Welcome to your chemistry 2006
| Element | H | He | b | C | N | O | F | Na | Mg | Al | Si | P | S |
| Z | 1 | 2 | 5 | 6 | 7 | 8 | 9 | 11 | 12 | 13 | 14 | 15 | 16 |
| A | 1.0 | 4.0 | 10.8 | 12.0 | 14.0 | 16.0 | 19.0 | 22.98 | 24.30 | 26.98 | 28.08 | 30.97 | 32.1 |
| Element | Cl | Ca | Cr | Mn | Fe | Ni | Cu | Zn | Ag | Cd | Xe | Pb |
| Z | 17 | 24 | 24 | 25 | 26 | 28 | 29 | 30 | 47 | 48 | 54 | 82 |
| A | 35.5 | 40.1 | 52.0 | 54.9 | 55.9 | 58.7 | 63.5 | 65.4 | 107.9 | 112.4 | 131.3 | 207.2 |
1.
Which of the following is NOT a conjugate acid-base pair?
2.
Which of the following is correct?
3.
Commercially, liquid vegetable oils are converted to solid fats such as margarine by:
4.
What is the chemical name for Aspirin?
5.
Which of the following statement(s) is (are) true of an ideal liquid-liquid solution?
6.
The unit cell in a certain lattice consists of a cube formed by an anion at each corner, an anion in the center, and a cation at the center of each face. How many cations and how many anions does the unit cell have?
7.
In a reaction, A + B → product, the rate is doubled when the concentration of B is doubled, and the rate increases by a factor of 8 when the concentrations of both the reactants (A and B) are doubled, the rate law for the reaction can be written as:
8.
. Answer the following question using the phase diagram below. At which point can only the solid and liquid phases coexist?
9.
Which electron transition in a hydrogen atom releases the largest energy?
10.
The simplest formula for a compound containing Mn4+ and O2- is
11.
What is the ratio of the energy of a photon of 300 nm wavelength radiation to that of 600 nm radiation?
12.
Which one of the following chemicals is used to disinfect water?
13.
During the titration of a known volume of a strong acid with a strong base, there is
14.
A solution with a PH of 7.5 would be described as:
15.
The electrolysis of molten NaCl is an industrial process. What does the electrolysis produce?
16.
Butane burns in oxygen according to the equation below. 2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O(l). If 11.6g of butane is burned in 11.6 g of oxygen, which is the limiting reagent?
17.
A beaker filled to the 100mL mark with salt (the salt has a mass of 100g) and another beaker to the 100mL mark with water (the water has a mass of 100g) are mixed together in a bigger beaker until the salt is completely dissolved. What will be the mass of the solution
18.
Which one of the following is NOT an intensive property?
19.
Which of the following is natural polymer?
20.
Which of the following metals forms a volatile compound during the extraction process?
21.
Which one of the following atoms in its ground state has the greatest number of unpaired electrons?
22.
Which statement is true about chemical reactions at equilibrium?
23.
Which compound contains both covalent and ionic bonds?
24.
Which set of quantum numbers (n, l, ml, ms) is not possible?
25.
Which of the following particles contains more electrons than neutrons? I. 11H II. 1735Cl- III. 3919 K+
26.
Which molecule or ion does NOT have a tetrahedral shape?
27.
Why are metals soft and malleable?
28.
In which region of the Periodic Table would the element with the electronic structure below be located? 1s22s22p63s23p63d104s24p64d65s2
29.
Which factors will influence the rate of the reaction shown below?
30.
How many π bonds are present in CO2?
31.
Which pair of monomers forms polyesters?
32.
Which changes will increase the amount of SO3(g) at equilibrium?
33.
Which compound is a carboxylic acid?
34.
The mechanism of a reaction is shown below.
35.
What is the equilibrium constant expression for the following reaction? 2Hg (g) + O2 (g) ⇄ 2HgO (s)
36.
A triacylglycerol that is solid at room temperature is called:
37.
Which compound is an ester?
38.
If a solute dissolves in an endothermic process,
39.
A solution is made by dissolving 250.0g of potassium chromate crystals (K2CrO4, molar mass, 194.2g) in 1.00kg of water. What will be the freezing point of the solution? (Kf for water is 1.860cm-1).
40.
How many moles of sodium hydroxide are present in 2.5L of 0.5M aqueous solution?
41.
Which species CANNOT act as a Lewis acid?
42.
Which of the following statements is true?
43.
Three acids, HA, HB, HC have the following Ka values.
44.
If the solute-solvent interactions are greater than the solute-solute and solvent-solvent interactions, what will be the total vapour pressure of the solution?
45.
Which of the following procedures will produces will produce a buffered solution?
46.
For which conversion is an oxidizing agent required?
47.
What volume of 0.500M NaOH is required to neutralize 25.0 mL of 1.2 MH2SO4? (Assume complete ionization of the acid).
48.
A gas is confined to a cylinder under constant atmospheric pressure. When the gas undergoes a particular chemical reaction, it releases 135kJ of heat to its surroundings and does 63kJ of P-V work on its surroundings. What are the values of ∆H and ∆E for the process?
49.
The oxidation numbers of nitrogen in NH3, HNO3 and NO2 are respectively.
50.
Which statement about the following reaction is correct? 2FeS (s) + 3CO2 (g) → Fe2O3 (s) + 3CO (g) ∆H0 = +26.6kJ
51.
Which of the following metals is extracted by thermal reduction process?
52.
The two standard electrode potentials involved in the nickel cadmium rechargeable cell are given below. Calculate the ?G0 in kJ of the cells.
53.
Which of the following is a synthetic rubber produced from caprolactam (CPL)?
54.
Which of the following reaction is NOT a redox reaction?
55.
The half-reaction for formation of magnesium metal upon electrolysis of molten MgCl2 is:
56.
An aqueous solution is 70% nitric acid (HNO3) by mass. What is the concentration of HNO3 expressed in molality?
57.
Which of the following is a natural polymer?
58.
What is the ionization energy of an iron atom if it requires a radiation of 276nm to completely remove its outer most electron in the gaseous state?
59.
Which of the electron configurations describes the ground state electron configuration of Cl-?
60.
When 0.68 is divided by 14.364, the actual answer is 0.0473405. What will be the correct answer?
62.
Which of the following molecules or ions will exhibit delocalized bonding? NO2-, NH4+, N3-
63.
Based on molecular orbital theory, the bond orders of H2, H2+ and H2- are , respectively.
64.
How many 3d electrons are present in the ground state of chromium atom?
65.
When the following substances are arranged in order of increasing melting point (lowest melting point first), the correct order is:
66.
The half-life for the first order decomposition of nitromethane, CH3NO2, at 500k is 650 seconds. If the initial concentration of CH3NO2 is 0.500M, what will its concentration be (M) after 1300 seconds have elapsed?
67.
In a zero-order reaction for every 100 rise of temperature, the rate is doubled. If the temperature is increased from 100C to 1000C, the rate of the reaction will become
68.
Which of the following mathematical relationships between K, K1 and K2 is correct?
69.
Which of the following gives the correct order of decreasing acidity of carboxylic acids?
70.
The value of Kc for the following equilibrium reaction is 4.0 at a temperature of 373k.
71.
Which one of the following is true about an open system?
72.
Which of the following statements is true about the percent ionization of a weak acid?
73.
What is the value of ∆H for the reaction S(s) → S(g)?
74.
Which of these compounds is the ester formed from the reaction of acetic acid and 1-Propanol?
75.
A lab instructor is preparing 5.0 liters of a 0.10M Pb(NO3)2 (molecular mass 331) solution. What is the mass required?
76.
Which of the following is NOT a characteristic of the electrolytic cell containing aqueous solution of NaCl used in the manufacture of sodium hydroxide?
77.
The kinetic data are for the reaction:
78.
Which of the following metals has the highest electrical and thermal conductivities of any metal?
79.
Which of the following is a linear polymer?
80.
Which of the following is the most important source for the extraction of iron?
