To determine which gas's molecules would exert the greatest collision force, let's carefully analyze the given data and temperature effects.
First, it's important to understand the relationship between temperature and molecular collision force. The molecular collision force in a gas is directly related to the temperature of the gas; higher temperatures cause gas molecules to move faster, resulting in more vigorous collisions with the walls of the container (this is a consequence of the kinetic molecular theory of gases).
Given the temperatures for each gas:
- Gas P: 10.2°C
- Gas Q: 25.4°C
- Gas R: 25.9°C
- Gas S: 33.2°C
We need to identify which gas has the highest temperature, as this gas's molecules will exert the greatest collision force. Let's review the temperatures:
1. Gas P has a temperature of 10.2°C.
2. Gas Q has a temperature of 25.4°C.
3. Gas R has a temperature of 25.9°C.
4. Gas S has a temperature of 33.2°C.
Comparing these temperatures, we see that the highest temperature is 33.2°C, which corresponds to Gas S. Therefore, the molecules of Gas S, being at the highest temperature, will exert the greatest collision force.
As a result, the gas whose molecules would exert the greatest collision force is Gas S.
