What value in an equilibrium reaction does K have if the other values for the reaction HC₂H₃O₂ ⇌ H⁺ + C₂H₃O₂^- are [A^-] = 0.10 M and [HC₂H₃O₂] = 0.25 M?

A) 0.01
B) 0.04
C) 0.03
D) 0.25

Question

Zybrea Knight · Accepted Answer

Final Answer : B, Explanation :   The equilibrium constant   K K K   for the reaction is calculated using the concentrations of the products raised to their stoichiometric coefficients divided by the concentrations of the reactants raised to their stoichiometric coefficients. Given that the stoichiometry of the reaction is 1:1:1,   K = [ A S − ] [ C S O 4 − ] [ H 2 C S O 4 ] K = \frac{[AS^-][CSO_4^-]}{[H_2CSO_4]} K = [ H 2 ​ CS O 4 ​ ] [ A S − ] [ CS O 4 − ​ ] ​  . Substituting the given concentrations,   K = ( 0.10 ) ( 0.10 ) 0.25 = 0.04 K = \frac{(0.10)(0.10)}{0.25} = 0.04 K = 0.25 ( 0.10 ) ( 0.10 ) ​ = 0.04  .

What value in an equilibrium reaction does K have if the other values for the reaction HC₂H₃O₂ ⇌ H⁺ + C₂H₃O₂^- are [A^-] = 0.10 M and [HC₂H₃O₂] = 0.25 M?

A) 0.01
B) 0.04
C) 0.03
D) 0.25

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What value in an equilibrium reaction does K have if the other values for the reaction HC2H3O2 ⇌ H+ + C2H3O2- are [A-] = 0.10 M and [HC2H3O2] = 0.25 M?A) 0.01B) 0.04C) 0.03D) 0.25

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What value in an equilibrium reaction does K have if the other values for the reaction HC₂H₃O₂ ⇌ H⁺ + C₂H₃O₂^- are [A^-] = 0.10 M and [HC₂H₃O₂] = 0.25 M?

A) 0.01
B) 0.04
C) 0.03
D) 0.25