Question

question 6 (1 point)
use the following information to answer the next question.
the following reaction is an example of a homogeneous
equilibrium system
3clo₂⁻(aq) ⇌ 2clo₃⁻(aq) + cl⁻(aq)
the equilibrium expression for the reaction is
a) $k_{eq} = \frac{clo_3^-cl^-}{clo_2^-}$
b) $k_{eq} = \frac{clo_3^-^2cl^-}{clo_2^-}$
c) $k_{eq} = \frac{clo_3^-^2cl^-}{clo_2^-^3}$
d) $k_{eq} = \frac{clo_3^-cl^-}{clo_2^-^3}$
e) $k_{eq} = \frac{clo_3^-^2cl^-}{clo_2^-^2}$

Explanation:

Step1: Recall Equilibrium Expression Rule

For a reaction \( aA + bB
ightleftharpoons cC + dD \), the equilibrium expression \( K_{eq}=\frac{[C]^c[D]^d}{[A]^a[B]^b} \), where concentrations of products are in numerator (raised to their stoichiometric coefficients) and reactants in denominator (raised to their stoichiometric coefficients).

Step2: Apply to Given Reaction

The reaction is \( 3\ce{ClO2^-}(aq)
ightleftharpoons 2\ce{ClO3^-}(aq) + \ce{Cl^-}(aq) \). Here, product concentrations: \( [\ce{ClO3^-}] \) with coefficient 2, \( [\ce{Cl^-}] \) with coefficient 1. Reactant concentration: \( [\ce{ClO2^-}] \) with coefficient 3. So \( K_{eq}=\frac{[\ce{ClO3^-}]^2[\ce{Cl^-}]}{[\ce{ClO2^-}]^3} \).

Answer:

c) \( K_{\text{eq}} = \frac{[\ce{ClO_3^-}]^2 [\ce{Cl^-}]}{[\ce{ClO_2^-}]^3} \)