Download GTU (Gujarat Technological University) BE/BTech (Bachelor of Engineering / Bachelor of Technology) 2019 Summer 3rd Sem New 2133606 Material And Energy Balance Calculations Previous Question Paper
Seat No.: ________ Enrolment No.___________
GUJARAT TECHNOLOGICAL UNIVERSITY
BE - SEMESTER ?III (NEW) EXAMINATION ? SUMMER 2019
Subject Code: 2133606 Date: 18/06/2019
Subject Name: Material & Energy Balance Calculations
Time: 02:30 PM TO 05:00 PM Total Marks: 70
Instructions:
1. Attempt all questions.
2. Make suitable assumptions wherever necessary.
3. Figures to the right indicate full marks.
Marks
Q.1 (a) Define the quantities with SI units: i) Density ii) Pressure iii) Volume. 03
(b) The mass velocity of a gas through a duct is 1000 Kg/m
2
.h. Express the velocity
in to lb/ft
2
.s
04
(c) A chemist is interested in preparing 500 ml of 1 normal, 1 molar and 1 molal
solution of H 2SO 4. Assuming the density of H 2SO 4 solution to be 1.075 g/cm
3
,
calculate the quantities of H 2SO 4 to be taken to prepare these solutions.
07
Q.2 (a) Define the following: Molarity , Molality and Normality 03
(b) The average molar mass of a flue gas sample is calculated by two different
engineers. One engineer uses the correct molar mass of 28 for N 2 and determines
the average molar mass to be 30.08, the other engineer, using an incorrect value
of 14, calculates the average molar mass to be 18.74. (i) Calculate the volume %
of nitrogen in the flue gases, (ii) If the remaining components of the flue gases are
CO 2 and O 2, calculate the volume % each of them
04
(c) Cracked gas from a petroleum refinery has the following composition by volume,
methane 45%, Ethane10%, ethylene 25%, Propane 7%, Propylene 8%, n-Butane
5% . Find (a) Average mol. wt. of gas mixture. (b) the composition by weight %
and (c) Specific gravity of the gas mixture at STP.
07
OR
(c) A weight of 1.10 kg of Carbon dioxide occupies a volume of 0.033 m
3
at 300 K.
Using the Van der Waals equation of state, calculate the pressure.
Data: For CO 2 gas, take a = 3.60 [(m
3
)
2
.kPa] / (kmol)
2
and b = 4.3 x 10
-2
m
3
/kmol.
07
Q.3 (a) State : Dalton?s law and Raoult?s law 03
(b) The spent acid from a nitrating process contains 33% H 2SO 4, 36% HNO 3 and 31%
water by weight. This acid is to be strengthened by the addition of concentrated
sulphuric acid containing 95% H 2SO 4 and concentrated nitric acid containing 78%
HNO 3. The strengthened mixed acid is to contain 40% H 2SO 4 and 43% HNO 3.
Calculate the quantities spent and concentrated acids that should be mixed together
to yield 1500 kg of the desired mixed acid
04
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1
Seat No.: ________ Enrolment No.___________
GUJARAT TECHNOLOGICAL UNIVERSITY
BE - SEMESTER ?III (NEW) EXAMINATION ? SUMMER 2019
Subject Code: 2133606 Date: 18/06/2019
Subject Name: Material & Energy Balance Calculations
Time: 02:30 PM TO 05:00 PM Total Marks: 70
Instructions:
1. Attempt all questions.
2. Make suitable assumptions wherever necessary.
3. Figures to the right indicate full marks.
Marks
Q.1 (a) Define the quantities with SI units: i) Density ii) Pressure iii) Volume. 03
(b) The mass velocity of a gas through a duct is 1000 Kg/m
2
.h. Express the velocity
in to lb/ft
2
.s
04
(c) A chemist is interested in preparing 500 ml of 1 normal, 1 molar and 1 molal
solution of H 2SO 4. Assuming the density of H 2SO 4 solution to be 1.075 g/cm
3
,
calculate the quantities of H 2SO 4 to be taken to prepare these solutions.
07
Q.2 (a) Define the following: Molarity , Molality and Normality 03
(b) The average molar mass of a flue gas sample is calculated by two different
engineers. One engineer uses the correct molar mass of 28 for N 2 and determines
the average molar mass to be 30.08, the other engineer, using an incorrect value
of 14, calculates the average molar mass to be 18.74. (i) Calculate the volume %
of nitrogen in the flue gases, (ii) If the remaining components of the flue gases are
CO 2 and O 2, calculate the volume % each of them
04
(c) Cracked gas from a petroleum refinery has the following composition by volume,
methane 45%, Ethane10%, ethylene 25%, Propane 7%, Propylene 8%, n-Butane
5% . Find (a) Average mol. wt. of gas mixture. (b) the composition by weight %
and (c) Specific gravity of the gas mixture at STP.
07
OR
(c) A weight of 1.10 kg of Carbon dioxide occupies a volume of 0.033 m
3
at 300 K.
Using the Van der Waals equation of state, calculate the pressure.
Data: For CO 2 gas, take a = 3.60 [(m
3
)
2
.kPa] / (kmol)
2
and b = 4.3 x 10
-2
m
3
/kmol.
07
Q.3 (a) State : Dalton?s law and Raoult?s law 03
(b) The spent acid from a nitrating process contains 33% H 2SO 4, 36% HNO 3 and 31%
water by weight. This acid is to be strengthened by the addition of concentrated
sulphuric acid containing 95% H 2SO 4 and concentrated nitric acid containing 78%
HNO 3. The strengthened mixed acid is to contain 40% H 2SO 4 and 43% HNO 3.
Calculate the quantities spent and concentrated acids that should be mixed together
to yield 1500 kg of the desired mixed acid
04
2
(c) Soyabean seeds are extracted with the hexane in batch extractors. The flaked seeds
are found to contain 18.6% oil, 69% solids, 12.4% moisture (by weight). At the
end of the extraction process, cake is separated from hexane-oil mixture. The cake
is analyzed to contain 0.8% oil, 87.7% solids and 11.5% moisture (by weight).
Find the percent recovery of oil
07
OR
Q.3 (a) Define the terms: (a) Conversion (b) Yield (c) Selectivity 03
(b) 2000 kg of wet solids containing 70% solids by weight are fed to tray dyer where
it is dried by hot air. The product finally obtained is found to contain 1% moisture
by weight, calculate: (1) kg of water removed from wet solids (2) kg of the product
obtained.
04
(c) A solution contains 50% Benzene, 30% Toluene and 20% Xylene by weight at a
temperature of 100 ?C. The vapors are in contact with solution. Calculate the total
pressure and molar % compositions of liquid and the vapor. The vapor pressures
and the molecular weights are as follows:
Components vapor pressure at 100
o
C Mol. weight
Benzene 1340 mm Hg 78
Toluene 560 mm Hg 92
Xylene 210 mm Hg 106
07
Q.4 (a) Explain: Limiting reactant, Excess reactant and Percent excess reactant 03
(b) Ammonia reacts with sulphuric acid giving ammonium sulphate:
2NH 3 +H 2SO 4 ?( NH 4) 2SO 4
a) 20 m
3
of ammonia at 1.2 bar and 300 k reacts with 40 kg of
sulphuric acid. Which one is the excess reactant and what is the
percent excess?
b) How much ammonium sulphate is obtained
04
(c) 1 kg nitrogen is mixed with 3.5 m
3
of hydrogen at 300 K and 101.3 kPa and sent
to the ammonia converter. The product leaving the converter analysed 13.7 %
ammonia, 70.32 % hydrogen and 15.98 % nitrogen.
(a) Identity the limiting reactant.
(b) What is the present excess of excess reactant?
(c) What is the present conversion of the limiting reactant?
07
OR
Q.4 (a) State the basic principle of material balance 03
(b) Calculate the following for the reaction:
C 2H 4 + 2Cl 2 ? C 2HCl 3 + H 2 + HCl
(1) The stoichiometry ratio of Cl 2 to C 2H 4
(2) If 4 kmol Cl 2 is used per kmol of C 2H 4, find the % excess Cl 2
04
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1
Seat No.: ________ Enrolment No.___________
GUJARAT TECHNOLOGICAL UNIVERSITY
BE - SEMESTER ?III (NEW) EXAMINATION ? SUMMER 2019
Subject Code: 2133606 Date: 18/06/2019
Subject Name: Material & Energy Balance Calculations
Time: 02:30 PM TO 05:00 PM Total Marks: 70
Instructions:
1. Attempt all questions.
2. Make suitable assumptions wherever necessary.
3. Figures to the right indicate full marks.
Marks
Q.1 (a) Define the quantities with SI units: i) Density ii) Pressure iii) Volume. 03
(b) The mass velocity of a gas through a duct is 1000 Kg/m
2
.h. Express the velocity
in to lb/ft
2
.s
04
(c) A chemist is interested in preparing 500 ml of 1 normal, 1 molar and 1 molal
solution of H 2SO 4. Assuming the density of H 2SO 4 solution to be 1.075 g/cm
3
,
calculate the quantities of H 2SO 4 to be taken to prepare these solutions.
07
Q.2 (a) Define the following: Molarity , Molality and Normality 03
(b) The average molar mass of a flue gas sample is calculated by two different
engineers. One engineer uses the correct molar mass of 28 for N 2 and determines
the average molar mass to be 30.08, the other engineer, using an incorrect value
of 14, calculates the average molar mass to be 18.74. (i) Calculate the volume %
of nitrogen in the flue gases, (ii) If the remaining components of the flue gases are
CO 2 and O 2, calculate the volume % each of them
04
(c) Cracked gas from a petroleum refinery has the following composition by volume,
methane 45%, Ethane10%, ethylene 25%, Propane 7%, Propylene 8%, n-Butane
5% . Find (a) Average mol. wt. of gas mixture. (b) the composition by weight %
and (c) Specific gravity of the gas mixture at STP.
07
OR
(c) A weight of 1.10 kg of Carbon dioxide occupies a volume of 0.033 m
3
at 300 K.
Using the Van der Waals equation of state, calculate the pressure.
Data: For CO 2 gas, take a = 3.60 [(m
3
)
2
.kPa] / (kmol)
2
and b = 4.3 x 10
-2
m
3
/kmol.
07
Q.3 (a) State : Dalton?s law and Raoult?s law 03
(b) The spent acid from a nitrating process contains 33% H 2SO 4, 36% HNO 3 and 31%
water by weight. This acid is to be strengthened by the addition of concentrated
sulphuric acid containing 95% H 2SO 4 and concentrated nitric acid containing 78%
HNO 3. The strengthened mixed acid is to contain 40% H 2SO 4 and 43% HNO 3.
Calculate the quantities spent and concentrated acids that should be mixed together
to yield 1500 kg of the desired mixed acid
04
2
(c) Soyabean seeds are extracted with the hexane in batch extractors. The flaked seeds
are found to contain 18.6% oil, 69% solids, 12.4% moisture (by weight). At the
end of the extraction process, cake is separated from hexane-oil mixture. The cake
is analyzed to contain 0.8% oil, 87.7% solids and 11.5% moisture (by weight).
Find the percent recovery of oil
07
OR
Q.3 (a) Define the terms: (a) Conversion (b) Yield (c) Selectivity 03
(b) 2000 kg of wet solids containing 70% solids by weight are fed to tray dyer where
it is dried by hot air. The product finally obtained is found to contain 1% moisture
by weight, calculate: (1) kg of water removed from wet solids (2) kg of the product
obtained.
04
(c) A solution contains 50% Benzene, 30% Toluene and 20% Xylene by weight at a
temperature of 100 ?C. The vapors are in contact with solution. Calculate the total
pressure and molar % compositions of liquid and the vapor. The vapor pressures
and the molecular weights are as follows:
Components vapor pressure at 100
o
C Mol. weight
Benzene 1340 mm Hg 78
Toluene 560 mm Hg 92
Xylene 210 mm Hg 106
07
Q.4 (a) Explain: Limiting reactant, Excess reactant and Percent excess reactant 03
(b) Ammonia reacts with sulphuric acid giving ammonium sulphate:
2NH 3 +H 2SO 4 ?( NH 4) 2SO 4
a) 20 m
3
of ammonia at 1.2 bar and 300 k reacts with 40 kg of
sulphuric acid. Which one is the excess reactant and what is the
percent excess?
b) How much ammonium sulphate is obtained
04
(c) 1 kg nitrogen is mixed with 3.5 m
3
of hydrogen at 300 K and 101.3 kPa and sent
to the ammonia converter. The product leaving the converter analysed 13.7 %
ammonia, 70.32 % hydrogen and 15.98 % nitrogen.
(a) Identity the limiting reactant.
(b) What is the present excess of excess reactant?
(c) What is the present conversion of the limiting reactant?
07
OR
Q.4 (a) State the basic principle of material balance 03
(b) Calculate the following for the reaction:
C 2H 4 + 2Cl 2 ? C 2HCl 3 + H 2 + HCl
(1) The stoichiometry ratio of Cl 2 to C 2H 4
(2) If 4 kmol Cl 2 is used per kmol of C 2H 4, find the % excess Cl 2
04
3
(3) The amount of HCl produced from 50 kg C 2H 4 assuming reaction goes to
completion
(c) A coal containing C=67.9%, H=4.4%, S=0.8%, N=1.6%, O=7.9%, ash =4.5% and
water =12.9 % is burnt in a furnace. The product of combustion dry gas , analyses,
CO 2 =14.5%, O 2 =4.7 and rest N 2.Calculate
1). The theoretical volume of air used for the complete combustion of 100 kg of
coal.
2). The percent excess air used.
07
Q.5 (a) Define: i) Heat capacity ii) Sensible heat and iii) Latent heat 03
(b) A heat exchanger for cooling hot oil uses 10000 kg/hr of cooling water, which
enters the exchanger at 294 K. The hot oil at the rate of 5000 kg/hr enters at 423
K and leaves at 338 K and has an average heat capacity of 2.51 KJ/kg K. Calculate
the outlet temperature of the water
04
(c) Calculate the theoretical flame temperature for CO when it is burnt with 100 %
excess air. Both the reactants are at 373K. The heat capacities (J/mol.K) (may be
assumed constant) are 29.23 for CO, 34.83 for O 2 ,33.03 for N 2 and 53.59 for CO 2.
The standard heat of combustion at 298K is -282.99 kJ/mol CO
07
OR
Q.5 (a) Define : Heat of formation and Heat of combustion 03
(b) Pure methane is heated from 303 K to 523 K at atmospheric pressure. Calculate
the heat added per kmol methane using the following data:
Cp= 26.586 + 7.5820 ? 10
-3
T ? 1.1200 ? 10
-6
T
2
, kJ/(kmol-K)
04
(c) Calculate the change in enthalpy between reactants and products if both are at 298
K (25
0
C) and if 5 mole of ethylene oxide is produced as per the following reaction:
C 2H 4(g) + 1/2 O 2(g) = C 2H 4O (g)
Data:
Component ?H
0
f, kJ/mol at 298.15 K(25
0
C)
C 2H 4(g) 52.50
C 2H 4O(g) -52.63
07
***************
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This post was last modified on 20 February 2020