basic revision questions on calculation of moles and chemicals for industry

1. REVISION Manufactured substance in industry= the answers are on slideshow ppoint same topics
Name:…………………………………………………………..class………………………….teacher ………………..
1) Manufacture of sulphuric acid
Dry
Hot air oxygen Water
X
sulphur Sulphur Sulphur Oleum Sulphuric
dioxide trioxide acid
Stage 1 Stage 2 Stage 3
a) State the name of the process to manufacture sulphuric acid in industry ……………………………..
b) Sulphur is heated in air in stage 1. Write chemical equation ……………………………..
c) Stage 2 is the production of sulphur trioxide.
i) Write the equation ………………………………………………………………………….….
ii) State the conditions Temp………………….pressure………….catalyst ……………..….
d) Stage 3 is the production of sulphuric acid
i) State substance X ………………………………………..Write equation for the formation of oleum ………………………………………
ii) Oleum is mixed with water to form sulphuric acid. Write the equation
……………………………………………………………………………..
e) State 2 uses of sulphuric acid…………………………………………………………………………………………………………………………………….…
2) Manufacture of ammonia
Nitrogen + hydrogen Ammonia
a) State the name of the process to manufacture ammonia in industry ……………………………..
b) Write chemical equation …………………………………………………..
c) State conditions. Temp………………….pressure………….catalyst ……………..….
d) State 2 uses of ammonia in industry ……………………………………………………………………………
3) Fill in the table below
Alloy Mixture of metals Alloy Mixture of metals
Steel Bronze
Brass Magnelium
4) Fill in the table below

2. Name of polymer Structure of monomer Structure of polymer uses
polythene
Polyvinyl chloride
Polypropene
5) Which type of glass? Fill in the table below
Type of glass Uses Type of glass Uses
1.? Cheap glass containers, mirrors 3.? Optical lenses, spectrometer
2. ? Decorative glass and lamps 4. ? Cooking utensils
REVISION Chemical formulae and equation
1) Relative atomic mass of magnesium is 24. Explain this statement in terms of
i) Hydrogen standard ………………………………………………………………………………………………
ii) Carbon-12 standard………………………………………………………………………………………………………………………
2) If an atom W is 32 times heavier than 1/12 of the mass of 1 atom carbon -12, what is its relative atomic mass?
…………………………………………………………………………………………….
3) An atom of metal M is 1.6 times heavier than an atom of calcium. What is the relative atomic mass of M? ( Ca=40)
……………………………………………………………………………………………………………………………….
4) How many times a lead atom is heavier than a carbon atom? ( Pb= 207, C=12)………………………………………………………..
5) A compound has the formula of NaXO3. The relative molecular mass is 151. Find the relative atomic mass of X
(given RAM of Na, 23: O,16)
……………………………………………………………………………………………………………………………………………………………………..
6) What is meant by empirical formula and molecular formula? ……………………………………………………………………………….
………………………………………………………………………………………………………………………………………………………………………………………..

3. ………………………………………………………………………………………………………………………………………………………………………………….
7) Determine the empirical formula for substance below
substance Molecular formula Empirical formula substance Molecular Empirical formula
formula
a) benzene C6H6 b) Glucose C6H12O6
c) Propene C3H6 d) ammonia NH3
8) Metal X combines with 4.32 g of oxygen to form 13.68 g of metal oxide X. What is the empirical formula of the metal oxide?given
Ram O is 16
…………………………………………………………………………………………………………………………………………………………………………………………
9) The empirical formula of a compound is CH2. If its molecular formula is 56, what is its molecular formula?
……………………………………………………………………………………………………………………………………………………………………………
10) A compound contain 40% carbon, 53.3 % oxygen ,and the rest is hydrogen If the molar mass of the compound is 180, find
i) Empirical formula ………………………………………………………………………………………………………………………………………….
ii) Molecular formula ………………………………………………………………………………………………………………………………………
11) Complete the formula below
Mole = mass/ Mole = volume of gas / Mole = number of particles/
CuCO3
CuO + CO2
12) 6.2 gram
From the reaction above, calculate ( given RAM of Cu,64: C,12: O,16)
a) Mole of copper carbonate used ………………………………………………b) Mass of copper oxide formed ………………………………………………..
c) Volume of carbon dioxide released …………………………………………………
d) Number of molecules of carbon dioxide released …………………………………………………..

4. e) Number of atoms of carbon dioxide released ………………………………………………………………………………………………….END