Study the information in the table below and answer the questions that follow. (The letters do not represent the actual symbols of the elements)

Select the element which is

(a) Likely to be in group II of the periodic table            (1mk)

(b) Could be used to make electric cables.        (1mk)

(c) Likely to be graphite.                   (1mk)

Study the experiment set-up below and answer the questions that follow.

State the observations made after heating in             

(i) Test tube A            (1mk)

(ii) Test tube B.       (1mk)

(iii) Write the equation for the reaction that take place in tube B.       (1mk)

Excess carbon (II) oxide gas was passed over heated sample of an oxide of iron. Study it and answer the questions that follow:

Mass of empty dish = 10.98g

Mass of empty dish + oxide of iron = 13.14g

Mass of empty dish + Residue = 12.66g

Determine the simplest formula of the oxide of iron.   (Fe = 56 , O = 16)              (3mks)

Calculate the number of hydrogen ions in 5cm³ of 0.5M phosphoric acid.    (L = 6.0 x 10²³)       (3mks)

A metal Y with atomic number 11 burns in chlorine to produce a white solid X.

(a) Describe the following properties of X.

i) Solubility         (1mk)

ii) Electrical conductivity.         (1mk)

(b) Write an equation to show the formula of X            (1mk)

(a) Define Graham’s law of diffusion           (1mk)

(b) 60cm³ of oxygen gas diffused through porous partition in 50 seconds. How long would it take for 60cm³ of Sulphur (IV) oxide gas to diffuse through the same partition under the same condition?   (S = 32.0 , O = 16.0)                                       (2mks)

A student reacted Silver Nitrate and Barium chloride solutions to prepare two salts.

(a) Write an equation for the reaction that took place         (1mk)

(b) Write the ionic equation for the reaction.         (1mk)

(c) Name the method above used in preparing salts mentioned.       (1mk)

A fixed mass of a certain gas has a volume 96cm³ at 69⁰C and 700mmHg Pressure. Find the volumethe gas would occupy at s.t.p.             (3mks)

20.0cm³ of NaOH solution containing 8.0gdm^-3  were required for complete neutralization of 0.118g of a dibasic acid. Calculate the Relative Molecular Mass (R.M.M) of the acid.    (Na = 23 , O = 16 , H = 1)                 (3mks)

0.28g of iron burns in air to form Iron (II) Oxide. Calculate the mass of Iron (II) Oxide formed (O = 16 , Fe = 56)         (3mks)