Question

imagine two pure samples of gas in identical closed, rigid containers: gas a and gas b. gas a has a higher gas pressure than gas b. which gass particles exert a greater total force on the walls of their container? gas a gas b what factors could contribute to this difference in force? select all that apply. the temperature of each gas the number of particles in each gas

Explanation:

Step1: Recall pressure - force relationship

Pressure $P=\frac{F}{A}$, where $F$ is force and $A$ is area. Since containers are identical, area $A$ is the same. Given $P_A > P_B$, from $F = P\times A$, we can conclude that the force exerted by gas A is greater.

Step2: Analyze factors affecting pressure

According to the ideal - gas law $PV = nRT$ (where $P$ is pressure, $V$ is volume, $n$ is the number of moles which is related to the number of particles, $R$ is the ideal gas constant, and $T$ is temperature), in identical closed, rigid containers ($V$ is constant), both temperature $T$ and the number of particles (related to $n$) can affect the pressure. Higher temperature or more particles can lead to higher pressure.

Answer:

First question: gas A
Second question: the temperature of each gas, the number of particles in each gas