Write the Ke q expressions for the following reactions: 𝐚· 4 H3O^+(a q)+2 Cl^-(a q)+MnO2(s)

step 1 So we have some reactions, and we want to write the equilibrium constant expressions. And it's c

Write the Ke q expressions for the following reactions: ...

Write the $K_{e q}$ expressions for the following reactions: $$\begin{array}{c}{\mathbf{a} \cdot 4 \mathrm{H}_{3} \mathrm{O}^{+}(a q)+2 \mathrm{Cl}^{-}(a q)+\mathrm{MnO}_{2}(s) \rightleftarrows} \\ {\mathrm{Mn}^{2+}(a q)+6 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Cl}_{2}(g)} \\ {\text { b. } \mathrm{As}_{4} \mathrm{O}_{6}(s)+6 \mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows 4 \mathrm{H}_{3} \mathrm{AsO}_{3}(a q)}\end{array}$$

Write the $K_{e q}$ expressions for the following
reactions:
$$\begin{array}{c}{\mathbf{a} \cdot 4 \mathrm{H}_{3} \mathrm{O}^{+}(a q)+2 \mathrm{Cl}^{-}(a q)+\mathrm{MnO}_{2}(s) \rightleftarrows} \\ {\mathrm{Mn}^{2+}(a q)+6 \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Cl}_{2}(g)} \\ {\text { b. } \mathrm{As}_{4} \mathrm{O}_{6}(s)+6 \mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows 4 \mathrm{H}_{3} \mathrm{AsO}_{3}(a q)}\end{array}$$

Key Concepts

Equilibrium Constant Expression

This concept involves writing a mathematical expression that relates the concentrations or partial pressures of products to those of reactants at equilibrium, with each term raised to the power of its stoichiometric coefficient. It is a fundamental tool in chemical thermodynamics that quantifies the relationship between reactants and products when a reaction has reached equilibrium.

Activity of Species

In equilibrium expressions, the effective concentration of a species, known as its activity, is used. Activities account for non-ideal behavior and are generally approximated by concentrations for solutes or partial pressures for gases. They are dimensionless numbers that reflect the driving force of the chemical reaction.

Exclusion of Pure Solids and Liquids

In the formulation of equilibrium constant expressions, pure solids and liquids are omitted because their activities are constant and defined as one. This simplification means that these phases do not appear in the equilibrium constant expression, streamlining calculations by focusing only on the species whose concentrations change.

Reaction Quotient

The reaction quotient, although structured like the equilibrium constant expression, is evaluated at any moment in time rather than at equilibrium. It is used to compare with the equilibrium constant to predict the direction in which a reaction will proceed to achieve equilibrium.

Transcript

Please give Ace some feedback