Many metabolites are maintained at steady state concentrations that are far from equilibrium. A comparison K'_eq and Q, the mass-action ratio, can determine whether a metabolic reaction is far from equilibrium. Calculate K'_eq for this reaction at T= 25.0 degree C delta G degree ' = -14.2 kj/mol Calculate the mass-action ratio. Q, from the approximate physiological concentrations for rat heart tissue shown at the right. Select the true statements about the PFK-1 reaction The PFK-1 reaction in heart tissue does not reach equilibrium. In heart tissue, the PFK-1 products are more abundant than reactants. In heart tissue, the PFK-1 reaction will be driven toward product formation. Under standard conditions, the PFK-1 reaction reaches equilibrium when the concentrations_of all products and reactants are equal.

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Answerthis solution will not form a precipitateexplanationsolubility equilbrium:         pbf₂(s)  ⇄ pb²⁺(aq) + 2 f⁻(aq)the solubility product expression is    (we exclude solids from the equilibrium expression).now suppose we have the trial ion product q, which we can define as    then, we can interpret  q as the product of the concentration of the ions that we have and ksp as the product of the ion concentrations that are needed to form a saturated solution.if q > ksp, then that implies that there will be a surplus of ions that exceed the amount that is required to form a saturated solution. a precipitate will then form (the precipitate continually  forms until the surplus ions are removed and q is decreased to ksp's value).if q = ksp, the saturated solution that forms is barely saturated and the precipitate will be minimal.if q < ksp, then the ion concentration will not be enough to form a saturated solution (so no precipitate).using our information, we calculate the trial ion product:     since q = 2.7  × 10⁻⁸ < ksp =  4  ×  10⁻⁸, a precipitate will not form.

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