The equilibrium constant Kc for this reaction is 0.16 at 25^∘ C, and the standard reaction entha

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The equilibrium constant Kc for this reaction is 0.16 at...

The equilibrium constant $K_{\mathrm{c}}$ for this reaction is 0.16 at $25^{\circ} \mathrm{C},$ and the standard reaction enthalpy is $16.1 \mathrm{~kJ}$. $$ 2 \mathrm{NOBr}(\mathrm{g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})+\mathrm{Br}_{2}(\ell) $$ Predict the effect of each of these changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of these changes is made for a constant-volume system. (a) Adding more $\mathrm{Br}_{2}$ (b) Removing some $\mathrm{NOBr}$ c). Lowering the temnerature

The equilibrium constant $K_{\mathrm{c}}$ for this reaction is 0.16 at $25^{\circ} \mathrm{C},$ and the standard reaction enthalpy is $16.1 \mathrm{~kJ}$.
$$
2 \mathrm{NOBr}(\mathrm{g}) \rightleftharpoons 2 \mathrm{NO}(\mathrm{g})+\mathrm{Br}_{2}(\ell)
$$
Predict the effect of each of these changes on the position of the equilibrium; that is, state which way the equilibrium will shift (left, right, or no change) when each of these changes is made for a constant-volume system.
(a) Adding more $\mathrm{Br}_{2}$
(b) Removing some $\mathrm{NOBr}$
c). Lowering the temnerature

Key Concepts

Le Chatelier's Principle

This fundamental concept in chemical equilibrium states that if a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium will shift to counteract the change. It is the guiding principle for predicting the direction in which a reaction will proceed when the concentration, pressure, or temperature is altered.

Concentration Effects on Equilibrium

When the concentration of either reactants or products is altered, the equilibrium responds by favoring the reaction that tends to reduce that change in concentration. For example, adding more product will shift the equilibrium toward the reactants, whereas removing a reactant will shift the equilibrium toward the side that produces more of that reactant.

Temperature Effects on Equilibrium

Temperature changes affect the equilibrium position depending on whether the reaction is endothermic or exothermic. In an endothermic process, increasing the temperature favors the forward reaction by supplying additional energy, while lowering the temperature favors the reverse reaction. Conversely, for an exothermic reaction, lowering the temperature shifts the equilibrium toward the forward reaction.

Phase Considerations in Equilibrium

Different phases (gas, liquid, solid) are treated distinctly when considering equilibrium. In equilibrium expressions, the concentrations or pressures of pure solids and pure liquids are typically omitted because they are constant. However, changes in the amount of a species in a particular phase can indirectly affect the equilibrium if they alter the system's conditions.

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