Gases Flashcards
1
Q
What equation links pressure and temperature (pressure law)?
A
P₁ ÷ T₁ = P₂ ÷ T₂
2
Q
How does one change Celsius to kelvin and vice versa?
A
0°C = 273K
To change from Celsius to kelvin you add 273.
To change from kelvin to Celsius you minus 273.
3
Q
What equation links pressure and volume (Boyle’s Law)?
A
P₁ x V₁ = P₂ x V₂
4
Q
How is the KE of particles in a gas proportional to temperature?
A
- By increasing the temperature of a gas, one is giving the particles more energy.
- If you double the temperature (IN KELVIN), the average kinetic energy of the particles doubles.
5
Q
Brownian motion:
A
- Robert Brown observed that pollen grains in water jerk around in random movements.
- This observation can be applied to the movements of gas and liquid particles - they are moving around continually and are bumping into each other and into tiny particles (such as pollen grains).
- If there are more collisions on one side of a pollen grain than on the other, the pollen grain will change its direction or speed of movement.
6
Q
How does the motion of gas particles produce a pressure inside their container?
A
- As the gas particles move about, they are banging into each other and also the walls of their container.
- As they collide with the walls of a container, they exert a force on it and create an outward pressure.
7
Q
Why does the air pressure in tyres increase during a long car journey?
A
- The temperature of the tryes increases as there is more kinetic energy.
- The gas particles are colliding with the walls of the tyre more frequently.
- There is a greater force exerted on the walls, which means there is greater pressure.
8
Q
How does Brownian motion support the idea that matter is made from tiny particles in continuous motion?
A
- The tiny particles are hitting each other.
- This causes the larger (observable) particles to move.
- The larger particles move about randomly as a result.
