| Particle Motion 3 Facts | 1) The force acting on the container due to these collisions is at right angles to the container
2) The pressure from gas molecules may increase if there are more molecules colliding each second or if the molecules are moving faster
3) The pressure in the atmosphere (atmospheric pressure) at sea level is about 100,000 N/m2 |
| Equation for Pressure | Pressure = force ÷ area
-Pressure (N/m^2)
-force (N)
-area (m^2) |
| Relationship between Pressure and Temperature | 1) the pressure of a gas increases as its temperature increases. As a result, the gas particles will be travelling faster and will collide with the walls of the container more frequently, and with more force ∴ pressure is directly proportional to temperature
2) If the temperature of a gas stays the same, the pressure of the gas increases as the volume of its container decreases because the same number of particles collides with the walls of the container more frequently as there is less space. However, the particles still collide with the same amount of force |
| Relationship between Pressure and Volume | 1) Inversely proportional.
2) pressure × volume = constant (pressure-Pa, Volume-m^3)
3) Robert Boyle poured mercury into a J-shaped tube (sealed on the lower end). He trapped a bubble of air, the volume of mercury in the higher column, the greater the pressure on the trapped air, the smaller the it became |
| Equation for Change in Pressure | p1 × V1=p2 × V2 |
