Here are the essential concepts you must grasp in order to answer the question correctly.
Dalton's Law of Partial Pressures
Dalton's Law states that in a mixture of non-reacting gases, the total pressure exerted is equal to the sum of the partial pressures of each individual gas. This principle helps us understand how gases behave in mixtures and allows us to relate the partial pressures to the number of moles of each gas present.
Recommended video:
Dalton's Law: Partial Pressure (Simplified) Concept 3
Mole Concept
The mole concept is a fundamental principle in chemistry that relates the amount of substance to its mass and volume. One mole of any gas at standard temperature and pressure (STP) occupies the same volume, which means that the number of moles can be directly related to the number of particles, such as atoms or molecules, in a given volume.
Recommended video:
Ideal Gas Law
The Ideal Gas Law (PV=nRT) describes the relationship between pressure (P), volume (V), temperature (T), and the number of moles (n) of a gas. This law allows us to understand how changes in one variable affect the others, and it is particularly useful for comparing the behavior of different gases under the same conditions, such as in the case of helium and oxygen in this question.
Recommended video: