Wednesday 27 May 2020

CBSE Class 11 - Chemistry - Chapter: Equilibrium - What are Irreversible and Reversible Reactions? (#eduvictors)(#cbse2020)(#class11Chemistry)

What are Irreversible and Reversible Reactions? 

CBSE Class 11 - Chemistry - Chapter: Equilibrium 

CBSE Class 11 - Chemistry - Chapter: Equilibrium  - What are  Irreversible and Reversible Reactions? (#eduvictors)(#cbse2020)(#class11Chemistry)


Q1: What is equilibrium?

Answer: It is a state in a process when two opposing processes (forward and reverse) occur simultaneously at the same rate. The free
energy change at equilibrium state is zero i.e., ΔG = 0.


Q2: What are reversible reactions? Give examples.

Answer:  Chemical reactions in which the entire amounts of reactants are converted into products are termed irreversible reactions.  
Irreversible reactions form the basis of quantitative chemical analysis such as volumetric analysis.

Examples are:

The reaction between led nitrate and potassium chromate is an irreversible reaction.

Pb(NO₃)₂ (aq)  + K₂CrO₄ (aq)   →    PbCrO₄ (s)   + 2KNO₃ (aq)

The reaction between a strong acid and strong base are irreversible.

HCl + NaOH  →  NaCl  + H₂O



Q3: What are reversible reactions? Give examples.

Answer: The reactions in which only a part of the total amount of reactants is converted into products are called reversible reactions. When molecules begin to react, the rate of the forward reaction is faster than the rate of the reverse reaction. In the chemical equations for the reversible reactions, the reactants and products are separated by the symbols ().

Examples are:

Neutralisation between an acid and a base either of which or both are weak like
CH₃CHOOH + NaOH    ⇌   CH₃COONa + H₂O

Esterification reaction
CH₃CHOOH + C₂H₅OH ⇌  CH₃COOC₂H₅ + H₂O

Evaporation of water in a closed container.
H₂O (l)  ⇌ H₂O (g)

Thermal decomposition of Calcium carbonate
CaCO₃(s) ⇌ CaO(s) + CO₂(g)


Q4: Under what condition, a reversible process becomes irreversible?

Answer: If one of the products (gaseous) is allowed to escape out (i.e., in an open vessel) or the reaction results in the formation of a precipitate.


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