Question

when pressure _i_and volume _ii_the reaction in an equilibrium system shifts in the direction that produces _iii_ particles. the statement given above is completed by the information given in the row: row i ii iii a decreases increases more b increases decreases more c decreases increases less d decreases increases the same number of e increases decreases the same number of a b c d e question 8 (1 point) which does not occur from the addition of an inert gas to an equilibrium system? the pressure increases the concentration of products increase the concentration of reactants increase the system remains at equilibrium the inert gas reacts with the components of the system question 9 (1 point) which of these affects the equilibrium constant, $k_{eq}$. concentration pressure volume temperature all of the above

Explanation:

Question 8

Inert gases are non - reactive. Adding an inert gas to an equilibrium system at constant volume increases the total pressure. But since the concentrations (moles per unit volume) of reactants and products remain the same (because the volume is constant and the moles of reactants and products are unchanged), the equilibrium does not shift. So, the concentration of products and reactants does not increase due to the addition of inert gas (as there is no shift in equilibrium), and the inert gas does not react with the components of the system.

The equilibrium constant \(K_{eq}\) is only affected by temperature. According to Le - Chatelier's principle, for an exothermic reaction (\(\Delta H<0\)), increasing the temperature decreases \(K_{eq}\) and for an endothermic reaction (\(\Delta H > 0\)), increasing the temperature increases \(K_{eq}\). Changes in concentration, pressure, and volume only cause the system to shift to re - establish equilibrium (by changing the amounts of reactants and products) but do not change the value of \(K_{eq}\) itself.

Answer:

the inert gas reacts with the components of the system

Question 9