Calawod, Stiffa Love
Condino, Simel Grace
Moran, Brant
Reactors
Google Docs Link:
https://docs.google.com/document/d/18gAkMR_SkyUKlD74IMVuCOCF_HaZ_z_XStuJa-VNh4o/
edit
Mock Boards
General Engineering:
1. Ultrasound refers to sounds whose frequencies are above __________.
A. 10,000 Hz
B. 20,000 Hz
C. 30,000 Hz
D. 40,000 Hz
2. Water is pouring into a swimming pool. After t hours, there are t + √t gallons in the pool. At
what rate is the water pouring into the pool when t = 9 hours?
A.
B.
C.
D.
4/3 gph
5/2 gph
1 gph
3/2 gph
Soln. (9+√9)/9 = 12/9 = 4/3
For questions 3 to 5: A projectile is fired by a Pyro Gunslinger with an initial speed of 65 m/s at
an angle of 30 degrees above the horizontal on a long flat firing range.
3. Determine the total time of the projectile in the air.
A. 3.32 s
B. 8.78 s
C. 5.86 s
D. 6.64 s
4. Determine the maximum height reached by the projectile.
A. 94.42 m
B. 53.89 m
C. 89. 36 m
D. 79.28 m
5. Determine range of the projectile.
A.
B.
C.
D.
373.77 m
539.44 m
315.80 m
296.68 m
6. If 24 people joined a quiz bowl, in how many ways can these people be seated in the first,
second and third seat?
A.
B.
C.
D.
255024
12144
32760
360360
Soln: 24P3=12144
7. How many significant digits do 10.097 have?
A.
B.
C.
D.
5
4
3
2
8. 7 + 0i is?
A.
B.
C.
D.
Irrational number
Real number
Imaginary
Even
9. Which of the following cannot be a probability
A.
B.
C.
D.
1
0
1/e
0.21682
10. Integrate dx/(x+3) from -2 to 8
A. 5/12
B. 1/8
C. ln 11
D. ln 10
Soln: ln(8+3) - ln(-2+3) = ln(11) - ln(1) = ln(11)
11. Express decimally: Fourteen Ten thousandths
A.
B.
C.
D.
0.14
0.00014
0.0014
0.1410000
12. MCMXCIV is equivalent to what number?
A.
B.
C.
D.
1994
1974
1984
1964
For questions 13-14: The Crux is 690 m away from the Guyun Stone Forest that defends the
Liyue Harbor. A Guizhong Ballista at sea level fires javelins at an initial velocity of 91 m/s at an
angle of 42 degrees.
13. Determine the maximum height of the javelin.
A.
B.
C.
D.
272.30 m
189.26 m
235.16 m
132.13 m
14. Determine the total time traveled by the javelin in the air.
A.
B.
C.
D.
14. 91 s
7.45 s
6.21 s
12.43 s
15. What is the value in degrees of 1 radian?
A.
B.
C.
D.
360
0.0174533
57.3
90
16. 4800 mils is equivalent to ____ degrees.
A.
B.
C.
D.
145
270
320
270
17. What is the absolute temperature of the freezing point of water in degree Rankine?
A.
B.
C.
D.
492
478
482
456
18. The standard acceleration due to gravity is
A.
B.
C.
D.
9.8 ft/s²
32.2 ft/s²
27 ft/s²
24.7 ft/s²
19. Factor the expression x^2 + 6x + 8 as completely as possible
A.
B.
C.
D.
(x-4) (x+2)
(x+4) (x+2)
(x-2) (x-4)
(x+2) (x-4)
20. What is the least common multiple of 15 and 18?
A.
B.
C.
D.
60
30
36
90
21. The arithmetic mean of a and b is
A.
B.
C.
D.
(a+b)/2
(a+b)/b
(a+b)/a
(a+b)/(a+b)
22. The moment of inertia of an object is dependent on which of the following?
A.
B.
C.
D.
The object’s size and shape
The object’s mass
The location of the axis of rotation
All of these
23. The terms of a sum may be grouped in any manner without affecting the result. this is law
known as
A.
B.
C.
D.
Associative Law
Commutative Law
Distributive Law
Republic Law
24. What is another term for a vector product of two vectors?
A.
B.
C.
D.
Cross product
Vector product
Dot product
Plus product
25. “The ratio of the sines of the angles of incidence and refraction is equal to the ratio of the
speeds of light in the two media”. This statement is known as ________.
A.
B.
C.
D.
Huygen’s principle
Snell’s law
Maxwell’s hypothesis
Mandela effect
26. What refers to the effect when a beam containing more than one frequency is split into a
corresponding number of different beams when it is refracted?
A. Flux
B. Refraction
C. Reflection
D. Dispersion
27. The standard acceleration due to gravity is
A. 32.2 m/s2
B. 382 in/s2
C. 0.0061 mi/s2
D. 9.8 mm/s2
28. Air exerts force that is opposite to the car’s motion. What is this force called?
A.
B.
C.
D.
Reverse effective force
Air force
Drag force
Aerodynamic force
29. Roll a pair of dice. What is the probability that the sum of two numbers is 11?
A.
B.
C.
D.
1/36
1/9
1/18
1/20
Soln: (2/6)*(1/6)=1/18
30. Determine the probability of drawing either a king or a diamond in a single draw from a pack
of 52 playing cards
A.
B.
C.
D.
2/13
3/13
4/13
1/13
Soln: There are 13 diamond cards and 4 kings but 1 of those kings is a diamond thus,
(13/52)+(3/52) = 16/52 or 4/13
31. Find the 4th term of the expansion of (x^3+2)^11
A.
B.
C.
D.
4455x^24
4475x^24
4485x^24
4505x^24
Soln: (p+q)^n=nC(r-1)p^(n-r+1)q(r-1)
11C3 * (x^3)^(11-4+1) * 3^(4-1)
165*(x^24)*(3)^3
4455x^24
32. In how many ways can you invite one or more of your 8 friends in a party?
A.
B.
C.
D.
255
254
226
245
Soln: 8C8+8C7+8C6+8C5+8C4+8C3+8C2+8C1=255
33. What is the number of permutations of the letters in the word CHEMICAL?
A.
B.
C.
D.
2520
1380
5440
5040
Soln: 7!/2!=2520
Chemical Engineering
Physical and Chemical Principles:
1. A student adds 0.1 mol of oxalic acid and 0.1 mol of sodium dihydrogen phosphate to enough
water to make 1.0 L of solution. The following equilibrium is established with the concentrations
of the products greater than the concentrations of the reactants. Which of the statements about
the equilibrium system is correct?
H2C2O4(aq) + H2PO4–(aq) HC2O4–(aq) + H3PO4(aq)
A. The dihydrogen phosphate anion, H2PO4–, is a stronger acid than oxalic acid.
B. The hydrogen oxalate anion, HC2O4–, is a stronger base than the dihydrogen
phosphate anion, H2PO4–.
C. Water is a stronger acid than either oxalic or phosphoric acids.
D. Oxalic acid is a weaker acid than phosphoric acid.
E. Phosphoric acid is a weaker acid than oxalic acid.
2.Which one of the following substances will give an aqueous solution of pH < 7?
A. CH3OH
B. Na2CO3
C. NH4Br
D. CH3COONa
E. KI
Soln: NH4Br is the only base among the choices.
3. Butyric acid is responsible for the odor in rancid butter. A solution of 0.25 M butyric acid has a
pH of 2.71. What is the Ka for the acid?
A. 0.36
B. 1.5 × 10–5
C. 2.4 × 10–2
D. 7.8 × 10–3
E. none of the above
Soln:
4.For which of the following processes would ΔS° be expected to be most positive?
A.
B.
C.
D.
E.
O2(g) + 2H2(g) → 2H2O(g)
H2O(l) → H2O(s)
NH3(g) + HCl(g) → NH4Cl(g)
2NH4NO3(s) → 2N2(g) + O2(g) + 4H2O(g)
N2O4(g) → 2NO2(g)
Reasoning: Positive ΔS° means higher disorder, phase change from solid to liquid or
solid to gas have positive entropy change due to increasing disorder of the nature of
their molecules.
5. Which of the following is true?
A. By spontaneous we mean that the reaction or process will always proceed to the right
(as written) even if very slowly. Increasing the temperature may speed up the reaction,
but it does not affect the spontaneity of the reaction.
B. By spontaneous we mean that the reaction or process will always proceed to the left (as
written) even if very slowly. Increasing the temperature may speed up the reaction, but it
does not affect the spontaneity of the reaction.
C. By spontaneous we mean that the reaction or process will always proceed to the left (as
written) even if very slowly. Increasing the temperature may speed up the reaction and it
generally affects the spontaneity of the reaction.
D. By spontaneous we mean that the reaction or process will always proceed to the
right (as written) even if very slowly. Increasing the temperature may speed up the
reaction, and it generally affects the E. spontaneity of the reaction.
E. None of the above is true.
6.CH4(g) + 4Cl2(g) → CCl4(g) + 4HCl(g), ΔH = -434 kJ
Based on the above reaction, what energy change occurs when 1.2 moles of methane (CH4)
reacts?
a.
b.
c.
d.
e.
5.2 × 105 J are released.
5.2 × 105 J are absorbed.
3.6 × 105 J are released.
3.6 × 105 J are absorbed.
4.4 × 105 J are released.
Soln:
7.The heat combustion of acetylene, C2H2(g), at 25°C is -1299 kJ/mol. At this temperature,
ΔHf° values for CO2(g) and H2O(l) are -393 and -286 kJ/mol, respectively. Calculate ΔHf° for
acetylene.
A.
B.
C.
D.
E.
2376 kJ/mol
625 kJ/mol
227 kJ/mol
-625 kJ/mol
-227 kJ/mol
Soln:
8.Consider the reaction:
C2H5OH(l) + 3O2(g) → 2CO2(g) + 3H2O(l); ΔH = -1.37 × 103 kJ
Consider the following propositions:
I. The reaction is endothermic
II. The reaction is exothermic.
III. The enthalpy term would be different if the water formed was gaseous.
Which of these propositions is (are) true?
a.
b.
c.
d.
e.
I
II
III
I, II
II, III
9.Which of the following does not have a standard enthalpy of formation equal to zero at 25°C
and 1.0 atm?
A.
B.
C.
D.
E.
F2(g)
Al(s)
H2O(l)
H2(g)
They all have a standard enthalpy equal to zero.
10.Consider the following balanced redox reaction
Mn2+(aq) + S2O82–(aq) + 2H2O(l) → MnO2(s) + 4H+(aq) + 2SO42–(aq)
Which of the following statements is true?
A. Mn2+(aq) is the reducing agent and is reduced.
B. Mn2+(aq) is the oxidizing agent and is oxidized.
C. Mn2+(aq) is the oxidizing agent and is reduced.
D. Mn2+(aq) is the reducing agent and is oxidized.
E. Manganese does not change its oxidation number in this reaction.
11.Which of the statements below correctly describes the combustion of glucose, shown below?
C6H12O6 + 6O2 → 6CO2 + 6H2O
A.
B.
C.
D.
E.
Oxygen in O2 is being oxidized.
Carbon in C6H12O6 is being oxidized.
Hydrogen in C6H12O6 is the reducing agent.
Oxygen in C6H12O6 is the oxidizing agent.
Hydrogen in C6H12O6 is being reduced.
Soln: C charge in glucose is 0 while C in CO2 is +4
C(x)+H(+1)+O(-2) = 0
6x+12(1)+6(-2) = 0
X=0
C(x)+O(-2) = 0
x+2(-2) = 0
X = +4
12.Which one of the following is not a redox reaction?
A. Cl2(g) + 2KBr(aq) → Br2(l) + 2KCl(aq)
B. 2H2(g) + O2(g) → 2H2O(l)
C. 6FeSO4(aq) + K2Cr2O7(aq) + 7H2SO4(aq) → Cr2(SO4)3(aq) + 3Fe2(SO4)3(aq) +
K2SO4(aq) + 7H2O(l)
D. H2O(l) + NH3(g) → NH4+(aq) + OH–(aq)
E. Zn(s) + H2SO4(aq) → ZnSO4(aq) + H2(g)
Soln: There are ion exchange or change in charge.
13.Which of the following solids is commonly used as an inactive electrode in electrochemical
cells
A.
B.
C.
D.
E.
sodium
copper
iron
zinc
graphite
14.The line notation, Pt | H2(g) | H+(aq) || Cu2+(aq) | Cu(s), indicates that
A.
B.
C.
D.
E.
Cu2+ is the reducing agent.
hydrogen gas (H2) is a product of the cell reaction.
Cu is the anode.
Pt is the cathode.
Copper metal is a product of the cell reaction.
15.What is the E°cell for the cell represented by the combination of the following half-reactions?
2Hg2+(aq) + 2e– Hg22+(aq) E° = 0.92 V
Cr3+(aq) + 3e– Cr(s)
E° = –0.74 V
A. 1.28 V
B. –0.18 V
C. 2.12 V
D. 0.18 V
E. 1.66 V
Soln: E° = 0.92V - (-0.74 V) = 1.66 V
16.Which of the following statements about voltaic and electrolytic cells is correct?
A.
B.
C.
D.
The free energy change, ΔG, is negative for an electrolytic cell.
The electrons in the external wire flow from cathode to anode in both types of cell.
Reduction occurs at the anode in an electrolytic cell.
The cathode is labeled as positive (+) in a voltaic cell but negative (–) in an
electrolytic cell.
E. Oxidation occurs at the cathode only in a voltaic cell.
17.Examine the following half-reactions and select the strongest reducing agent among the
species listed.
PbI2(s) + 2e– Pb(s) + 2I–(aq)
E° = –0.365 V
Ca2+(aq) + 2e– Ca(s)
E° = –2.868 V
Pt2+(aq) + 2e– Pt(s)
E° = 1.18 V
Br2(l) + 2e– 2Br–(aq)
E° = 1.066 V
A.
B.
C.
D.
E.
Pt(s)
Br–(aq)
Pt2+(aq)
Pb(s)
Ca(s)
Soln: The negative the value of E° cell the stronger its reducing power.
18.Which of the following conditions is most likely to apply to a fully-charged secondary cell?
A.
B.
C.
D.
E.
E°cell = 0
Ecell = E°cell
Q<K
Q=K
Q=1
19.What product forms at the cathode during the electrolysis of molten lithium iodide?
A.
B.
C.
D.
E.
Li+(l)
I–(l)
I3–(l)
Li(l)
I2(g)
Soln: Cathode in electrolysis is negatively charged thus it attracts positive ions making
Li(l) the product in the cathode.
20.What mass of silver will be formed when 15.0 A are passed through molten AgCl for 25.0
minutes? (Ag = 107.87 g/mol; Faraday’s constant = 96485 C/mol e)
A.
B.
C.
D.
E.
33.4 g
6.29 g
12.6 g
25.2 g
0.419 g
Soln:
Chemical Engineering Principles:
1. ________ receives the output signal to change the valve settings.
A. Controller
B. Actuator
C. Regulator
D. Sensor
2. The operating point in a pumping system is identified by
A. Point of intersection of pump curve and theoretical power curve
B. Cannot be determined by the pump characteristic curves
C. Point of intersection of system curve and efficiency curve
D. Point of intersection of pump curve and system curve
3. Joule Thomson expansion is the ____.
A. Upstream enthalpy equals to downstream enthalpy
B. Difference between upstream and downstream enthalpy
C. Overall enthalpy is the sum of upstream and downstream enthalpy
D. Net Enthalpy
For questions 4, 5 and 6 refer to the problem below:
A three-stage adiabatic compressor is required to compress air from 140 kN/m2 and 283 K to
4000 kN/m2. It may be assumed that the interstage cooling is provided to cool the air to the
initial temperature.
4. Calculate the ideal intermediate pressures in kN/m2 (P1’ and P2’).
A. P1’= 1409.58 and P2’= 430.06
B. P1’= 1504.02 and P2’= 468.47
C. P1’= 1280.83 and P2’= 451.89
D. P1’= 1308.47 and P2’= 428.02
5. Calculate the work required per kilogram of gas (J/kg).
A. 740,220 J/kg
B. 319,170 J/kg
C. 320,136 J/kg
D. 321,156 J/kg
6. Calculate the isothermal efficiency of the process.
A. 85.14%
B. 84.88%
C. 86.59%
D. 83.76%
7. A cooling coil, consisting of a single length of tubing through which water is circulated, is
provided in a reaction vessel, the contents of which are kept uniformly at 360 K by means of a
stirrer. The inlet and outlet temperatures of the cooling water are 280 K and 320 K respectively.
If the overall heat transfer coefficient is assumed to be constant over the length of the tube and
independent of the water temperature, what would be the outlet water temperature if the length
of the cooling coil were increased by 6 times?
A. 357.50 K
B. 356.70 K
C. 358.75 K
D. 353.80 K
8. Air flows at 15 m/s through a pipe of inside diameter 35 mm. The rate of heat transfer by
convection between the pipe and the air is 60 W/m2 K. Neglecting the effects of temperature
variation, estimate the pressure drop per meter length of pipe (kPa per meter).
A. 0.1152 kPa per meter
B. 0.1069 kPa per meter
C. 0.1029 kPa per meter
D. 0.1089 kPa per meter
For items 9 and 10, refer to item below:
A simple rectifying column consists of a tube arranged vertically and supplied at the bottom with
a mixture of benzene and toluene as vapor. At the top, a condenser returns some of the product
as a reflux which flows in a thin film down the inner wall of the tube. The tube is insulated and
heat losses can be neglected. At one point in the column, the vapor contains 70 mol% benzene
and the adjacent liquid reflux contains 59 mol% benzene. The temperature at this point is 365 K.
The molar latent heats of the two materials can be taken as equal. The vapor pressure of
toluene at 365 K is 54.0 kN/m2 and the diffusivity of the vapors is 0.051 cm2/s.
9. Calculate the partial pressure of toluene in the liquid phase (PT1) and vapor phase (PT2).
A. PT1= 22.14 kN/m2;PT2= 30.39 kN/m2
B. PT1= 22.30 kN/m2;PT2= 30.22 kN/m2
C. PT1= 22.78 kN/m2;PT2= 30.74 kN/m2
D. PT1= 22.69 kN/m2;PT2= 30.83 kN/m2
10. Assuming the diffusional resistance to vapor transfer to be equivalent to the diffusional
resistance of a stagnant vapor layer 0.2 mm thick, calculate the rate of interchange of benzene
and toluene between vapor and liquid (kmol/m2⋅s).
A. NB = 6.797x10-5 kmol/m2⋅s; NT = -6.797x10-5 kmol/m2⋅s
B. NB = 6.689x10-5 kmol/m2⋅s; NT = -6.689x10-5 kmol/m2⋅s
C. NB = 6.933x10-5 kmol/m2⋅s; NT = -6.933x10-5 kmol/m2⋅s
D. NB = 6.837x10-5 kmol/m2⋅s; NT = -6.837x10-5 kmol/m2⋅s
11. Maximum work that could be secured by expanding the gas over a given pressure range is
the __________ work.
A.
B.
C.
D.
Isentropic
Adiabatic
Exothermal
Isothermal
12. Heating of water under atmospheric pressure is an __________ process.
A.
B.
C.
D.
Adiabatic
Isothermal
Isochoric
Isobaric
13. Which of the following properties of a fluid is responsible for offering resistance to shear ?
A.
B.
C.
D.
Specific Gravity
Surface Tension
Sheer strength
Viscosity
14. Fundamental principle of refrigeration is based on the __________ law of thermodynamics.
A.
B.
C.
D.
Second
Zeroth
First
Third
15. A refrigerator may be termed as a
A.
B.
C.
D.
Heat compressor
Carnot Engine
Heat pump
All of the above
16. If pH value of a solution is 8, then its pOH value will be
A.
B.
C.
D.
7
9
0
6.
17. A sample of well water contains 140 gm/m3 Ca2+ ions and 345 gm/m3 Na+ ions. The
hardness of the sample of water, expressed in terms of equivalent CaCO3 in gm/m3 is
(assuming atomic masses of Ca :40, Na : 23, C : 12, O : 16)
A.
B.
C.
D.
300
240
350
340
Soln.
Atomic mass of ca 40.
MW of caco3 is 100.
Therefore 40 g of ca = 100 g of caco3.
Then 140 g of ca = ? g of caco3.
Simplifying 100(140) / 40.
W of caco3 = 350.
18. In a solution containing 0.30 Kg mole of solute and 600 kg of solvent, the molality is
A.
B.
C.
D.
0.3
1
0.4
0.5
Soln.
Molality = Number of gram moles of solute per
kilogram of solvent.
Molality= 0.3 x 1000 / 600 = 0.5.
1 kg = 1000 g
19. Fourier's law applies to the heat transfer by
A.
B.
C.
D.
Conduction
Convection
Induction
Radiation
20. The heat flux (from outside to inside) across an insulating wall with thermal conductivity, K=
0.04 W/m.°K and thickness 0.16m is 10 W/m2. The temperature of the inside wall is - 5°C. The
outside wall temperature is
A.
B.
C.
D.
35°C
25°C
32°C
28°C
Soln.
Q = KA(T2-T1)/dx.
Q = 10,
K = .04,
T1 = -5,
dx = .16,
A = 1.
10 = .04*(T2+5)/.16.
T2 + 5 = 40,
T2 = 40-5,
T2 = 35.