The Islamic University of Gaza
/ /Chemistry Department
Chemical Engineering (CHEM 1203) / Time: 2 hours / 50اسم الطالب...... الرقم الجامعي ......
اسم المدرس...... الشعبة......
Answer the following questions and mark your answer using (X) in the following answer sheet.
Answer / No / Answer / No / Answer / Nod / c / b / a / 25 / d / c / b / a / 13 / d / c / b / a / 1
d / c / b / a / 26 / d / c / b / a / 14 / d / c / b / a / 2
d / c / b / a / 27 / d / c / b / a / 15 / d / c / b / a / 3
d / c / b / a / 28 / d / c / b / a / 16 / d / c / b / a / 4
d / c / b / a / 29 / d / c / b / a / 17 / d / c / b / a / 5
d / c / b / a / 30 / d / c / b / a / 18 / d / c / b / a / 6
d / c / b / a / 31 / d / c / b / a / 19 / d / c / b / a / 7
d / c / b / a / 32 / d / c / b / a / 20 / d / c / b / a / 8
d / c / b / a / 33 / d / c / b / a / 21 / d / c / b / a / 9
d / c / b / a / 34 / d / c / b / a / 22 / d / c / b / a / 10
d / c / b / a / 35 / d / c / b / a / 23 / d / c / b / a / 11
d / c / b / a / 24 / d / c / b / a / 12
IA / VIIIA
1 / 2
H / He
1.008 / IIA / IIIA / IVA / VA / VIA / VIIA / 4.003
3 / 4 / 5 / 6 / 7 / 8 / 9 / 10
Li / Be / B / C / N / O / F / Ne
6.941 / 9.012 / 10.81 / 12.01 / 14.01 / 15.99 / 19.00 / 20.18
11 / 12 / 13 / 14 / 15 / 16 / 17 / 18
Na / Mg / Al / Si / P / S / Cl / Ar
22.99 / 24.31 / IIIB / IVB / VB / VIB / VIIB / ┌──── / VIIIB / ────┐ / IB / IIB / 26.98 / 28.09 / 30.97 / 32.07 / 35.45 / 39.94
19 / 20 / 21 / 22 / 23 / 24 / 25 / 26 / 27 / 28 / 29 / 30 / 31 / 32 / 33 / 34 / 35 / 36
K / Ca / Sc / Ti / V / Cr / Mn / Fe / Co / Ni / Cu / Zn / Ga / Ge / As / Se / Br / Kr
39.10 / 40.08 / 44.96 / 47.88 / 50.94 / 52.00 / 54.94 / 55.85 / 58.93 / 58.69 / 63.55 / 65.39 / 69.72 / 72.61 / 74.92 / 78.96 / 79.90 / 83.80
37 / 38 / 39 / 40 / 41 / 42 / 43 / 44 / 45 / 46 / 47 / 48 / 49 / 50 / 51 / 52 / 53 / 54
Rb / Sr / Y / Zr / Nb / Mo / Tc / Ru / Rh / Pd / Ag / Cd / In / Sn / Sb / Te / I / Xe
85.47 / 87.62 / 88.91 / 91.22 / 92.91 / 95.94 / (98) / 101.1 / 102.9 / 106.4 / 107.9 / 112.4 / 114.8 / 118.7 / 121.8 / 127.6 / 126.9 / 131.3
55 / 56 / 57 / 72 / 73 / 74 / 75 / 76 / 77 / 78 / 79 / 80 / 81 / 82 / 83 / 84 / 85 / 86
Cs / Ba / La / Hf / Ta / W / Re / Os / Ir / Pt / Au / Hg / Tl / Pb / Bi / Po / At / Rn
132.9 / 137.3 / 138.9 / 178.5 / 180.9 / 183.9 / 186.2 / 190.2 / 192.2 / 195.1 / 197 / 200.6 / 204.4 / 207.2 / 209.0 / (209) / (210) / (222)
87 / 88 / 89 / 104 / 105 / 106 / 107 / 108 / 109
Fr / Ra / Ac / Rf / Db / Sg / Bh / Hs / Mt
(223) / 226 / 227 / (261) / (262) / (263) / (264) / (265) / (268)
Choose the correct answer:
1- Perform the following experimental operation:
(67.323 - 67.1)(12.6 + 1.972) /3.1 =
a) 0.9 b) 1.0 c) 0.94 d) 1
2- Which of the following is an extensive property?
a) specific heat b) heat capacity c) boiling point d) molarity
3- The empirical formula of acetic acid, CH3COOH, is
a) CH3CO2H b) C2H4O c) C2H2O d) CH2O
4- An aluminum ion, Al3+, has:
a) 13 protons and 13 electrons b) 27 protons and 24 electrons
c) 16 protons and 13 electrons d) 13 protons and 10 electrons
5- One formula unit of Al2(SO4)3 contains
a) 8 oxygen atoms b) 4 oxygen atoms
c) 6 Aluminum atoms d) 12 oxygen atoms
6- How many oxygen atoms are in 51.4 g CaSO4 (F. Wt. = 136)?
(Avogadro’s No. = 6.022 x 1023).
a) 4 b) 9.10 x 1023 c) 2.28 x 1023 d) 6.022 x 1023
7- Ammonia boils at - 33.4oC. What is its temperature in Fahrenheit scale?
a) - 60.1oF b) - 92.1oF c) - 28.1oF d) - 18.5oF
8- In the combustion of a certain hydrocarbon 18.0 g of CO2 is produced, which represents
a 80% yield. What is the theoretical yield?
a) 14.4 g b) 8.1 g c) 22.5 g d) 22.0 g
9- Which of these elements is a transition element?
a) Ge b) F c) Cr d) Na
10- Calculate the mass of excess reagent remaining at the end of the reaction in which 90.0 g of SO2 are
mixed with 100.0 g of O2.
2SO2 + O2 2SO3
a) 11.5 g b) 22.5 g c) 67.5 g d) 77.5 g
11- The percent composition by mass of tartaric acid is: 32.01% C, 4.03% H, and 63.96% O.Given that the molecular mass of tartaric acid is 150 amu, determine its molecular formula
a) C2H3O3 b) H3C2O3 c) C4H6O6 d) C2H4O2
12- Which of the following processes is endothermic?
a) O2(g) + 2H2(g) 2H2O(g)
b) H2O(g) H2O(l)
c) 3O2(g) + 2CH3OH(g) 2CO2(g) + 2H2O(g)
d) H2O(s) H2O(l)
13- The symbol ΔHof[HNO3(l)] refer to?
a) H(g) + N(g) + O3(g) HNO3(l)
b) 1/2H2(g) + 1/2N2(g) + 3/2O2(g) HNO3(l)
c) HNO3(l) 1/2H2(g) + 1/2N2(g) + 3/2O2(g)
d) H2(g) + N2(g) + O3(g) HNO3(l)
14- Calculate ΔHorxn for the following reaction.
2H2O2(l) 2H2O(l) + O2(g)
Given ΔHof (H2O2(l)) = -187.6 kJ/mol ; ΔHof (H2O(l)) = -285.8 kJ/mol
a) 196.4 kJ b) -196.4 kJ c) 98.2 kJ d) -98.2 kJ
15- A gas is compressed in a cylinder by a constant pressure of 10 atm from a volume of 20 L to 2.0 L. Calculate the work done on the system.
Given 1 L·atm = 101.3 J.
a) 1.01 104 J b) -180 J c) 1.82 104 J d) -1.82 104 J
16- How many unpaired electrons does an atom of sulfur have?
a) 0 b) 1 c) 3 d) 2
17- Transition metal elements have atoms or ions with partially filled:
a) s subshells b) p subshells c) d subshells d) a and b
18- What is the electronic configuration of Cr ?
a) 1s2, 2s2, 2p6, 3s2, 3p6, 3d5, 4s1 b) 1s2, 2s2, 2p6, 3s2, 3p6, 3d6
c) 1s2, 2s2, 2p6, 3s2, 3p6, 3d4, 4s2 d) None of the above
19- What is the four quantum numbers of the electron in the outermost orbital of K atom?
a) n = 4; l = 0; ml = 0; ms = 1/2 b) n = 4; l = 0; ml = 1; ms = 1/2
c) n = 4; l = 1; ml = 0; ms = 1/2 d) n = 4; l = 1; ml = 0; ms = 1/2
20- Which pair of elements would be most likely to form an ionic compound?
a) Cl and I b) Al and K c) Cl and Mg d) C and S
21- Which of the following bonds has the greatest polarity (highest percent ionic character)?
a) Si ─ P b) Si ─ S c) Si ─ Cl d) Si ─ I
22- What is the formal charge on the oxygen atom in N2O, which has two double bonds?
a) 0 b) +1 c) -1 d) -2
23- Which one of the following compounds does not follow the octet rule?
a) NF3 b) CF4 c) PF5 d) AsH3
24- Which one of the following substances should exhibit hydrogen bonding in the liquid state?
a) PH3 b) H2S c) CH4 d) CH3OH
25- Which of the following liquids should have the highest viscosity at the same temperature?
a) CH3OCH3 b) HOCH2CH2OH c) C2H5OH d) CH2Cl2
26- Which of the following substances would be expected to have the highest vapor pressure at room temperature?
a) ethanol bp = 78oC b) methanol bp = 65oC
c) water bp = 100oC d) acetone bp = 56oC
27- The solubility of CO2 gas in water:
a) increases with increasing temperature. b) decreases with decreasing temperature.
c) decreases with increasing temperature. d) decreases with increasing gas pressure.
28- Calculate the amount of heat that must be absorbed by 10.0 g of ice at -20oC to convert it to liquid water at 61.0oC.
Given: Specific heat (ice) = 2.1 J/g oC, Specific heat (water) = 4.18 J/g oC, DHfus = 6.0 kJ/mol
a) 420 J b) 2900 J c) 6300 J d) 63 kJ
29- Arrange the following in order of increasing boiling point: RbCl, CH3Cl, CH3OH, CH4.
a) CH3OH < CH4 < CH3Cl < RbCl b) RbCl < CH3Cl < CH3OH < CH4
c) CH4 < CH3OH < CH3Cl < RbCl d) CH4 < CH3Cl < CH3OH < RbCl
30- Which of the following characteristics indicates the presence of weak intermolecular forces in a liquid?
a) a high heat of vaporization b) a high critical temperature
c) a high vapor pressure d) a high boiling point
31- When sugar is dissolved in water, the resulting solution
a) has a higher boiling point than pure water.
b) has a higher freezing point than pure water.
c) has a higher conductivity than pure water.
d) None of the above
32- Which of the following compounds will be soluble in CCl4?
a) NaCl b) H2O c) NaOH d) C8H18
33- The vapor pressure of water at 20oC is 17.5 mmHg. What is the vapor pressure of water over a solution prepared from 200 g of sucrose (M.Wt = 342) and 350 g water (M.Wt = 18)?
a) 17.0 mm Hg b) 16.0 mm Hg c) 0.51 mm Hg d) 18.0 mm Hg
34- A solution of a non-electrolyte, X, contains 84 g per kg of water and freezes at –1.46 °C. What is the molar mass of X? Kf for water = 1.86 °C/m
a) 228 g/mol b) 107 g/mol c) 66 g/mol d) 0.32 g/mol
35- What is the molarity of a solution that is 26.0 % by mass phosphoric acid (H3PO4) and that has a density of
1.155 g/mL?
a) 2.30 10 ─ 3 M b) 0.30 M c) 2.30 M d) 3.06 M
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