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MID SEMESTER EXAMINATION
Faculty of Engineering
COURSE CODE : CHEM4005
LEVEL / SEMESTER : 4/1
COURSE TITLE : Reaction Engineering
ACADEMIC YEAR : 2010-2011
DATE : Monday, 06 December 2010
TIME : 09:00
DURATION : 2 Hours
MAXIMUM MARK : 100
COURSE COORDINATOR : Ahmed J. Ali Al-Dallal
STUDENT NAME
STUDENT ID GROUP NO
INSTRUCTIONS TO CANDIDATES
This question paper consists of3 pages only. AnswerALL questions. Write yourID, NAME and GROUP NUMBER clearly on allof your answer books.
Follow all examination rules.
Do not bring books or other related materials into theexamination room.
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Question 1: [40 marks]
The following elementary, reversible, gas-phase reaction takes place in a continuous stirred-tank
reactor (CSTR): A + B CThe following information are known:
- Forward reaction constant (kf) = 0.5 L/mol.s @ 50oC
- Equilibrium constant based on concentration (Kc) = 1.2 L/mol @ 50oC
- Total inlet flowrate is 10 L/min, with initial concentrations of CAO= 1M & CBO= 2M.
- The reactor is maintained under isothermal conditions at 50oC and at 1 atm.
i) Complete the following Stoichiometric Table Q1 for this reaction (fill in shaded areas):
Table Q1: Stoichiometric Table
ii) Write each species concentration in terms of conversion, XA.
iii) Solve for the equilibrium conversion at 500C.
iv)What CSTR volume is required to achieve 80% of the equilibrium conversion?
Question 2: [30 marks]
Pure gaseous (A) at about 3 atm and 30C, with initial concentration C A0=120 mmole/liter, is fed into a
1 liter CSTR at various flow rates. Reactant (A) decomposes in the reactor and the exit concentration ofA (CA) is measured for each flow rate (v0). The flow rate and concentration data are given in Table Q2.
The reaction is: A 3P
Table Q2: Flow rate and concentration data
v0 (Liter/min) 0.06 0.48 1.5 8.1
CA (mmole /Liter) 30 60 80 105
i) Write the mole balance for the CSTR where a 2nd order reaction is taking place.
ii) Show how you will plot the above data to obtain a straight line, and thus determine the
reaction rate constant (k).
Question 3: [30 marks]
The homogeneous gas decomposition of phosphine, 4 PH3(g) P4(g) +6 H2(g), proceeds at 649C
(rate constant = 10 hr-1) in a plug flow reactor operating at 649C and 460 kPa which produce 80%
conversion of a pure feed consisting of 40 mol/hr of pure phosphine.
i) Write the mole balance, rate law and stoichiometry equations for the system.
ii) Combine the three equations in (a).
iii) Estimate the volume of reactor.
Additional Data
R (Gas Constant) = 0.0821 atm.L/mol. K
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= 8.314 Pa.m3/ mol. K
STUDENT NAME
STUDENT ID GROUP NO
Graph Paper for Q2
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