Question

i. Why reversible reactions never complete?
ii. What is a static equilibrium, explain with an
example.
iii. Why the amounts of reactants and products do
not change in a reversible reaction.
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Answer 1

Answer:

(i) Reactions in which products are converted back into reactants under similar conditions are known as reversible reactions. These reactions proceed in either direction (forward as well as backward). A reversible reaction never go for completion. It has a tendency to attain a state of equilibrium.

(ii)We are all familiar with dynamic equilibrium, in which the rates of opposing processes are equal. Static equilibrium occurs when there is no exchange between reactants and products. An example of static equilibrium is diamond turning into graphite.

(iii)The concentrations of reactants and products are not necessarily the same between them. A reaction in equilibrium means only that the forward and reverse reactions happen at the same rate and that the individual concentration of reactants and products does not change significantly.

Explanation:

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Answer 2

Answer: Why reversible reaction never complete?

Explanation:

Reversible reactions are those which can recombine to form reactants and they never go to completion because they proceed in both ways i.e. forward and reverse reaction.