1
Species that appear in some steps but do not appear in the net equation are
Intermediates
In a single step reaction represented by the equation A + B --> C, the rate law for the forward one-step reaction is:
R=K[A][B]
forward reaction rate equals reverse reaction rate
Equilibrium
If the pressure on the equilibrium system is increased
2CO(g) + O2(g) --> 2CO2(g)
then:
equilibrium will shift to the right to make more CO2
DE is +ve
Endothermic reaction
Sequence of steps in a reaction
Reaction Mechanism
process used to speed up chemical reactions
Catalysis
value of equilibrium constant changes with
Temperature
Changing concentration of a zero-order reactant will lead to:
a. increases the reaction rate
b. decreases the reaction rate
c. might increase or decrease the reaction rate
d. doesn’t affect the reaction rate
d. doesn’t affect the reaction rate
chemical equilibrium expression for the equation
Fe(OH)3(aq) ⇌ Fe3+(aq) + 3OH-(aq)
Keq = [Fe3+] [OH-]3 / Fe(OH)3
Minimum energy required for an effective collision
Activation Energy
the slowest step in a reaction
Rate-determining step
If K is more than 1 which substances are favored, Products or reactants?
Products
Adding a catalyst will:
a. increases the reaction rate
b. decreases the reaction rate
c. might increase or decrease the reaction rate
d. doesn’t affect the reaction rate
a. increases the reaction rate
Two conditions needed for a reaction to reach equilibrium
Closed container and reversible reaction
short-lived transitional structure formed during a collision
Activated-Complex
It provides an alternative pathway with a lower activation energy
Catalyst
Increasing surface area (using powder instead of lumps) will:
a. increases the reaction rate
b. decreases the reaction rate
c. might increase or decrease the reaction rate
d. doesn’t affect the reaction rate
a. increases the reaction rate
Reactions whose reactants and products exist in a single phase
Homogeneous reactions
Energy absorbed in breaking bonds
Energy released in forming bonds
What is Endothermic?
What is Exothermic?
In an energy profile the activated complex is found at the
Peak of the curve
A reaction is zero order in reactant A and first order in reactant B. What happens to the reaction rate when the concentrations of both reactants are doubled?
the reaction rate is doubled (increases by a factor of 2)
In an energy profile, this is the difference between products and reactants
Energy Change DE
If doubling the concentration of a reactant quadruples the rate of the reaction, the concentration of the reactant appears in the rate law with an exponent of ___________
2
Observe the following equation:
C(s) + H2O (g) + Heat ⇌ CO (g) + H2 (g)
If the temperature is increased the equilibrium will shift in which direction?
Shift to the right