Reaction kinetics
- First order
- ln(CA/CA0) = −kt
- Half-life (first order)
- t½ = ln 2/k
- Second order
- 1/CA = 1/CA0 + kt
- Arrhenius
- k = A·e−Ea/(RT)
- Two temperatures
- ln(k2/k1) = (Ea/R)(1/T1 − 1/T2)
Chemical Reaction Engineering: cram pack
Formula sheets, the key method steps for every topic and 8 practice problems, with full solutions at the back.
1Formulas and methods
Reactor sizing (CSTR & PFR)
- Space time
- τ = V/Q
- CSTR, first order
- τ = X/(k·(1 − X)), CA = CA0/(1 + kτ)
- PFR, first order
- τ = ln(1/(1 − X))/k, CA = CA0·e−kτ
- Conversion from volume
- CSTR: X = kτ/(1 + kτ), PFR: X = 1 − e−kτ
- N equal CSTRs in series
- X = 1 − 1/(1 + kτi)N
Chemical equilibrium
- Equilibrium constant
- Kc = [C]c[D]d/([A]a[B]b)
- ICE table
- Initial, Change (×coefficient), Equilibrium
- Quadratic
- x = (−b + √(b² − 4ac))/(2a)
Method
- Write Kc with products over reactants, each raised to the power of its coefficient.
- Set up an ICE table: Initial, Change (in steps of x times the coefficients), Equilibrium.
- Put the equilibrium expressions into Kc and solve for x.
- Check whether x is small enough for an approximation; otherwise solve the quadratic.
Mass balance
- Steady state
- in = out
- Total balance
- ṁ1 + ṁ2 = ṁ3
- Component balance
- ṁ1x1 + ṁ2x2 = ṁ3x3
- Evaporator
- F·xF = P·xP, W = F − P
2Practice problems
1.Reaction kineticsMedium
A first-order reaction in a batch reactor has k = 0.01 min⁻¹. How long does it take to reach 90% conversion? Find t.
k = 0.01 min⁻¹X = 90 %
t = min
2.Reaction kineticsHard
A reaction has a rate constant of 0.02 min⁻¹ at 25 °C and an activation energy of 100 kJ/mol. Find the rate constant k2 at 65 °C.
k1 = 0.02 min⁻¹T1 = 25 °CT2 = 65 °CEa = 100 kJ/molR = 8.314 J/(mol·K)
k2 = min⁻¹
3.Reactor sizing (CSTR & PFR)Medium
A liquid-phase first-order reaction A → B (k = 0.1 min⁻¹) runs in a 200 L plug-flow reactor (PFR). The feed enters at 50 L/min with CA0 = 1.5 mol/L. The density is constant and the reactor is at steady state. Find the outlet concentration CA.
V = 200 LQ = 50 L/mink = 0.1 min⁻¹CA0 = 1.5 mol/L
CA = mol/L
4.Reactor sizing (CSTR & PFR)Hard
A first-order liquid-phase reaction (k = 0.08 min⁻¹) runs in a 2000 L CSTR fed at 40 L/min. The density is constant and the reactor is at steady state. Find the conversion X in percent.
V = 2000 LQ = 40 L/mink = 0.08 min⁻¹
X = %
5.Chemical equilibriumMedium
0.1 mol/L of H₂ and 0.1 mol/L of I₂ are put in a container and react: H₂ + I₂ ⇌ 2HI, with Kc = 49. Find the equilibrium concentration [HI].
[H₂]₀ = [I₂]₀ = 0.1 mol/LKc = 49
[HI] = mol/L
6.Chemical equilibriumHard
PCl₅ decomposes: PCl₅ ⇌ PCl₃ + Cl₂, with Kc = 0.05 at the reaction temperature. A container starts with 0.1 mol/L of PCl₅ only. Find the equilibrium concentration [PCl5].
[PCl₅]₀ = 0.1 mol/LKc = 0.05
[PCl5] = mol/L
7.Mass balanceMedium
How much of stream 2 must be added each hour to stream 1 so that the blended product contains 35% NaOH? Find ṁ2.
ṁ1 = 300 kg/hx1 = 40 %x2 = 15 %x3 = 35 %
ṁ2 = kg/h
8.Mass balanceHard
An evaporator concentrates a salt solution by boiling off pure water. Find the product flow P in kg/h.
F = 700 kg/hxF = 13 %xP = 50 %
P = kg/h
3Solutions
1.Reaction kinetics
Answer: t = 230.3 min
Reaction rates: for a first-order reaction −dC/dt = kC, so C = C₀·e−kt and the half-life ln 2/k does not depend on concentration. For a second-order reaction 1/C = 1/C₀ + kt. The rate constant rises with temperature following Arrhenius: k = A·e−Ea/(RT).
Conversion and concentration
C/C0 = 1 − X = 0.1
Solve for the time
t = −ln(1 − X)/k = −ln(0.1)/0.01 = 230.3 min
Answer
t = 230.3 min
2.Reaction kinetics
Answer: k2 = 2.363 min⁻¹
Reaction rates: for a first-order reaction −dC/dt = kC, so C = C₀·e−kt and the half-life ln 2/k does not depend on concentration. For a second-order reaction 1/C = 1/C₀ + kt. The rate constant rises with temperature following Arrhenius: k = A·e−Ea/(RT).
Absolute temperatures
T1 = 298.1 K, T2 = 338.1 K
Arrhenius ratio
ln(k2/k1) = −(100000/8.314)·(1/338.1 − 1/298.1) = 4.772
k2 = 0.02·e4.772 = 2.363 min⁻¹
Answer
k2 = 2.363 min⁻¹
3.Reactor sizing (CSTR & PFR)
Answer: CA = 1.005 mol/L
Ideal reactors, first-order reaction (−rA = k·CA) at steady state, with space time τ = V/Q. A CSTR is perfectly mixed, so the whole volume reacts at the low outlet concentration: τ = X/(k·(1 − X)) and CA = CA0/(1 + k·τ). In a PFR each slice of fluid reacts like a small batch reactor: τ = ln(1/(1 − X))/k and CA = CA0·e−k·τ. For the same conversion a CSTR always needs more volume than a PFR.
Space time
τ = V/Q = 200/50 = 4 min
Outlet concentration
CA = 1.5·e−0.1·4 = 1.005 mol/L
Answer
CA = 1.005 mol/L
Conversion: X = 32.97%.
4.Reactor sizing (CSTR & PFR)
Answer: X = 80 %
Ideal reactors, first-order reaction (−rA = k·CA) at steady state, with space time τ = V/Q. A CSTR is perfectly mixed, so the whole volume reacts at the low outlet concentration: τ = X/(k·(1 − X)) and CA = CA0/(1 + k·τ). In a PFR each slice of fluid reacts like a small batch reactor: τ = ln(1/(1 − X))/k and CA = CA0·e−k·τ. For the same conversion a CSTR always needs more volume than a PFR.
Space time
τ = V/Q = 2000/40 = 50 min, kτ = 0.08·50 = 4
Conversion
X = kτ/(1 + kτ) = 4/(1 + 4) = 80%
Answer
X = 80%
5.Chemical equilibrium
Answer: [HI] = 0.1556 mol/L
Chemical equilibrium: for aA + bB ⇌ cC + dD, the equilibrium constant is Kc = [C]c[D]d/([A]a[B]b), using concentrations at equilibrium. An ICE table (Initial, Change, Equilibrium) links the starting amounts to the equilibrium amounts through one unknown x, scaled by the coefficients.
Equilibrium expression
49 = (2x)²/(0.1 − x)²
Take the square root
7 = 2x/(0.1 − x) → x = 0.1·7/(2 + 7) = 0.07778 mol/L
Equilibrium concentration
[HI] = 2x = 0.1556 mol/L
Answer
[HI] = 0.1556 mol/L
6.Chemical equilibrium
Answer: [PCl5] = 0.05 mol/L
Chemical equilibrium: for aA + bB ⇌ cC + dD, the equilibrium constant is Kc = [C]c[D]d/([A]a[B]b), using concentrations at equilibrium. An ICE table (Initial, Change, Equilibrium) links the starting amounts to the equilibrium amounts through one unknown x, scaled by the coefficients.
Equilibrium expression
0.05 = x²/(0.1 − x) → x² + 0.05·x − 0.005 = 0
Solve the quadratic
x = (−0.05 + √(0.05² + 4·0.005))/2 = 0.05 mol/L
Equilibrium concentration
[PCl₅] = 0.1 − 0.05 = 0.05 mol/L
Answer
[PCl5] = 0.05 mol/L
7.Mass balance
Answer: ṁ2 = 75 kg/h
Steady-state mass balance: in = out for the total and for each component. Blending problems combine both.
Balances
Total: ṁ3 = ṁ1 + ṁ2
NaOH: ṁ1x1 + ṁ2x2 = (ṁ1 + ṁ2)x3
Solve for ṁ2
ṁ2 = ṁ1(x1 − x3)/(x3 − x2) = 300·(40 − 35)/(35 − 15) = 75 kg/h
Answer
ṁ2 = 75 kg/h
8.Mass balance
Answer: P = 182 kg/h
Tie component: a component that passes through unchanged in one stream (here the solute) links the flows directly. Then the total balance gives the rest.
Solute balance
F·xF = P·xP → P = 700·13/50 = 182 kg/h
Answer
P = 182 kg/h
ExamProblems · examproblems.com/courses/chemical-reaction-engineering