QQuestion
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
✓Answer
(b) 1 and 3
Explanation:
(1) The molar mass of O2 = 2 × atomic mass of oxygen ≈ 32 g/mol.
So, 32 grams of O2 is equivalent to 1 mole of O2. 1 mole of any gas at S.T.P. occupies 22.4 liters.
(2) 2 moles of hydrogen gas will occupy 2 x 22.4 = 44.8 litres
(3) 1 mole of NH3 contains 6.022 × 1023 molecules and occupies 22.4 liters at S.T.P. Therefore, 6.022 × 1023 molecules of NH3 will also occupy 22.4 liters at S.T.P.
Related Questions
More ICSE Easy level questions
The vapour density of CH₃OH is ............... (At. Wt. C=12, H=1, O=16) (a) 32 (b) 18 (c) 16 (d) 34
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
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]
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.
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?
Choose the correct answer from the list given below: zinc blende, C2H2, calamine, CH, haematite (a) The ore which is concentrated by magnetic separation. (b) The empirical formula of Ethyne.
Define the following terms: (a) Molar volume (b) Normal salt
Ammonia burns in oxygen as shown below. If 240 cc of ammonia is burnt in 300 cc of oxygen, find out the composition of the resultant gaseous mixture at room temperature.
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 ]
Define / State: (a) Electronegativity. (b) Gay-Lussac’s law of combining volumes.