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COMPILATION OF FINAL EXAMINATION QUESTIONCHE594 CHEMICAL REACTION ENGINEERING

CHAPTER 2

EXAMINATION: DEC 2014

QUESTION 2

(PO1, CO1, CO2, C2, C3, C4)

Gas phase decomposition of nitrogen dioxide producing nitrogen oxide and oxygen wascarried out in a constant volume batch reactor as depicted in Reaction 2 as follows:

22  22   ONONO    

Reaction 2.

a) Setup a stoichiometric table for Reaction 2 above. (6 marks)

b) The decomposition a reaction of Reaction 2 was run at 5.3 atm and at 350 K. Assumingthe reaction was at isobaric and isothermal condition, determine the reaction order andrate constant, k  with unit s-1 for Reaction 2 based on data concentration of nitrogen oxideindicated in Table 2.

Table 2. Measurement of Nitrogen Oxide concentration at different level of conversion

Conversion(s) Concentration, CNO

(mol/L)Time (s)

82.6%75.4%65%

50.4%29.6%

0

0.1530.1390.1200.0930.055

0

50403020100

(12 marks)

c) Express the complete rate law for this reaction, taking the answer in (a) and (b) into

consideration. (2 marks) 

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EXAMINATION: JUNE 2014

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EXAMINATION: DECEMBER 2013

TEST 1: OCTOBER 2014

QUESTION 1

 An elementary reaction of liquid solution was carried out in sealed beaker and placed into aconstant temperature bath. The beaker is considered as batch reactor. After various reactiontimes, the beaker was removed and quickly cooled to room temperature to stop the reaction.The chemical reaction equation can be described as follows:

 A → Product 

From the amount of product collected, the conversion was recorded in table below:

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Table1: Experiment 1

Time (min) Conversion (%)

1 0.36

2 0.59

3 0.73

4 0.83

5 0.89

6 0.93

7 0.95

8 0.97

9 0.98

10 0.99

In addition, the temperature dependence of rate constant also has been measured inseparate experiment. The experimental data are summarized as below:

Table 2: Experiment 2

T (K) k (s-1)

300 0.2

500 0.4

700 0.6

900 0.8

1200 0.95

a) If these data consistent with first order reaction rate, determine the rate constant, k  forexperiment 1

(11 marks)

b) Using an appropriate approach, determine the activation energy (E ) and pre-exponentialfactor ( A or k 0 ) for reaction in experiment 2. R  is given as 8.314 J/mol∙K.

(11 marks)

c) From data collected in both experiment above, calculate the temperature of reaction inexperiment 1.

(3 marks)