Equilibrium Questions and Answers

equilibria is 1 1 36 2 1 1 3 1 3 4 1 9 4 A vessel at 1000 K contains CO with a pressure of 0 5 atm Some of the CO is converted into CO on the addition of graphite If the total pressure at equilibrium is 0 8 atm the value of K is AIEEE 2011 1 0 3 atm 4 3 atm 2NO g at temperature T is 2 0 18 atm 3 1 8 atm 5 The equilibrium constant Kc for the reaction N g O2 g

A 9 B Between 6 and 7 C 7 14 8 gm NaOH and 4 9 gm H SO4 are present in one litre of the solution What is its pH A 1 B 13 C 12 D 2 D 4 0 g What is the quantity of NaOH present in 250 cc of the solution so that it gives a pH 13

50 mL of 0 1 M NaOH is added to 75 mL of 0 1 M NH CI to make a basic buffer If pK of NH is 9 26 calculate pH Lof 12 Moolution of pyridine CH N K 15x10 9

When sulphur is heated at 800 K the initial pressure of 1 atm decreases by 20 at equilibrium K of the reaction S g 4S g ono A 4 2 is 1 0 2 2 0 512 3 1 51

If 0 5 mole H is reacted with 0 5 mole I in a ten litre container at 444 C and at same temperature value of equilibrium constant K is 49 the ratio of HI and will be 1 1 7 4 49 2 3 1 7

The degree of hydrolysis of a salt of weak acid HA and weak base BOH in its 0 1 M solution is found to be 10 If the molarity of the solution is 0 05 M the percentage hydrolysis of the salt should be offolod zwoller 2 10 1 5 3 20 4 None

4 w at isothermal AIPMT 2014 For the reaction X O4 l 2XO2 g AU 2 1 kCal AS 20 cal K at 300 K Hence AG is 1 2 7 kCal 3 9 3 kCal 2 2 7 kCal 4 9 3 kCal AIIMS 2014

9 57 The rapid change of pH near the stoichiometric point of an acid base titration is the basis of indicator detection pH of the solution is related to ratio of the concentrations of the conjugate acid HIn and base In forms of the indicator by the expression A log C log Hin In In Hin pK pH In pH pK In B log D log Hin In In Hin pH pK In pK pH In

4 100 cm of 1 M CH3COOH was mixed with 100 c 2M CH3OH to form an ester The change in the initial rate each solution is diluted with equal volume of water would be KCET 2015 a 0 5 times c 0 25 times b 2 times d 4 times

Two moles of ammonia is introduced in a evacuated 500 ml vessel at high temperature The decomposition reaction is N g 311 g 2NI 1 g N g At the equilibrium NI I becomes 1 mole then the K would be 1 0 42 3 1 7 d 2 6 75 4 1 5

Which of the following cations is not hydrolyzed in aqueous solution ii Ca iii Na 3 i ii iii iv i Mg2 1 i ii 2 iii iv 11 iv K 4 i ii iii

5 What is the OH in the final solution prepared by mixing 20 0 mL of 0 050 M HCl with 30 0 mL of 0 10 M Ba OH a 0 10 M c 0 0050 M b 0 40 M d 0 12 M

When CO is dissolved in water following equilibrium is established CO 2H O H O HCO3 for which equilibrium constant is 3 8 10 7 and pH 6 0 The ratio HCO3 CO would be 1 3 8 10 13 X 2 3 8 10 1 3 6 0 4 13 4 16

the pressure at which PCI will be 20 dissociated temperature remaining same PCI dissociates according to the reaction PC1 PC13 g Cl g At 523 K K 1 78 atm Find the density of the equilibrium mixture at a total pressure of 1 atm P The gr N

4 difficult to compute without 7 NH COONH s 2NH g CO g If equilibrium pressure is 3 atm for the above reaction K will be 3 4 27 4 1 27

29 A buffer of pH 9 26 is made by dissolving x moles of ammonium sulphate and 0 1 mole of ammonia into 100 mL solution If pK of ammonia is 4 74 calculate value of x

sample of 0 15 g of the compound Pt NH3 Bry 2 zBr ignited and heated to decomposition oduced 0 0502 g of Pt A second 0 15 g sample was dissolved in water and titrated rapidly with 01 M AgNO3 solution 51 50 mL was required to precipitate all the ionic bromide A third 0 15 g ample was heated for two hours on a steam bath in a solution to which 0 2 mole of AgNO3 has een added This precipitated all the bromide no just the free ionic Br as AgBr The weight of ne precipitate thus produced was 0 20 g Find x y and z Pt 195 Ag 108 Br 80 N 14 and H 1

26 For the reaction PCI g PCI g Cl g the forward reaction at constant temperature is favoured by A introducing an inert gas at constant volume B introducing chlorine gas at constant volume C introducing an inert gas at constant pressure D increasing the volume of the container

The following reaction is performed at 298 K 2NO g O g 2NO g The standard free energy of formation of NO g is 86 6 kJ mol at 298 K What is the standard f of formation of NO g at 298 K K 1 6 x 10 2 JEE Ma 1 86600 In 1 6 10 R 298 2 0 5 2 x 86 600 R 298 In 1 6 x 1012 3 R 298 In 1 6 x 1012 86600 10101

PC13 g Cl2 g PC15 heat cont 5 g The equilibrium will shift in forward direction 1 By increasing conc of PCI 5 g 2 By decreasing pressure 3 By decreasing conc of PCL and Cl 3 g 2 g 4 By increasing pressure and decreasing temp

54 When 0 02 moles of NaOH are added to a litre of buffer solution its pH changes from 5 75 to 5 80 What is its buffer capacity A 0 4 B 0 05 N 5 5 acetic acid was titrated with N 10 C 0 05 D 2 5 NaOH When 25 50 and 75 of titration is over then

Karnataka Me b Pt H 1 atm HC1 2M 2 1 d Pt H 1 atm HCl 0 5M 141 Which one of the following has a potential more than zero a Pt H latm HCl 1M 2 1 c Pt H 1 atm HCl 0 1M 2

pH of 0 1 M NaCN solution is 11 then the percentage hydrolysis is 1 0 1 3 0 01 2 1 4 10

The amount of NH SO in g which must be added to 500 ml of 0 2 M NH to yield a solution of pH 9 35 K for NH 1 78 x 10 A 5 248 g B 4 625 gm C 5 821 gm D 3 756 gm

HOT 29 At equilibrium 500mL vessel contains 1 5 M of each A B C D If 0 5M of C and D expelled out than what would be the K 41 1 2 1 9 3 4 9 4 5 9

The standard Gibbs energy change at 300 K for the reaction 2A B C is 2494 2J At a given tim 1 1 2 2 the composition of the reaction mixture is A B 2 and C R 8 314 J K mol e 2 718 1 forward direction because Q K 2 reverse direction because Q K 3 forward direction because Q Kc 4 reverse direction because OSK The reaction proceeds in the JEE Main 2015

Calculate pH of following solutions 0 1 M HCl a b c d f on 0 1 M CH COOH K 1 8 x 10 5 log 1 8 0 13 0 1 M NH OH K 1 8 10 5 10 8 M HCI 401 20 02 log 1 051 0 03 10 10 M NaOH 10 6 M CH COOH K 1 8 10 5 10 8 M CH COOH K 1 8 x 10 5 401 20 02 log 1 051 0 031 h Decimolar solution of Baryta Ba OH diluted 100 times 10 3 mole of KOH dissolved in 100 L of water i Equal volume of HCl solution PH 4 0 0019 N HCl solution

When 1 L of NaOH 1M is mixed with 1 L of HCI 1 M the temperature of reaction mixture rises by 10 C When 1 L of NaOH 1 M is mixed with 2 L 0 5 M HCI the temperature of reaction mixture rises approximately by 1 10 C 2 5 C 3 6 67 C 4 3 33 C

3g of activated charcoal was added to 50 mL of acetic acid solution 0 06N in a flask After an hour it was filtered and the strength of the filtrate was found to be 0 042 N The amount of acetic acid adsorbed per gram of charcoal is JEE Main 2015 1 42 mg 4 36 mg 3 18 mg 2 54 mg

Calculate pH of following solutions ay 0 1 M HCI b c d e f g h i 1 0 1 M CH COOH K 1 8 x 10 5 log 1 8 0 13 0 1 M NH OH K 1 8 10 5 10 8 M HCI 401 20 02 log 1 051 0 03 10 10 M NaOH 10 6 M CH3COOH K 1 8 10 5 10 8 M CH COOH K 1 8 x 10 5 401 20 02 log 1 051 0 03 Decimolar solution of Baryta Ba OH diluted 100 times 10 3 mole of KOH dissolved in 100 L of water Equal volume of HCl solution PH 4 0 0019 N HCl solution

C 4 9 10 9 D 4 9 10 7 At 30 C In which of the one litre solution the solubility of Ag CO3 solubility product 8x 10 2 be maximum C 0 05 M AgNO D 0 05 M NH 4 10 5 A 0 05 M Na CO B Pure water Read the following i An equimolar coluti

5 C d e f h 1 1 0 1 M HCI 0 1 M CH COOH K 1 8 10 5 log 1 8 0 13 0 1 M NH OH K 1 8 10 5 10 8 M HCI 401 20 02 log 1 051 0 03 10 10 M NaOH 10 6 M CH COOH K 1 8 10 5s 10 8 M CH COOH K 1 8 x 10 5 401 20 02 log 1 051 0 03 Decimolar solution of Baryta Ba OH diluted 100 times 10 3 mole of KOH dissolved in 100 L of water Equal volume of HCl solution PH 4 0 0019 N HCl solution

5 14 Calculate H CH COO and C H O in a solution that is 0 02 M in acetic acid and 0 0 in benzoic acid K acetic 1 8 x 10 5 K benzoic 6 4 10 5 a POLYPROTIC ACIDS RACES

2 In the reaction N O 2NO at equilibrium the concentrations of N O and NO are 0 25 0 05 and 1 M respectively Calculate initial concentrations of N and O 2 1 0 25 M 0 35 M 2 0 05 M 0 35 M 3 0 75 M 0 55 M 4 0 75 M 0 45 M

2 25 One mole of X is mixed with one mole of Y in a flask of volume 1 litre If at equilibrium 0 5 mole of Y are obtained Then find out K for reaction 2 P LICAT X Y 2XY 2 g 1 12 2 9 g 3 4 4 36

solubility product of Ca OH is 10 11 the pH which Ca OH precipitate from a solutio containing decimolar concentration of Ca is 1 5 3 9 2 9 pH 5 4 9 pH 7

2 At 490 C the equilibrium constant for the synthesis of HI is 50 The value of K for the dissociation of HI will be A 20 0 B 2 0 C 0 2 D 0 02

PCI PCI Cl is 0 5 at 500 K What is the state of vessel shown below 8 PCI X f Zh Lo p PCI fo C 8 1 The contents of the vessel are not in equilibrium with an excess of PC15 2 The contents of vessel are in equilibrium 3 The contents of the vessel are not in equilibrium with an excess of PCI and Cl 4 Nothing can be predicted regarding the o equilibrium just from the diagram given above ad llw onny noi

0 45 On addition of NaOH to CH3COOH solution 60 of the acid is neutralised If pK of CH COOH is 4 7 then the pH of the resulting solution is A More than 4 7 but less than 5 0 C More than 5 0 ill B Less than 4 7 but more than 4 0 D Remains unchanged able acidic when

The concentration of hydrogen ion in a sample of soft drink is 3 8 x 10 M what is its pH Solution pH log 3 8 x 10 1 log 3 8 log 10 0 58 3 0 2 42 2 42 Therefore the pH of the soft drink is 2 43 and it can be inferred that it is acidic

53 The equilibrium constant K for the reaction 2HI g H g 1 g at room temperature is 2 85 and that at 698 K is 1 4 x 102 This implies that A HI is an exothermic compound B HI is very stable at room temperature C HI is relatively less stable than H and I D HI is resonance stabilized 60

Composition of the equilibrium mixture Cl 2CI which is attained at 1200 C is determined by measuring rate of effusion through a pin hole It is observed that at 1 80 mm Hg pressure the mixture effuses 1 16 times as fast as Krypton effuses under the same conditions Calculate the fraction of chlorine molecules dissociated into atoms IIT 95 Relative atomic mass of Kr 84

a Methanol a liquid fuel that could possibly replace gasoline can be prepared from water gas and additional hydrogen at high temperature and pressure in the presence of a suitable catalyst Write the expression for the equilibrium constant for the reversible reaction 2H g CO g CH OH g AH 90 2 kJ Assume that equilibrium has been established and predict how the concentration of H CO and CH OH will differ at a new equilibrium if 1 more H is added 2 CO is removed 3 CH OH is added 4 the pressure on the system is increased 5 the temperature of the system is increased 6 more catalyst is added on of steam

0 05 g of a commercial sample of KCIO3 on decomposition liberated just sufficient oxygen for complete oxidation of 20 mL CO at 27 C 750 mm pressure Calculate of KClO3 in the sample

3 For two reactions in equilibrium in same container 1 A s 2B g C g Kp 27 atm 1 D s 2B g E g K 81 atm Pressure of B g at equilibrium will be 1 6 atm 2 3 atm 3 5 atm 4 9 atm

Calculate H H PO HPO2 and PO3 in a 0 01M solution of H PO4 Take K 10 K 10 8 K 10 13 HO

i An equimolar solution of NaNO and HNO can act as a Buffer solution ii Between Nat Agt ion Ag is a stronger Lewis acid iii Salts of strong acids and weak bases undergo cationic hydrolysis 2 iv If the salts M X QY and PZ have same solubilities 1 their Kvalues are related M X QY PZ3 Select the correct code for above A TFTT B FTFT C TTTT D FTTT

One mole of A reacts with one mole of B to form 0 1 mole of C and 0 1 mole of D What will be the value of the equilibrium constant 1 0 01 2 100 4 81 3 1 81

150 mL of 0 0008 M ammonium sulphate is mixed with 50 mL of 0 04 M calcium nitrate The ionic product of CaSO will be 4 K 2 4 x 10 5 for CaSO4 sp 1 K 2 K sp sp 3 K sp 4 None of these assd sticend vhoqanov p valsdial 2 pristni

10 M pyridine solution to which 0 3 mol of pyridinium chloride CH NH CI has been added assuming no change in volume Calculate the pH of a solution which results from the mixing of 50 0 ml of 0 3 M HCl with 50 0 ml of 9 4 MINH K NH 1 8 10 5 33 Calculate the pH of a solution made by mixing 50 0 ml of 0 2M NH CI 75 0 ml of 0 1 M NaOH 0 32