Question

in this simulation, you will be exploring the relationship between temperature and pressure while keeping volume constant. click here to begin. select the explore box. answer the questions as you perform the steps. 1. raise and push down the pressure pump handle to add gas molecules to the container. the initial temperature is 300 k (27°c) and the pressure has a range of 5.4 - 6.2 atm. notice the pressure values change as the particles collide with the wall. 2. click on the bucket to raise the temperature of the container to approximately 400 k (127°c). what happened to the pressure? decreased 3.5 - 4.3 atm √ approximately what pressure range did you observe? 3. click on the bucket to reduce the temperature to approximately 200 k (-73°c). what happened to the pressure? decreased approximately what pressure did you observe? stayed the same increased decreased

Explanation:

Step1: Recall the ideal - gas law

The ideal - gas law is \(PV = nRT\). When \(V\) (volume), \(n\) (number of moles), and \(R\) (gas constant) are constant, \(P\propto T\) (pressure is directly proportional to temperature).

Step2: Analyze the increase in temperature

When the temperature \(T\) increases from 300 K to 400 K, according to \(P\propto T\), the pressure \(P\) should increase.

Step3: Analyze the decrease in temperature

When the temperature \(T\) decreases from 300 K to 200 K, according to \(P\propto T\), the pressure \(P\) should decrease.

Answer:

1. When the temperature is raised from 300 K to 400 K (while keeping volume constant), the pressure increased. The initial pressure range is 5.4 - 6.2 atm and the pressure range when the temperature is 400 K is 3.5 - 4.3 atm. Since the pressure values at higher temperature are higher than the initial - state pressure values, the pressure increased.
2. When the temperature is decreased from 300 K to 200 K (while keeping volume constant), the pressure decreased.
3. When the temperature is decreased from 300 K to 200 K, the pressure decreased.