Write equilibrium constant expressions for these reactions: (a) Ni(s)+4 CO(g) ⇌Ni(CO),(g) (b) HF

step 1 So here we're asked to write equilibrium constants. In our first case, we have the reaction of s

Write equilibrium constant expressions for these reactions:...

Write equilibrium constant expressions for these reactions: (a) $\mathrm{Ni}(\mathrm{s})+4 \mathrm{CO}(\mathrm{g}) \rightleftharpoons \mathrm{Ni}(\mathrm{CO}),(\mathrm{g})$ (b) $\mathrm{HF}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{F}^{-}(\mathrm{aq})$ (c) $\mathrm{Cl}_{2}(\mathrm{~g})+2 \mathrm{Br}^{-}(\mathrm{aq}) \rightleftharpoons \mathrm{Br}_{2}(\ell)+2 \mathrm{CI}^{-}(\mathrm{aq})$

Write equilibrium constant expressions for these reactions:
(a) $\mathrm{Ni}(\mathrm{s})+4 \mathrm{CO}(\mathrm{g}) \rightleftharpoons \mathrm{Ni}(\mathrm{CO}),(\mathrm{g})$
(b) $\mathrm{HF}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\ell) \rightleftharpoons \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{F}^{-}(\mathrm{aq})$
(c) $\mathrm{Cl}_{2}(\mathrm{~g})+2 \mathrm{Br}^{-}(\mathrm{aq}) \rightleftharpoons \mathrm{Br}_{2}(\ell)+2 \mathrm{CI}^{-}(\mathrm{aq})$

Key Concepts

Equilibrium Constant Expression

This concept refers to setting up an expression that relates the concentrations or partial pressures of the products and reactants in a reaction at equilibrium. The expression is derived from the law of mass action, where each concentration or pressure term is raised to the power corresponding to its stoichiometric coefficient in the balanced chemical equation.

Use of Activities Instead of Concentrations or Pressures

In equilibrium expressions, the 'activity' of each species is used rather than its concentration or pressure directly. Activities account for non-ideal behavior in real systems. However, for ideal conditions, the concentrations for solutes and partial pressures for gases can be used directly in the expression.

Exclusion of Pure Solids and Liquids

Pure solids and liquids have constant concentrations and do not affect the position of equilibrium. As a result, they are not included in the equilibrium constant expression. This simplifies the expression to only include species whose concentrations or pressures change during the reaction.

Stoichiometry in Equilibrium Expressions

Each species’ concentration or pressure in the equilibrium expression is raised to a power equal to its coefficient in the balanced chemical equation. This mathematical representation ensures that the expression accurately reflects the reaction's stoichiometric relationships and quantitative behavior at equilibrium.

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