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Chapter 15: Problem 2

Explain the difference between physical equilibrium and chemical equilibrium. Give two examples of each.

Short Answer

Expert verified
Physical equilibrium involves a balance of physical processes, like melting or evaporation, with no chemical reactions. Chemical equilibrium, on the other hand, involves a balance of forward and backward chemical reactions. Examples of physical equilibrium include the melting and freezing of ice at a consistent temperature, and the evaporation and condensation of water in a closed container. Examples of chemical equilibrium include the Haber Process for producing ammonia, and the formation and decomposition of hydrogen iodide.

Step by step solution

01

Define Physical Equilibrium

Physical equilibrium refers to the state where the physical processes (like melting, boiling, evaporation etc.) in the system are occurring at the same rate forward and backward. In physical equilibrium, no chemical reaction happens; it is only the physical state changes. Some of the system's properties, such as pressure, volume or temperature, may exhibit steady-state behavior.
02

Examples of Physical Equilibrium

1. When ice melts, it becomes liquid water. In a closed system at a stable temperature, the rate of ice melting will be equal to the rate of water freezing, maintaining equilibrium.\n2. In a closed container partially filled with water, the rate of evaporation of water will be equal to the rate of condensation of the water vapor. This is another example of physical equilibrium.
03

Define Chemical Equilibrium

Chemical equilibrium is the state in which both reactants and products are present in concentrations which have no further tendency to change with time. It typically involves visible chemical changes, such as the decomposition of a chemical compound in a reaction. Even though the concentration of the substances doesn't change over time in chemical equilibrium, the chemical reaction still proceeds but at an equal rate in both directions (forward and reverse).
04

Examples of Chemical Equilibrium

1. The Haber Process for the production of Ammonia is an example. In this process, Nitrogen and Hydrogen react to form Ammonia gas. The reaction proceeds equally in both directions - formation and decomposition of Ammonia, achieving a chemical equilibrium.\n2. The reaction between Hydrogen and Iodide ions to form Hydrogen iodide is another example. Here too, the forward and backward reactions proceed at an equal rate, achieving chemical equilibrium.

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Most popular questions from this chapter

The equilibrium constant \(K_{P}\) for the reaction $$ \mathrm{PCl}_{5}(g) \rightleftharpoons \mathrm{PCl}_{3}(g)+\mathrm{Cl}_{2}(g) $$ is 1.05 at \(250^{\circ} \mathrm{C}\). The reaction starts with a mixture of \(\mathrm{PCl}_{5}, \mathrm{PCl}_{3},\) and \(\mathrm{Cl}_{2}\) at pressures of \(0.177 \mathrm{~atm}\) 0.223 atm, and 0.111 atm, respectively, at \(250^{\circ} \mathrm{C}\). When the mixture comes to equilibrium at that temperature, which pressures will have decreased and which will have increased? Explain why.

Baking soda (sodium bicarbonate) undergoes thermal decomposition as $$ 2 \mathrm{NaHCO}_{3}(s) \rightleftharpoons \mathrm{Na}_{2} \mathrm{CO}_{3}(s)+\mathrm{CO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g) $$ Would we obtain more \(\mathrm{CO}_{2}\) and \(\mathrm{H}_{2} \mathrm{O}\) by adding extra baking soda to the reaction mixture in (a) a closed vessel or (b) an open vessel?

Industrially, sodium metal is obtained by electrolyzing molten sodium chloride. The reaction at the cathode is \(\mathrm{Na}^{+}+e^{-} \longrightarrow \mathrm{Na}\). We might expect that potassium metal would also be prepared by electrolyzing molten potassium chloride. However, potassium metal is soluble in molten potassium chloride and therefore is hard to recover. Furthermore, potassium vaporizes readily at the operating temperature, creating hazardous conditions. Instead, potassium is prepared by the distillation of molten potassium chloride in the presence of sodium vapor at \(892^{\circ} \mathrm{C}\) : $$ \mathrm{Na}(g)+\mathrm{KCl}(l) \rightleftharpoons \mathrm{NaCl}(l)+\mathrm{K}(g) $$ In view of the fact that potassium is a stronger reducing agent than sodium, explain why this approach works. (The boiling points of sodium and potassium are \(892^{\circ} \mathrm{C}\) and \(770^{\circ} \mathrm{C}\), respectively.)

What effect does an increase in pressure have on each of these systems at equilibrium? (a) \(\mathrm{A}(s) \rightleftharpoons 2 \mathrm{~B}(s)\) (b) \(2 \mathrm{~A}(l) \rightleftharpoons \mathrm{B}(l)\) (c) \(\mathrm{A}(s) \rightleftharpoons \mathrm{B}(g)\) (d) \(\mathrm{A}(g) \rightleftharpoons \mathrm{B}(g)\) (e) \(\mathrm{A}(g) \rightleftharpoons 2 \mathrm{~B}(g)\) The temperature is kept constant. In each case, the reacting mixture is in a cylinder fitted with a movable piston.

Outline the steps for calculating the concentrations of reacting species in an equilibrium reaction.
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