Consider the equilibrium reaction: 3ClO-(aq) ClO3-(aq) + 2Cl-(aq) Kc = 3.2 x 103

Question

Consider the equilibrium reaction: 3ClO-(aq) ClO3-(aq) + 2Cl-(aq) Kc = 3.2 x 103 [Cl-] = 0.5 mol/L; [ClO-3] = 0.32 mol/L; [ClO-] = 0.24 mol/L Show the calculations to determine if this mixture is at equilibrium and, if not, in which direction will the reaction proceed?

Explanation / Answer

FOLLOW THIS he expression for an equilibrium reaction is determined by the coefficients in the balanced equation. Large K > 1 products are "favored" they dominate the mixture K = 1 neither reactants nor products are favored Small K < 1 reactants are "favored" they dominate the mixture The term "favored" means that side of the equation has higher numbers of moles and higher concentrations than the other. A large K is more than '1' and can be huge, 1 x 1034 K = 1 neither reactants nor products are favored A small K is less than 1 and can be tiny, 4 x 10-41

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