An organic compound has a vapour density of 22. The molecular formula of the organic compound is: [Atomic weight: C = 12, H = 1]

(a) CH₄

(b) C₂H₄

(c) C₂H₆

(d) C₃H₈

(a) State Avogadro’s Law. (b) Define Co-ordinate bond.

A gas cylinder can hold 150 g of hydrogen under certain conditions of temperature and pressure. If an identical cylinder with the same capacity can hold 450 g of gas ‘G’ under the same conditions of temperature and pressure, find: (a) the vapour density of the gas ‘G’. (b) the molecular weight of gas ‘G’.

40 cm3 of methane (CH4) is reacted with 60 cm3 of oxygen according to the equation: CH4 + 2O2 ⟶ CO2 + 2H2O All volumes are measured at the same temperature and pressure. What total volume of gas remains after the reaction at room temperature? (a) 60 cm3 (b) 40 cm3 (c) 45 cm3 (d) 50 cm3

State the terms for the following: (a) The group obtained by removing one hydrogen atom from the parent alkane. (b) Two metal plates or wires through which the current enters and leaves the electrolytic cell. (c) The amount of substance which contains the same number of units as the number of atoms in carbon-12. (d) The tendency of an atom to pull a shared pair of electrons towards itself in a compound. (e) The formula which represents the simplest ratio between the atoms of elements present in a compound.

Define / State: (a) Electronegativity. (b) Gay-Lussac’s law of combining volumes.

State the terms/process for the following: (a) The energy released when an atom in the gaseous state accepts an electron to form an anion. (b) Tendency of an element to form chains of identical atoms. (c) The name of the process by which Ammonia is manufactured on a large scale. (d) A type of salt formed by partial replacement of hydroxyl radicals with an acid radical. (e) The ratio of the mass of a certain volume of gas to the same volume of hydrogen measured under the same conditions of temperature and pressure.

Zn + 4HNO3 ⟶ Zn(NO3)2 + 2H2O + 2NO2 32.5 g of zinc reacts with concentrated nitric acid as given in the above equation. (a) How many moles of zinc was required in the reaction? (b) Find the mass of nitric acid needed to react with 32.5 g of zinc. (c) Find the volume of nitrogen dioxide liberated in (b). [Atomic weight: H=1, N=14, O=16, Zn=65]

Arrange the following according to the instructions given in brackets: (a) C2H2, C3H6, CH4, C2H4 (In the increasing order of the molecular weight) (b) Cu2+, Na+, Zn2+, Ag+ (The order of Preferential discharge at the cathode)

Equal volumes of ammonia gas and chlorine gas are kept in two different containers under the same conditions of temperature and pressure. Find the number of molecules contained in chlorine gas when the mass of ammonia is 34 g. [Atomic weight: Cl=35.5, H=1, N=14]

Complete the following sentences by choosing the correct option from the brackets: (a) The oxide that dissolves in caustic potash (KOH) is ............... . [ZnO / CuO] (b) The reaction that takes place at the anode during the electrolysis of molten lead bromide is ............... . [2Br − 2e− ⟶ 2Br− / 2Br− − 2e− ⟶ Br2] (c) The volume occupied by 8 grams of oxygen gas at STP is ............... litres. [5.6 / 8.96] [Atomic weight of O = 16] (d) ............... does not give hydrogen gas when it reacts with cold and very dilute nitric acid. [Cu / Mn] (e) ............... is a polar covalent compound. [HCl / CCl4]

5.6 litres of gas Z weighs 32 g at STP. What is the molecular weight and vapour density of Z?

Calcium carbonate reacts with dilute hydrochloric acid as given below: (a) What is the mass of 5 moles of calcium carbonate? (Relative molecular mass of calcium carbonate is 100) (b) How many moles of HCl will react with 5 moles of calcium carbonate? (c) What is the volume of carbon dioxide liberated at S.T.P. at the same time?