Q1: The number of atoms of oxygen present in 11.2 litres of ozone (O₃) at N.T.P. are

ANS:C - 9.03 x 10²⁴

To solve this problem, we need to use Avogadro's law, which states that equal volumes of gases at the same temperature and pressure contain equal numbers of molecules. At standard temperature and pressure (NTP), which is 0°C (273.15 K) and 1 atmosphere pressure, one mole of any gas occupies 22.4 liters. Ozone (O₃) has a molar mass of approximately 48 grams per mole. So, to find the number of oxygen atoms in 11.2 liters of ozone at NTP, we first need to find the number of moles of ozone in 11.2 liters and then multiply by the number of oxygen atoms per molecule.

1. Calculate the number of moles of ozone: Volume of ozone=11.2 litersVolume of ozone=11.2liters Molar volume at NTP=22.4 liters/molMolar volume at NTP=22.4liters/mol

Number of moles of ozone=11.2 liters22.4 liters/molNumber of moles of ozone=22.4liters/mol11.2liters​ Number of moles of ozone=0.5 molesNumber of moles of ozone=0.5moles

2. Each molecule of ozone (O₃) contains 3 oxygen atoms.
3. Now, calculate the number of oxygen atoms in 0.5 moles of ozone: Number of oxygen atoms=0.5 moles×3 atoms/moleculeNumber of oxygen atoms=0.5moles×3atoms/molecule

Number of oxygen atoms=1.5 molesNumber of oxygen atoms=1.5moles

4. Finally, convert the number of oxygen atoms to atoms: Number of oxygen atoms=1.5 moles×6.02×1023 atoms/moleNumber of oxygen atoms=1.5moles×6.02×1023atoms/mole

Number of oxygen atoms=9.03×1023 atomsNumber of oxygen atoms=9.03×1023atoms So, the correct option is 9.03×10239.03×1023