Chapter 6

What are instantaneous reactions? Give two examples.

Define a reversible reaction. Give an example.

Rusting of iron is a _____ reaction.

What is meant by irreversible reaction? Give an example.

How can you make a reversible reaction irreversible? Give an example.

Define rate of reaction? How do we represent it mathematically?

What is meant by activation energy?

During a chemical reaction _____ takes place between the reactant molecules.

What are negative catalysts? Give an example.

State Le Chatelier's principle.

State the law of mass action.

How does a catalyst influence the rate of a reaction?

What is meant by dynamic equilibrium?

Explain the dynamic nature of chemical equilibrium.

How can you recognize the state of equilibrium?

Energy possessed by molecules resulting in effective collisions is called _____.

What is meant by threshold energy?

Units of equilibrium constant of the reaction \(\mathrm{BaO}_{2}(\mathrm{~s}) \rightleftharpoons \mathrm{BaO}(\mathrm{s})+\frac{1}{2} \mathrm{O}_{2}(\mathrm{~g})\) is _____.

Define equilibrium constant.

The units of rate of reaction are _____.

What are instantaneous reactions, slow reactions and moderate reactions? Give examples.

How do you represent rate of a reaction with respect to reactants and products? What are the units?

What are the characteristics of dynamic equilibrium?

State law of mass action. Apply it to the following equilibria. (a) \(2 \mathrm{SO}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})} \rightleftharpoons 2 \mathrm{SO}_{3(\mathrm{~g})}\) (b) \(3 \mathrm{Fe}_{(\mathrm{s})}+4 \mathrm{H}_{2} \mathrm{O}_{(\mathrm{g})} \rightleftharpoons \mathrm{Fe}_{3} \mathrm{O}_{4(\mathrm{~s})}+4 \mathrm{H}_{2(\mathrm{~g})}\)

For the reaction \(\mathrm{H}_{2}+\mathrm{I}_{2} \rightleftharpoons 2 \mathrm{HI}\), express the rate of reaction with respect to all reactants and products.

Apply the law of mass action to the following equilibria (a) \(\mathrm{PCl}_{5} \rightleftharpoons \mathrm{PCl}_{3}+\mathrm{Cl}_{2}\) (b) \(2 \mathrm{NO}+\mathrm{O}_{2} \rightleftharpoons 2 \mathrm{NO}_{2}\)

Explain how it is possible to show the dynamic nature of chemical equilibrium by an experiment.

Explain the effect of concentration on rate of reaction on the basis of collision theory.

What are the characteristics of equilibrium constant?

Explain Le Chatelier's principle. Apply it to the following equilibria (a) \(2 \mathrm{SO}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})} \rightleftharpoons 2 \mathrm{SO}_{3(\mathrm{~g})}+\) heat (b) \(\mathrm{N}_{2} \mathrm{O}_{4(\mathrm{~g})} \rightleftharpoons 2 \mathrm{NO}_{2(\mathrm{~g})}\) - heat

Explain the effect of catalyst on the rate of reaction?

Explain the effect of temperature on rate of reaction on the basis of collision theory.

List out two applications of equilibrium constant.

Give differences between reversible and irreversible reactions.

State and explain the law of mass action. Apply it to the following equilibria. (i) \(\mathrm{H}_{2(\mathrm{~g})}+\mathrm{I}_{2(\mathrm{~g})} \rightleftharpoons 2 \mathrm{HI}\) (ii) \(\mathrm{NH}_{4} \mathrm{HS}_{(\mathrm{S})} \rightleftharpoons \mathrm{NH}_{3_{(\mathrm{g})}}+\mathrm{H}_{2} \mathrm{~S}_{(\mathrm{g})}\) (iii) \(2 \mathrm{SO}_{2_{(\mathrm{g})}}+\mathrm{O}_{2_{(\mathrm{g})}} \rightleftharpoons 2 \mathrm{SO}_{ \left.3_{(\mathrm{g}}\right)}\)

State and explain the postulates of the collision theory of reaction rates.

State Le Chatelier's principle and apply it to the following equilibria. (i) \(2 \mathrm{NH}_{3(\mathrm{~g})} \rightleftharpoons \mathrm{N}_{2(\mathrm{~g})}+3 \mathrm{H}_{2(\mathrm{~g})}-\) heat (ii) \(2 \mathrm{NO}_{(\mathrm{g})} \rightleftharpoons \mathrm{N}_{2(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})}+\) heat

One mole of \(\mathrm{PCl}_{5}\) is subjected to heating in a one litre vessel. The number of moles of \(\mathrm{PCl}_{3}\) formed at equilibrium is 0.6. Calculate the equilibrium constant for the dissociation of \(\mathrm{PCl}_{5}\).

Explain the effect of temperature and concentration on the rate of reaction by an experiment.