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2024 Tahsili Chemistry: Reaction Rates
Rate Of Reaction
Rate |
- ΔReactants / Δt = Δproducts / Δt |
Reactants are negative |
Collision Theory |
states that particles must collide for a reaction to occur, and must have the right orientation and enough energy |
Activated Complex |
a complex that exists very briefly in the time between the breaking down of reactants and forming of products |
Activation Energy |
the minimum amount of energy needed to form the activated complex |
Exothermic Reaction |
a reaction that releases energy; the products end up having less energy that the reactants |
Endothermic reaction |
a reaction that must absorb enough energy to overcome the energy barrier; the products have more energy at the end |
Factors that affect the rate |
catalysts - the nature of the substances - Concentration - Surface Area - Temperature |
Factors Affecting Equilibrium
Characteristics of equilibrium |
1- fixed ratio, 2- closed system, 3-fixed temp, 4- dynamic equilibrium |
Le Chatelier's Principle |
a change in one variable that describes a system produces a shift in the position of the equilibrium, countering the change |
Effects of Changing Concentration: |
higher reactant concentration = reaction shifts to the right, and vice versa |
Effects of Changing Temperature |
adding heat to and exothermic reaction = more reactants; adding heat to an endothermic reaction = more products |
Effects of Changing Pressure and Volume |
Higher pressure + lower volume = lower number of moles; lower pressure + higher volume = more moles |
if the number of moles are equal on both sides, pressure and volume will have no effect |
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Rate Law
Rate Law |
R = k [A]x [B]y |
Order of the reaction |
x+y |
Rate Constant (k) |
is only affected by temp |
Rate Constant Units |
s-1 , L/mol.s , L2/mol2.s |
A and B are the molar concentrations of reactants; the rate is directly proportional to the concentrations |
the coefficients are the exponents |
Reversible Reactions and Equilibrium
Complete Reaction |
when reactants change to products (→) |
Reversible reaction |
can go both ways (⇆) |
Equilibrium |
when the rate of the forward reaction equals the rate of the backwards one |
Chemical Equilibrium Law |
states that at a certain temperature, the ratio of the reactants and products can remain constant |
for aA + bB = cC +dD |
Chemical Equilibrium Law Formula |
K eq = [C]c[D]d / [A]a[B]b |
if K eq > 1, the products have a higher concentration, if K eq < 1 the reactants have a higher concentration |
Homogeneous Equilibrium |
when the reactants and products are in the same state of matter |
Heterogeneous Equilibrium |
when the reactants and products are in multiple states (the pure solid and liquids are removed from the equation) |
Temperature and The Equilibrium Constant
K eq is directly proportional to temp id the equation is: |
endothermic |
K eq is inversely proportional to temp id the equation is: |
exothermic |
catalyst |
increases the speed at which a reaction reaches equilibrium, but does not change the equilibrium |
K sp = solubility product constant |
Q sp = ionic product |
if K sp > Q sp |
unsaturated, no precipitate |
if K sp = Q sp |
saturated, no precipitate |
if K sp < Q sp |
saturated, precipitate is formed |
Temperature and The Equilibrium Constant
K eq is directly proportional to temp id the equation is: |
endothermic |
K eq is inversely proportional to temp id the equation is: |
exothermic |
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