6. Which of the following gas sample has maximum number of atoms? (A) 44.8 L of O3 at STP (B) 49.2 L of H2 at 1 atm, 300 K (C) 22.4 L of O2 at 2 atm, 546 K (D) 11.2 L of N2O at STP

To answer this question, we need to understand the concept of molar volume. At Standard Temperature and Pressure (STP), one mole of any gas occupies 22.4 L. This is known as the molar volume of a gas.

(A) 44.8 L of O3 at STP: Since 22.4 L of any gas at STP is 1 mole, 44.8 L would be 2 moles. Since O3 has 3 atoms per molecule, this sample contains 2*3 = 6 moles of atoms.

(B) 49.2 L of H2 at 1 atm, 300 K: The conditions are not at STP, so we cannot directly calculate the number of moles. We would need more information (like the ideal gas constant) to calculate this.

(C) 22.4 L of O2 at 2 atm, 546 K: Again, the conditions are not at STP, so we cannot directly calculate the number of moles. We would need more information to calculate this.

(D) 11.2 L of N2O at STP: Since 22.4 L of any gas at STP is 1 mole, 11.2 L would be 0.5 moles. Since N2O has 3 atoms per molecule, this sample contains 0.5*3 = 1.5 moles of atoms.

So, based on the information given, the gas sample with the maximum number of atoms is (A) 44.8 L of O3 at STP.