Final answer:
A mole of ozone does not occupy more volume than a mole of diatomic oxygen at STP; both occupy the same molar volume of 22.4 L. Therefore, there is no difference in volume at STP between these two gases.
Step-by-step explanation:
To calculate how much more volume a mole of ozone (O₃) would occupy than a mole of diatomic oxygen (O₂) at STP (Standard Temperature and Pressure), we need to use the concept of molar volume. According to Avogadro's law, at STP, every mole of any gas occupies the same volume of 22.4 liters, regardless of its molar mass.
This means that one mole of ozone and one mole of diatomic oxygen, both gases at STP, will occupy the same molar volume of 22.4 L. Therefore, there is no difference in volume between one mole of ozone and one mole of diatomic oxygen at STP, and the volume that one mole of ozone occupies is not more than the volume one mole of diatomic oxygen occupies.
The correct answer to your question is that a mole of ozone does not occupy a greater volume than a mole of diatomic oxygen at STP, so the idea of it occupying a certain number of liters more, such as 22.4 L, 11.2 L, 16.8 L, or 19.2 L more, is incorrect.