This set of Chemical Reaction Engineering Multiple Choice Questions & Answers (MCQs) focuses on “Rate Laws and Stoichiometry Definitions”.
1. Hydrogenation of oil is an example of ___________ reactor
a) Homogeneous
b) Heterogeneous
c) Autocatalytic
d) Insufficient data
View Answer
Explanation: The reactants are of different phases i.e. Hydrogen (Gas phase) and oil (Liquid phase). Ni catalyst (Solid) is also used.
2. Arrhenius first suggested the temperature dependence of the rate constant.
a) True
b) False
View Answer
Explanation:
k = \(koe^{\frac{-E}{RT}}\)
This is known as Arrhenius equation and it gives the relation between temperature and rate constant.
3. The slope of the line in the graph gives the ___________
a) Activation energy
b) Rate constant
c) Frequency factor
d) Insufficient data
View Answer
Explanation: The Arrhenius equation k=\(koe^{\frac{-E}{RT}}\) can be modified as
ln(k)=ln(ko) – \((\frac{E}{R})\frac{1}{T} \)
The slope of the line gives E/R from which Activation energy can be determined.
4. Arrhenius equation to determine the activation energy.
a) ln\((\frac{k1}{k2}) = \frac{E}{R} (\frac{1}{T2}-\frac{1}{T1}) \)
b) ln\((\frac{k1}{k2}) = \frac{E}{R} (\frac{1}{T2}+\frac{1}{T1}) \)
c) ln\((\frac{k1}{k2}) = -\frac{E}{R} (\frac{1}{T2}-\frac{1}{T1}) \)
d) ln\((\frac{k1}{k2}) = \frac{E}{R} (\frac{T1}{T2}) \)
View Answer
Explanation: When we have two values of k and T
k1 = ko\(e^{-\frac{E}{RT1}}\) and k2 = ko\(e^{-\frac{E}{RT2}} \)
Modifying it gives
ln(k1) = ln(ko) – \((\frac{E}{R})\frac{1}{T1}\) and ln(k2) = ln(ko) – \((\frac{E}{R})\frac{1}{T2} \)
On further simplification we get ln\((\frac{k1}{k2}) = \frac{E}{R} (\frac{1}{T2}-\frac{1}{T1}). \)
5. Temperature dependence of rate constant according to transition state theory is ______
a) k=ko\(e^{-\frac{E}{RT}} \)
b) k=\(e^{-\frac{E}{RT}} \)
c) k=koT\(e^{-\frac{E}{RT}} \)
d) k=ko\(e^{-\frac{1}{RT}} \)
View Answer
Explanation: According to transition state theory the relationship between temperature and rate constant is given by = koT\(e^{-\frac{E}{RT}}. \)
6. Value of m to obtain the collision theory relation for temperature dependency of rate constant is ________
a) 1
b) 0
c) -1
d) 0.5
View Answer
Explanation: The general equation for temperature dependency is k=koTm \(e^{-\frac{E}{RT}} \)
If m = 0 → Arrhenius equation
m = 1 → transition state theory
m = 0.5 → Collision theory.
7. Calculate the activation energy for the following data using transition state theory.
| T in deg C | k |
| 0 | 0.002 |
| 80 | 0.08 |
a) 30.07 KJ/mol
b) 50.43 KJ/mol
c) 34.37 KJ/mol
d) 82.31 KJ/mol
View Answer
Explanation: When we have two values of k and T
k1=koT1\(e^{-\frac{E}{RT1}} \) and k2=koT2\(e^{-\frac{E}{RT2}} \)
Modifying it gives
ln(k1)=ln(ko)+ln(T1) – \((\frac{E}{R})\frac{1}{T1}\) and ln(k2)=ln(ko)+ln(T2) – \((\frac{E}{R})\frac{1}{T2} \)
On further simplification we get ln\((\frac{k1}{k2})\)=ln\((\frac{T1}{T2}) – \frac{E}{R}(\frac{1}{T1}-\frac{1}{T2}) \)
ln\((\frac{0.002}{0.08})\)=ln\((\frac{273}{353})-\frac{E}{8.314}(\frac{1}{273} – \frac{1}{353}) \)
E = 34.377 KJ/mol.
8. The reaction rate of a bimolecular reaction at 300K is 10 times the reaction rate at 150K. Calculate the activation energy using collision theory.
a) 4928 J/mol
b) 5164 J/mol
c) 3281 J/mol
d) 1296 J/mol
View Answer
Explanation: T1 = 150K, T2 = 300K and k2 = 10k1
When we have two values of k and T
k1=ko\(\sqrt{T1}e^{-\frac{E}{RT1}}\) and k2=ko\(\sqrt{T2}e^{-\frac{E}{RT2}}\)
Modifying it gives
ln(k1)=ln(ko)+0.5ln(T1) – \((\frac{E}{R})\frac{1}{T1}\) and ln(k2)=ln(ko) – \((\frac{E}{R})\frac{1}{T2} \)
On further simplification we get ln\((\frac{k1}{k2}) = 0.5ln(\frac{T1}{T2}) \frac{E}{R} (\frac{1}{T1}-\frac{1}{T2}) \)
ln\((\frac{k1}{10k1})\)=0.5ln\((\frac{150}{300}) – \frac{E}{8.314}(\frac{1}{300} – \frac{1}{150}) \)
E = 4928 J/mol.
9. For the reaction -rA = \(\frac{1670[A][Po]}{6+CA} \frac{kmol}{ml.hr}\) write the units for constants 6 and 1670.
a) kmol/ml and 1/hr
b) 1/hr and 1/hr
c) kmol and kmol
d) data insufficient
View Answer
Explanation: To get the final units
-rA = \(\frac{1670[\frac{kmol}{ml}][\frac{kmol}{ml}]}{6+\frac{kmol}{ml}} \)
The units of constants have to be 1/hr for 1670 and kmol/ml for 6.
10. Which theory is the basis for Arrhenius equation?
a) Collision theory
b) Kinetic theory of gases
c) Ideal gas law
d) Charles and Boyles law
View Answer
Explanation: Arrhenius equation is based on Kinetic theory of gases.
Sanfoundry Global Education & Learning Series – Chemical Reaction Engineering.
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