The Empirical formula of an organic compound is CHCl2. If its relative molecular mass is 168, what is its molecular formula? [At. Wt. C = 12, H = 1, Cl = 35.5]

Which of the following occupies 22.4 L at STP? (1) 32 g of O₂ (2) 2 mol of H₂ (3) 6.022 × 10²³ molecules of NH₃ (a) 1 and 2 (b) 1 and 3 (c) 2 and 3 (d) 1, 2 and 3

What volume of carbon dioxide is produced at STP when 5 litres of propane is burnt completely according to the equation given below? (a) 10 litres (b) 15 litres (c) 20 litres (d) 25 litres

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

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)

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.

Ethane burns in oxygen according to the chemical equation: 2C2H6 + 7O2 → 4CO2 + 6H2O If 80 ml of ethane is burnt in 300 ml of oxygen, find the composition of the resultant gaseous mixture when measured at room temperature.

Calculate: (a) The percentage of phosphorus in the fertilizer super phosphate Ca(H2PO4)2 correct to 1 decimal point. (b) Write the empirical formula of C8H18 [At. Wt. H=1, P=31, O=16, Ca=40]

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

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

An organic compound ‘X’ contains carbon, oxygen and hydrogen only. The percentage of carbon and hydrogen are 47.4% and 10.5% respectively. The relative molecular mass of ‘X’ is 76. Find the empirical formula and the molecular formula of ‘X’. [ Atomic weight: C = 12, O = 16, H = 1 ]

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.