Chemical Equilibrium and Rates of Reactions Flashcards

Factors that affect reaction rate
Conditions at equilibrium
Shifts in equilibrium

817904529	True or False: Reaction rate is proportional to the number of effective collisions.	True! Reactions happen due to collisions
817904530	List 4 ways to increase collisions and thus increase reaction rate.	1) Increase temperature (for solids) - this increases energy= increases movement = increases collisions 2) Increase surface area by crushing the reactants into smaller pieces - This increases the # of particles having collisions 3) Add a catalyst - this lowers the activation energy so reactants don't have to gain as much energy to react 4) Increase the concentration of the reactants = increases the # of particles colliding
817904531	In a potential energy diagram for a reaction, the presence of a catalyst will be shown with what?	It will be shown with a dashed line that is below the original activation energy curve.
817904532	What does chemical equilibrium mean?	Equal rates of forward (reactants to products) and reverse (products to reactants) reactions. Does NOT mean equal amounts of the reactant and product just equal rates of transfer!
817904533	In an equilibrium expression, the _____ go on top in brackets.	Products
817904534	A K (equilibrium constant) greater than 1 tells you that the reaction:	proceeds mostly to completeion (to products)
817904535	When a reaction is at equilibrium and the pressure is increased, how will it react?	It will shift to the side with less mess - side with less stuff on it!
817904536	A reaction is at equilibrium. One of the reactants is increased. What happens?	Shift to the product side to use up extra reactant.
817904537	A reaction is at equilibrium. One of the reactants is constantly removed from the reaction. What happens?	Shift to the reactant side to replace the removed reactant.