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Compare a system with a large K value to one with a small K value at equilibrium.
Large K: Favors products, higher [products]/[reactants] | Small K: Favors reactants, lower [products]/[reactants]
Differentiate between a reaction that has shifted 'right' versus one that has shifted 'left'.
Shift Right: More products are formed, reactants decrease | Shift Left: More reactants are formed, products decrease
Compare initial conditions to equilibrium conditions in a reversible reaction.
Initial: Reactants present, no products | Equilibrium: Reactants and products present in constant ratio.
Define 'particulate models' in chemistry.
Representations showing matter as individual particles to visualize reactions.
What does a high equilibrium constant (K) indicate?
Indicates a higher concentration of products relative to reactants at equilibrium.
What does a low equilibrium constant (K) indicate?
Indicates a higher concentration of reactants relative to products at equilibrium.
Define chemical equilibrium.
The state where the rate of the forward reaction equals the rate of the reverse reaction, resulting in no net change in reactant and product concentrations.
What does it mean for equilibrium to be dynamic?
The forward and reverse reactions continue to occur, even though the concentrations of reactants and products remain constant.
Define Le Chatelier's principle.
If a change of condition is applied to a system in equilibrium, the system will shift in a direction that relieves the stress.
What is the effect of increasing the temperature on an exothermic reaction at equilibrium?
The equilibrium shifts to the left, favoring reactants.
What is the effect of decreasing the volume (increasing pressure) on a gaseous reaction at equilibrium?
The equilibrium shifts to the side with fewer moles of gas.
What happens to the concentrations of reactants and products when a catalyst is added to a system at equilibrium?
The equilibrium position remains unchanged, but the rate at which equilibrium is reached increases.
What is the effect of adding an inert gas to a system at constant volume?
No change in the equilibrium position.
What happens to the equilibrium position if more reactant is added to a system at equilibrium?
The equilibrium will shift to the right, favoring the formation of products.