From the phet virtual lab on gas laws, determine the size of the heavy particle using the simulation tools, then relate their molecular size to something in your real world that you are familiar. Show your calculations with units clearly labeled.
The Correct Answer and Explanation is:
To determine the size of a heavy particle using the PHET virtual lab on gas laws, we can follow a method that involves applying concepts such as particle motion and ideal gas laws to understand how molecular size affects the behavior of gases.
Steps:
- Set up the Simulation:
In the PHET simulation for gas laws, you would typically choose a gas (e.g., oxygen, nitrogen, etc.). There is often an option to adjust the particle size or mass to simulate different types of gases, and the simulation will show how particles move in the gas phase under different conditions (e.g., pressure, temperature, volume). - Measure the Particle Size:
To measure the size of a heavy particle, look for a tool in the simulation that allows you to control or observe the mass and size of the molecules. These tools usually display the molecular dimensions and mass in units of atomic mass unit (amu) or kilograms. For example, if you are working with a gas like Argon, you can find that the molecular size or diameter of an Argon atom is approximately 0.37 nm (nanometers). - Use Ideal Gas Law for Calculation:
The Ideal Gas Law, PV=nRTPV = nRTPV=nRT, can help relate pressure, volume, and temperature to the number of molecules present. To determine molecular size, we often need to consider the molecular collisions and kinetic theory, which connects the behavior of gas molecules to temperature and pressure. - Relating the Size to Real-World Objects:
If the molecular size of Argon is 0.37 nm, this is still very small compared to everyday objects. To give a relatable comparison, imagine the size of a single red blood cell, which has a diameter of about 7-8 µm (micrometers), or 7000-8000 nm. So, in comparison, Argon atoms are more than 10,000 times smaller than a red blood cell. - Final Calculation:
For instance, if you wanted to calculate how many molecules fit in a small volume, you would use the ideal gas law and include the molar mass and molecular size into a derived calculation of the volume that a single molecule would occupy. This typically involves advanced methods like the Van der Waals equation, but the general takeaway is that molecular sizes in gases are on the order of nanometers, while everyday objects are orders of magnitude larger.
Conclusion:
Gas particles, even heavy ones, are extremely tiny on the molecular scale. The size of particles like Argon can be compared to something like a virus, which can be a good reference when explaining molecular sizes in gases to someone unfamiliar with atomic measurements. The size of these molecules determines how gases behave under different conditions of temperature and pressure, making them key to understanding gas laws.
