NCERT Solutions for Class 11 Chemistry Chapter 7 Equilibrium

Topics and Subtopics in NCERT Solutions for Class 11 Chemistry Chapter 7 Equilibrium:

Section Name	Topic Name
7	Equilibrium
7.1	Equilibrium in Physical Processes
7.2	Equilibrium in Chemical Processes – Dynamic Equilibrium
7.3	Law of Chemical Equilibrium and Equilibrium Constant
7.4	Homogeneous Equilibria
7.5	Heterogeneous Equilibria
7.6	Applications of Equilibrium Constants
7.7	Relationship between Equilibrium Constant K, Reaction Quotient Q and Gibbs Energy G
7.8	Factors Affecting Equilibria
7.9	Ionic Equilibrium in Solution
7.10	Acids, Bases and Salts
7.11	Ionization of Acids and Bases
7.12	Buffer Solutions
7.13	Solubility Equilibria of Sparingly Soluble Salts

NCERT Solutions Class 11 Chemistry Chemistry Lab Manual Chemistry Sample Papers

NCERT TEXTBOOK QUESTIONS SOLVED

Question 1. A liquid is in equilibrium with its vapours in a sealed container at a fixed temperature. The volume of the container is suddenly increased, (i) What is the initial effect of the change on the vapour pressure? (ii) How do the rates of evaporation and condensation change initially? (iii) What happens when equilibrium is restored finally and what will be the final vapour pressure?
Answer: (i) On increasing the volume of the container, the vapour pressure will initially decrease because the same amount of vapours are now distributed over a larger space.
(ii) On increasing the volume of the container, the rate of evaporation will increase initially because now more space is available. Since the amount of the vapours per unit volume decrease on increasing the volume, therefore, the rate of condensation will decrease initially.
(iii) Finally, equilibrium will be restored when the rates of the forward and backward processes become equal. However, the vapour pressure will remain unchanged because it depends upon the temperature and not upon the volume of the container.

Question 2. What is K_c for the following reaction in state of equilibrium?

Answer:

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Question 3.

Answer:

Question 4. Write the expression for the equilibrium constant for each of the following reactions

Answer:

What is the dilution factor formula? For dilution factor you should divide the volume of your final solution by the weight of sediment used.

Question 5. Find the value of K_c for each of the following equilibria from the value of K

Answer:

Question 6. For the following equilibrium, K =6.3 x 10¹⁴ at 1000 K. NO(g)+O₃—–>NO₂(g) + O₂(g) Both the forward and reverse reactions in the equilibrium are elementary bimolecular reactions. What is K_c for the reverse reaction?
Answer:

Question 7. Explain why pure liquids and solids can be ignored while writing the value of equilibrium constants.
Answer: This is because molar concentration of a pine solid or liquid is independent of the amount present.

Since density of pure liquid or solid is fixed and molar mass is also fixed. Therefore molar concentration are constant.

How To Find Kp In Chemistry

Question 8. Reaction between nitrogen and oxygen takes place as follows:

If a mixture of 0.482 mol of N₂ and 0.933 mol of O₂ is placed in a reaction vessel of volume 10 L and allowed to form N₂O at a temperature for which K_c – 2.0 x 10^-37, determine the composition of the equilibrium mixture.
Answer: Let x moles of N₂(g) take part in the reaction. According to the equation, x/2 moles of O₂ (g) will react to form x moles of N₂O(g). The molar concentration per litre of different species before the reaction and at the equilibrium point is:

The value of equilibrium constant (2.0 x 10^-37) is extremely small. This means that only small amounts of reactants have reacted. Therefore, is extremely small and can be omitted as far as the reactants are concerned.

Question 9. Nitric oxide reacts with bromine and gives nitrosyl bromide as per reaction given below:

When 0.087 mole of NO and 0.0437 mole of Br₂ are mixed in a closed container at constant temperature, 0.0518 mole of NOB_r is obtained at equilibrium. Determine the compositions of the equilibrium mixture.
Answer: The balanced chemical equation for the reaction is:
According to the equation, 2 moles of NO (g) react with 1 mole of Br₂(g) to form 2 moles of NOB_r (g). The composition of the equilibrium mixture can be calculated as follows:
No. of moles of NOB_r (g) formed at equilibrium = 0.0518 mol (given)
No. of moles of NO (g) taking part in reaction = 0.0518 mol
No. of moles of NO (g) left at equilibrium = 0.087 – 0.0518 = 0.0352 mol
No. of moles of Br₂ (g) taking part in reaction = 1/2 x 0.0518 = 0.0259 mol
No. of moles of Br₂ (g) left at equilibrium = 0.0437 – 0.0259 = 0.0178 mol
The initial molar concentration and equilibrium molar concentration of different species may be represented as:
2NO (g) + Br₂(g) ——————> 2NOB_r(g)
Initial moles 0.087 0.0437 0
Moles at eqm. point: 0.0352 0.0178 0.0518

Question 10.

Answer:

Question 11. A sample of HI (g) is placed in a flask at a pressure of 0.2 atm. At equilibrium partial pressure of HI (g) is 0.04 atm. What is K_p for the given equilibrium?

Answer:

Question 12. A mixture of 1.57 mol of N₂, 1.92 mol of H₂ and 8.13 mol of NH₃is introduced into a 20 L reaction vessel at 500 K. At this temperature, the equilibrium constant K_c for the reaction

Is this reaction at equilibrium? If not, what is the direction of net reaction?
Answer:

Question 13. The equilibrium constant expression for a gas reaction is,

Write the balanced chemical equation corresponding to this expression.
Answer: Balanced chemical equation for the reaction is 4

Question 14. If l mole of H₂0 and 1 mole of CO are taken in a 10 litre vessel and heated to 725 K, at equilibrium point 40 percent of water (by mass) reacts with carbon monoxide according to equation.

Calculate the equilibrium constant for the reaction.
Answer: Number of moles of water originally present = 1 mol
Percentage of water reacted =40%
Number of moles of water reacted = 1 x 40/100 = 0.4 mol
Number of moles of water left = (1 – 0.4) = 0.6 mole According to the equation, 0.4 mole of water will react with 0.4 mole of carbon monoxide to form 0.4 mole of hydrogen and 0.4 mole of carbon dioxide.
Thus, the molar cone, per litre of the reactants and products before the reaction and at the equilibrium point are as follows:

Question 15. What is the equilibrium concentration of each of the substances in the equilibrium when the initial concentration of ICl was 0.78 M?

Answer:

Question 16. K =0.04 atm at 898 K for the equilibrium shown below. What is the equilibrium concentration ok C₂H₆ when it is placed in a flask at 4 atm pressure,and allowed to come to equilibrium.

Answer:

Question 17. The ester, ethyl acetate is formed by the reaction of ethanol and acetic acid and the equilibrium is represented as:
CH₃COOH(l) + C2H5OH(l)——-> CH₃COOC₂H₅(l) + H₂O(l)
(i) Write the concentration ratio (concentration quotient) Q for this reaction. Note that water is not in excess and is not a solvent in this reaction.
(ii) At 293 K, if one starts with 1.000 mol of acetic acid and 0.180 mol of ethanol, there is 0.171 mol of ethyl acetate in the final equilibrium mixture. Calculate the equilibrium constant.
(iii) Starting mth 0.50 mol of ethanol and 1.0 mol of acetic acid and maintaining it at 293 K, 0.214 mol of ethyl acetate is found after some time. Has equilibrium been reached?
Answer:

Since Q_c is less than K_c this means that the equilibrium has not been reached. The reactants are still taking part in the reaction to form the products.

Question 18. A sample of pure PCl₅was introduced into an evacuated vessel at 473 K. After equilibrium was reached, the concentration of PCl₅ was found to be 0.5 x 10^-1 mol L^-1. If K_c is 8.3 x 10^-3 what are the concentrations of PCl₃ and Cl₂ at equilibrium?
Answer: Let the initial molar concentration of PCl₅ per litre = x mol
Molar concentration of PCl₅ at equilibrium = 0.05 mol
.’. Moles of PCl₅ decomposed = (x – 0.05) mol
Moles of PCl₃ formed = (x – 0.05) mol
Moles of Cl₂ formed = (x – 0.05) mol
The molar conc./litre of reactants and products before the reaction and at the equilibrium point are:

Question 19. One of the reactions that takes place in producing steel from iron ore is the reduction of iron
(II) oxide by carbon monoxide to give iron metal and C0₂
FeO(s) + CO(g) ———>Fe(s) + C0₂(g) ; K_p = 0.265 atm at 1050 K
What are the equilibrium partial pressures of CO and C0₂at 1050 K if the initial pressures are: P_CO = 1.4 atm and P_CO2 = 0.80 atm?
Answer:

Since Q_p>K_p(0.265), this means that the reaction will move in the backward direction to attain the equilibrium. Therefore, partial pressure of C0₂ will decrease while that of CO will increase so that the equilibrium may be attained again. Let p atm be the decrease in the partial pressure of C0₂. Therefore, the partial pressure of CO will increase by the same magnitude i.e., p atm.

Question 20.

Answer:

Question 21. Bromine monochloride (B_rCl ) decomposes into bromine and chlorine and reaches the equilibrium:

The value of Kc is 32 at 500 K. If initially pure B_rCl is present at a concentration of 3.3 x10^-3mol L^-1what is its molar concentration in the mixture at equilibrium?
Answer: Let x moles of B_rCl decompose in order to attain the equilibrium. The initial molar concentration and the molar concentration at equilibrium point of different species may be represented as follows:

Question 22. At 1127 K and 1 atmosphere pressure, a gaseous mixture of CO and C0₂ in equilibrium with solid carbon has 90.55% CO by mass.

Calculate K_c for the reaction at the above temperature.
Answer:

Question 23. Calculate (a) ∆G^– and (b) the equilibrium constant for the formation of N0₂ from NO and 0₂ at 298 K

Answer:

Question 24. Does the number of moles of reaction products increase, decrease or remain same when each of the following equilibria is subjected to a decrease in pressure bp increasing the volume?

Answer: (i) Pressure will increase in the forward reaction and number of moles of products will increase.
(ii) Pressure will increase in backward reaction and number of moles of products will decrease.
(iii) The change in pressure will have no effect on the equilibrium constant and there will be no change in the number of moles.

Question 25. Which of the following reactions will get affected by increase in pressure ? Also mention whether the change will cause the reaction to go to the right or left direction.

Answer: Only those reactions will be affected by increasing the pressure in which the number of moles of the gaseous reactants and products are different (n_p ≠ n_r) (gaseous). With the exception of the reaction (1); all the reamaining five reactions will get affected by increasing the pressure. In general,

The reaction will go to the left if n_p> n_r.
The reaction will go to the right if n_r > n_p .
Keeping this in mind,

(i) Increase in pressure will not affect equilibrium because n_p = n_r = 3.
(ii) Increase in pressure will favour backward reaction because n_p (2) > n_r (1)
(iii) Increase in pressure will favour backward reaction because n_p (10) > n_r (9)
(iv) Increase in pressure will favour forward reaction because n_p (1) < n_r (2)
(v) Increase in pressure will favour backward reaction because n_p (2) > n_r(1)
(vi) Increase in pressure will favour backward reaction because n_p (1) > n_r (0).

Question 26. The equilibrium constant for the following reaction is 1.6 x 10⁵at 1024 K.
Find the equilibrium pressure of all gases if 10.0 bar of HB_r is introduced into a sealed container at 1024 K.

Ans.

Question 27. Hydrogen gas is obtained from the natural gas by partial oxidation with steam as per the following endothermic reaction:

Write the expression for Kp for the above reaction
How will the value of K_p and composition of equilibrium mixture be affected by:
(i) increasing the pressure, (ii) increasing the temperature, (iii) using a catalyst?
Answer: The expression for K_pfor the reaction is:

(i) By increasing the pressure, the number of moles per unit volume will increase. In order to decrease the same, the equilibrium gets shifted to the left or in the backward direction. As a result, more of reactants will be formed and the value of K_p will decrease.
(ii) If the temperature is increased, according to Le Chatelier’s principle, the forward reaction will be favoured as it is endothermic. Therefore, the equilibrium gets shifted to the right and the value of K_p will increase.
(iii) The addition of catalyst will not change the equilibrium since it influences both the forward and the backward reactions to the same extent. But it will be attained more quickly.

Question 28. What is the effect of:
(i) addition of H₂ (ii) addition of CH₃OH
(iii) removal of CO (iv) removal of CH₃OH

Answer: (i) Equilibrium will be shifted in the forward direction.
(ii) Equilibrium will be shifted in the backward direction.
(iii) Equilibrium will be shifted in the backward direction.
(iv) Equilibrium will be shifted in the forward direction.

Question 29. At 473 K, the equilibrium constant K_c for the decomposition of phosphorus pentachloride (PCl₅) is 8.3 x 10^-3. if decomposition proceeds as:

(a) Write an expression for K_c for the reaction
(b) What is the value of K_c for the reverse reaction at the same temperature.
(c) What would be the effect on K_c if
(i) More of PCl₅is added (ii) Temperature is increased.
Answer:

(c) (i) By adding more of PCl₅, value of K_c will remain constant because there is no change in temperature.
(ii) By increasing the temperature, the forward reaction will.be favoured since it is endothermic in nature. Therefore, the value of equilibrium constant will increase.

Question 30. Dihydrogen gas used in Haber’s process is produced by reacting methane from natural gas with high temperature steam. The first stage of two stage reaction involves the formation of CO and H₂ In second stage, CO formed in first stage is reacted with more steam in water gas shift reaction.

If a reaction vessel at 400°C is charged with an equimolar mixture of CO and steam so that P_CO = PH₂O = 4.0 bar, what will be the partial pressure of H₂ at equilibrium? K_p = 0.1 at 400°C.
Answer:

Question 31. Predict which of the following will have appreciable concentration of reactants and products:

Answer: Following conclusions can be drawn from the values of K_c .
(a) Since the value of K_c is very small, this means that the molar concentration of the products is very small as compared to that of the reactants.
(b) Since the value of K_c is quite large, this means that the molar concentration of the products is very large as compared to that of the reactants.
(c) Since the value of K_c is 1.8, this means that both the products and reactants have appreciable concentration.

Question 32.The value of K_c for the reaction 30₂(g) —>20₃(g) is 2.0 x 10^-50 at 25°C. If equilibrium concentration of 02 in air at 25°C is 1.6 x 10^-2, what is the concentration of O₃?
Answer:

Question 33.

Answer:

Question 34. What is meant by conjugate acid-base pair? Find the conjugate acid/base for the following species: HNO₂, CH^–, HClO₄ , OH^–, CO₃^2-, S^2-
Answer: An acid-base pair which differs by a proton only (HA———> A^– + H⁺) is known as conjugate acid-base pair.
Conjugate acid:HCN,H₂0,HCO₃^–,HS^–.
Conjugate base:NO₂^–,ClO₄^–,O₂^–

Question 35. Which of the following are Lewis Acids?
H₂O,BF₃, H⁺ and NH⁴⁺,
Answer: BF₃, H⁺ ions are Lewis acids.

Question 36. What will be the conjugate bases for the Bronsted acids?HF, H₂S0₄ and H₂C0₃?
Answer: Conjugate bases: F^–, HSO^–₄ , HCO^–₃.

Question 37. Write the conjugate acids for the following Bronsted bases:
NH₂, NH₃ and HCOO^–
Answer: NH₃, NH₄⁺ and HCOOH

Question 38.The species H₂0, HCO₃^–, HSO₄^– and NH₃ can act both as Bronsted acid and base. For each case, give the corresponding conjugate acid and base.
Answer:

Question 39. Classify the following species into Lewis acids and Lewis bases and show how these can act as Lewis acid/Lewis base?
(a) OH^–ions (b) F^–(c) H⁺ (d) BCl₃
Answer: (a) OH^– ions can demate an electron pair and act as Lewis base.
(b) F^– ions can donate an electron pair and act’as Lewis base.
(c) H⁺ ions can accept an electron pair and act as Lewis acid.
(d) BCl₃ can accept an electron pair since Boron atom is electron deficient. It is a Lewis acid.

Question 40. The concentration of hydrogen ions in a sample of soft drink is 3.8 x 10^-3M. What is the pH value?
Answer: pH = – log [H⁺] = – log (3.8 x 10^-3) = – log 3.8 + 3 = 3 – 0.5798 = 2.4202 = 2.42

Question 41. The pH of a sample of vinegar is 3.76. Calculate the concentration of hydrogen ion in it.
Answer: pH = – log [H⁺] or log [H⁺] = – pH = – 3.76 = 4.24
.-. [H⁺] = Antilog 4.24 = 1.738 x 10^-4 = 1.74 x 10-4 M

Question 42. The ionization constant of HF, HCOOH and HCN at 298 K are is 6.8 x 10^-4 , 1.8 x 10^-4 and 4.8 x 10^-9respectively, Calculate the ionization constant of the corresponding conjugate base.
Answer: For F^–, K_b =K_w/K_a= 10^-14/(6.8 x 10^-4) = 1.47 x 10^-11 = 1.5 x 10^-11 .
For HCOO-, K_b = 10^-14/(1.8 x 10^-4) = 5.6 x 10^-11
For CN^–, K_b= 10^-14/(4.8 X 10^-9) = 2.08 x 10^-6

Question 43. The ionization constant of phenol is 1.0 x 10^-10. What is the concentration of phenolate ion in 0.05 M solution of phenol? What will be its degree of ionization if the solution is also 0.01 M in sodium phenolate?
Answer:

Question 44. The-first ionization constant of H₂S is 9.1 x 10^-8. Calculate the concentration of HS^– ions in its 0.1 M solution and how will this concentration be affected if the solution is 0.1 M in HCl also? If the second dissociation constant of H₂S is 1.2 x 10^-13, calculate the concentration of S^2-under both conditions.
Answer:

Question 45. The ionization constant of acetic acid is 1.74 x 10^-5. Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ions in the solution and its pH.
Answer:

Question 46. It has been found that the pH of a 0.01 M solution of an organic acid is 4.15. Calculate the concentration of the anion, the ionization constant of the acid and its PK_a.
Answer:

Question 47. Assuming complete dissociation, calculate the pH of the following solutions:
(a) 0.003 M HCl (b) 0.005 M NaOH (c) 0.002 M HBr (d) 0.002 M KOH
Answer:

Question 48. Calculate the pH of the following solutions:
(a) 2g ofTlOH dissolved in water to give 2 litre of the solution
(b) 0.3 g of Ca(OH)₂dissolved in water to give 500 mL of the solution
(c) 0.3 g of NaOH dissolved in water to give 200 mL of the solution
(d) l mL of 13.6 M HCl is diluted with water to give 1 litre of the solution.
Answer:

Question 49. The degree of ionization of a 0.1 M bromoacetic acid solution is 0.132. Calculate the pH of the solution and the PK_a of bromoacetic acid.
Answer:

Question 50. The pH of0.005 M codeine (C₁₈H₂₁N0₃) solution is 9.95. Calculate the ionization constant and PK_b.
Answer:

NCERT Solutions for Class 11 Chemistry Chapter 7 Very Short Answer Type Questions

Question 1. What is meant by equilibrium?
Answer: Equilibrium is a state at which rate of forwarding reaction is equal to the rate of backward reaction.

Question 2. State the law of mass action?
Answer: It states that the rate at which a substance reacts is directly proportional to its molar concentration.

Question 3. What is meant by reaction quotient?
Answer: It is defined as the ratio of the product of molar concentration of products to the product of molar concentration of reactants at any stage of the reaction.

Ionic Strength Calculator displays the ionic strength in a solution.

Question 4. Define ionic equilibrium.
Answer: The equilibrium between ions and unionised molecules is called ionic equilibrium.

Question 5. What is meant by ionic product of water (k_w)?
Answer: It is the product of concentration of [ H₃O⁺] and [OH^–] at a specific temperature.
Kw = [H₃O⁺] [OH^–]
= 1.0 x 10-14 at 298 K

Question 6. Define solubility product.
Answer: It is product of molar concentration of ion raised to the power of number of ions produced per compound in saturated solution.

Question 7. How does common ion affect the solubility of electrolyte?
Answer: Solubility of electrolyte decreases due to common ion effect.

Question 8. Write conjugate add and conjugate base of H₂O?
Answer: Conjugate acid is H₃O⁺ and conjugate base is OH^–.

Question 9. Give two characteristics of a buffer solution.
Answer:

Its pH does not change on the addition of small amount of acid or base.
Its pH does not change on dilution or standing.

Question 10. How does a catalyst affect the equilibrium constant?
Answer: The equilibrium constant is not affected by a catalyst.

Question 11. State Ostwald’s dilution law.
Answer: Ostwald’s dilution law states that the degree of dissociation of weak electrolyte is inversely proportional to square root of its concentration.

Where, Kfl and Kfc are acid dissociation and base dissociation constants.

Question 12. What is basic buffer?
Answer: Basic buffer is the buffer whose pH is more than 7. It is a mixture containing weak base and its salt with a strong acid, e.g., NH₄Cl + NH₄OH

Question 13. S0₃^2-is Bronsted base or acid and why?
Answer: S0₃^2-is Bronsted base because it can accept H⁺.

Question 14.

What is the relationship between K_p and K_c?
Answer: K_p = K_c
because ∆n = 0.

Question 15. Define common ion effect.
Answer: The supervision in concentration of one of the ions by adding other ion as common ion is called common ion effect.

NCERT Solutions for Class 11 Chemistry Chapter 7 Short Answer Type Questions

Question 1. The following concentration were obtained for the formation of NH₃ from N₂ and H₂at equilibrium at 500 K.[N₂(g)] = 1.5 x 10^-2M [H₂ (g)] = 3.0 x 10^-2 M [NH₃] = 1.2 x 10^-2M. Calculate equilibrium constant.
Answer:

Question 2. Write the equilibrium constant (K_c) expression for the following reactions.

Answer:

Question 3. Given the equilibrium N₂O₄ (g) ——->2NO₂ (g) K=0.15 atm at 298 K
(a) What is K_p using pressure in torr?
(b) What is K_cusing units of moles per litre.

Answer:

Question 4. In the reaction A + B———> C + D, what will happen to the equilibrium if concentration of A is increased?
(b) The equilibrium constant for a reaction is 2 x 10^-23 at 25°C and 2 x 10^-2 at 50°C. Is the reaction endothermic or exothermic?
(c) Mention at least three ways by which the concentration of S0₃ can be increased in the following reaction in a state of equilibrium.
Answer: (a) The reaction will shift in the forward direction.
(b) Endothermic
(c) (i) lowering the temperature (ii) increasing pressure.
(iii) increasing concentration of oxygen.

Question 5. (i) Define Le Chatelier’s principle.
(ii) Following reactions occur in a Blast furnace.
Fe₂0₃(s) + 3CO(g) ———–>2Fe(s) + 3CO₂(g)
use Le chatelier’s principle to predict the direction of reaction when equilibrium mixture is disturbed by
(a) adding Fe₂0₃ (b) removing CO₂ .
(c) removing CO.
Answer: (a) When a system under equilibrium is subjected to a change in temperature, pressure or concentration, then the equilibrium shifts in such a direction so as to undo the effect of the change.
(ii) (a) On adding Fe₂0₃(s), the equilibrium will remain unaffected.
(b) By removing CO₂(g), the equilibrium will be shifted in the forward direction.
(c) By removing CO(g), the equilibrium will be shifted in the backward direction.

NCERT Solutions for Class 11 Chemistry Chapter 7 Long Answer Type Questions

Question 1. (i) Point out the differences between ionic product and solubility product.
(ii) The solubility of AgCl in water at 298 K is 1.06 x 10^-5 mole per litre. Calculate its solubility product at this temperature.
Answer: (i)

Question 2. At certain temperature and under a pressure of 4 atm, PCl₅ is 10% dissociated. Calculate the pressure at which PCl₅ will be 20% dissociated at temperature remaining constant.
Answer: Calculation of K_p

NCERT Solutions for Class 11 Chemistry Chapter 7 Multiple Choice Questions

Question 1. The equilibrium expression, K_c= [C0₂] represents the reaction.

Question 2. Hydrogen molecule (H₂) can be dissociated into hydrogen atoms (H). Which one of the following changes will not increase the number of atoms present at equilibrium?
(a) adding H atoms (b) increasing the temperature
(c) increasing the total pressure (d) increasing the volume of the container
Question 3. What is the expression for K_eq? for the reaction

Question 4. A catalyst will increase the rate of a chemical reaction by
(a) shifting the equilibrium to the right (b) shifting the equilibrium to the left (c) lowering the activation energy (d) increasing the activation energy
Question 5. What is the correct expression for the representation of the solubility product constant of Ag₂Cr0₄?

Question 6. In a closed system

Question 7. H₂+ S ——->H₂S + energy.
In this reversible reaction, select the factor which will shift the equilibrium to the right.
(a) adding heat (b) adding H₂S
(c) blocking hydrogen gas reaction (d) removing hydrogen sulphide gas
Question 8. What effect does a catalyst have on the equilibrium position of a reaction?
(a) a catalyst favours the formation of products
(b) a catalyst favours the formation of reactants
(c) a catalyst does not change the equilibrium position of a reaction
(d) a catalyst may favour reactants or product formation, depending upon the directiofi in which the reaction is written.
Question 9. A chemist dissolves an excess of BaSO₄ in pure water at 25°C if its K_sp= 1 x 10^-10 what is the concentration of barium in the water?
(a) 10^-4M (b) 10^-5M (C) 10^-15M (d) 10^-6 M
Question 10. If in a mixture where Q = k is combined, then what happens?
(a) the reaction shift towards products
(b) the reaction shift towards reactants
(c) nothing appears to happen, but forward and reverse are continuing at the same rate
(d) nothing happens
Answer: 1.(b) 2.(c) 3.(c) 4.(c) 5.(a)
6.(d) 7.(a) 8.(c) 9.(c) 10.(c)

NCERT Solutions for Class 11 Chemistry Chapter 7 HOTS Questions

Question 1. For the equilibrium 2 NOCl(g)——-> 2NO(g) + Cl₂(g) the value of the equilibrium constant Kc is 3.75 x 10^-6 at 1069 K. Calculate the K_pfor the reaction at this temperature?
Answer: We know that K_p = K_c(RT)^∆n
For the above reaction, ∆n = (2 + 1) – 2 = 1 K_p = 3.75 x 10’6 (0.0831 x 1069)
K_p = 0.033.

Question 2. The values of Ksp of two sparingly soluble salts Ni(OH)₂and AgCN are 2.0 x 10^-15 and 6 x 10^-17 respectively. Which salt is more soluble? Explain.
Answer:

Question 3. The value of Kc for the reaction 2A——>B + C is 2 x 10^-3. At a given time, the composition of reaction mixture is [A] = [B] = [C] = 3 x 10^-4 M. In which direction the reaction will proceed?
Answer: For the reaction the reaction quotient Q_c is given by Q_c = [B] [C]/[A]2 as [A] = [B] = [C] = 3 x 10-4 M Q_c = (3 x 10^-4) (3 x10^-3)/(3 x 10) = 1
as Q_c > K_c, so, the reaction will proceed in the reverse direction.

Question 4. PCl₅, PCl₃ and Cl₂ are at equilibrium at 500 K and having concentration 1.59M PCl₅ 1.59M Cl₂ and 1.41M PCl₅. Calculate K_c for the reaction PCl₅———>PC₁₃+ Cl₂
Answer: The equilibrium constant Kc for the above reaction can be written as:

Question 5. Dihydrogen gas is obtained from natural gas by partial oxidation with steam as per following endothermic reaction:
CH₄(g) + H₂O(g) ——> CO(g) + 3 H₂(g)
(a) Write an expression for K_pfor the above reaction.
(b) How will the values of K_p and composition of equilibrium mixture be affected by (i) increasing the pressure (ii) increasing the temperature (iii) using a catalyst?
Answer:

(b) (i) value of K_p will not change, equilibrium will shift in backward direction.
(ii) value of K_p will increase and reaction will proceed in forward direction.
(iii) no effect.

NCERT Solutions for Class 11 Chemistry Chapter 7 Equilibrium