Equilibrium
What would be the effect on the equilibrium constant (K) for a reaction that is already at equilibrium, due to the temperature change?
If a student designs an experiment to determine the effect of temperature on the equilibrium constant (K) for an exothermic reaction, which outcome would correctly reflect the principles of chemical equilibrium?
If the equilibrium constant for the reaction A2 + B2 ⇌ 2AB is significantly larger than 1, what will be the effect on the concentration of AB if both A2 and B2 are initially present in equal molar amounts?
For student-designed experiments investigating solubility equilibria using various salts, what observation would affirm that concentrations present within saturated solutions are controlled by distinct ksp values specific per salt?
Considering two substances with similar molar masses but different types of predominant intermolecular forces, which one would you expect to have a lower vapor pressure at room temperature?
In an exothermic reaction where heat is on the product's side, what effect would increasing temperature have on the value of K?
Consider aqueous solution reactions involving weak acids strong bases; why might pH not always provide reliable indication about equilibria states?
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What will happen if you double only reactant concentrations for a reaction at equilibrium with an overall positive ΔG⁰ value?
What happens to the position of an exothermic reaction’s equilibrium if pressure is increased by reducing volume, assuming gaseous components are present?
When writing the expression for the equilibrium constant (K), what is not included in the expression?