I am totally confused. Does my answer make sense or do I need to start over? The more I read it the more I doubt my answer. I am also confused when it states Please be specific. Is it looking for a specific number for the temperature and pressure or just the conditions?
Under what conditions of temperature and pressure do you think that the gas laws would work best? Please be specific.
I think that the gas laws would work best at high and low temperatures and pressures. Either high temperature and pressure or low temperatures and pressures since the gas molecules move more rapidly than standard (STP) or they move slower. Under the gas laws the molecules are held closer together at high and low temperatures causing the best conditions for them.
You are on the wrong track. The most deviation is for HIGH pressure; therefore, for the laws to work best you want low pressure and moderate temperatures (say around room T). Under the conditions you have (high P and low T), the gas molecules are CLOSER to each other and that causes them to attract each other (which the ideal gas law assumes does NOT happen) AND the volume occupied by each molecule has a larger effect (the ideal gas law assumes negligible volume).
Thanks, I will start over. I appreciate your help.
Your answer does provide some insight, but it could benefit from being more specific. When the question asks for specific conditions of temperature and pressure, it is referring to numerical values rather than just high and low ranges.
To determine the best conditions for the gas laws to work effectively, you need to consider the behavior of gases and how they relate to temperature and pressure. The gas laws, including Boyle's Law, Charles's Law, and Avogadro's Law, describe the relationships between these variables.
To find a specific temperature and pressure for the gas laws to work best, you can consider the following:
1. High temperature and low pressure: Gases behave ideally under low pressures and high temperatures. As the temperature increases, the gas molecules gain more kinetic energy, leading to increased molecular motion and collisions. Assuming the pressure is low, the gas molecules would move freely and not experience significant interactions with each other.
2. Low temperature and high pressure: Under low temperatures and high pressures, gases tend to be in a more condensed state. At low temperatures, gas molecules have lower kinetic energy, resulting in reduced motion and fewer collisions. With high pressures, the gas molecules are forced to be closer together, increasing intermolecular interactions.
Therefore, stating specific temperature and pressure values would enhance your answer. For instance, you could mention that the gas laws work best at temperatures above 500°C and pressures below 1 atm, or at temperatures below -50°C and pressures above 10 atm. These specific conditions provide a clearer understanding of the range in which the gas laws are most applicable.