, the volume remaining the same. Which of the following is are true? [ ISM Dhanbad 1994]
  • a)The pressure inside the container will not change
  • b) The temperature will not change
  • c)The temperature will increase
  • d)The temperature will decrease
Q.5
On the basis of Le Chatellier principle, predict which of the following conditions would be unfavorable for the formation of SO3? Given that 2SO2 + O2 ↔ 2SO3 ; ΔH=-42 kcal .. [ MP PET 1998]
  • a) Low pressure
  • b) High pressure
  • c)high temperature
  • d)high concentration of SO2
Q.6
4 moles of A are mixed with 4 moles of B when 2 moles of C are formed at equilibrium according to the reactionA + B ↔ C + D The value of the equilibrium constant is ..[ CPMT 1992]
  • a) 4
  • b) 1
  • c)1/2
  • d)1/4
Q.7
The rate of forward reaction is two times that of the reverse reaction at a given temperature and identical concentration. K is
  • a) 0.5
  • b) 1.5
  • c) 2.5
  • d) 2
Q.8
Consider the reaction PCl5(g) ↔ PCl3(g) + Cl2(g) in a closed container at equilibrium. At a fixed temperature what will be the effect of adding more PCl5 on the equilibrium concentration of Cl2(g)? [ BHU 1991]
  • a)It decreases
  • b) It increases
  • c)It remains unaffected
  • d)It can not be predicted without the value of Kp
Q.9
Which of the following is not affected by pressure change? [ Pb CET 1999]
  • a) 2NO2(g) ↔ N2O4(g)
  • b) CO2(g) + H2O (l)↔ CO2 (solution)
  • c)H2(g) + I2(g) ↔ 2HI(g)
  • d)2O3(g) ↔ 3O2(g)
Q.10
An equilibrium mixture for the reaction2H2S (g) ↔ 2H2(g) + S2(g) had one mole of hydrogen sulphide, 0.2 mole of H2 and 0.8 mole of S2 in a two litre vessel. the value of K in mole/litre is [ IIT 1991]
  • a) 0.005
  • b) 0.016
  • c)0.08
  • d)0.160
Q.11
In the reaction PCl5(g) ↔ PCl3 + Cl2(g) the equilibrium concentration of PCl5 and PCl3 are 0.4 and 0.2 mole/litre respectively. If the value of K is 0.5, what is the concentration of Cl2 mole/litre [ EAMCET 2003]
  • a) 2.0
  • b) 1.5
  • c) 1.0
  • d) 0.5
Q.12
The first and second dissociation constant of an acid H2A are 1.0×10⁻⁵ and 5.0 ×10⁻¹⁰ respectively. The overall dissociation constant of the acid will be [ AIEEE 2007]
  • a) 0.2 × 105
  • c) 5.0 × 1015
  • b) 5.0 × 10⁻⁵
  • d) 5.0 × 10⁻¹⁵
Q.13
A weak acid HX has the dissociation constant 1 × 10⁻⁵M. It forms a salt NaX on reaction with alkali. The degree of hydrolysis of 0.1M solution of NaX is
  • a) 0.0001%
  • b) 0.01%
  • c) 0.1%
  • d) 0.15%
Q.14
The equilibrium constant for the reaction H2(g) + I2(g) ↔ 2HI(g) is 32 at given temperature. the equilibrium concentrations of I2 and HI are 0.5×10⁻³ and 8×10⁻³ M respectively. the equilibrium concentration of H2 is ..[Pb CET sample paper 1988]
  • c)2 ×10⁻³
  • a) 1 ×10⁻³ M
  • b) 0.5 ×10⁻³ M
  • d)4 ×10⁻³
Q.15
The decomposition of N2O4 to NO2 is carried out at 280°C in chloroform. When equilibrium is reached 0.2 mol of N2O4 and 2×10⁻³ mol of nO2are present in 2 litre solution. The equilibrium constant for the reaction N2O4 ↔ 2NO2 is ..[AIIMS 1984]
  • a) 1 ×10⁻³
  • b) 2 ×10⁻³
  • c)1 ×10⁻⁵
  • d)2 ×10⁻⁵
Q.16
in a chemical reaction, the rate constant for the backward reaction is 7.5×10⁻⁴ and the equilibrium constant is 1.the rate constant for forward reaction is ..[KCET 1989]
  • a) 5 ×10⁻⁴
  • b)2 ×10⁻³
  • c) 1.125 ×10⁻³
  • d) 9 ×10⁻⁴
Q.17
For the reaction equilibrium N2O4(g) ↔ 2NO2(g)the concentration of N2O4 and NO2 at equilibrium are 4.8×10⁻² and 1.2×10⁻² molL-1 respectively. the value of K for reaction is ..[AIEEE 2003]
  • a) 3×10⁻¹ molL-1
  • b) 3×10⁻³ molL-1
  • c) 3×103 molL-1
  • d) 3.3×102 molL-1
Q.18
The equilibrium constant for reaction, N2(g) + O2 is 4×10⁻⁴ at 2000KIn presence of a catalyst, equilibrium is attended ten times faster. therefore, the equilibrium constant, in presence of the catalyst, at 2000 K is : [ MLNR 1994]
  • d)difficult to compute without more data
  • a)40 ×10⁻⁴
  • b) 4 ×10⁻⁴
  • c)4 × 10⁻³
Q.19
Find out the solubility of Ni(OH)2 in 0.1 M NaOH. Given that the ionic product of Ni(OH)2 is 2 × 10-15.... [NEET 2020]
  • b) 1 × 108 M
  • a) 1 × 10⁻¹³ M
  • c) 2 × 10⁻¹³ M
  • d) 2 × 10⁻⁸ M
Q.20
pH of a saturated solution of Ca(OH)2isThe solubility product (Ksp ) of Ca(OH)2 is: ... [ NEET 2019]
  • a) 0.5 × 10⁻¹⁵
  • b) 0.25 × 10⁻¹⁰
  • c)0.125 × 10⁻¹⁵
  • d) 0.5 × 10⁻¹⁰
Q.21
The solubility of BaSO4 in water is 2·42 × 10⁻³ gL–1 at 298 K. The value of its solubility product (Ksp) will be ... [NEET 2018] (Given molar mass of BaSO4 = 233 g mol–1)
  • a) 1·08 × 10⁻¹⁴ mol2 L–2
  • b) 1·08 × 10⁻¹² mol2 L–2
  • c) 1·08 × 10⁻¹⁰ mol2 L–2
  • d) 1·08 × 10⁻⁸ mol2 L–2
Q.22
The dissociation constant of weak 0.1M acid solution is 4.9×10⁻⁸, its percentage ionization is .. [ AFMC 1999]
  • a) 0.07%
  • b) 0.007%
  • c)0.7%
  • d)0.0007%
Q.23
Ionization constant of acetic acid is 1.8 ×10-The concentration of H+ ions in 0.1M solution is .. [ AFMC 2000]
  • a) 1.8×10⁻³M
  • b) 1.8×10⁻⁵M
  • c) 1. 3×10⁻³M
  • d) 1.34×10⁻³M
Q.24
Solubility product of PbCl2 at 298 K is 10-At this temperature solubility of PbCl2 in mol/L is .. [ AFMC 2006]
  • a)(10-6) 1/2
  • b) (10-6) 1/3
  • c)(0.25×10⁻⁶) 1/3
  • d)(0.25×10⁻⁶) 1/2
Q.25
If 0.1M of a weak acid is taken, and its percentage of degree of ionization is 1.34%, then its ionization constant will be..[ AFMC 2005]
  • d)none of the above
  • a) 0.8×10⁻⁵
  • b) 1.79×10⁻⁵
  • c)0.182×10⁻⁵
Q.26
The pH of 10-8 M HCl solution is [ AFMC 2008]
  • a) 8
  • b) more than 8
  • c)between 6 and 7
  • d)slightly more than 7
Q.27
Ag+ + NH3 → [Ag(NH3)+] ;   K1=6.8 × 10⁻³ [Ag(NH3)+] + NH3 → [Ag(NH3)2]2+   K2=1.6 × 10⁻³ then the formation constant of [Ag(NH3)2]2+ is [ IIT 2006]
  • d) None of these
  • a) 1.08 × 10⁻⁷
  • b) 1.08 × 10⁻⁵
  • c) 1.08 × 10⁻⁹
Q.28
Calculate the partial pressure of carbon monoxide from the following data CO2 + C ↔ 2CO ; Kp=8 × 10⁻² CaCo3 ⇔ CaO + CO2 ; Kp=2 [ Orissa JEE 2004]
  • a)0.2
  • b) 0.4
  • c)1.6
  • d)4.0
Q.29
When 0.1 mol of CH3NH2 ( ionization constant,Kb=5 ×10⁻⁴) is mixed with 0.08 mol HCl and the volume is maid up toFind the [H+] of resulting solution. [ IIT 2005]
  • a) 8 × 10⁻⁵
  • b) 2 × 10⁻¹¹
  • c) 1.23 × 10⁻⁴
  • d) 8 × 10⁻¹¹
Q.30
In a saturated solution of the sparingly soluble strong electrolyte AgIO3 molecular mass=283, the equilibrium which sets in is AgIO3 ⇔ Ag+ + IO3- If the solubility product constant Ksp of AgIO3 at given temperature is 1.0 ×10⁻⁸, what is the mass of AgIO3 contained in 100 ml of its saturated solution [ AIEEE 2007]
  • a)1.0 ×10⁻⁴ g
  • b) 28.3 ×10⁻² g
  • c)2.83 ×10⁻³ g
  • d)1.0 ×10⁻⁷ g
0 h : 0 m : 1 s