ChE Reaction Flashcards
It involves a catalyst in the progression of chemical reaction
It is a chemical reaction in which a catalyst increases the rate of reaction. These catalysts increase the reaction rate by reducing the activation energy of the reaction.
Catalytic Reaction
It does not involve a catalyst in the reaction.
These are chemical reactions in which a catalyst does not involve in the reaction process. Therefore, in these reactions, the
reaction rate does not increase by any external influence.
Non-catalytic Reaction
It involves reactants, products, and catalyst in the same phase of matter.
Homogeneous catalytic reactions
It involves reactants and products in the same phase of matter.
Homogeneous non-catalytic reactions
It involves reactants, products, and catalyst in the different phase of matter.
Heteregeneous catalytic reactions
It involves reactants and products in the different phase of matter.
Heteregenenous non-catalytic reactions
Burning of flames
Homogenenous or Heterogeneous
Non-catalytic or Catalytic
Homogeneous non-catalytic reaction
It only exist in vapor.
Liquid reactions and enzyme/microbial reactions
Homogenenous or Heterogeneous
Non-catalytic or Catalytic
Homogenous catalytic reaction
Burning of coal (as feed)
Homogenenous or Heterogeneous
Non-catalytic or Catalytic
Heteregeneous non-catalytic reaction
Burning of coal (as feed)
Homogenenous or Heterogeneous
Non-catalytic or Catalytic
Heteregeneous non-catalytic reaction
Roasting of ores
Homogenenous or Heterogeneous
Non-catalytic or Catalytic
Heteregeneous non-catalytic reaction
Gas absorption with chemical reactions
Homogenenous or Heterogeneous
Non-catalytic or Catalytic
Heteregeneous non-catalytic reaction
Ammonia synthesis
Homogenenous or Heterogeneous
Non-catalytic or Catalytic
Heteregeneous catalytic reaction
Cracking of crude oil
Homogenenous or Heterogeneous
Non-catalytic or Catalytic
Heteregeneous catalytic reaction
HV -» lighter valueable components
Oxidation of ammonia
Homogenenous or Heterogeneous
Non-catalytic or Catalytic
Heteregeneous catalytic reaction
It produces HNO3
Rate Equation
aA + bB –> cC + dD
-rᴀ = 1/V (dNᴀ/dt)
-rᴀ = -dCᴀ/dt
Expressions of Rate
aA + bB –> cC +dD
-rᴀ/a = -rʙ/b = rc/c = rᴅ/d
-1/a (dCᴀ/dt) = -1/b (dCʙ/dt)
= 1/c (dCc/dt) = 1/d (dCᴅ/dt)
Law of Mass Action
ORDER
r α Cᵣₑₐₜₐₙₜⁿ
A + B —> P
-rᴀ = kCᴀᵃCʙᵝ
n = α+β
Type of Reaction:
2A + B —> P
-rᴀ = kCᴀ²Cʙ¹
Elementary Reaction
Type of Reaction:
2A + B —> P
-rᴀ = kCᴀ²
Non-elementary Reaction
Unit Rate of Constant, k
k = Vⁿ⁻¹ / molⁿ⁻¹ · t
V/mol = 1/conc.
Zero Order
3
-rᴀ = kCᴀo = k
- Cᴀo - Cᴀ = kt
- Cᴀo•xᴀ = kt
- Cᴀ = Cᴀo(1-xᴀ) ; Constant Vol. Batch Reactor Only
First Order
2
-rᴀ = kCᴀ
- ln(Cᴀo/Cᴀ) = kt E7-170
- -ln(1-xᴀ) = kt
lnCᴀ = -kt + lnCᴀo
Second Order
2
-rᴀ = kCᴀ²
- 1/Cᴀ - 1/Cᴀo = kt
- xᴀ/(1-xᴀ) = ktCᴀo
Nth Order
2
-rᴀ = kCᴀⁿ
- Cᴀ¹⁻ⁿ - Cᴀo¹⁻ⁿ = (n-1)kt
ln(-rᴀ) = n ln Cᴀ + ln k (E7-168)
General Proportionality Between Half Life and Initial Concentration
t½ α Cᴀo¹⁻ⁿ α 1/ Cᴀoⁿ⁻¹
Use E7-171
Temperature Dependence of k
k = kₒTᵐ e⁻ᴱ/ᴿᵀ (E7-9)
ln(k) = ln(kₒ) - E/R (1/T) (E7-169)
ln[k₂/k₁(T₁/T₂)ᵐ] = E/R (1/T₁ - 1/T₂)
where: kₒ = pre-proportional factor
k₂ T₁
k₁ T₂
Arrhenius Law
ln[k₂/k₁]
= E/R (1/T₁ - 1/T₂)
m=0
no T1 and T2
Collision Theory
ln[k₂/k₁ · √(T₁/T₂)]
= E/R (1/T₁ - 1/T₂)
m= 1/2
square root T2 and T2
Transition State Theory
ln[(k₂/k₁)(T₁/T₂)]
= E/R (1/T₁ - 1/T₂)
m=1
multiply T1 and T2
Parallel Reactions
. k₁
A —> R -rᴀ₁ = k₁Cᴀ = rʀ
k₂
A —> S -rᴀ₂ = k₂Cᴀ = rꜱ
-rᴀ = k₁Cᴀ + k₂Cᴀ
- ln(Cᴀo/Cᴀ) = (k₁ + k₂)t
- k₁/k₂ = Cʀ/Cs = nʀ/ns
Cᴀo - Cᴀ is equal to
Cᴀoxᴀ
