NEET Chemistry Chemical Equilibrium Revision Notes

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Chapter-wise Revision Notes for Full Course Chemical Equilibrium Chemical Equilibrium

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Chemical Equilibrium Revision Notes for Full Course Chemical Equilibrium

Revision Notes on Chemical and Ionic Equilibrium
 
Equilibrium
 
• Equilibrium is the state of a process in which the properties like temperature, pressure, and concentration etc of the system do not show any change with passage of time.
• In all processes which attain equilibrium, two opposing processes are involved.
• Equilibrium is attained when the rates of the two opposing processes become equal.
• If the opposing processes involve only physical changes, the equilibrium is called Physical Equilibrium.
• If the opposing processes are chemical reactions, the equilibrium is called Chemical Equilibrium.
 
Physical Equilibrium
 
NEET Chemistry Chemical Equilibrium Revision Notes
 
Equilibrium in Chemical Process
 
• Reversible reaction: A reaction in which not only the reactants react to form the products under certain conditions but also the products react to form reactants under the same conditions
NEET Chemistry Chemical Equilibrium Revision Notes Reaction
 
•  Irreversible reaction: A reaction cannot take place in the reverse direction, i.e. the products formed do not react to give back the reactants under the same condition.
 
Example: AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(g)
 
•  Generally, a chemical equilibrium is represented as NEET Chemistry Chemical Equilibrium Revision Notes Reaction1
 
Where A, B are reactants and C, D are products.
NEET Chemistry Chemical Equilibrium Revision Notes R
 
• The equilibrium state is dynamic and not static in nature. A reaction is said to have attained equilibrium when the rate of forward reaction equals that of backward reaction
 
NEET Chemistry Chemical Equilibrium Revision Notes R2
 
• Homogeneous Equilibrium: All the reactants and products of any reaction under equilibrium are in same physical state.
Example:
NEET Chemistry Chemical Equilibrium Revision Notes Reaction2
 
• Heterogeneous Equilibrium :Physical state of one or more of the reacting species may differ i.e. all the reactants and products are not in same physical state.
Example
 
NEET Chemistry Chemical Equilibrium Revision Notes Reaction3
 
Characteristics of Equilibrium State
• It can be attained only if the reversible reaction is carried out in closed vessel.
• It can be attained from either side of the reaction.
• A catalyst can hasten the approach of equilibrium but does not alter the state of equilibrium.
• It is dynamic in nature i.e. reaction does not stop but both forward and backward reactions take place at equal rate.
• Change of pressure, concentration or temperature favours one of the reactions (forward or backward) resulting in shift of equilibrium point in one direction.
 
Law of Mass Action & Equilibrium Constant
 
“The rate at which a substance reacts is directly proportional to its active mass and rate of a chemical reaction is directly proportional to product of active masses of reactants each raised to a power equal to corresponding stoichiometric coefficient appearing in the balanced chemical equation”.
 
NEET Chemistry Chemical Equilibrium Revision Notes Reaction4
 
where K is rate constant or velocity constant of the reaction at that temperature.
 
Unit of rate constant (K)
 
NEET Chemistry Chemical Equilibrium Revision Notes Reaction5
 
(where n is order of reaction.)
For unit concentration of reactants rate of the reaction is equal to rate constant or specific reaction rate.
 
NEET Chemistry Chemical Equilibrium Revision Notes Reaction6
NEET Chemistry Chemical Equilibrium Revision Notes Reaction7
 
Equilibrium Quotient or Mass Action Ratio:
Consider the equilibrium
 
NEET Chemistry Chemical Equilibrium Revision Notes Reaction8
 
When the reaction is not at equilibrium this ratio is called ‘QC’ i.e., QC is the general term used for the above given ratio at any instant of time. And at equilibrium QC becomes KC.
• If the reaction is at equilibrium, Q = Kc
• A net reaction proceeds from left to right (forward direction) if Q < KC.
• A net reaction proceeds from right to left (the reverse direction) if Q >Kc
 
The Le–Chatelier’s Principle:
Statement:
“When a chemical reaction at equilibrium is subjected to any stress, then the equilibrium shifts in that direction in which the effect of the stress is reduced.”
 
Effect of Addition of Inert Gases:
 
• Addition of inert gas at constant volume: No effect on equilibrium.
• Addition of inert gas at constant pressure: Equilibrium shifts in a direction where there is increase in number of moles of gases.
 
Effect of Change in Temperature:
 
• In a system at equilibrium, both exothermic and endothermic reactions take place simultaneously.
• Increase in temperature would shift the equilibrium in the direction of endothermic reaction.
• Decrease in temperature would shift the equilibrium in the direction of exothermic reaction.
 
Effect of Change in Concentration:
 
• When the concentration of reactants increased, equilibrium shifts in forward direction.
• When the concentration of the products is increases, equilibrium shifts in backward direction.\ Effect of Change in Pressure:
• Increase in pressure shifts the equilibrium in the direction of lesser number of gaseous molecules.
• Decrease in pressure shifts the equilibrium in the direction of larger number of gaseous molecules.
 
Effect of Catalyst:
 
Catalyst does not change the equilibrium.
 
Thermodynamics of chemical equilibrium:
NEET Chemistry Chemical Equilibrium Revision Notes Reaction9
NEET Chemistry Chemical Equilibrium Revision Notes Reaction10
 
Acids and Bases:
 
1. Arrhenius Definition:
 
a. Acids give H+ ions aqueous solutions.
b. Bases give OH- ions in aqueous solution.
 
2. Bronsted – Lowry Definition:
a. Acid is a proton donor .
b. Base is a proton acceptor.
 
3. Strong and Weak Acids:
a. Strong acid dissociate completely in aqueous solution.
Example: HCl
 
b. Weak acid dissociates partially in aqueous solution.
Examples: CH3COOH
Degree of dissociation (a) =(Ka/C)1/2
Where,
Ka = [CH3COO-][H+]/[CH3COOH]
And
C = Initial concentration of acid.
Also
[H+] = Ca = (Ka×C)1/2
 
c. Ionic Product of Water:
H2O H+ + OH–
K[H2O] = [H+] [OH–] = 10-14
 
Common Ion effect:
 
The addition of an ion to equilibrium, having the same ion makes the equilibrium `reaction move in a direction to consume that ion.
 
NEET Chemistry Chemical Equilibrium Revision Notes Reaction11
 
This implies that water would dissociate less in the presence of HCl.
 
Hydrolysis of salts:
 
1. Salt of a Weak Acid and Strong Base:
[H+] = (Kw Ka / C )1/2
2. Salt of a Weak Base and Strong Acid
[H+] = (Kw / Kb C )1/2
3. Salt of a Weak Acid and Weak Base
[H+] = (Kw Ka / Kb )1/2
 
• Buffer Solutions: Resists change in its pH when such a change is caused by the addition of a small amount of acid or base.
 
1. Weak acid–Salt buffer:
 
Formed by combination of a weak acid and a salt of the acid with a strong base. Example
CH3COOH & CH3COONa
pH = pKa + log [Conjugated base]/ [Acid]
For weak dibasic acid
pH = (pKa1 + pKa2 )/2
Where pKa1 and pKa2 are 1st and 2nd dissociation constant of the acid.
 
2. Weak base–salt buffer: Formed by combination of a weak base and a salt of the base with a strong acid. Example, NH4OH and NH4Cl
pH = pKb + log [Conjugated acid]/ [Base]
 
Solubility and Solubility Product :
 
1. Amount (moles) of the salt that has made the solution saturated per liter of solution is called the solubility of the salt.
2. For salt AB.
NEET Chemistry Chemical Equilibrium Revision Notes Reaction12
 
3. Solution cannot have the product of the concentration of the ions more than KSP of the salt in solution.
 
Ionic Product:
 
a) Product of ionic concentration due to ions already present in water or from a salt.
b) I.P. may be and may not be equal to Ksp.
c) If ionic Product (IP) > Ksp ; precipitation takes place till I.P. equals Ksp
d) If Ionic Product < Ksp ; a precipitate will not be formed and the solution will be unsaturated.
e) If Ionic Product = Ksp ; a precipitate will not form an the solution is saturated in that salt.
 

Question. Which of the following conditions represents an equilibrium?
a. Freezing of ice in a open vessel, temperature of ice is constant
b. Few drops of water is present along with air in a balloon, temperature of balloon is constant
c. Water is boiling in an open vessel over stove, temperature of water is constant
d. All the statements (a), (b) and (c) are correct for the equilibrium
Answer : B

Question. The reaction CaCO3 CaO + CO2 (g) ⇌ goes to completion in lime kiln because:
a. of the high temperature
b. CaO is more stable than CaCO2
c. CaO is not dissociated
d. CO2 escapes continuously
Answer : D

Question. A reversible reaction is one which?
a. Proceeds in one direction
b. Proceeds in both directions
c. Proceeds spontaneously
d. All the statements are wrong
Answer : B

Question. Which of the following is a characteristic of a reversible reaction?
a. Number of moles of reactants and products are equal
b. It can be influenced by a catalyst
c. It can never proceed to completion
d. None of the above
Answer : C

Question. The decomposition of N2 O4 to NO2 is carried out at 280K in chloroform. When equilibrium has been established, 0.2 mol of N2 O4 and 2 x 10−3 mol of NO2 are present in 2 litre solution. The equilibrium constant for reaction N2 O4 ⇌ 2NO2 is:
a. 1 x 10−2
b. 2 x 10−2
c. 1 x 10−5
d. 2 x 10−5
Answer : C

Question. A reaction is A + B→ C + D. Initially we start with equal concentration of A and B. At equilibrium we find  the moles of C are two times of A. What is the equilibrium constant of the reaction?
a. 4
b. 2
c. 1 / 4
d. 1 / 2
Answer : A

Question. The rate constant for forward and backward reactions of hydrolysis of ester are 1.1 10−2 and 1.5 x 10−3 per minute respectively. Equilibrium constant for the reaction is CH3 COOC2 H5 + H2 O ⇌ CH3 COOH + C2 H5 OH
a. 4.33
b. 5.33
c. 6.33
d. 7.33
Answer : D

Question. 2 moles of PCl5 were heated in a closed vessel of 2 litre capacity. At equilibrium, 40% of PCl5 is dissociated into PCl3 and Cl3. The value of equilibrium constant is:
a. 0.266
b. 0.53
c. 2.66
d. 5.3
Answer : A

Question. Unit of equilibrium constant for the reversible reaction H2 + I2 ⇌ 2HI is:
a. mol–1 litre
b. mol–2 litre
c. 1 mol litre−
d. None of these
Answer : D

Question. For the chemical equilibrium, CaCO3 (s) ⇌ CaO(s) + CO2 (g), ΔHr° can be determined from which one of the following plots:

""NEET-Chemistry-Chemical-Equilibrium-Revision-Notes

Answer : A

Question. In which of the following equilibria, the value of Kp is less than Kc ?
a. H2 + I2 ⇌ 2HI
b. N2 + 3H2 ⇌ 2NH3
c. N2 + O2 ⇌ 2NO
d. CO + H2 O ⇌ CO2 + H2
Answer : B

Question. 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 H2 (g) + I2 (g) ⇌ 2HI(g) is?
a. 1
b. 10
c. 5
d. 0.33
Answer : A

Question. An equilibrium mixture of the reaction 22H2 S(g) ⇌ 2H2 (g) +S2 (g) had 0.5mole H2 S ,0.10 mole H2 and 0.4 mole S2 in one litre vessel. The value of equilibrium constant (K) in mole litre-1 is:
a. 0.004
b. 0.008
c. 0.016
d. 0.160
Answer : C

Question. At 3000 K the equilibrium pressures of CO2, CO and O2 are 0.6,0.4 and 0.2 atmospheres respectively. p K for the reaction, 2CO2 ⇌ 2CO + O2 is:
a. 0.089
b. 0.0533
c. 0.133
d. 0.177
Answer : A

Question. The equilibrium SO2CI2(g) ⇌ SO2(g) + Cl2(g) is attained at 25°C in a closed container and an inert gas helium is introduced which of the following statement is correct?
a. More chlorine is formed
b. Concentration of SO2 is reduced
c. More SO2 Cl2 is formed
d. Concentration of SO2 Cl2 ,SO2 and Cl2 does not change
Answer : D

Question. Sodium sulphate dissolves in water with evolution of heat. Consider a saturated solution of sodium sulphate. If the temperature is raised, then according to Le-Chatelier principle:
a. More solid will dissolve
b. Some solid will precipitate out from the solution
c. The solution will become supersaturated
d. Solution concentration will remain unchanged
Answer : B

Question. Consider the equilibrium: N2 (g) + 3H2 (g) ⇌ 2NH3 (g) ; ΔH = – 93.6 KJ.
The maximum yield of ammonia is obtained by:
a. Decrease of temp. and increase of pressure
b. Increase of temp. and decrease of pressure
c. Decrease of both the temp. and pressure
d. Increase of both the temp. and pressure
Answer : A

Question. Amongst the following chemical reactions the irreversible reaction is:
a. H2 + I2 ⇌ HI
b. AgNO3 + NaCl ⇌ AgCl + NaNO2
c. CaCO3 ⇌ CaO + CO2
d. O2 + 2SO2 ⇌ 2SO2
Answer : B

Question. In chemical reaction A ⇌  B, the system will be known in equilibrium when?
a. A completely changes to B
b. 50% of A changes to B
c. The rate of change of A to B and B to A on both the sides are same
d. Only 10% of A changes to B Irreversible and Reversible Reactions
Answer : C

Question. For the reaction H2 (g) + I2 (g) ⇌ 2HI(g), the equilibrium constant changes with:
a. Total pressure
b. Catalyst
c. The amounts of H2 and I2 taken
d. Temperature
Answer : D

Question. Calculate ΔG° for conversion of oxygen to ozone 3/ 2 O2 (g)→ O3 (g) at 298 K, if Kp for this conversion is 2.47 x 10−29 
a. 163 kJ mol−1
b. 2.4 x 102 kJ mol−1
c. 1.63 kJ mol−1
d. 2.38 x 106 kJ mol−1
Answer : A

Question. When the pressure is applied over system ice ⇌ water what will happen?
a. More water will form
b. More ice will form
c. There will be no effect over equilibrium
d. Water will decompose in H2 and O2
Answer : A

Question. The reactionA + B ⇌ C+ D+ heat has reached equilibrium.
The reaction may be made to proceed forward by:
a. Adding more C
b. Adding more D
c. Decreasing the temperature
d. Increasing the temperature
Answer : C

Question. Following gaseous reaction is undergoing in a vessel C2 H4 + H2 ⇌ C2 H6 ;ΔH = −32.7 Kcal Which will increase the equilibrium concentration of C2 H6 :
a. Increase of temperature
b. By reducing temperature
c. By removing some hydrogen
d. By adding some C2 H6
Answer : B

Question. N2 + O2 ⇌ 2NO − Qcals In the above reaction which is the essential condition for the higher production of NO
a. High temperature
b. High pressure
c. Low temperature
d. Low pressure
Answer : A

Question. Which of the following reactions proceed at low pressure?
a. N2 + 3H2 ⇌ 2NH3
b. H2 + I2 ⇌ 2HI
c. PCl5 ⇌ PCl3 + Cl2
d. N2 + O2 ⇌ 2NO
Answer : C

Question. In the following reversible reaction 2SO2 + O2 ⇌ 2SO3 + QCal Most suitable condition for the higher production of SO3 is:
a. High temperature and high pressure
b. High temperature and low pressure
c. Low temperature and high pressure
d. Low temperature and low pressure
Answer : C

Question. The effect of increasing the pressure on the equilibrium 2A + 3B⇌ 3A + 2B is:
a. Forward reaction is favoured
b. Backward reaction is favoured
c. No effect
d. None of the above
Answer : C

Question. For the equilibrium 2NO2 (g) ⇌ N2 O4 (g) + 14.6k cal the increase in temperature would:
a. Favour the formation of N2 O4
b. Favour the decomposition of N2 O4
c. Not alter the equilibrium
d. Stop the reaction 
Answer : B

Question. On the velocity in a reversible reaction, the correct explanation of the effect of catalyst is:
a. It provides a new reaction path of low activation energy
b. It increases the kinetic energy of reacting molecules
c. It displaces the equilibrium state on right side
d. It decreases the velocity of backward reaction
Answer : A

Question. According to Le-chatelier principle, if heat is given to solid-liquid system, then:
a. Quantity of solid will reduce
b. Quantity of liquid will reduce
c. Increase in temperature
d. Decrease in temperature
Answer : A

Question. In the reactionA(g) + 2B(g) ⇌ C(g) +QkJ, greater product will be obtained or the forward reaction is favoured by:
a. At high temperature and high pressure
b. At high temperature and low pressure
c. At low temperature and high pressure
d. At low temperature and low pressure
Answer : C

Question. Consider the reaction HCN(aq) H+(aq) CN−(aq) At equilibrium, the addition of (aq) CN−(aq) would:
a. Reduce HCN(aq) concentration
b. Decrease the H+(aq) ion concentration
c. Increase the equilibrium constant
d. Decrease the equilibrium constant
Answer : B

Question. In the gaseous equilibrium H2 X2 + heat ⇌ 2HX, the formation of HX will be favoured by:
a. High pressure and low temperature
b. High temperature and low pressure
c. Low temperature and low pressure
d. High temperature and high pressure
Answer : B

Question. In which of the following gaseous equilibrium an increase in pressure will increase the yield of the products?
a. 2HI ⇌ H2 + I2
b. 2SO2 + O2 ⇌ 2SO3
c. H2 + Br2 ⇌ 2HBr
d. H2 O + CO ⇌ H2 + CO2
Answer : B

Question. Which of the following factors will favour the reverse reaction in a chemical equilibrium?
a. Increase in the concentration of one of the reactants
b. Removal of at least one of the product at regular time intervals
c. Increase in the concentration of one or more products 
d. None of these
Answer : C

Question. In the formation of SO3 by contact process, the conditions used are:
a. Catalyst, optimum temperature and higher conce ntration of reactants
b. Catalyst, optimum temperature and lower concentration of reactants
c. Catalyst, high temperature and higher concentration of reactants
d. Catalyst, low temperature and lower concentration of reactants
Answer : A

Question. Given reaction is 2X(gas) + Y(gas) ⇌ 2Z(gas) + 80 kcal which combination of pressure and temperature gives the highest yield of Z at equilibrium?
a. 1000 atm and 500 °C
b. 500 atm and 500 °C
c. 1000 atm and 100 °C
d. 500 atm and 100 °C
Answer : C

Question. The formation of NO2 in the reaction 2NO + O2 ⇌ 2NO2 + heat is favoured by:
a. Low pressure
b. High pressure
c. Low temperature
d. Reduction in the mass of
Answer : B, C

Question. The exothermic formation of ClF3 is represented by the equation Cl2(g) + 3F2(g) ⇌ 2ClF3(g) ; ΔH = −329 kJ Which of the following will increase the quantity of ClF3
in an equilibrium mixture of Cl2 ,F2 and ClF3 ?
a. Increasing the temperature
b. Removing Cl2
c. Increasing the volume of the container
d. Adding F2
Answer : D

Question. Raising the temperature of an equilibrium system:
a. Favours the exothermic reaction only
b. Favours the endothermic reaction only
c. Favours both the exothermic and endothermic reactions
d. Favours neither the exothermic nor endothermic reactions
Answer : B

Question. The endothermic reaction (M+ N ⇆ P) is allowed to attain equilibrium at 25°. Formation of P can be increased by:
a. Raising temperature
b. Lowering temperature
c. Keeping temperature constant
d. Decreasing the concentration of M and N
Answer : A

Question. According to Le-chatelier's principle, an increase in the temperature of the following reaction will: N2 + O2 ⇌ 2NO − 43, 200kcal
a. Increase the yield of NO
b. Decrease the yield of NO
c. Not effect the yield of NO
d. Not help the reaction to proceed in forward direction
Answer : A

Question. In the manufacture of NH3 by Haber's process, the condition which would give maximum yield is: N2 + 3H2 ⇌ 2NH3 +Qkcal
a. High temperature, high pressure and high concentrations of the reactants
b. High temperature, low pressure and low concentrations of the reactants
c. Low temperature and high pressure
d. Low temperature, low pressure and low concentration of H2
Answer : C

Question. Suppose the reaction PCl5(s) ⇌ PCl3(s) + Cl2(g) is in a closed vessel at equilibrium stage. What is the effect on equilibrium concentration of Cl2(g) by adding PCl5 at constant temperature?
a. Decreases
b. Increases
c. Unaffected
d. Cannot be described without the value of Kp
Answer : B

Question. In which of the following equilibrium reactions, the equilibrium would shift to the right, if total pressure is increased?
a. N2 + 3H2 ⇌ 2NH3
b. H2 + I2 ⇌ 2HI
c. H2 + Cl2 ⇌ 2HCl
d. N2 O4 ⇌ 2NO
Answer : A

Question. Formation of SO3 takes place according to the reaction 2SO2 + O2 ⇌ 2SO ;ΔH = −45.2 kcal
Which of the following factors favours the formation of SO3 ?
a. Increase in temperature
b. Increase in pressure
c. Removal of oxygen
d. Increase in volume
Answer : B

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NEET Full Course Chemical Equilibrium Chemical Equilibrium Notes

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