Welcome to your chemistry 2010
2.
The reaction between alcohols and acyl chlorides produces
3.
Which one of the following aqueous solutions will have the LOWEST freezing point?
4.
When a student draws a plausible Lewis structure for hydrazine molecule (N2H4), how many lone pair of electrons are available?
5.
Who used the cathode Ray tube to discover the electron and determine its charge to mass ratio?
6.
Compounds that contain the carboxyl (carbonyl and hydroxyl) group are said to be:
7.
The main ore of lead is called:
8.
During nitrification, bacterial convert into
9.
Which one of the following metals exists in a free state?
10.
A ___ ∆H corresponds to an ___ process.
11.
Which of the following is NOT both a Bronsted-Lowry acid and a Bronsted-Lowry base?
12.
Chlorine has an oxidation number of +5 in:
13.
What is a measure of the closeness of a measurement to its true value?
14.
The monomer of neoprene is:
15.
What is the sum of 3.72 x 108 and 4.62 x 107 to the correct significant figure?
16.
Which of the following is a natural polymer?
17.
When a sodium chromate Na2CrO4 solution is acidified, it is converted to:
19.
Which quantum number is used to be determine sub shells?
20.
The maximum kinetic energy of a photoelectron emitted from a metal is 1.03 x 10-19J when light that has a 656 nm wavelength shines on the surface. What is the threshold frequency for this metal?
21.
What is the maximum number of electrons in an atom that can have the principal quantum number n = 4?
22.
Which of the following questions expresses de Broglie's hypothesis?
23.
What skill is a scientist using when he/she listens to the sounds that animals make?
24.
Which of the following is fundamentally different from the others?
25.
What is (are) the bond angle (s) in SF6?
26.
The number of resonance structures for CO3-2 are:
27.
In the following equation, what type of hybridization change, if any occurs at the Xe atom? XeF2(s) + F2(g) → XeF4(s)
28.
Which of the following compounds does NOT contain an ionic bond?
29.
Which of the following statements about oxygen and fluorine is NOT correct?
30.
What will be the charges on the ions formed when silicon reacts with nitrogen?
31.
The equilibrium constant for the ionization of HCN is 4.9 x 10-10
32.
The rate equation for the decomposition of nitramide, H2NNO2 → N2O + H2O is rate = k[H2 NNO2][H+]-1 which of the following mechanisms is consistent with this rate equation?
33.
Given the equilibrium constant values:
34.
Which of the following factors does NOT affect the rate of a chemical reaction?
35.
If a reaction is zero order in A, tripling the concentration of A will cause the reaction rate to:
36.
The phrase "like dissolves like" refers to the fact that:
37.
An ester has the structural formula shown below. On hydrolysis, the ester would produce
38.
You are given a bottle of solid x and three aqueous solutions of Y, the first saturated the second unsaturated and the third supersaturated. Which of the following is correct, if you add a small amount of the solid solute to each solution?
39.
Consider the following equilibrium:
40.
For a certain gas phase reaction
41.
Which of the following compounds would be the most soluble in H2O?
42.
A 0.2M solution of a weak acid HA is 1% ionized at 250CKa for the acid is equal to:
43.
What species of ions are present in a 0.1M solution of HCl and what will be their equilibrium concentrations?
44.
A solution in which prop ionic acid is 0.94% ionized has a PH of 2.85. What is the value of the acid ionization constant (Ka) for prop ionic acid?
45.
Commercial concentrated sulphuric acid (density = 1.831gcm-3) is 94.0% H2SO4 by mass. What is the normality of H2)
46.
2.3g of ethanol (CH3CH2OH) is added to 500g of water. What is the molality of the resulting solution?
47.
A 0.5L and 0.1 MHNO3 solution is to be prepared by dilution process form a 13M nitric acid. How many ml conc. HNO3 and how many ml of water are required to prepare the dilute solution?
48.
During the electrolysis of CuSO4(aq) using carbon electrodes, which of the following is the correct half reaction for the anode electrode?
49.
During the electrolysis of a concentrated aqueous solution of NaCl, what substance is formed at the cathode?
50.
In a voltaic cell, electrons flow from the___________ to the __________
51.
What is the PH of a mixture of 15.0ml of 0.126M NaOH and 21.0M H2SO4?
52.
Which of the following statement is true?
53.
What is final temperature when 150.0ml of water at 90.00C is added to 100.0ml of water at 30.00C?
54.
Which of the following correctly lists electromagnetic waves in order from shortest to longest wavelength?
55.
The relationship between Pico meter (pm) and nanometre (nm) is:
56.
What would be the wavelength of a radio wave having a frequency of 3 MHz?
57.
The process of vulcanization of rubber makes it
58.
Which of the following is NOT the decomposition product of HNO3?
59.
The determine the volume of an irregularly shaped glass vessel, the vessel is weighed empty (121.3g) and when filled with CCl4 (283.2g). What is the volume capacity of the vessel, given that the density of CCl4 is 1.59g/cm3?
60.
The diagram below shows the range of energies of collision of a collection of reactants at two temperatures, T1 and T2. Which of the following is true regarding T1 and T2?
61.
For the reaction C6H14(g) → C6H6(g) + 4H2(g), ∆p(H2)/∆t was found to be 2.5 x 10-2 atm/s, where ∆p(H2) is change in the pressure of hydrogen. Determine ∆p(H6H14)/∆t in units of atm/s for this reaction at the same time.
62.
The decomposition of a compound at 4000C is first order with a half - life of 1570 seconds what fraction of an initial amount of the compound remains after 4710 seconds?
63.
Given the following AFn species, BF3, BeF2, CF4, NF3, OF2. What is the correct order of F - A - F bond angles?
64.
From CO2, H2O, BeCl2 and N2O which have the same molecular geometry?
65.
How many electrons are present in the σ2p molecular orbital of N2+?
66.
A solution of NH4Cl made by dissolving 3.16g NH4Cl in 30.14g H2O has a density of 1.0272g cm-3. What is the mole fraction of NH4Cl?
67.
Which of the following is true regarding the solution formation process?
68.
What volume of 1.40M H2SO4 solution is needed to react exactly with 10.0g of aluminium according of the following reaction?
69.
Which of the following statements is NOT true in relation to the triple point on a single component phase diagram?
70.
Consider the following equilibrium:
71.
Which acid is produced when toluene is subjected to KMnO4 oxidation?
72.
Which of the following statement is true?
73.
Calculate ∆H for the following reaction using the bond energies given below H - H(g) + I - I(g) → 2H - I (g) bond energies: H - H = 436KJ/mol, I - I = 151KJ/mol, H - I = 297KJ/mol
74.
How long has a current of 3 ampere to be applied through a solution of silver nitrate to coat a metal surface of 80cm2 with 0.005cm thick layer? Density of silver = 10.5gcm-3
75.
Which of the following is an organic acid?
76.
What is the freezing point of a 0.1m solution of NaCl (in 0C)? KT = 1.860C/m and the freezing point of pure water is (0C)
77.
During a titration what volume of 0.500M KOH is necessary to completely neutralize 10.0ml of 2.00M CH3COOH?
78.
What is the standard cell potential of the oxidation of ammonia, given below?
79.
Two electrolytic cells were placed in series, one of AgNO3 and the other of CuSO4. If 1.273g Ag is deposited, how much Cu was deposited, how much Cu was deposited at the same time?
