Question
2. Use the particle model to explain why the pressure of a gas rises with temperature __ ..................... .................. ................ .. . .... .....
Answer
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(141 Votes)
Hugo
Elite · Tutor for 8 years
Answer
As the temperature increase, the average kinetic energy of the gas particles also increases, leading to more frequent and energetic collisions with the container walls, which in turn causes the pressure of the gas to rise, as per the particle model of gases and the ideal gas law.
Explanation
## Step 1: Understand the ConceptsRecognize that this problem relies on an understanding of the behavior of particles in a gas as dictated by the kinetic theory of gases. This theory states that particles in a gas are in constant random motion, and these movements are responsible for the pressure exerted by gas on the sides of its container. ## Step 2: Link Temperature and Pressure in GasesRecognize that according to the said theory, temperature is a measure of the average kinetic energy of the gas particles, i.e., the speed of their motion. The greater the average kinetic energy means particles on average are moving faster.## Step 3: Identify the Result Connect these insights to understand why pressure increases with temperature. As temperature (more precisely, kinetic energy) increases, the particles move more quickly and collide with the walls of their container more often. These more frequent and energetic collisions lead to an increase in tower pressure, so long as the volume or number of gas atoms does not change.### The key equation that conceptualizes this concept is the ideal gas law: ###
### When the number of particles and volume of the gas are constant, the pressure is directly proportional to its absolute temperature.