Each of the following questions consists of two statements, I in the left-hand column and II in the right-hand column. For each question, determine whether statement I is true or false and whether statement II is true or false. Select the appropriate answer combination from the choices below. Choices with a filled CE oval denote that statement II is a correct explanation of the true statement I.
|If some acetic acid, , is added to the equilibrium mixture represented by the equation above, the concentration of decreases||BECAUSE||the equilibrium constant of a reaction changes as the concentration of the reactants changes.|
Select an Answer
When a system at equilibrium is disturbed, the system will shift in a way that partially offsets the effect of the disturbance (Le Châtelier’s principle). Thus, when is added to the equilibrium mixture, the equilibrium will shift to the right. This increases the concentration of and . Statement I is therefore false. Changes in the concentrations of reactants and products do not affect the value of the equilibrium constant; if the temperature does not change, the value of the equilibrium constant does not change. Statement II is therefore false. The correct answer is false, false.