Q 8/9

in order for a reaction to occur, particles must….

collide at the correct orientation and with a minimum energy to break bonds

minimum energy to break bonds is called…..

activation energy

rate law for 2A+B—>C+D

rate=k[A]2[B]

rate constant units for 1st order ____ and 2nd order ____

s-1, M-1s-1

1st order graph is linear for….

ln[A] vs time

2nd order graph is linear for….

1/[A] vs time

absolute value of the slope of a rate graph is…..

k

ways to speed up a reaction….

add a catalyst, increase reactant concentration, increase surface area, increase pressure of gases, increase temperature

adding a catalyst….

lowers the activation energy

increasing reactant concentration…..

more collisions

increasing surface area…..

more collisions

increase pressure of gases….

increases the concentration of the gas, so there are more collisions

increase temperature….

more collisions and more of them have the minimum activation energy

half life for a 1st order process

0.693/k

a 1st order reaction has a constant ____ regardless of the initial concentration

half life

radioactive decay is a _____ process

1st order

the taller the activation energy…..

the slower the reaction

the slow step is also called the….

rate determining step

the slow step will dictate the…..

speed of the reaction

the slow step will determine the…..

rate law

_____ are produced in one step and used up in a later step

intermediates

_____ are used up in one step and produced in a later step

catalysts

Keq=[products]^x/[reactants]^y. x and y represent…..

the coefficients in the balanced chemical equation

only ____ and ____ appear in an equilibrium expression

aq and g

use ____ for molarity and ____ for atm

[ ], (Pgas)

a large Keq means that there are more _____ at equilibrium

products

a small Keq means there are more _____ at equilibrium

reactants

reversing a reaction

1/Keq

doubling a reaction

(Keq)^2

adding reactions

multiply the Ks together

LeChateliers Principle is all about determining…..

Q

if Q > Keq, the reaction shifts ____, towards the ____

to the left, reactants

if Q < Keq, then the reaction shifts ____ towards the ____

to the right, products

____ and _____ do not shift an equilibrium

catalysts and inert gases

changing the volume in a container changes the…..

pressure

changes in pressure can shift an equilibrium only if…..

the number of gas particles are different in each side

an increase in the pressure favors a shift in the equilibrium towards…..

the side with less miles of gas

as volume increases…..

pressure decreases