Modeling and Analysis of Dynamic Systems
|
|
- Gertrude Garrett
- 5 years ago
- Views:
Transcription
1 Modeling and Analysis of Dynamic Systems Dr. Guillaume Ducard Fall 2017 Institute for Dynamic Systems and Control ETH Zurich, Switzerland G. Ducard c 1 / 66
2 Outline 1 Lecture 9 - A: Chemical Systems Example: Continuously Stirred Tank Reactor Simulation Simulation Objectives Simulation Setup Simulation Results G. Ducard c 2 / 66
3 - Simulation Outline Example: Continuously Stirred Tank Reactor 1 Lecture 9 - A: Chemical Systems Example: Continuously Stirred Tank Reactor Simulation Simulation Objectives Simulation Setup Simulation Results G. Ducard c 3 / 66
4 - Simulation Chemical Systems Example: Continuously Stirred Tank Reactor Definition A chemical reaction is a transformation during which reactants are transformed into products. Remark: during a chemical reaction, molecules may appear/disappear to be transformed in other molecules, but in all cases the atoms are conserved, and thus the total mass is preserved. Chemical reactions typically involve two reactants αa+βb γc +δd the integer coefficients {α, β, γ, δ} describe the stoichiometry of the reaction and the double arrow indicates that the reaction can evolve in both directions. G. Ducard c 4 / 66
5 - Simulation Chemical Systems: examples Example: Continuously Stirred Tank Reactor Combination sodium + chlorine sodium chloride 2 Na(s) + Cl 2 (g) 2 NaCl(s) Combustion burning of propane C 3 H 8 (g) + 5 O 2 (g) 3 CO 2 (g) + 4 H 2 O(l) burning of coal (carbon) gives carbon dioxide C(s)+O 2 (g) CO 2 (g) Other types of reactions include: Reduction Oxidation Precipitation reactions etc. G. Ducard c 5 / 66
6 - Simulation Chemical Systems Example: Continuously Stirred Tank Reactor Chemical reactions typically involve two reactants αa+βb γc +δd Chemical reactions are best described on a molecular basis n A, n B, n C, n D with numbers of mol (quantity of element) n A = 1 mol is molecules of that species (Avogadro constant), Molar mass M A is the mass of 1 mol of A. m A = n A M A. Concentration [A] is the number of molecules n A in a given volume V: [A] = n A V G. Ducard c 6 / 66
7 - Simulation Example: Continuously Stirred Tank Reactor Chemical reaction kinetics We define the reaction advancement ξ, as the variation of the reactants quantity: dn A α = dn B β = dn C γ = dn D δ = dξ The reaction rate or speed of the reaction, or formation speed is thus v f = dξ dt v f = dξ dt = 1 dn A α dt = 1 β dn B dt = 1 γ dn C dt = 1 δ dn D dt If you divide by the volume V of the mixed reacting elements, the volumic speed of the reaction is v = 1 V dξ dt = 1 d[a] = 1 d[b] = 1 d[c] = 1 d[d] α dt β dt γ dt γ dt where [x] denotes the concentration of element x in [mol/m 3 ] G. Ducard c 7 / 66
8 - Simulation Example: Continuously Stirred Tank Reactor Chemical reaction kinetics v = 1 V dξ dt = 1 d[a] = 1 d[b] = 1 d[c] = 1 d[d] α dt β dt γ dt δ dt The reaction rate is also defined as v = r[a] p [B] q where p and q are called partial reaction orders. Remark: the coefficients p and q are often not equal to the stoichiometric coefficients, must be determined experimentally. G. Ducard c 8 / 66
9 - Simulation Case of First-order Reaction Example: Continuously Stirred Tank Reactor Consider the reaction A+B C Assume the reaction is first order in both reactants, then the reaction rate is: v = r [A][B] since the reaction rate is also it yields v = d[a] dt d[a] dt = r [A][B] G. Ducard c 9 / 66
10 - Simulation Case of equilibrium or opposed reactions Example: Continuously Stirred Tank Reactor The forward reaction rate αa+βb γc +δd (causing element A to disappear ) is also defined as: v = r [A] α [B] β. and thus the concentration change rate of reactant A is obtained as : 1 d [A] = r [A] α [B] β α dt d [A] = α r [A] α [B] β dt Remark: in this formulation, the probability that the reaction takes place is proportional to the probability that the necessary number of molecules A and B are in contact (concentration). G. Ducard c 10 / 66
11 - Simulation Case of equilibrium or opposed reactions Example: Continuously Stirred Tank Reactor The backward reaction rate (causing element A to appear ) is also defined as: v + = r + [C] γ [D] δ and thus the concentration change rate of reactant A is obtained as : 1 d + [A] = r + [C] γ [D] δ α dt d + [A] = α r + [C] γ [D] δ dt Total rate of formation of the species A (in mol/(s m 3 )) d [A] = α ( r + [C] γ [D] δ r [A] α [B] β) dt G. Ducard c 11 / 66
12 - Simulation Example: Continuously Stirred Tank Reactor The value of the reaction constants r +, and r, depend on: the pressure, and most importantly on the temperature. An Arrhenius model is used r + = k + (ϑ,p,...) e E+ /(Rϑ) R = J/mol K: universal gas constant. The constant k + is referred to as the the pre-exponential factor, E + is the activation energy. The Boltzmann term: exp{ E + /(Rϑ)} indicates the fraction of all collisions that have sufficient energy to start the reaction. G. Ducard c 12 / 66
13 - Simulation Example: Continuously Stirred Tank Reactor r + = k + (ϑ,p,...) e E+ /(Rϑ) r/k Rϑ/E Figure: Arrhenius function. Remark: it reminds of a probability function; see influence of temperature G. Ducard c 13 / 66
14 - Simulation Example: Continuously Stirred Tank Reactor Similarly, the reaction kinetic for the backward reaction r = k (ϑ,p,...)e E /(Rϑ) The four parameters: {k +,k,e +,E } must be determined experimentally. G. Ducard c 14 / 66
15 - Simulation Outline Example: Continuously Stirred Tank Reactor 1 Lecture 9 - A: Chemical Systems Example: Continuously Stirred Tank Reactor Simulation Simulation Objectives Simulation Setup Simulation Results G. Ducard c 15 / 66
16 - Simulation Example: Continuously Stirred Tank Reactor Example: continuously stirred tank reactor (CSTR) Assumptions A+B C 1 The concentration [B] can be assumed to remain constant (amount of B in inflow and in tank always more than necessary for the reaction.) 2 The dissociation A+B C is negligible. 3 The mass m and the density ρ of the fluid in the CSTR are constant. 4 The CSTR is perfectly insulated, the only heat transfer occurs through the controllable heat exchanger. G. Ducard c 16 / 66
17 - Simulation Example: Continuously Stirred Tank Reactor Example: continuously stirred tank reactor (CSTR) [A i (t)],ϑ i (t), m i Q (t) m ρ c ϑ(t) [A(t)],[C(t)] LC [C(t)],ϑ(t), m o Figure: Chemical reactor. G. Ducard c 17 / 66
18 - Simulation Modeling of the Chemical Reactor Example: Continuously Stirred Tank Reactor Step 1: Define Inputs and Outputs Control input = Q(t): rate of heat transferred by the heat exchanger Outputs = concentration of C and temperature ϑ(t) Disturbances = [A i (t)] and ϑ i (t) Notice that m i = m o = m (constant level control = constant mass in rector) and V i = V o = V= m /ρ G. Ducard c 18 / 66
19 - Simulation Modeling of the Chemical Reactor Example: Continuously Stirred Tank Reactor Step 2: Energy reservoirs Using the assumptions mentioned, three reservoirs must be modeled: n A : the amount of species A in the CSTR, level variable [A]; n C : the amount of species C in the CSTR, level variable [C]; U: the internal energy in the CSTR, level variable ϑ. G. Ducard c 19 / 66
20 - Simulation Modeling of the Chemical Reactor Example: Continuously Stirred Tank Reactor Step 3: Conservation laws For species A, the conservation laws yield d dt n A(t) = V [A i (t)] V [A(t)] V k [B] e E/(Rϑ) [A(t)] for species C d dt n C(t) = V [C(t)]+V k [B] e E/(Rϑ) [A(t)] and for the CSTR energy d dt U(ϑ(t),n A(t),n B (t),n C (t)]) = Hi(ϑ i (t)) H(ϑ(t))+ Q(t) Notice that the concentration [B] is (assumed to be) a constant. G. Ducard c 20 / 66
21 - Simulation Modeling of the Chemical Reactor Example: Continuously Stirred Tank Reactor Step 4: Express of internal energy as a function of temperature and composition du(ϑ,n A,n B,n C ) = U ϑ dϑ + U n A dn A + U n B dn B + U n C dn C = ρvc v dϑ +H A dn A +H B dn B +H C dn C where H A, H B, and H C are the enthalpies of formation for the corresponding species. Remark: Neither C v nor H A, H B, and H C are assumed to depend on the temperature ϑ. G. Ducard c 21 / 66
22 - Simulation Example: Continuously Stirred Tank Reactor du = ρvc v dϑ +H A dn A +H B dn B +H C dn C du dϑ dn = ρvc v dt +H A dn A dt +H B dn B dt +H C C dt dϑ 1 dn = ρc v dt +H A 1 dn A V dt +H B 1 B V dt +H C V dt 1 du V dt 1 du V dt = ρc v dϑ dt dϑ 1 dt = ρ C v [ 1 V du dt with internal energy variation du(t) dt +H A d[a] dt H A d[a] dt +H B d[b] dt H B d[b] dt +H C d[c] dt dn C dt H C d[c] dt ] = Hi(ϑ i (t)) H(ϑ(t))+ Q(t) = ρ VC p (ϑ i (t) ϑ(t))+ Q(t) Variations of elements due to chemical reactions: d[a] dt = d[b] dt = d[c] dt = r [A] G. Ducard c 22 / 66
23 - Simulation Example: Continuously Stirred Tank Reactor ( dϑ(t) 1 dt = 1 du ρ C v V dt H A d[a] d[b] dt H B ( 1 1 = ρ C v V ρ Consider: C p C v for liquids V dϑ(t) dt V VC p (ϑ i (t) ϑ(t))+ 1 V + 1 ρ C v (H A +H B H C )r [A](t) = ϑ i (t) ϑ(t)+ τ dϑ(t) dt = ϑ i (t) ϑ(t)+ 1 ρc v Q(t) + V V ρ C v d[c] dt H C dt Q(t) (H A +H B H C ) r [A](t) ρ C v V Q(t) + τ H 0 C vρ ke E/(Rϑ) [A(t)] V where the residence time τ, the overall reaction rate k and the reaction enthalpy H 0 are defined by τ := V/ V, k := k [B], H 0 = H A +H B H C ) ) G. Ducard c 23 / 66
24 - Simulation Example: Continuously Stirred Tank Reactor Step 5: Inserting the last equation in the conservation laws yields: τ d dt [A(t)] = [A i(t)] ( 1+τ k e E/(Rϑ)) [A(t)] τ d dt [C(t)] = [C(t)]+τ k e E/(Rϑ) [A(t)] τ d dt ϑ(t) = ϑ i(t) ϑ(t)+ 1 Q(t) k ρc v +τ H 0 C V vρ e E/(Rϑ) [A(t)] where the residence time τ, the overall reaction rate k and the reaction enthalpy H 0 are defined by τ := V/ V, k := k [B], H 0 = H A +H B H C Remark: H x > 0 if energy is needed to form species x. G. Ducard c 24 / 66
25 - Simulation Example: Continuously Stirred Tank Reactor Static behavior of the CSTR: i.e., Q = 0, rate of heat transferred by the heat exchanger, ϑ i = constant, and [A i ] = constant. Heat removed by the in- and out-flowing mass flow Hflow(ϑ)+ Q chem (ϑ) = 0 where Hflow(ϑ) = m C p (ϑ i ϑ) Vke E/(Rϑ) Q chem (ϑ) = H 0 1+τke E/(Rϑ)[A i] G. Ducard c 25 / 66
26 - Simulation Example: Continuously Stirred Tank Reactor P 3 Hflow Q chem P 2 P 1 Rϑ/E Figure: Steady-state points as a function of temperature. G. Ducard c 26 / 66
27 - Simulation Outline 1 Lecture 9 - A: Chemical Systems Example: Continuously Stirred Tank Reactor Simulation Simulation Objectives Simulation Setup Simulation Results G. Ducard c 27 / 66
28 - Simulation G. Ducard c 28 / 66
29 - Simulation Objectives 1 Illustrate the steps necessary to model a system that includes elements from : mechanical, thermodynamic, fluid dynamic subsystems. 2 Introduce the notion of so-called hybrid systems. G. Ducard c 29 / 66
30 - Simulation Problem Definition Water-propelled Rocket (WPR) V(t) p(t) v(t) (absolute) h(t) m w (t) w(t) (relative) G. Ducard c 30 / 66
31 - Simulation Bottle: mass m l and volume V l Initial conditions At start, filled with water: mass of water m w (0) occupying a volume V w (0) according to: V w (0) = m w(0) ρ w The rest of the volume is filled with air: V a (0) according to: at a certain pressure p(0). V a (0) = V l V w (0), G. Ducard c 31 / 66
32 - Simulation Flight sequence: At t = 0, the nozzle is opened. 1 0 < t < t 1 : Lift force due to water jet (until there is no water anymore), 2 t 1 < t < t 2 :Thrust due to pressurized air (until the air pressure in the rocket reaches atmospheric pressure), 3 t > t 2 : Ballistic mode. G. Ducard c 32 / 66
33 - Simulation Hybrid system: Definition A system that changes its dynamic behavior depending on discrete events is referred to as a hybrid system. In this WPR example the discrete events are switching conditions : when all the water has been flushed away: m w (t) = 0 when there is no more pressurized air: m air (t) = 0 Consequence: the 3 phases (water thrust, air thrust, ballistic flight) will be modeled separately. G. Ducard c 33 / 66
34 - Simulation Assumptions 1 Only the vertical motion is modeled (WPR assumed to only move up or downward). 2 Only 2 forces are considered: - gravity - thrust (from water, air). Aerodynamic forces are neglected. 3 The expansion of the pressurized air inside the WPR is isentropic (no heat transfer, no friction considered) 4 Compared to the mass of water, the air mass is neglected. m a m w 5 The flow of the fluids through the nozzle may be modeled using Bernoulli s law (fluid assumed incompressible without friction). G. Ducard c 34 / 66
35 - Simulation Outline 1 Lecture 9 - A: Chemical Systems Example: Continuously Stirred Tank Reactor Simulation Simulation Objectives Simulation Setup Simulation Results G. Ducard c 35 / 66
36 - Simulation time t time t+dt v(t) m(t) m(t) v(t)+dv(t) dm(t) w(t) v(t) dm(t) Figure: Illustration of the momentum balance equations. The velocity of the water or air, respectively, ejected through the nozzle is w(t). This velocity is relative to the WPR and is positive when flowing in the direction indicated in the Figure. G. Ducard c 36 / 66
37 - Simulation time t time t+dt v(t) dm(t) m(t) m(t) v(t)+dv(t) w(t) v(t) dm(t) Figure: Illustration of the momentum balance equations. Momentum balance: db(t) = B(t+dt) B(t) G. Ducard c 37 / 66
38 - Simulation time t time t+dt v(t) m(t) m(t) v(t)+dv(t) dm(t) w(t) v(t) dm(t) db(t) = B(t+dt) B(t) = [m(t)(v(t)+dv(t)) dm(t)(w(t) v(t))] [m(t) + dm(t)]v(t) = m(t) dv(t) dm(t) w(t) G. Ducard c 38 / 66
39 - Simulation Newton s law db(t) = F e (t) dt = g m(t) dt Combining equations: m(t) dv(t) dm(t) w(t) = g m(t) dt m(t) dv(t) = dm(t) w(t) g m(t) dt m(t) dv(t) = dm(t) w(t) g m(t) dt dt G. Ducard c 39 / 66
40 - Simulation Water mass flow F: nozzle area [m 2 ] dm(t) dt = m = ρ F w(t) Dynamic equations vertical motion of the WPR : m(t) d dt v(t) = g m(t)+ρ F w2 (t) }{{} T w mass change of the WPR: d dt m R(t) = ρ F w(t) Now, can we find a way to express w(t)? G. Ducard c 40 / 66
41 - Simulation p(t) air p(t), velocity= 0 water nozzle area F p a,w(t) Velocity w(t) of the water in the nozzle defined by the pressure difference over the nozzle p(t) p a (Bernoulli, water considered incompressible) 1 2 ρ w2 (t)+p a = p(t) Are neglected, the increase of pressure due to: 1 gravity 2 and acceleration. G. Ducard c 41 / 66
42 - Simulation p(t) air p(t), velocity= 0 water nozzle area F p a,w(t) Velocity w(t) is obtained as: 2 w(t) = p(t) p a ρ G. Ducard c 42 / 66
43 - Simulation Description of the pressure p(t) in side the WPR The pressure p(t) is the pressure of the air inside the WPR (starts at p(0)). Water gets off the WPR the volume available for air increases the pressure p(t) decreases V(t) = V l m w(t) ρ Assuming isentropic conditions (PV κ = cst) ( ) V(0) κ p(t) = p(0) V(t) where κ = c p /c v 1.4 for air. G. Ducard c 43 / 66
44 - Simulation Outline 1 Lecture 9 - A: Chemical Systems Example: Continuously Stirred Tank Reactor Simulation Simulation Objectives Simulation Setup Simulation Results G. Ducard c 44 / 66
45 - Simulation Phase 2: Air-thrust, t 1 < t < t 2 Thrust due to the compressed air flow. 1 In phase 1: only 1 state variable is sufficient to describe quantities for both fluids in the rocket: water mass m w. 2 In phase 2: the mass of the air in the rocket is not constant anymore 2 state variables are used to describe the behavior of the gas flow (air): air mass m air and air internal energy U. Mass of air contained in the rocket? The air mass at the beginning of the air-thrust phase (t = t 1 ) is equal to the mass of air at the beginning of the water-thrust phase at t = 0. m air (t 1 ) = m air (0) G. Ducard c 45 / 66
46 - Simulation Phase 2: Air-thrust, t 1 < t < t 2 Air mass m air (t 1 ) = m air (0) Using the ideal-gas law: P(0) V(0) = n air R u T = m air M air R u T m air (0) = P(0) V(0) M air R u T = cst for t < t 1 with the universal gas constant: R u = 8.31 [J. K 1. mol 1 ], molar mass of air: M air = [kg. mol 1 ]. G. Ducard c 46 / 66
47 - Simulation Phase 2: Air-thrust, t 1 < t < t 2 Thrust due to air mass flow ( m out )? m out = d dt m air = ρ air F w(t) db(t) = B(t+dt) B(t) = m(t) dv(t) dm(t) w(t) db(t) = m(t) g dt G. Ducard c 47 / 66
48 - Simulation Neglecting the mass of air m air compared to mass of the rocket m R m air m R m(t) = m R db(t) = m R g dt = m R dv(t) dm(t) w(t) = m R dv(t) ρ air F w(t)dt w(t) Rocket dynamics equation during the air-thrust phase m R dv(t) dt = m R g +ρ air F w 2 (t) }{{} T air Remark: compare with the dynamic equation during water-thrust phase: m(t) d dt v(t) = m(t) g +ρ w F w 2 (t) G. Ducard c 48 / 66
49 - Simulation Phase 2: Air-thrust, t 1 < t < t 2 Thrust due to Pressurized Air Air thrust T air (t) = ρ air F w 2 (t) = ρ air F w(t) w(t) }{{} m air (t) = m air (t) = m 2 air (t) ρ air F m air (t) ρ air F Remark: this is a trick (to use the air mass flow m air ) in order not to have to compute explicitly the relative airflow speed w(t). G. Ducard c 49 / 66
50 - Simulation Phase 2: Air-thrust, t 1 < t < t 2 Air Mass-flow: m air (t) The air rocket is modeled as a gas receiver (see previous lecture) and the nozzle can be seen as a valve that restricts the exit area of the gas flow. p in (t) p out (t) m in (t),ϑ in (t),p in (t) m out (t),ϑ out (t),p out (t) ϑ in (t) ϑ out (t) G. Ducard c 50 / 66
51 - Simulation If we assume conditions of perfect gases: p m in (t) air (t) = c d F R ϑin (t) Ψ(p in(t),p out (t)) where Ψ(.) is approximated (air and many other gases OK) by: Ψ(p in (t),p out (t)) = In this case: 1 2 [ ] 2p out p in 1 pout p in for 2p out < p in for 2p out p in p in (t) is the pressure of air inside the rocket: P air (t), p out (t) is the pressure of atmosphere: P a, ϑ in (t) is the temperature of air in the rocket: ϑ(t) G. Ducard c 51 / 66
52 - Simulation Approximation (unrealistically large threshold: π tr = 0.9) Ψ(Π) (-) Ψ exact (solid) and approximated (dashed)(κ = 1.4), laminar part (dash-dot) Π (-) G. Ducard c 52 / 66
53 - Simulation Air Pressure P air (t) during the Air-thrust Phase See Gas Receiver example p.45 and p.46 in the script. (lecture 6) d κr { min p(t) = (t)ϑ in (t) m out (t)ϑ(t)} dt V taking m in (t) = 0, we get: with: d { mout } p(t) = κr (t)ϑ(t) dt V l V l : total volume of the rocket (bottle) ϑ(t): temperature of air in the rocket. G. Ducard c 53 / 66
54 - Simulation Air Temperature ϑ(t) during the Air-thrust Phase See Gas Receiver example p.45 and p.46 in the script. (lecture 6) d ϑ(t) R { } ϑ(t) = c p min ϑ in c p mout ϑ ( m in m out )c v ϑ dt p(t) V l c v taking m in = 0, we get: d dt ϑ(t) = = ϑ(t) R { } c p mout (t) ϑ(t)+ m out (t) c v ϑ(t) p(t) V l c v ϑ(t) R { (c p c v ) m } out (t) ϑ(t) p(t) V l c v knowing that for ideal gas R = c p c v in [J (kg K) 1 ], we finally obtain: d dt ϑ(t) = ϑ2 (t) R 2 m out (t) p(t) V l c v G. Ducard c 54 / 66
55 - Simulation Outline Simulation Objectives Simulation Setup Simulation Results 1 Lecture 9 - A: Chemical Systems Example: Continuously Stirred Tank Reactor Simulation Simulation Objectives Simulation Setup Simulation Results G. Ducard c 55 / 66
56 - Simulation Simulation Objectives Simulation Objectives Simulation Setup Simulation Results 1 What is the optimum mass of water that you should put in the rocket to reach maximum height? 2 What is the maximum reachable height? G. Ducard c 56 / 66
57 - Simulation Outline Simulation Objectives Simulation Setup Simulation Results 1 Lecture 9 - A: Chemical Systems Example: Continuously Stirred Tank Reactor Simulation Simulation Objectives Simulation Setup Simulation Results G. Ducard c 57 / 66
58 - Simulation Simulation Objectives Simulation Setup Simulation Results Simulation Setup: Water-thrust Phase Simulation of the rocket from start to "water burn out" total mass of the "rocket" time t isentropic expansion m p pressure air in plenum nozzle behavior p w relative velocity of water leaving nozzle water mass balance w m w T thrust generation thrust m T vertical motion G. Ducard c 58 / 66
59 - Simulation Simulation Setup: Phase Switch Simulation Objectives Simulation Setup Simulation Results m(t) 0 0 h t 0 t 0 time t Figure: Iterative state-event detection. G. Ducard c 59 / 66
60 - Simulation Simulation Objectives Simulation Setup Simulation Results Simulation Setup: Air-thrust Phase G. Ducard c 60 / 66
61 - Simulation Outline Simulation Objectives Simulation Setup Simulation Results 1 Lecture 9 - A: Chemical Systems Example: Continuously Stirred Tank Reactor Simulation Simulation Objectives Simulation Setup Simulation Results G. Ducard c 61 / 66
62 - Simulation Simulation Results Simulation Objectives Simulation Setup Simulation Results 20 Maximum height reached 20 Maximum speed reached Height [m] Height [m] Speed [m/s] Water content in % of WPR volume Water content in % of WPR volume Height trajectory at optimum water content speed trajectory at optimum water content Speed [m/s] Time t Time t G. Ducard c 62 / 66
63 - Simulation Simulation Results Simulation Objectives Simulation Setup Simulation Results Top two plots Maximum height and maximum speed reached during the flight of the WPR for varying initial water levels. The crosses in the top left diagram indicate measured values. Bottom two plots Height and speed trajectories for a WPR with optimal water content at start. The dashed curves are obtained when neglecting the thrust contribution of the air after water burn out. G. Ducard c 63 / 66
64 - Simulation Simulation Objectives Simulation Setup Simulation Results Discussion on the Simulation Results Qualitatively, this result can be explained by the following arguments: 1 If the WPR is filled with very little water: a large amount of energy can be stored in the pressurized air. However, this energy will not produce much thrust because of the lack of sufficient propellant. 2 If too much water is used: very little energy can be stored in the pressurized air. Moreover, the WPR will be very heavy and lifting that mass will require a large amount of the energy stored in the pressurized air. G. Ducard c 64 / 66
65 - Simulation Simulation Materials Simulation Objectives Simulation Setup Simulation Results Model Equations Complete model equations can be downloaded at http : modeling.html G. Ducard c 65 / 66
66 - Simulation Simulation Objectives Simulation Setup Simulation Results Thank you for your attention. G. Ducard c 66 / 66
Modeling and Analysis of Dynamic Systems
Modeling and Analysis of Dynamic Systems by Dr. Guillaume Ducard c Fall 2016 Institute for Dynamic Systems and Control ETH Zurich, Switzerland 1/59 Outline 1 2 Introduction Example: Continuously Stirred
More informationModeling and Analysis of Dynamic Systems
Modeling and Analysis of Dynamic Systems Dr. Guillaume Ducard Fall 2017 Institute for Dynamic Systems and Control ETH Zurich, Switzerland G. Ducard c 1 / 34 Outline 1 Lecture 7: Recall on Thermodynamics
More informationModeling and Analysis of Dynamic Systems
Modeling and Analysis of Dynamic Systems Dr. Guillaume Ducard Fall 2017 Institute for Dynamic Systems and Control ETH Zurich, Switzerland G. Ducard c 1 / 46 Outline 1 Lecture 6: Electromechanical Systems
More informationExercise 7 - Fluiddynamic Systems
Exercise 7 - Fluiddynamic Systems 7.1 Valves The flow of fluids between reservoirs is determined by valves, whose inputs are the pressure up- and downstream, denoted by p in and p out respectively. Here,
More informationChemical reactors. H has thermal contribution, pressure contribution (often negligible) and reaction contribution ( source - like)
Chemical reactors - chemical transformation of reactants into products Classification: a) according to the type of equipment o batch stirred tanks small-scale production, mostly liquids o continuous stirred
More informationAerodynamics. Basic Aerodynamics. Continuity equation (mass conserved) Some thermodynamics. Energy equation (energy conserved)
Flow with no friction (inviscid) Aerodynamics Basic Aerodynamics Continuity equation (mass conserved) Flow with friction (viscous) Momentum equation (F = ma) 1. Euler s equation 2. Bernoulli s equation
More informationAAE COMBUSTION AND THERMOCHEMISTRY
5. COMBUSTIO AD THERMOCHEMISTRY Ch5 1 Overview Definition & mathematical determination of chemical equilibrium, Definition/determination of adiabatic flame temperature, Prediction of composition and temperature
More informationModeling and Analysis of Dynamic Systems
Modeling and Analysis of Dynamic Systems by Dr. Guillaume Ducard Fall 2016 Institute for Dynamic Systems and Control ETH Zurich, Switzerland 1/22 Outline 1 Lecture 5: Hydraulic Systems Pelton Turbine:
More informationChemical Reaction Engineering Lecture 5
Chemical Reaction Engineering g Lecture 5 The Scope The im of the Course: To learn how to describe a system where a (bio)chemical reaction takes place (further called reactor) Reactors Pharmacokinetics
More informationCHAPTER 7 ENTROPY. Copyright Hany A. Al-Ansary and S. I. Abdel-Khalik (2014) 1
CHAPTER 7 ENTROPY S. I. Abdel-Khalik (2014) 1 ENTROPY The Clausius Inequality The Clausius inequality states that for for all cycles, reversible or irreversible, engines or refrigerators: For internally-reversible
More informationRate of Heating and Cooling
Rate of Heating and Cooling 35 T [ o C] Example: Heating and cooling of Water E 30 Cooling S 25 Heating exponential decay 20 0 100 200 300 400 t [sec] Newton s Law of Cooling T S > T E : System S cools
More informationLesson 6 Review of fundamentals: Fluid flow
Lesson 6 Review of fundamentals: Fluid flow The specific objective of this lesson is to conduct a brief review of the fundamentals of fluid flow and present: A general equation for conservation of mass
More informationDevelopment of Dynamic Models. Chapter 2. Illustrative Example: A Blending Process
Development of Dynamic Models Illustrative Example: A Blending Process An unsteady-state mass balance for the blending system: rate of accumulation rate of rate of = of mass in the tank mass in mass out
More informationequation 4.1 INTRODUCTION
4 The momentum equation 4.1 INTRODUCTION It is often important to determine the force produced on a solid body by fluid flowing steadily over or through it. For example, there is the force exerted on a
More informationThe Bernoulli Equation
The Bernoulli Equation The most used and the most abused equation in fluid mechanics. Newton s Second Law: F = ma In general, most real flows are 3-D, unsteady (x, y, z, t; r,θ, z, t; etc) Let consider
More informationChapter 5: The First Law of Thermodynamics: Closed Systems
Chapter 5: The First Law of Thermodynamics: Closed Systems The first law of thermodynamics can be simply stated as follows: during an interaction between a system and its surroundings, the amount of energy
More informationRocket Thermodynamics
Rocket Thermodynamics PROFESSOR CHRIS CHATWIN LECTURE FOR SATELLITE AND SPACE SYSTEMS MSC UNIVERSITY OF SUSSEX SCHOOL OF ENGINEERING & INFORMATICS 25 TH APRIL 2017 Thermodynamics of Chemical Rockets ΣForce
More informationModeling and Analysis of Dynamic Systems
Modeling and Analysis of Dynamic Systems Dr. Guillaume Ducard Fall 2017 Institute for Dynamic Systems and Control ETH Zurich, Switzerland G. Ducard c 1 / 21 Outline 1 Lecture 4: Modeling Tools for Mechanical
More informationModeling and Analysis of Dynamic Systems
Modeling and Analysis of Dynamic Systems by Dr. Guillaume Ducard Fall 2016 Institute for Dynamic Systems and Control ETH Zurich, Switzerland based on script from: Prof. Dr. Lino Guzzella 1/33 Outline 1
More informationChemical Reaction Engineering. Lecture 2
hemical Reaction Engineering Lecture 2 General algorithm of hemical Reaction Engineering Mole balance Rate laws Stoichiometry Energy balance ombine and Solve lassification of reactions Phases involved:
More informationIntroduction to Aerodynamics. Dr. Guven Aerospace Engineer (P.hD)
Introduction to Aerodynamics Dr. Guven Aerospace Engineer (P.hD) Aerodynamic Forces All aerodynamic forces are generated wither through pressure distribution or a shear stress distribution on a body. The
More informationAdvanced Physical Chemistry CHAPTER 18 ELEMENTARY CHEMICAL KINETICS
Experimental Kinetics and Gas Phase Reactions Advanced Physical Chemistry CHAPTER 18 ELEMENTARY CHEMICAL KINETICS Professor Angelo R. Rossi http://homepages.uconn.edu/rossi Department of Chemistry, Room
More informationPROPULSIONE SPAZIALE. Chemical Rocket Propellant Performance Analysis
Chemical Rocket Propellant Performance Analysis Sapienza Activity in ISP-1 Program 15/01/10 Pagina 1 REAL NOZZLES Compared to an ideal nozzle, the real nozzle has energy losses and energy that is unavailable
More informationThermal Energy Final Exam Fall 2002
16.050 Thermal Energy Final Exam Fall 2002 Do all eight problems. All problems count the same. 1. A system undergoes a reversible cycle while exchanging heat with three thermal reservoirs, as shown below.
More information4.1 LAWS OF MECHANICS - Review
4.1 LAWS OF MECHANICS - Review Ch4 9 SYSTEM System: Moving Fluid Definitions: System is defined as an arbitrary quantity of mass of fixed identity. Surrounding is everything external to this system. Boundary
More informationPHEN 612 SPRING 2008 WEEK 1 LAURENT SIMON
PHEN 612 SPRING 2008 WEEK 1 LAURENT SIMON Chapter 1 * 1.1 Rate of reactions r A A+B->C Species A, B, and C We are interested in the rate of disappearance of A The rate of reaction, ra, is the number of
More informationChapter 3: Chemical Reactions and the Earth s Composition
Chapter 3: Chemical Reactions and the Earth s Composition Problems: 3.1-3.3, 3.5, 3.11-3.86, 3.95-3.115, 3.119-3.120, 3.122, 3.125-3.128, 3.132, 3.134, 3.136-3.138-3.141 3.2 The Mole Stoichiometry (STOY-key-OM-e-tree):
More informationC H E M 1 CHEM 101-GENERAL CHEMISTRY CHAPTER 5 GASES INSTR : FİLİZ ALSHANABLEH
C H E M 1 CHEM 101-GENERAL CHEMISTRY CHAPTER 5 GASES 0 1 INSTR : FİLİZ ALSHANABLEH CHAPTER 5 GASES Properties of Gases Pressure History and Application of the Gas Laws Partial Pressure Stoichiometry of
More informationMultistage Rocket Performance Project Two
41 Multistage Rocket Performance Project Two Charles R. O Neill School of Mechanical and Aerospace Engineering Oklahoma State University Stillwater, OK 74078 Project Two in MAE 3293 Compressible Flow December
More informationEnthalpy and Adiabatic Changes
Enthalpy and Adiabatic Changes Chapter 2 of Atkins: The First Law: Concepts Sections 2.5-2.6 of Atkins (7th & 8th editions) Enthalpy Definition of Enthalpy Measurement of Enthalpy Variation of Enthalpy
More informationThe underlying prerequisite to the application of thermodynamic principles to natural systems is that the system under consideration should be at equilibrium. http://eps.mcgill.ca/~courses/c220/ Reversible
More informationModeling and Analysis of Dynamic Systems
Modeling and Analysis of Dynamic Systems by Dr. Guillaume Ducard Fall 2016 Institute for Dynamic Systems and Control ETH Zurich, Switzerland 1/21 Outline 1 Lecture 4: Modeling Tools for Mechanical Systems
More informationIntroduction to Aerospace Engineering
Introduction to Aerospace Engineering Lecture slides Challenge the future 3-0-0 Introduction to Aerospace Engineering Aerodynamics 5 & 6 Prof. H. Bijl ir. N. Timmer Delft University of Technology 5. Compressibility
More informationTheoretical Models of Chemical Processes
Theoretical Models of Chemical Processes Dr. M. A. A. Shoukat Choudhury 1 Rationale for Dynamic Models 1. Improve understanding of the process 2. Train Plant operating personnel 3. Develop control strategy
More informationThermodynamic Processes and Thermochemistry
General Chemistry Thermodynamic Processes and Thermochemistry 박준원교수 ( 포항공과대학교화학과 ) 이번시간에는! Systems, states, and processes The first law of thermodynamics: internal energy, work, and heat Heat capacity,
More informationRocket Propulsion. Combustion chamber Throat Nozzle
Rocket Propulsion In the section about the rocket equation we explored some of the issues surrounding the performance of a whole rocket. What we didn t explore was the heart of the rocket, the motor. In
More informationChapter 6: Thermochemistry
Chem 1045 General Chemistry by Ebbing and Gammon, 8th Edition George W.J. Kenney, Jr Last Update: 24-Oct-2008 Chapter 6: Thermochemistry These Notes are to SUPPLIMENT the Text, They do NOT Replace reading
More informationChapter 5. Chemistry for Changing Times, Chemical Accounting. Lecture Outlines. John Singer, Jackson Community College. Thirteenth Edition
Chemistry for Changing Times, Thirteenth Edition Lecture Outlines Chemical Accounting John Singer, Jackson Community College Chemical Sentences: Equations Chemical equations represent the sentences in
More informationLecture 4. Mole balance: calculation of membrane reactors and unsteady state in tank reactors. Analysis of rate data
Lecture 4 Mole balance: calculation of membrane reactors and unsteady state in tank reactors. nalysis of rate data Mole alance in terms of Concentration and Molar Flow Rates Working in terms of number
More informationRocket propulsion Prof. K. Ramamurthi Department of Mechanical Engineering Indian Institute of Technology, Madras. Lecture 09 Theory of Nozzles
Rocket propulsion Prof. K. Ramamurthi Department of Mechanical Engineering Indian Institute of Technology, Madras Lecture 09 Theory of Nozzles (Refer Slide Time: 00:14) Good morning. We will develop the
More information5/6/ :41 PM. Chapter 6. Using Entropy. Dr. Mohammad Abuhaiba, PE
Chapter 6 Using Entropy 1 2 Chapter Objective Means are introduced for analyzing systems from the 2 nd law perspective as they undergo processes that are not necessarily cycles. Objective: introduce entropy
More informationCompressible Flow - TME085
Compressible Flow - TME085 Lecture 13 Niklas Andersson Chalmers University of Technology Department of Mechanics and Maritime Sciences Division of Fluid Mechanics Gothenburg, Sweden niklas.andersson@chalmers.se
More informationGases. Properties of Gases Kinetic Molecular Theory of Gases Pressure Boyle s and Charles Law The Ideal Gas Law Gas reactions Partial pressures.
Gases Properties of Gases Kinetic Molecular Theory of Gases Pressure Boyle s and Charles Law The Ideal Gas Law Gas reactions Partial pressures Gases Properties of Gases All elements will form a gas at
More informationReaction rate. reaction rate describes change in concentration of reactants and products with time -> r = dc j
Reaction rate ChE 400 - Reactive Process Engineering reaction rate describes change in concentration of reactants and products with time -> r = dc j /dt r is proportional to the reactant concentrations
More informationThe First Law of Thermodynamics. By: Yidnekachew Messele
The First Law of Thermodynamics By: Yidnekachew Messele It is the law that relates the various forms of energies for system of different types. It is simply the expression of the conservation of energy
More informationCOMBUSTION CHEMISTRY COMBUSTION AND FUELS
COMBUSTION CHEMISTRY CHEMICAL REACTION AND THE RATE OF REACTION General chemical reaction αa + βb = γc + δd A and B are substracts and C and are products, α, β, γ and δ are stoichiometric coefficients.
More informationWell Stirred Reactor Stabilization of flames
Well Stirred Reactor Stabilization of flames Well Stirred Reactor (see books on Combustion ) Stabilization of flames in high speed flows (see books on Combustion ) Stabilization of flames Although the
More informationRichard Nakka's Experimental Rocketry Web Site
Página 1 de 7 Richard Nakka's Experimental Rocketry Web Site Solid Rocket Motor Theory -- Nozzle Theory Nozzle Theory The rocket nozzle can surely be described as the epitome of elegant simplicity. The
More informationChapter 7. Entropy. by Asst.Prof. Dr.Woranee Paengjuntuek and Asst. Prof. Dr.Worarattana Pattaraprakorn
Chapter 7 Entropy by Asst.Prof. Dr.Woranee Paengjuntuek and Asst. Prof. Dr.Worarattana Pattaraprakorn Reference: Cengel, Yunus A. and Michael A. Boles, Thermodynamics: An Engineering Approach, 5th ed.,
More informationThermodynamics ENGR360-MEP112 LECTURE 7
Thermodynamics ENGR360-MEP11 LECTURE 7 Thermodynamics ENGR360/MEP11 Objectives: 1. Conservation of mass principle.. Conservation of energy principle applied to control volumes (first law of thermodynamics).
More informationChapter 8 Thermochemistry: Chemical Energy. Chemical Thermodynamics
Chapter 8 Thermochemistry: Chemical Energy Chapter 8 1 Chemical Thermodynamics Chemical Thermodynamics is the study of the energetics of a chemical reaction. Thermodynamics deals with the absorption or
More informationFundamentals of compressible and viscous flow analysis - Part II
Fundamentals of compressible and viscous flow analysis - Part II Lectures 3, 4, 5 Instantaneous and averaged temperature contours in a shock-boundary layer interaction. Taken from (Pasquariello et al.,
More informationFinal S2 (2011) - Practice Test - Ch 11, 12, 13, 14, 15, 16, 18, 19, 22, 23
Final S2 (2011) - Practice Test - Ch 11, 12, 13, 14, 15, 16, 18, 19, 22, 23 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. If 12.0 g of a gas at 2.5 atm
More informationLecture 8. Mole balance: calculations of microreactors, membrane reactors and unsteady state in tank reactors
Lecture 8 Mole balance: calculations of microreactors, membrane reactors and unsteady state in tank reactors Mole alance in terms of Concentration and Molar Flow Rates Working in terms of number of moles
More informationIsentropic Efficiency in Engineering Thermodynamics
June 21, 2010 Isentropic Efficiency in Engineering Thermodynamics Introduction This article is a summary of selected parts of chapters 4, 5 and 6 in the textbook by Moran and Shapiro (2008. The intent
More informationENTHALPY, INTERNAL ENERGY, AND CHEMICAL REACTIONS: AN OUTLINE FOR CHEM 101A
ENTHALPY, INTERNAL ENERGY, AND CHEMICAL REACTIONS: AN OUTLINE FOR CHEM 101A PART 1: KEY TERMS AND SYMBOLS IN THERMOCHEMISTRY System and surroundings When we talk about any kind of change, such as a chemical
More informationChapter 8 Thermochemistry: Chemical Energy
Chapter 8 Thermochemistry: Chemical Energy 國防醫學院生化學科王明芳老師 2011-11-8 & 2011-11-15 Chapter 8/1 Energy and Its Conservation Conservation of Energy Law: Energy cannot be created or destroyed; it can only be
More informationTheoretical Models for Chemical Kinetics
Theoretical Models for Chemical Kinetics Thus far we have calculated rate laws, rate constants, reaction orders, etc. based on observations of macroscopic properties, but what is happening at the molecular
More informationGeneral Chemistry I. Dr. PHAN TẠI HUÂN Faculty of Food Science and Technology Nong Lam University. Module 4: Chemical Thermodynamics
General Chemistry I Dr. PHAN TẠI HUÂN Faculty of Food Science and Technology Nong Lam University Module 4: Chemical Thermodynamics Zeroth Law of Thermodynamics. First Law of Thermodynamics (state quantities:
More informationME Thermodynamics I
Homework - Week 01 HW-01 (25 points) Given: 5 Schematic of the solar cell/solar panel Find: 5 Identify the system and the heat/work interactions associated with it. Show the direction of the interactions.
More informationTHERMODYNAMICS I. TERMS AND DEFINITIONS A. Review of Definitions 1. Thermodynamics = Study of the exchange of heat, energy and work between a system
THERMODYNAMICS I. TERMS AND DEFINITIONS A. Review of Definitions 1. Thermodynamics = Study of the exchange of heat, energy and work between a system and its surroundings. a. System = That part of universe
More informationCH10007/87. Thermodynamics. Dr Toby Jenkins
CH10007/87 Thermodynamics Dr Toby Jenkins 1 Objectives To introduce the basic concepts of thermodynamics To apply them to chemical systems To develop competence in thermodynamics calculations 2 Equilibrium
More informationV (r,t) = i ˆ u( x, y,z,t) + ˆ j v( x, y,z,t) + k ˆ w( x, y, z,t)
IV. DIFFERENTIAL RELATIONS FOR A FLUID PARTICLE This chapter presents the development and application of the basic differential equations of fluid motion. Simplifications in the general equations and common
More informationPART 0 PRELUDE: REVIEW OF "UNIFIED ENGINEERING THERMODYNAMICS"
PART 0 PRELUDE: REVIEW OF "UNIFIED ENGINEERING THERMODYNAMICS" PART 0 - PRELUDE: REVIEW OF UNIFIED ENGINEERING THERMODYNAMICS [IAW pp -, 3-41 (see IAW for detailed SB&VW references); VN Chapter 1] 01 What
More informationReactors. Reaction Classifications
Reactors Reactions are usually the heart of the chemical processes in which relatively cheap raw materials are converted to more economically favorable products. In other cases, reactions play essential
More informationUnderstanding Equations
Chemical Reactions Chemical reaction: a process of chemically changing both the physical and chemical properties of a substance to a new substance with different physical and chemical properties. Video
More information2 Reaction kinetics in gases
2 Reaction kinetics in gases October 8, 2014 In a reaction between two species, for example a fuel and an oxidizer, bonds are broken up and new are established in the collision between the species. In
More informationChapter 4. Chemical Quantities and Aqueous Reactions
Lecture Presentation Chapter 4 Chemical Quantities and Aqueous Reactions Reaction Stoichiometry: How Much Carbon Dioxide? The balanced chemical equations for fossilfuel combustion reactions provide the
More informationChapter Elements That Exist as Gases at 25 C, 1 atm. 5.2 Pressure basic physics. Gas Properties
5.1 Elements That Exist as Gases at 25 C, 1 atm Chapter 5 The Gaseous State YOU READ AND BE RESPONSIBLE FOR THIS SECTION! Gaseous compounds include CH 4, NO, NO 2, H 2 S, NH 3, HCl, etc. Gas Properties
More informationIntroduction to Aerospace Engineering
Introduction to Aerospace Engineering Lecture slides Challenge the future 4-0-0 Introduction to Aerospace Engineering Aerodynamics 3 & 4 Prof. H. Bijl ir. N. Timmer Delft University of Technology Challenge
More informationReview of Fundamentals - Fluid Mechanics
Review of Fundamentals - Fluid Mechanics Introduction Properties of Compressible Fluid Flow Basics of One-Dimensional Gas Dynamics Nozzle Operating Characteristics Characteristics of Shock Wave A gas turbine
More informationwhere R = universal gas constant R = PV/nT R = atm L mol R = atm dm 3 mol 1 K 1 R = J mol 1 K 1 (SI unit)
Ideal Gas Law PV = nrt where R = universal gas constant R = PV/nT R = 0.0821 atm L mol 1 K 1 R = 0.0821 atm dm 3 mol 1 K 1 R = 8.314 J mol 1 K 1 (SI unit) Standard molar volume = 22.4 L mol 1 at 0 C and
More informationStoichiometry of Gases
CHAPTER 13 Stoichiometry of Gases Now that you have worked with relationships among moles, mass, and volumes of gases, you can easily put these to work in stoichiometry calculations. Many reactions have
More informationPractice Examinations Chem 393 Fall 2005 Time 1 hr 15 min for each set.
Practice Examinations Chem 393 Fall 2005 Time 1 hr 15 min for each set. The symbols used here are as discussed in the class. Use scratch paper as needed. Do not give more than one answer for any question.
More informationSection 2: Lecture 1 Integral Form of the Conservation Equations for Compressible Flow
Section 2: Lecture 1 Integral Form of the Conservation Equations for Compressible Flow Anderson: Chapter 2 pp. 41-54 1 Equation of State: Section 1 Review p = R g T " > R g = R u M w - R u = 8314.4126
More informationThis follows from the Clausius inequality as a consequence of the second law of thermodynamics. Therefore. (for reversible process only) (22.
Entropy Clausius inequality can be used to analyze the cyclic process in a quantitative manner. The second law became a law of wider applicability when Clausius introduced the property called entropy.
More informationPlug flow Steady-state flow. Mixed flow
1 IDEAL REACTOR TYPES Batch Plug flow Steady-state flow Mixed flow Ideal Batch Reactor It has neither inflow nor outflow of reactants or products when the reaction is being carried out. Uniform composition
More informationChapter 5. Mass and Energy Analysis of Control Volumes
Chapter 5 Mass and Energy Analysis of Control Volumes Conservation Principles for Control volumes The conservation of mass and the conservation of energy principles for open systems (or control volumes)
More informationCompressible Flow - TME085
Compressible Flow - TME085 Lecture 14 Niklas Andersson Chalmers University of Technology Department of Mechanics and Maritime Sciences Division of Fluid Mechanics Gothenburg, Sweden niklas.andersson@chalmers.se
More informationChapter Two. Basic Thermodynamics, Fluid Mechanics: Definitions of Efficiency. Laith Batarseh
Chapter Two Basic Thermodynamics, Fluid Mechanics: Definitions of Efficiency Laith Batarseh The equation of continuity Most analyses in this book are limited to one-dimensional steady flows where the velocity
More informationAME 436. Energy and Propulsion. Lecture 15 Propulsion 5: Hypersonic propulsion
AME 436 Energy and Propulsion Lecture 5 Propulsion 5: Hypersonic propulsion Outline!!!!!! Why hypersonic propulsion? What's different about it? Conventional ramjet heat addition at M
More informationIntroduction. In general, gases are highly compressible and liquids have a very low compressibility. COMPRESSIBLE FLOW
COMRESSIBLE FLOW COMRESSIBLE FLOW Introduction he compressibility of a fluid is, basically, a measure of the change in density that will be produced in the fluid by a specific change in pressure and temperature.
More informationLecture 8. Mole balance: calculations of microreactors, membrane reactors and unsteady state in tank reactors
Lecture 8 Mole balance: calculations of microreactors, membrane reactors and unsteady state in tank reactors Mole alance in terms of oncentration and Molar low Rates Working in terms of number of moles
More informationSteady-State Molecular Diffusion
Steady-State Molecular Diffusion This part is an application to the general differential equation of mass transfer. The objective is to solve the differential equation of mass transfer under steady state
More informationChemical Reaction Engineering
Chemical Reaction Engineering Dr. Yahia Alhamed Chemical and Materials Engineering Department College of Engineering King Abdulaziz University General Mole Balance Batch Reactor Mole Balance Constantly
More information(Heat capacity c is also called specific heat) this means that the heat capacity number c for water is 1 calorie/gram-k.
Lecture 23: Ideal Gas Law and The First Law of Thermodynamics 1 (REVIEW) Chapter 17: Heat Transfer Origin of the calorie unit A few hundred years ago when people were investigating heat and temperature
More informationOutline of the Course
Outline of the Course 1) Review and Definitions 2) Molecules and their Energies 3) 1 st Law of Thermodynamics 4) 2 nd Law of Thermodynamics 5) Gibbs Free Energy 6) Phase Diagrams and REAL Phenomena 7)
More informationGases: Their Properties & Behavior. Chapter 09 Slide 1
9 Gases: Their Properties & Behavior Chapter 09 Slide 1 Gas Pressure 01 Chapter 09 Slide 2 Gas Pressure 02 Units of pressure: atmosphere (atm) Pa (N/m 2, 101,325 Pa = 1 atm) Torr (760 Torr = 1 atm) bar
More informationCONTENTS Real chemistry e ects Scramjet operating envelope Problems
Contents 1 Propulsion Thermodynamics 1-1 1.1 Introduction.................................... 1-1 1.2 Thermodynamic cycles.............................. 1-8 1.2.1 The Carnot cycle.............................
More informationDisorder and Entropy. Disorder and Entropy
Disorder and Entropy Suppose I have 10 particles that can be in one of two states either the blue state or the red state. How many different ways can we arrange those particles among the states? All particles
More informationCHEMICAL ENGINEERING THERMODYNAMICS. Andrew S. Rosen
CHEMICAL ENGINEERING THERMODYNAMICS Andrew S. Rosen SYMBOL DICTIONARY 1 TABLE OF CONTENTS Symbol Dictionary... 3 1. Measured Thermodynamic Properties and Other Basic Concepts... 5 1.1 Preliminary Concepts
More informationrate of reaction forward conc. reverse time P time Chemical Equilibrium Introduction Dynamic Equilibrium Dynamic Equilibrium + RT ln f p
Chemical Equilibrium Chapter 9 of Atkins: Sections 9.1-9.2 Spontaneous Chemical Reactions The Gibbs Energy Minimum The reaction Gibbs energy Exergonic and endergonic reactions The Description of Equilibrium
More informationThermodynamics is the study of the relationship between heat and other forms of energy that are involved in a chemical reaction.
Ch 18 Thermodynamics and Equilibrium Thermodynamics is the study of the relationship between heat and other forms of energy that are involved in a chemical reaction. Internal Energy (U) Internal energy
More informationEntropy and the Second Law of Thermodynamics
Entropy and the Second Law of Thermodynamics Reading Problems 7-1 7-3 7-88, 7-131, 7-135 7-6 7-10 8-24, 8-44, 8-46, 8-60, 8-73, 8-99, 8-128, 8-132, 8-1 8-10, 8-13 8-135, 8-148, 8-152, 8-166, 8-168, 8-189
More informationBIO134: Chemical Kinetics
BIO134: Chemical Kinetics K Ando School of Chemistry, University of Birmingham http://www.chem.bham.ac.uk/labs/ando/bio134/ Last updated: February 18, 2005 Contents 1 Thermodynamics 3 1.1 The 1st and 2nd
More informationNon-Newtonian fluids is the fluids in which shear stress is not directly proportional to deformation rate, such as toothpaste,
CHAPTER1: Basic Definitions, Zeroth, First, and Second Laws of Thermodynamics 1.1. Definitions What does thermodynamic mean? It is a Greeks word which means a motion of the heat. Water is a liquid substance
More informationUNIT I Basic concepts and Work & Heat Transfer
SIDDHARTH GROUP OF INSTITUTIONS :: PUTTUR Siddharth Nagar, Narayanavanam Road 517583 QUESTION BANK (DESCRIPTIVE) Subject with Code: Engineering Thermodynamics (16ME307) Year & Sem: II-B. Tech & II-Sem
More informationChemical Kinetics. Chapter 13. Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
Chemical Kinetics Chapter 13 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. Chemical Kinetics Thermodynamics does a reaction take place? Kinetics how fast does
More informationAP Chemistry Chapter 16 Assignment. Part I Multiple Choice
Page 1 of 7 AP Chemistry Chapter 16 Assignment Part I Multiple Choice 1984 47. CH 4 (g) + 2 O 2 (g) CO 2 (g) + 2 H 2 O(l) H = 889.1 kj H f H 2 O(l) = 285.8 kj mol 1 H f CO 2 (g) = 393.3 kj mol 1 What is
More informationpiston control surface
Lecture Thermodynamics 4 Enthalpy Consider a quasistatic hydrostatic constant pressure (isobaric) process weights piston, p gas Q control surface fi, p gas U -U 1 = Q +W = Q - Ú pdv = Q - p + p fi (U +
More information