What mass of water is produced when 8.0g of hydrogen reacts with excess oxygen? [H = 1, O = 16]

• A. 36.0g
• B. 8.0g
• C. 72.0g
• D. 16.0g

Chlorine atom forms CI by

• A. losing one electron
• B. Sharing one electron
• C. Donating lone pair of electrons
• D. Gaining one electron

0.25 mole of hydrogen chloride was dissolved in distilled water and the volume made up of 0.50 dm³. If 15.0 cm³ of the solution requires 12.50 cm³ of aqueous sodium trioxocarbonate (IV) for neutralization, calculate the concentration of the alkaline solution

• A. 0.30 mol dm³
• B. 0.40 mol dm³
• C. 0.50 mol dm³
• D. 0.60 mol dm³

Which of the following alkanes has a straight-chain structure?

• A. Cyclopentane
• B. Isobutane
• C. Butane
• D. Pentane

What volume of oxygen at s.t.p is required to burn completely 7.5 dm3 of methane according to the following equation? CH₄ g + 2O₂ g → CO₂ g + H₂Og

• A. 3.75 dm³
• B. 7.59 dm³
• C. 15.0 dm³
• D. 30.0dm³

Duralumin consists of aluminum, copper?

• A. Zinc and Gold
• B. Lead and Manganese
• C. Nickel and Silver
• D. Manganese and Magnesium

(i) Name two amorphous forms of carbon

(ii) State the reason why graphite is a lubricant but diamond is not.

(iii) Draw and label a diagram for the laboratory preparation of a dry sample of carbon (IV) oxide.

(b)(i) Give one example of the following: I. Soil pollutant; II. Water pollutant; III. Air pollutant.

(ii) State the major use of sulphur (IV) oxide in a chemical industry.

(c)(i) Explain in terms of the kinetic theory why petrol is volatile

(ii) State two criteria for determining the purity of a substance.

(iii) Mention one use of each of the following gases: I. Krypton; II. Argon

(d)(i) When zinc metal was added to aqueous copper (I) tetraoxosulphate (VI), the solution turned colourless. I. Name the compound in the colourless solution. II. Write the ionic equation for the reaction. Ill. State what would be observed when a few drops of sodium hydroxide solution is added to a portion of the colourless solution.

(ii) Calculate the volume of CO\(_2\) produced when 5.3g of Na\(_2\)CO\(_3\) reacted with excess HNO\(_{3(aq)}\) + Na\(_2\)CO\(_3\) + 2HNO\(_{3(aq)}\) \(\to\) 2NaNO\(_{3(aq)}\) + CO\(_{2(g)}\) + H\(_2\)O\(_{(l)}\) [H = 1, C = 12, N = 14, O = 16, Na = 23, 1 mole of a gas occupies 22.4 dm\(^3\) at s.t.p.]

An element X has isotopic masses of 6 and 7. if the relative abundance is 1 to 12.5 respectively, what is the relative atomic mass of X?

• A. 6.0
• B. 6.1
• C. 6.9
• D. 7.0

The ratio of the number of molecules in 2g of hydrogen to that in 16g of oxygen is

• A) 2:1
• B) 1:1
• C) 1:2
• D) 1:4

An example of an acidic oxide is

• A) NO
• B) CO
• C) SO2
• D) CuO