In the hypothetical equation A + B ⇌ K 1 K 2 C + D if equilibrium constant is 2 × 10 4 at 298 K . If forward rate constant K 1 = 4 × 10 3 mole 2 l i t – 2 at 298 K , the value of backward rate constant K 2 at same temperature is ?
A vessel contains A(g) and B(g) at 2 atm and 4 atm respectively at TK, the mixture is allowed to attain equilibrium at TK, according to the reaction 8 B ( g ) ⇌ 8 A ( g ) + C ( s ) At equilibrium n A n B eq. = n B n A initial Find the value of y if K c = 2 y
For the reaction, C ( s ) + CO 2 ( g ) ⇌ 2 CO ( g ) the partial pressures of CO 2 and CO are 2.0 and 4.0 atm respectively at equilibrium. The K, for the reaction is:
What is the molar solubility of Fe OH 2 K sp = 8.0 × 10 − 16 is pH = 13.0 ?
The physical parameters which do not change at equilibrium of a reaction mixture at constant temperature among the given are i) Color ii) Density iii) Concentration of species iv) Pressure v) Volume vi) Change in enthalpy vii) Rates of forward and backward reactions.
An acidified solution of 0.05 M Zn 2+ is saturated with 0.1 M H 2 S. What is the minimum molar concentration (M) of H + required to prevent the precipitation of ZnS? Use Ksp (ZnS) = 1.25 × 10 –22 and Overall dissociation constant of H 2 S , KNET = K 1 K 2 = 1 × 10 –21
Por the reaction H 2 ( g ) + I 2 ( g ) ⇌ 2 HI ( g ) , the equilibrium can be shifted in favour of product by
The equilibrium constant K p for a homogeneous gaseous reaction is 10 -8 . The standard Gibbs free energy change ∆ G ° for the reaction in kilocalories is——
In a closed container for the reaction H 2 ( g ) + I 2 ( g ) ⇌ 2 H I ( g ) the equilibrium concentrations H 2 = 0 . 5 M , I 2 = 0 . 5 M and [ H I ] = 1 . 25 M . If 0.5 moles of HI was added to 1 L of equilibrium mixture, then H 2 at new equilibrium mixture is
0.01 mole of A g N O 3 is added to 1 litre of a solution which is 0.1 M in N a 2 C r O 4 and 0.005 M in 0.005 M in N a I O 3 . Calculate the millimoles of precipitate formed at equilibrium. ( K s p values of A g 2 C r O 4 and A g I O 3 are 10 − 8 and 10 − 13 respectively).
The composition of the equilibrium mixture ( C l 2 ⇌ 2 C l ) , which is attained at 1200°C, is determined by measuring the rate of effusion through a pinhole. It is observed that at 1.80 mm Hg pressure, the mixture effuses 1.2 times as fast as krypton effuses under the same conditions. Calculate the fraction of chlorine molecules dissociated into atoms. (Atomic mass of Kr = 84, Cl = 35.5)
For the endothermic reaction 3 A ( g ) ⇌ B ( g ) + C ( g ) , select the option(s) by which equilibrium concentration of A(g) can be increased ?
The pairs of compounds which cannot exist together in aqueous solution are
A weak monobasic acid is 0.01% ionised, its concentration is 1 M. Hence, [OH – ] is
4 mole of A are mixed with 4 mole of B, when 2 mole of C are formed at equilibrium, according to the reaction, A + B ⇌ C + D . The equilibrium constant is :
For a reaction, 2 A + B ⇌ C , where initial concentration of A = 2M, B =1M and C = 0, the concentration of B at equilibrium is 0.5M. The value of equilibrium constant for the reaction is
When the pressure is applied over system, ice ⇌ water, which ones do not happen or seen?
pH of a solution made by mixing 50 mL of 0.2 M NH 4 Cl and 75 mL of 0.1 M NaOH is [pK b of NH 3 (aq) = 4.74. log 3 = 0.47]
Which set is not correct for the solubility product K s p solubility (Sg/litre) of sparingly soluble salt A 3 B 2 (mol. Wt. M) in water:.
A 0.1 M sodium acetate solution was prepared. The k h = 5.6 × 10 − 10
If K 1 and K 2 are the equilibrium constants at temperature T 1 and T 2 and T 2 > T 1 then
The equilibrium constant for the following reaction at 298 K is expressed as x × 10 y . 2 F e 3 + + 2 I − 2 F e 2 + + I 2 , E c e l l 0 = 0.235 V . The value of y is
Which of the following will produce a buffer solution when mixed in equal volumes?
K a for CH 3 COOH is 1 . 8 × 10 – 5 and K b for NH 4 OH is 1 . 8 × 10 – 5 . The pH of 0.01 M ammonium acetate will be
Pure gas –A was taken in a closed container at an initial pressure of 5atm the pressure in the container changed due to the reactions A g ⇌ B g + 2 C g C g ⇌ B g + D g If the total pressure due to the mixture of gases A, B,C and D was found to be 10atm at equilibrium in which pressure due to C was 3 atm then kp for the first equilibrium is
0.4 mole of CO taken in a 2 L flask is maintained along with a catalyst at 812 K so that the reaction : CO ( g ) + 2 H 2 ( g ) ⇌ CH 3 OH ( g ) can takes place , H 2 is introduced until total pressure of system is 20 atm & 0.2 moles of C H 3 O H is formed at equilibrium then the correct statements among the following:
H 0 is an acidic indicator K ln = 10 – 7 which dissociates into H + and In – in aqueous solution. It is added to a solution of 30 ml of 0.15 M H 3 PO 4 ( K 1 = 1 × 10 – 3 , K 2 = 1 × 10 – 7 = – 1 K 3 = 1 × 10 – 13 ) . If Hln and In – posses colour P and Q respectively and color P predominates over color Q, when concentration of HIn is 120 times than that of I n − and color Q predominates over P, and when concentration of I n − is 127 times of HIn. If this solution treated with 30 ml KOH, then correct statements among the following is/are :
If the percentage of H C O 3 − in the H 2 CO 3 – HCO 3 – buffer so that to have a neutral solutions is 10 × x the then the value of x is K a = 4 × 10 – 7
0.01 mole of AgNO 3 is added to 1 litre of a solution which is 0.1 M in Na 2 CrO 4 and 0.005 M in NaIO 3 . Calculate the millimol of precipitate formed at equilibrium. K s p values of Ag 2 CrO 4 and AgIO 3 are 10 – 8 and 10 – 13 respectively).
An arbitrary compound P 2 Q decomposes according to reaction: 2 P 2 Q ( g ) ⇌ 2 P 2 ( g ) + Q 2 ( g ) If one starts the decomposition reaction with 4 moles of P 2 Q and value of equilibrium constant K p is numerically equal to total pressure at equilibrium. Then which option is/are correct at equilibrium,.
The solubility of AgCl ( s ) in water is 10 – 5 mollitre – 1 . Which is/are correct statement(s)?
When 100 mL of 1.0 M HCl was mixed with 100mL of 1.0 M NaOH in an insulated beaker at constant pressure, a temperature increase of 5.7°C was measured for the beaker and its contents (Expt.1). Because the enthalpy of neutralization of a strong acid with a strong base is a constant (-57.0 kJ mol -1 ), this experiment could be used to measure the calorimeter constant. In a second experiment (Expt. 2), 100 mL of 2.0 M acetic acid (Ka = 2.0 × 10 -5 ) was mixed with 100mL of 1.0 M NaOH (under identical conditions to Expt.1) where a temperature rise of 5.6°C was measured.(Consider heat capacity of all solutions as 4.2 J g -1 K -1 and density of all solutions as 1.0 g mL -1
Thermal decomposition of gaseous X 2 to gaseous X at 298 K takes place according to the following equation: X 2 g ⇌ 2 X g . The standard reaction Gibbs energy, Δ r G 0 , of this reaction is positive. At the start of the reaction, there is one mole of X 2 and no X. As the reaction proceeds, the number of moles of X formed is given by b . Thus, β e q u i l i b r i u m is the number of moles of X formed at equilibrium . The reaction is carried out at a constant total pressure of 2 bar. Consider the gases to behave ideally. (Given : R=0.083 L bar K − 1 m o l − 1 )
A solution of 0.1 M weak base (B) is titrated with 0.1 M of a strong acid (HA). The variation of pH of the solution with the volume of HA added is shown in the figure below. What is the p? b of the base? The neutralization reaction is given by B+HA BH + + A − .
Two solid compounds X and Y dissociates at a certain temperature as follows X ( s ) ⇌ A ( g ) + 2 B ( g ) ; K P 1 = 9 × 10 − 3 atm 3 Y ( s ) ⇌ 2 B ( g ) + C ( g ) ; K p 2 = 4.5 × 10 − 3 atm 3 The total pressure of gases over a mixture of X and Y is:
K sp of PbBr 2 (Molar mass= 367 ) is 3 .2 x 10 -5 • If the salt is 80% dissociated in solution, calculate the solubility of salt in gram per litre. (in litre -1 )
H 2 A is a weak diprotic acid. If the pH of 0.1 M H 2 A solution is 3 and concentration of A 2- is 10 -12 at 25°C. Select correct statement(s)
Which are true for the reaction : A 2 ⇌ 2 C + D ?
In H 3 PO 4 which of the following is true?
pH of 10 − 8 M NaOH is
Which has maximum pH?
100 mL solution of pH = 6 is diluted to 1000 mL. Resulting solution has pH
pH of a mixture which is 0.1 M in CH 3 COOH and 0.05 M in (CH 3 COO) 2 Ba is [pK a of CH 3 COOH = 4.74]
pK b of aq. NH 3 is 4 .74 , hence pH of 0 .01 M NH 3 solution is
For which of the following reactions is K p = K c ?
For the reaction, A + B ⇌ C + D the initial concentration of A and B are equal, but the equilibrium concentration of C is twice that of equilibrium concentration of A. The equilibrium constant is:
The pressure at which equilibrium constant in term of pressure is found to be equal to that in terms of mole fraction for the equilibrium, PCl 5 ( g ) ⇌ PCl 3 ( g ) + Cl 2 ( g ) is :
If α is the fraction of HI dissociation at equilibrium in the reaction, 2 HI ⇌ H 2 + I 2 then starting with 2 mole of HI, the total number of moles of reactants and products at equilibrium is:
200 mL of 1 M HCI and 900 mL of 1 M H 2 SO 4 solution are mixed and the resultant solution is made 1 litre. The [H + ] is..
100 mL of a buffer solution contains 0.1 M each of weak acid HA and salt NaA. How many gram of NaOH should be added to the buffer so that it pH will be 6? (K a of HA = 10 -5 )
An aqueous solution of metal chloride MCl 2 (0.05 M) is saturated with H 2 S (0.1 M). The minimum pH at which metal sulphide will be precipitated is . K sp MS = 5 × 10 − 21 , K 1 H 2 S = 10 − 7 , K 2 H 2 S = 10 − 14
When 0.2 M solution of acetic acid is neutralised with 0.2 M NaOH in 500 mL of water, the pH of the resulting solution will be: [pK a of acetic acid = 4.74]
M ( OH ) x has K sp = 4 × 10 − 12 and solubility 1 × 10 − 4 M . What is the value of X ?
The vapour density of a mixture consisting of NO 2 and N 2 O 4 is 38.3 at 275 K. The number of mole of N 2 O 4 in 100 g of the mixture is
The equilibrium constant for the reaction w + x ⇌ y + z is 9. If one mole of each of w and x are mixed and there is no change in volume, the number of moles of y for formed is
One mole of SO 3 was placed in a litre reaction flask at a given temperature when the reaction equilibrium was established in the reaction. 2 SO 3 ⇌ 2 SO 2 + O 2 the vessel was found to contain 0.6 mol of SO 2 . The value of the equilibrium constant is
