imagine two pure samples of gas in identical closed, rigid containers: gas a and gas b. gas a has a higher…

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

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

Answer

Explanation:

Step1: Understand gas pressure concept

Gas pressure is due to particle - wall collisions. Higher pressure means more force exerted on the walls. Since gas A has higher pressure, its particles exert a greater total force on the walls of the container.

Step2: Recall factors affecting gas pressure

According to the ideal gas law $PV = nRT$ (where $P$ is pressure, $V$ is volume, $n$ is the number of moles/particles, $R$ is the gas constant, and $T$ is temperature), in identical closed, rigid containers ($V$ is constant), both temperature ($T$) and the number of particles ($n$) can affect pressure. Higher temperature means more energetic particles and more collisions, and more particles mean more collisions, both leading to higher pressure.

Answer:

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