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Question 1 of 50
1. Question
A normal body temperature is 37 oC, Kw = 2.4 x 10-14. Calculate [H3O+] and [OH–] for the body fluid at this temperature.
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Question 2 of 50
2. Question
Atoms of elements in a group on the Periodic Table have similar chemical properties. This similarity is most closely related to the atoms.
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Question 3 of 50
3. Question
How many atoms of Cu are present in 35.4 g of Cu? [Cu = 63.5 gmol-1]
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Question 4 of 50
4. Question
How would you prepare 250 cm3 of 0.25 M aqueous solution of NaCl? [Na= 23 g mol-1; Cl = 35.5 g mol-1]
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Question 5 of 50
5. Question
What is the shape of PCl3?
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Question 6 of 50
6. Question
Uranium -233 (233U92) decays by α – emission. What is the decay product?
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Question 7 of 50
7. Question
Arrange the following ions in order of decreasing charge density Ca2+, Mg2+, Al3+ and Ba2+
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Question 8 of 50
8. Question
Which of the following statements explain why caesium has a lower melting point than sodium?
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Question 9 of 50
9. Question
Transition metals can form complex ions because:
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Question 10 of 50
10. Question
How many equivalent hybrid orbitals are there in Sp2-hybridised carbon?
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Question 11 of 50
11. Question
When common names are used for acids, the underlined carbon atom in the molecule shown would be designated as the ________ C atom.
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Question 12 of 50
12. Question
Purification of a strip of impure copper metal in aqueous CuSO4 was carried out using a steady current. Which graph shows the change in mass of the cathode with time?
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Question 13 of 50
13. Question
Which gas closely approaches ideal behaviour at room temperature and pressure?
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Question 14 of 50
14. Question
A sample of a brown gas, a major air pollutant, is found to contain 2.34 g N and 5.34g O. Determine the empirical formula for this substance. [N = 14, O = 16]
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Question 15 of 50
15. Question
Why does the rate of a gaseous reaction increase when the pressure is increased at a constant temperature?
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Question 16 of 50
16. Question
Why is gaseous nitrogen less reactive than gaseous fluorine?
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Question 17 of 50
17. Question
The first stage in the manufacture of nitric acid is the oxidation of ammonia by oxygen.
wNH3(g) + xO2(g) → yNO(g) + zH2O(g)
What values for w, x, y and z are needed to balance the equation?
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Question 18 of 50
18. Question
The reaction of chlorine with methane is carried out in the presence of light. What is the function of the light?
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Question 19 of 50
19. Question
In the Solvay process, NaCl(aq) + NH3(g) + H2O(l) + CO2(g)   →       NaHCO3(s) + NH4Cl(aq)
What volume of carbon dioxide (at s.t.p) is required to produce 1.00 kg of sodium hydrogencarbonate? (I mole of gas at s.t.p occupies 22.4 dm3) [Na = 23, Cl = 35.5, C = 12,O=16,H=1,N=14]
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Question 20 of 50
20. Question
Which group of particles is in order of increasing size?
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Question 21 of 50
21. Question
River water in a chalky agricultural area may contain Ca2+, Mg2+, CO32-, HCO3–, Cl–, NO3– In a waterworks, such water is treated by adding a calculated quantity of calcium hydroxide. What will be precipitated following the addition of calcium hydroxide?
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Question 22 of 50
22. Question
The electronic configuration of the Fe3+ ion is ______________
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Question 23 of 50
23. Question
An element with an atomic number of 35 is _____ block element.
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Question 24 of 50
24. Question
Iodine trichloride, ICl3, is made by reacting iodine with chlorine.
By using the data above, what is the enthalpy change of the formation for solid iodine trichloride?
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Question 25 of 50
25. Question
The standard enthalpy changes of formation of TiO2(s) and CO(g) are –940 kJmol–1 and -110 kJ mol–1Â
respectively. TiO2(s) + 2C(s) → Ti(s) + 2CO(g)
What is the standard enthalpy change of this reaction?
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Question 26 of 50
26. Question
The standard enthalpy changes of formation of HCl and HI are –93 kJ mol–1 and +25 kJ mol–1 Which statement is most important in explaining this difference?
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Question 27 of 50
27. Question
What is the catalyst used in the Contact process?
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Question 28 of 50
28. Question
The main purpose of adding cryolite to the ore (bauxite) during the preparation of aluminium metal by electrolysis is?
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Question 29 of 50
29. Question
What type of bond needs to be broken for magnesium oxide to melt?
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Question 30 of 50
30. Question
A substance that contains the following elements by mass: C, 17.8%; H, 1.5%; Cl, 52.6%; F, 28.1% has molecular mass of 135. Determine the molecular formula.
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Question 31 of 50
31. Question
How many chiral centres does the compound below possess? CH2CO2H C(OH)CO2H CH2CO2H
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Question 32 of 50
32. Question
200 mol of a hydrocarbon undergoes complete combustion to give 35.2 g of carbon dioxide and 14.4 g of water as the only products. What is the molecular formula of the hydrocarbon?
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Question 33 of 50
33. Question
One of the original postulates of Dalton’s Atomic Theory is:
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Question 34 of 50
34. Question
The ions in a mass spectrophotometer are separated based on their mass:charge ratio by the
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Question 35 of 50
35. Question
Which of the following terms accurately describes the energy associated with the process: Li (g)→Li+(g) + e–
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Question 36 of 50
36. Question
If the activation energy in the forward direction of an elementary step is 52 kJ and the activation energy in the reverse direction is 74 kJ, what is the energy of reaction E for this step?
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Question 37 of 50
37. Question
Sodium peroxide dissolves in water in accordance with the following reaction:
The pH of the solution after reaction will be:
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Question 38 of 50
38. Question
Gunpowder is a mixture of saltpetre, sulphur and wood charcoal in the ratio of 6:1:1 by mass. The mixture burns with explosion because it produces a large volume of gases. Saltpetre in the mixture acts as:
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Question 39 of 50
39. Question
The oxidation state of Au in K[Au(OH)4] is:
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Question 40 of 50
40. Question
The most common type of chemical reaction which alkanes undergo is
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Question 41 of 50
41. Question
The boiling point of water is higher than that of methanol because
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Question 42 of 50
42. Question
In the Rutherford scattering experiment, Rutherford bombarded a thin piece of gold foil with a beam of _____
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Question 43 of 50
43. Question
When azimuthal quantum number (l = 2), what set of orbitals is designated?
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Question 44 of 50
44. Question
Sodium hydroxide is an Arrhenius base because it contains ________
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Question 45 of 50
45. Question
The standard state of an element or compound is determined at a pressure of and a temperature of _______
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Question 46 of 50
46. Question
Which of the following is a state function?
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Question 47 of 50
47. Question
The method that cannot be used for removing permanent hardness of water is _______
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Question 48 of 50
48. Question
In which of the following characteristics does hydrogen resemble halogens?
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Question 49 of 50
49. Question
Which alkali metal react directly with Nitrogen to form nitride?
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Question 50 of 50
50. Question
The isomerism which exists between CH3CHCI2 and CH2CI. CH2CI is _________
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