Chemical Equilibrium Flashcards
what is an irreversible
reactions in which the reactants convert to products and where the products cannot convert back to the reactants
what is a reversible
a reaction where the conversion of reactants to products and the conversion of products to reactants occur at the same time
has double arrows
dynamic equilibrium
the rate of the forward reaction is equal to the rate of the reverse reaction
closed system
the reactant and the products can’t leave or enter the system
reactants and products are trapped inside
favourable (an advantage) change
change that has a natural tendency to happen under certain conditions
entropy
the degree of disorder
what does spontaneous mean?
the reaction will take place
non-spontaneous
the reaction will not take place
what happens if the quotient equals the equilibrium constant
this means the system is in equilibrium
if the quotient is greater than the equilibrium constant
the system attains equilibrium by moving to the left, favouring the reactants
when the quotient is less than the equilibrium constant
the system attains equilibrium by moving to the right, favouring the products
when the quotient is greater than the equilibrium constant
the system reaches equilibrium by moving toward the reactants and moving towards the left
when the quotient is equal to the equilibrium constant
the system is at equilibrium
le chatelier principle
if a system at equilibrium is subjected to external stress, the equilibrium will shift as to minimize that stress.
external stress, in this case is a change in temperature, a change in pressure, a change in volume, or a change in concentration
when there is a decrease in volume and an increase in pressure which direction will the equilibrium shift?
system moves to the side with less moles
when there is an increase in volume and decrease in pressure which direction will the equilibrium shift
system move to the side with more moles
when the concentration of element goes up
the system shifts in the opposite direction
when concentration of element goes down which direction will the equilibrium shift?
the system moves in that same direction to make up for the concentration lost
when the reactants go down what happens to the products?
the products are used up
when the products go down what other change happens to the equilibrium system?
the reactants are used up
whats happens to equilibrium when there is an equal number of gas moles on each side?
there is no change in the position of equilibrium since changes, such as pressure or volume, affect each side equally, therefore it doesn’t cause a concentration to by higher than the other and there is no shift
what happens to equilibrium when there is an addition of an inert gas to a system at a constant volume
does not change the shift of the equilibrium
which side does an increase in temperature favour
will favour the reactant side, because this side will absorb heat and balance out the increase in temperature
what side does a decrease in temperature favour
will favour the product side, an exothermic reaction
describe the equilibrium shift when the equilibrium constant is greater than 1
products are favoured so the reaction shifts to the right
describe the equilibrium shift when the equilibrium constant is less than 1
the reactant is favoured so the system shifts to the left
describe the equilibrium shift when the equilibrium constant is greater than 1 times 10^10
reaction goes into completion when the products don’t go back to the reactants, only a forward reaction
describe the equilibrium shift when the equilibrium constant is less than 1 times 10^-10
the reaction will not take place
the meaning of a small equilibrium constant
when keq is small compared with the intial, the value of the initial minus x is equal to the initial concentration and the x is ignored
equilibrium constant (Keq)
the ratio of the mathematical product of the concentrations of the products of a reaction to the concentrations of the reactants of the reaction. Each concentration is raised to the power of its coefficient in the balanced chemical equation
Keq=[C}^c [D]^d[A]^a [B}^b
partial pressure formula
concentration of the products over concentration of reactants, no square brackets, used when every element in a reaction is a gas
law of chemical equilibrium
in a chemical system at equilibrium, there is a constant ratio between the concentration of products and the reactants
(the concentration of the reactants and products equal some constant)
