Thermodynamics and Basic Chemistry Assignment

This assignment delves into the fields of thermodynamics and basic chemistry. It focuses on calculations related to a diesel engine's operating cycle, including thermal efficiency, compression ratio, and fuel consumption. The assignment also covers topics in chemistry such as molar mass, chemical reactions, and equilibrium constants.

Introduction
The assignment focuses on thermodynamics and basic chemistry. Especially, the calculations
based on the operation cycle of a diesel engine.
Part A: Thermodynamics and Engines”
Question 1
“Thermal efficiency is given as n=1− Qout
Q¿
=1− mcv ( T 4−T 1 )
mcP ( T 3−T 2 )
Let CP
CV
=γ
Efficiency¿ 1− 1
γ ( ( T 4 −T1 )
( T3 −T2 ) )
all temperatures can be expressed in terms of T 3 from:
T 1= T 2
rv
γ −1 , T 2=T 3
V 2
V 3
=T 3
rc
, and T 4= T3
r v
γ−1
Therefore, η=1− 1
γ (
T 3
rv
γ −1 − T 3
rc rv
γ −1
T3 −T 3
rc
)
η=1− 1
γ
( (rc rv
γ −1−re
γ −1 )
re
γ −1 rc r v
γ−1 )
rx−1
rc
T 3
T 3

η=1− 1
γ
1
re
γ −1 rv
γ −1 [ rc ( re
γ −1 r c
γ−1 ) −re
γ −1
rc−1 ]
Hence, the thermal efficiency, η=1− 1
γ
1
rv
γ −1 [ r c
γ −1
r c−1 ]
But V 3
V 2
=rc=α and V 1
V 2
=rv=Ψ
Replacing these in the thermal efficiency equation yields:
η=1− 1
γ
1
Ψ γ −1 [ αγ −1
α −1 ]
Question 2
V 1=1949.56 litres, V 2=140 Litres , V 3
V 2
=1.86 , V 3=1.86 ×140=260.4 litres ,
V 4 =V 1=1949.56 litres
T 4=50 ° C , T3 =T 4 rv
γ −1 =50× 13.925(¿1.3 −1 )=110.18 ° C ¿
T 2=T 3
V 2
V 3
=110.18× 1
1.86 =59.24 ° C, T 1= T 2
rv
γ −1 = 59.24
13.925(¿1.3 −1)=26.88 ° C ¿
P2=P3 =150¯, P1=P4= P2
rv
γ −1 = 150
13.925(¿1.3−1)=68.07¯¿ ¿
Question 3
The specific heat capacity ratio¿ CP
CV
=γ =1.3
Swept volume ¿ V 1−V 2

¿ π
4 × D2 L
¿ π
4 ×0.962 ×2.5
¿ 1.80956 M3
V 1−V 2 =1.80956
V 1=1.80956+V 2=1.80956+140=1949.56 Litres
Compression ratio Ψ =V 1
V 2
= 1949.56
140 =13.925
Thermal efficiency, η=1− 1
γ
1
Ψ γ −1 [ αγ −1
α −1 ]
=1− 1
1.3 × 1
13.925( ¿1.3−1) [ 1.861.3−1
( 1.86−1 ) ]=0.4964=49.64 % ¿
Question 4”
Also, thermal efficiency= Heat
mass flow ×Calorific value = 80× 106
˙m× 45 ×106
˙m= 80× 106
0.4964 × 45 ×106 =3.5813 kg /s
Diesel consumption per day= ˙3.5813 ×24 × 3600=309.424 × 103 Kg
“Watt’s Governor
Question 1 and 2

If the Q ( l
s ) is the volume flow rate, V fuel= 0.001 Q
π
4 ×0.022
=3.1831Q m
s
ω= V fuel
0.05 = vω
0.15 , vω=9.5493 Q m
s
ωgear = vω
0.03 =318.31 Q rad
s , Q=0.0031416 ωgear
Q=0.031416× 30
π ωgear ∈rpm=0.03 ωgear (¿ rpm∧l
s )
“The MATLAB code used to implement the same is shown in figure 1 and the corresponding
plot is as shown:
Figure 1: MATLAB code”
Figure 2: “MATLAB PLOT”

“Question 3
To change to another working point, change the volume flow rate of the fuel.
Basic Chemistry”
“Question 1
The molar mass of CuS O4 is (63.5+32+16 × 4)=159.5 g
Question 2
Potassium oxide = K2 O
Molar mass=39 ×2+16=94 g
100g of K2 O has 100
94 Moles

But, each mole of K2 O produces 2 moles of potassium cations according to the dissociation
equation: K2 O(aq)→2 K+¿ ( aq ) + O2−¿( aq)¿ ¿
Therefore, the number of moles of potassium cations equals 100
94 ×2=200
94 Moles
But 1mole has 6.022 ×1023 ions
Hence, 200
94 Moles of potassiumhas 200
94 ×6.022 ×1023 ions=1.2813 ×1024 ions
Question 3
2 carats of diamond= ( 2 ×0.2 ) g=0.4 g
1 mole carbon=12g
Therefore, 0.4g carbon has 0.4
12 =0.03333 moles
The number of carbon atoms=0.03333 ×6.022 ×1023=2.00733× 1022 atoms
Question 4
3 Fe+4 H2 O → Fe3 O4 +4 H2
1 mole of water reacts with 1
4 ×3=0.75 moles of Fe
Therefore, 6 moles of water will react with 6 × 0.75moles=4.5 moles of Fe and the chemical
reaction becomes:
4.5 Fe+6 H2 O→ 1.5 Fe3 O4 +4 .5 H2

After the reaction 0.5 moles of Fe remain.
Question 5
H2 S O4 + 2 NaOH → Na2 S O4 +2 H2 O
Number of moles of H2 S O4 =Molarity× Volume= 0.3 × 50
1000 =0.015 moles
But, 1mole of H2 S O4 requires 2 moles of NaOH
0.015 moles of H2 S O4 will require 2 ×0.015=0.03 moles of NaOH
Volume of NaOH ( ml ) = No of Moles
Molarity × 1000= 0.3
0.75 × 1000=400 ml
Question 6
MnO2(s)+4HCl (aq)→MnCl2 (aq)+Cl2 (g) +2H2O (l)
1g of MnO2= 1
87 =0.01149 moles
Mole ratio Mn O2 :Cl2=1 :1
Cl2 moles = 0.01149
But 1 mole of Cl2 has a mass of 70.9g
Therefore, 0.01149 moles gives ( 0.01149 ×70.9 ) g=0.8149 g
But the density of Cl2 is 3.17g/L
Volume of Cl2= Mass
Density = 0.8149
3.17 ×1000=257 ml

In case 50g of Mn O2 are added:
50g of MnO2= 50
87 =0.5747 moles
Therefore, 0.5747 moles gives ( 0.5747 ×70.9 ) g=40.747 g
Volume of Cl2= Mass
Density = 40.747
3.17 =12.850 l
Question 7
2 ONCl ( g ) ⇄2 NO ( g ) +Cl2 (g)
“[ ONCl ]=0.09 ×1=0.09 M
2 ONCl ( g ) ⇄ 2 NO ( g ) +Cl2 (g)
Initial concentration” 1M 0 0
Change -0.09 +0.18 0.09
Equilibrium 0.91 0.18 0.09
Kc= [NO ]2 [Cl2 ]
[ONCl ]2 =[0.18]2 [0.09]
[ 0.91]2 =3.5213 ×10−3”
Question 8
“First, we make a table as follows
H2 ( g ) + CO2 ( g ) ⇄ H2 O ( g ) +CO (g)
Initial
concentration
0.01M 0.01M 0 0
Change -y -y +y +y

Equilibrium 0.01-y 0.01-y y y
The equilibrium constant, K= [ H2 O ] [CO ]
[ H 2 ] [CO2 ] = y ( y )
(0.01− y)(0.01− y ) =0.771
Substituting the numbers yields, y2
(0.01− y)2 =0.771
Finding the square roots of both sides
¿ y
0.01− y =0.878066, 0.878066 ( 0.01− y )= y
Rearranging and solving for y yields, y=4.675 ×10−3
So H2=CO=0.004675 M and H2=CO2=0.01−0.004675=0.005325 M
Question 9
The reaction is an endothermic process meaning that heat energy is absorbed. If you increase the
temperature, the rate of the reaction will increase and favor the production of more CO∧H2 O
Question 10”
{Ca} rsub {3} {(P {O} rsub {4} )} rsub {2} + {3H} rsub {2} S {O} rsub {4} → {2H} rsub {3} P {O} rsub {4}
Therefore, a=1 , b=3 , c=2 ,∧d=3
Conclusion
“The task helped me recall the thermodynamics and basic chemistry concepts taught in class.
Notably, the operation of the four-stroke gasoline engine and the calculations involved.