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Efrigerator. One is almost full. The other is almost empty. Slowly, the sodas are going flat. This is because the dissolved carbon dioxide is coming out of solution and going into the air space above. Of course, if you keep the bottle closed tightly, the soda doesn t go flat as fast. If the gas can t escape, it soon reaches equilibrium with the solution below. But are all equilibria the same? Does the almost empty bottle retain as much carbonation as the almost full bottle? The soda with the.

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There is only one set of equilibrium concentrations that equals the Kc value: At equilibrium, the rate of the forward reaction is the same as the rate of the reverse reaction: D) At equilibrium; the total concentration of products equals the total concentration of reactants_

3) Kc does depend on temperature. ⇒ If the Kc value is large (Kc >> 1), the equilibrium lies to the right and the reaction mixture contains mostly products. ⇒ If the Kc value is small (Kc <<1), the equilibrium lies to the left and the reaction mixture contains mostly reactants.

All reactant and product concentrations are constant at equilibrium.

Kc depends on the rate constants which in turn depend on the reaction (Ea) and temperature.

A reversible reaction can proceed in both the forward and backward directions. Equilibrium is when the rate of the forward reaction equals the rate of the reverse reaction. All reactant and product concentrations are constant at equilibrium.

Equilibrium can be established for both physical processes and chemical reactions.

Formula for Kc: The formula for Kc is Kc=[C]c[D]d[A]a[B]b K c = [ C ] c [ D ] d [ A ] a [ B ] b , where [C] and [D] are the molar concentrations of the products at equilibrium, and [A] and [B] are the molar concentrations of the reactants at equilibrium.

Because the concentrations are measured at equilibrium, the equilibrium constant remains the same for a given reaction independent of initial concentrations.

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