1. sulphur Sulphur dioxide Sulphur trioxide OleumSulphuric acidStage 1 Stage 2 Stage 3 Hot airDry oxygenXWater

2.

State the name of the process to manufacture sulphuric acid in industry

Sulphur is heated in air in stage 1. Write chemical equation

CONTACT PROCESS 3.

Stage 2 is the production of SO3.

Write the equation

State the conditions

Temp.pressure.catalyst

450-550 oC 1 atm VANADIUM PENTOXIDE 4.

Stage 3 is the production of sulphuric acid

State substance X

Write equation for the formation of oleum

Oleum is mixed with water to form sulphuric acid. Write the equation

Concentratedsulphuric acid 5. State 2 uses of sulphuric acid As Fertilisers As detergents Electrolyte in car batteries Manufacture of plastic and synthetic fibres Manufacture of pesticides 6.

Nitrogen +hydrogenAmmonia

State the name of the process

Write chemical equation

State conditions.

CONTACT PROCESS 7. State 2 uses of ammonia in industryManufacture fertilisers Manufacture explosives Manufacture nitric acidAs a cooling agentPrevent coagulation of latex 8. Fe + Cu Cu + Zn Cu + Sn Al + Mg Alloy Mixture of metals AlloyMixture of metals Steel Bronze Brass Magnelium 9. Plastic bag Name of polymerStructure monomer Structure polymer uses Polythene 10. Raincoat, pipes Name of polymerStructure monomer Structure polymer uses Polyvinyl chloride 11. Plastic chairs & tables Name of polymerStructure monomer Structure polymer uses Polypropene 12. Soda lime glass Lead glass Fused silicate glass Borosilicate glass Type of glass UsesType of glass UsesCheap glass containers, mirrors Optical lenses, spectrometer Decorative glass and lamps Cooking utensils 13. Relative atomic mass of magnesium is 24

Explain in terms of hydrogen standard

Explain in terms of carbon-12standard

14.

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?

32 15.

An atom of metal M is1.6times heavier than an atom of calcium. What is the relative atomic mass of M? ( Ca=40)

1.6 x 40=64 16.

How many times a lead atom is heavier than a carbon atom?

( Pb= 207, C=12)

207 / 12= 17.25 17.

A compound has the formula of NaXO 3 . The relative molecular mass is 151. Find the relative atomic mass of X (given RAM Na,23: O,16)

151 23 3(16) = 80 18.

What is meant by empirical formula and molecular formula?

Empirical formula is the simplest formula that shows s implest ratio of atomsin a molecule

Molecularformula is the real formula that showsactual number of atomsin a molecule

19. substance Molecular form Empirical form substance Molecular form Empirical form benzene Glucose 20. substance Molecular form Empirical form substance Molecular form Empirical form Propene ammonia 21.

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 X?[ RAM X, 52; O,16]

Mass of X = 13.68 -4.32 g =9.36 g Mole of X= 9.36/52 =0.18 Mole of O = 4.32/16 =0.27X: O 0.18 : 0.27 18: 27X: O 2: 3 22.

The empirical formula of a compound is CH 2 . If its molecular formula is 56, what is its molecular formula?

23.

A compound contain 40% carbon, 53.3 % oxygen ,hydrogen 6.7%.If the relative atomic mass of the compound is 180, find

Empirical formula

Mole of carbon= 40/12 =3.33 Mole of O = 53.3/16 =3.33C: O: H 3.33: 3.33 : 6.7 1:1:2C: O :H 1:1 :2 Mole of H = 6.7/1 =6.7 24.

If the relative atomic mass of the compound is 180, findMolecularformula

25. Mole =mass Mole =volume of gasMole =number of particles Molar mass Molar volume Avogadros constant 26.

Given that RAM Cu=64, C=12, O=16)

Moleof copper carbonateused

CuCO 3 6.2 gram CO 2CuO+ Mole= mass/ mmass Mole= 6.2/ 124 Mole= 0.05 27.

Mass of copper oxideformed

CuCO 3 6.2 gram CO 2CuO+ Mass= mole x mmass Mass= 0.05 x CuO = 0.05 x 80 = 4 g From the equation,CuCO3 :CuO 1:1 0.05 : 0.05 28.

Volume of carbon dioxidereleasedat room conditions

CuCO 3 6.2 gram CO 2CuO+ Volume of gas = mole x mvolumevolume= 0.05 x 24= 1.2 dm3 From the equation,CuCO3 :CO2 1:1 0.05 : 0.05 29.

Number ofmoleculesof carbon dioxide released

CuCO 3 6.2 gram CO 2CuO+ Mole of carbon dioxide = 0.05 No of molecules = mole x NA No of molecules = 30.

Number ofatoms of carbon dioxide released

CuCO 3 6.2 gram CO 2CuO+ No of atoms = 3 x no of molecules No of atoms =