CHEM 1411 Sample Final Exam
Name:
Score
Part I. Multiple choice questions. ( 2 points each)
Direction- Please bubblr your correct choice in scantron.
1. Perform the following calculations and round off the answers to the proper
significant figures
0.3614 x 2.75 =
A. 0.99385
B. 0.994
C. 0.99
D. 1.00
2. Which of the following expressed measurement 75,030.2 m in correct
scientific notation?
A. 7.50302x104 m
B. 7.503x104 m
C. 7.50x104 m
D. 7.5x104 m
3. What are the atomic number, Mass number, and number of electrons in
109Ag+?
A. 47, 109, 46
C. 109, 156, 156
B. 109, 47, 47
D. 47, 109, 47
4. What are the correct symbols for the elements (1) copper and (2) cobalt?
A. Co, CO
B. Cu, Cb
C. Cp, Cb
D. Cu, Co
5. How many nitrogen atoms are in 175 molecules of Cu(NO3)2
A. 800
B. 200
C. 350
D. 400
6. What is the equivalent of 130 K in degrees Fahrenheit?
A. - 225
B. - 200
C. 328
D. 54
7. Which of the following atoms has mass number 17, proton number 8,
neutron number 9, electron number 10
A.
35
17Cl
(-1 charge) B. 8O17 (-2 charge) C. 8O18 (-2 charge) D. 8O17
8. How many moles are in 112 g of anesthetic ethyl chloride (C2H5Cl)
A. 0.578
B. 1.74
C. 2.14
D. 1.12
9. How many grams of copper can be produced from 160 g of CuO
A. 32 g
B. 200 g
C. 128 g
D. 80
10. The empirical formula of a compound is C2H4O, and the weight of
1 mole of that compound is 88 g. What is its molecular formula?
A. C2H4O
B. C4H8O2
C. C6H12O3
D. C8H16O4
11. Molecules that undergo complete dissociation to form OH- in water are
called
A. Weak acid
C. Strong acid
B. Strong Base
D. Weak Base
12. A 100 ml solution is made by dissolving 890 mg of NaCl salt in Water.
What is the concentration of solution?
A. 0.015 M
B. 0.15 M
C. 1.5 M
D. 15 M
13. How many grams of NaCl are in 500.0 ml of a 5.000M solution?
A. 292.5 g
B. 29.25 g
C. 146.25 g
D. 14.6 g
14. The molarity of chloride ion, Cl-(aq), in 100.0mL of 1.00 M Aluminum
chloride, AlCl3, solution is:
A. 3.00 M
B. 1.00 M
C. 2.00 M
D. 10.00 M
15. What is the oxidation number of Cr in Cr2O72− ion
A. +2
B. + 7
C. + 6
D. − 6
16. In the following reaction which element is reduced?
NaI + 3HOCl  NaIO3 + 3HCl
A. Cl
B. I
C. O
D. Na
17. How many kJ of heat must be absorbed by 2 kg of water (specific
heat 4.184 J /g. °C ) to raise the temperature from 18.0°C to
30.0°C?
A. 2.5x10-2 kJ
B. 100 kJ
C. 100416 kJ
D. 2500 kJ
18. The heat of combustion of fructose, C6H12O6, is -2812 kJ/mole. Using
the following information, c
f for fructose.
C6H12O6 (s) + 6 O2(g)
 6 CO2(g) + 6 H2O (l)
ΔH°f ( CO2 ) = -393.5 KJ/mole
A. -210.3 kJ
B. 210.3 kJ
ΔH°f (H2O) = - 285.83 KJ/mole
C. -1264 kJ
D. 1264 kJ
19. Considering the following reaction,
ΔH˚ = 1430 kj
2CO2(g) + 3H2O(g)  C2H6(g) + 7/2 O2
What is the enthalpy change for the reaction if whole number
Coefficients are used?
A. 1430 kJ
B. -1430 kJ
C. -2860 kJ
D. 2860 kj
20. Use the information shown for equations 1 and 2 to determine the value
of ΔH˚ (in Kj) for equation 3.
1. 2S (s) + 3O2 (g) --------> 2SO3 (g) ΔH˚ = -790 Kj
2. S (s) + O2 (g) --------------> SO2 (g) ΔH˚ = - 297 Kj
3. 2SO2 (g) + O2 ---------------> 2SO3 (g) ΔH˚ = ?
A. −196 kj
B. 493 kj
C. −493 kj
D. 196 kj
21. 2CO (g) + O2 (g) ----> 2CO2 (g)
The value of heat exchange ΔH˚ for the above reaction is -482 Kj.
What the amount of heat (kj) exchanged when 12.5 g of CO ( g)
Completely reacts?
A. 107.6 kj
B. -3012.5 kj
C. -107.6 kj
D. non
22. What is the frequency of radiation that has a wavelength of
0.589 pm? (C = 3 x 108 m)
A. 1.96 x 10-21 s-1
B. 5.09 s-1
C. 5.09 x 108 s-1 D. 5.09 x 1020 s-1
23. What is the maximum number of electrons that can occupy the
subshell 4f?
A. 1
B. 3
C. 14
D. 10
24. The most stable electron configuration for the atom Cr, using the
appropriate noble-gas inner core for abbreviation is
A. [Ar]4s23d4
B. [Ar]4s24d4 C. [Ar]4s13d5 D. [Kr]4s13d6
25. Metallic character from right to left across a period of the periodic table:
A. Increases
B. Decreases
C. No change
D. non
26. Which element from the following has the greatest electronegativity?
A. F
B. Cl
C. Br
d) I
27. Determine the total number of sigma and pi bonds in the
following molecular structure.
H
O
H
H
H
H
H
A. 4 σ, 14 π
C. 14 σ , 4 π
B. 8 σ, 4π
D. none of these
28. Which one violates octet rule stability ?
A. S2-
B. Mg2+
C. O-
D. Fr+
29. What is the formal charge on sulfur in the following molecule?
O
H
O
S
O
H
O
A. +3
C. – 1
B. +2
D. 0
30. The electron-pair geometry and molecular geometry of
ammonia are ------ respectively
A. tetrahedral,tetrahedral
B. tetrahedral, trigonal planar
C. trigonal planar, trigonal planar
D. tetrahedral, trigonal pyramidal
31. How many moles of N2 gas occupy 33.6 liters volume at STP
condition?
A. 1.0 mol
B. 2.0 mol
C. 1.5 mol
D. cannot be determine
32. An unknown gas "X" effuses four times faster than a sample of
O2(g) through a porous container. Which of the following is the
unknown gas ?
A. H2
B. CH4
C. He
D. NO
33. What volume of air at 760 torr would have to be put into a car tire with a
volume of 15 L if the pressure in the car tire is to be 2.38 atm?
A. 6.3 L
B. 35.7 L
C. 0.05 L
D. 21.3 L
34. Which of the following molecules can not form a hydrogen bond?
A. SiH4
B. C2H5OH
C. H2O
D. HF
35. Ice floats on water because of
A. High density due to London forces
C. Low density due to Hydrogen bonding
B. Surface tension
D. Covalent bonding
Part II. Show all your work for complete credit.( 5 points each)
1. A bullet is fired at a speed of 2435 ft/s. What is this speed expressed in
kilometers per hour? (hint: 1 m = 3.2 ft)
2. Given the following data, calculate the average atomic mass of copper
isotopes
isotopic mass(amu)
abundance(%)
Cu-63
62.93
69.09
Cu-65
64.93
30.91
3. The sedative, anticonvulsant drug Phenobarbital contains 62.06% carbon,
5.21% hydrogen, 12.06% nitrogen, and 20.67% oxygen. What is its empirical
formula?
4. Phosphoric acid can be prepared according to the following reaction
PCl5 + 4H2O ------------- H3PO4 + 5HCl
In one experiment, 0.360 mol of PCl5 was slowly added to 2.88 mol of water
(a). In this reaction which reactant, if either, was limiting reactant?
(b). How many moles of HCl were formed in the reaction.
5.
From the following heats of reaction,
N2(g) + 2O2(g)  2NO2(g)
ΔH˚ = +67.6 kJ
2NO(g) + O2(g)  2NO2(g)
ΔH˚ = 113.2 kJ
calculate the heat of the reaction
N2(g) + O2(g)  2NO(g)
6. A. 5.00 g of metal was heated to 100 ºC and plunged into 100 g of
water at 24.0 ºC. The temperature of the resulting mixture became
28.0ºC.
a. How many joules did the water absorb?
b. How many joules did the metal lose?
c. What is the heat capacity of the metal?
CHEM 1411
Instructor: Shamsuddin Shaikh
Answer Key
Part I.
1. B
2. A
3. A
4. D
5. C
6. A
7. B
8. B
9. C
10. B
11. B
12. B
13. C
14. A
15. C
16. A
17. B
18. C
19. D
20. A
21. C
22. D
23. C
24. C
25. A
26. A
27. C
28. C
29. D
30. D
31. C
32. A
33.B
34. A
35. C
Part II.
1.
2.
3.
4.
5.
6.
2739.37 KM/h
63.55 amu
C12H12N2O3
a. PCl5, b. 1.8 moles of HCl
+ 180.8 kj
a. 1673.6 j, b. 1673.6 j, c. 23.24 j/ºC